Selection of Common Research Salts: A Task Map for Alkali Metal Salts & Alkaline Earth Metal Salts (with Product Tables 1–6)

I.Two Major Salt Families: What Are Alkali Metal Salts vs Alkaline Earth Metal Salts?

1.1 The first step in choosing a salt: distinguish M⁺ from M²⁺ (alkali vs alkaline earth)

In research and materials development, these two salt families frequently appear as the most basic sources of ions / precursors / supporting salts, for example:

1. Preparing solutions: adjusting ionic strength, serving as background electrolytes, building control systems

2. Making materials: acting as precursors (carbonates/halides/nitrates, etc.) for sintering, thin films, or solution routes

3. Electrochemistry: serving as conducting salts and sources of charge carriers (Li⁺/Na⁺/Mg²⁺/Ca²⁺ …)

They are all “salts,” but alkali metal salts typically provide monovalent cations M⁺ (e.g., Na⁺/K⁺), whereas alkaline earth metal salts typically provide divalent cations M²⁺ (e.g., Mg²⁺/Ca²⁺). The difference between +1 and +2 charge further affects solubility/hydration, coordination strength, and “structural roles” in materials.

1.2 What is a “salt”?

Chemically, a salt is a compound composed of cations and anions—this is the standard definition in the IUPAC Gold Book. When we later discuss “alkali metal salts / alkaline earth metal salts,” we are essentially discussing which element family the cation in the salt comes from.

1.3 Definitions and scope: what counts as an alkali metal salt? what counts as an alkaline earth metal salt?

A | Alkali metal salts (Alkali metal salts)

a) Alkali metals: Group 1 of the periodic table (excluding hydrogen): Li, Na, K, Rb, Cs, Fr.

b) Alkali metal salts: salts whose main cation is M⁺ (monovalent) formed by these elements (e.g., Na⁺, K⁺, Li⁺, Cs⁺, etc.).

B | Alkaline earth metal salts (Alkaline earth metal salts)

a) Alkaline earth metals: Group 2 of the periodic table: Be, Mg, Ca, Sr, Ba, Ra.

b) Alkaline earth metal salts: salts whose main cation is M²⁺ (divalent) formed by these elements (e.g., Mg²⁺, Ca²⁺, Sr²⁺, Ba²⁺, etc.).

1.4 One comparison table to tell them apart

Dimension	Alkali metal salts (Group 1)	Alkaline earth metal salts (Group 2)
Family definition	Group 1: Li/Na/K/Rb/Cs/Fr	Group 2: Be/Mg/Ca/Sr/Ba/Ra
Typical cation	M⁺ (monovalent)	M²⁺ (divalent)
“Common roles” in formulations	More often used as background salts / ionic environment / charge-carrier sources; also often serve as A-site or compensating ions in materials (depending on the system)	More often associated with bridging/crosslinking and inorganic-framework-related ions; also common as precursor sources for refractory materials, glass-ceramics, and oxide systems
Common anion families	Halides, nitrates, carbonates, phosphates, (electrolytes) PF₆⁻/TFSI⁻, etc.	Halides, nitrates, carbonates, sulfates, phosphates, etc.

Note: Be is in Group 2, but due to its high charge density and strong polarization, many beryllium halides, etc. are more covalent in character and do not follow the typical empirical intuition for “ionic M²⁺ salts.” The rules discussed here—such as “divalent ions more readily bridge/crosslink”—primarily apply to Mg/Ca/Sr/Ba systems.

II.How to choose salts: locate the task → check the cation (M⁺/M²⁺) first → then check the anion type

2.1 “Task → salt choice” navigation table

Research task / need	Recommended to look at first	Why this is prioritized (core reason)	Representative “salt keywords” (examples)
Background salt / ionic strength / solution control (avoid introducing precipitation)	Alkali metal salts first	Generally higher solubility; can stably provide ionic strength over a wider concentration range; typically weaker structural/bridging effects on the system. For the anion, prioritize types that minimally perturb the system.	NaCl, KCl, NaNO₃, KNO₃
Electrochemistry / electrolyte environment (charge carriers, conducting salts)	In most cases, alkali metal salts first	Common charge carriers are Li⁺/Na⁺/K⁺; practical success often hinges on anion chemistry and solvent compatibility	Li⁺/Na⁺ salts (further divided by system)
Need “bridging/crosslinking/hard-water ions” (materials–interface, gels/polymers, inorganic networks)	Alkaline earth metal salts first	The “divalent” nature of M²⁺ more readily produces bridging effects (under comparable conditions, it tends to “bind/bridge” more strongly than M⁺)	CaCl₂, MgCl₂, Ca(NO₃)₂, MgSO₄
Inorganic material precursors (calcination/solid-state/solution routes): target phase contains Li/Na/K or Mg/Ca/Sr/Ba	Depends on the target element	Here the salt’s role is an element source; prioritize purity, handling convenience, decomposition pathway, and whether unwanted anions are introduced	Nitrates / carbonates / halides (route-dependent)
Want certain ions to “precipitate out” or “avoid precipitation” (removal, separation, phase control)	Either family may be used, but start with anion rules	Solubility is often jointly determined by anion family + cation family; e.g., carbonates are often insoluble, while sulfates have classic exceptions	CO₃²⁻, SO₄²⁻, PO₄³⁻, etc.

Note: The electrochemical “charge carrier” depends on the system: Li/Na/K electrolytes mainly rely on Li⁺/Na⁺/K⁺, whereas multivalent systems (Mg/Ca, etc.) rely on Mg²⁺/Ca²⁺ salts and are even more sensitive to anion choice, solvent window, and coordination compatibility.

2.2 Quick empirical solubility rules (aqueous solutions at room temperature)

Scope: The following are empirical rules of thumb for common inorganic ionic compounds in water, near room temperature, under dilute-solution conditions.

1. Group 1 (alkali metal) salts are usually soluble (a similar rule often applies to NH₄⁺ salts).

i. Common exception reminder: some lithium salts (e.g., LiF, Li₂CO₃) have markedly lower solubility and should be checked individually.

2. Nitrates (NO₃⁻) are usually soluble. Chlorates/perchlorates are often soluble, but there are typical low-solubility exceptions such as KClO₄. If precipitation/separation is involved, consult solubility data specifically.

3. Carbonates (CO₃²⁻) are usually insoluble. Group 2 carbonates (e.g., CaCO₃/SrCO₃/BaCO₃) are typically insoluble; the main exceptions are Group 1 and NH₄⁺ carbonates.

i. Note: although Li₂CO₃ belongs to Group 1, it is only sparingly soluble/low-solubility and should not be treated as “fully soluble.”

4. Sulfates (SO₄²⁻) are often soluble, but BaSO₄ and SrSO₄ are usually insoluble, and CaSO₄ is often sparingly soluble/low-solubility.

2.3 Quick Reference: Anion Catalog

Anion type	Examples (alkali metal salts, M⁺)	Examples (alkaline earth metal salts, M²⁺)	Typical uses + key reminders
Halides (Cl⁻/Br⁻/I⁻)	NaCl, KCl, CsI	MgCl₂, CaCl₂, SrCl₂	Commonly used as background salts / ion sources / precursors. If the system is sensitive to halides (coordination, corrosion, side reactions), choose cautiously.
Nitrates (NO₃⁻)	NaNO₃, KNO₃	Mg(NO₃)₂, Ca(NO₃)₂	Convenient, measurable metal-ion sources in many systems; often used as an entry point for solution-based precursor routes.
Carbonates / Bicarbonates (CO₃²⁻/HCO₃⁻)	Na₂CO₃, NaHCO₃, K₂CO₃	CaCO₃, SrCO₃, BaCO₃	Common for precipitation/phase control, inorganic precursors, and fillers. Group 2 carbonates are typically low-solubility—often used as a “handle” for controlled precipitation.
Sulfates (SO₄²⁻)	Na₂SO₄, K₂SO₄	MgSO₄, CaSO₄, BaSO₄	Often used in separation, precipitation control, and inorganic system controls. Low-solubility sulfates (e.g., BaSO₄) make this a classic system for precipitation/scale studies and process control.
Phosphates (PO₄³⁻ and related)	Na₃PO₄, K₃PO₄ (also NaH₂PO₄/Na₂HPO₄, etc.)	Ca₃(PO₄)₂	Frequently form low-solubility precipitates or show strong coordination/buffering effects—useful for precipitation control, inorganic framework construction, and buffer formulations. Distinguish acid salts vs normal salts (e.g., NaH₂PO₄/Na₂HPO₄/Na₃PO₄): their use cases and effective pH ranges differ substantially.
Organic acid salts (acetates, etc.)	CH₃COONa, CH₃COOK	Ca(CH₃COO)₂, Mg(CH₃COO)₂	Often used as milder ion sources / coordination environments. Organic anions may participate in complexation or reactions; mechanism-sensitive systems should evaluate these effects.

III.Alkali Metal Salts (Alkali metal salts): Find representative salts and common uses by anion type

3.1 Anion-type index: representative alkali metal salts and selection notes

Anion type	Common representative alkali metal salts	Common uses (typical roles)	Selection notes (risks / cautions)
Halides (Cl⁻/Br⁻/I⁻)	LiCl, NaCl, KCl; CsI/CsBr	Background electrolyte / ionic-strength controls; halide sources and materials precursors (crystals, films, solution routes)	Halides may trigger precipitation in systems containing certain metal ions (e.g., Ag⁺/Pb²⁺/Hg₂²⁺) or participate in coordination/corrosion/side reactions. Systems sensitive to halides should be handled cautiously.
Nitrates (NO₃⁻) (and chlorates/perchlorates)	LiNO₃, NaNO₃, KNO₃	Common soluble salts and carriers for metal-ion sources; controls in solution chemistry and precipitation reactions	Nitrates are often “general-purpose soluble salts.” If using chlorates/perchlorates, pay attention to oxidizing properties and safety/compliance requirements.
Weak-acid anions such as acetates/bicarbonates (AcO⁻/HCO₃⁻)	CH₃COONa, CH₃COOK; NaHCO₃	Mild ion sources; formulation salts / buffer-related systems; tuning the solution environment	May participate in acid–base and complexation equilibria. In mechanism-sensitive or “as inert as possible” systems, evaluate anion effects.
Sulfates (SO₄²⁻)	Na₂SO₄, K₂SO₄	Inorganic salt controls; separation/precipitation-control studies; building ionic environments	If Ba²⁺/Sr²⁺/Ca²⁺/Pb²⁺, etc. are present, adding SO₄²⁻ may trigger low-solubility sulfate precipitation. This can be used for precipitation/separation; if clarity is required, avoid such combinations.
Carbonates & phosphates (CO₃²⁻ / PO₄³⁻) (incl. acid phosphates)	Na₂CO₃, K₂CO₃; Na₃PO₄, K₃PO₄ (also NaH₂PO₄/Na₂HPO₄, etc.)	“Alkalinity reserve/acid scavenging,” precipitation driving and separation tools; inorganic material precursor routes; phosphates also used in buffers/formulations	CO₃²⁻/PO₄³⁻ cause many metal ions to form low-solubility salts and precipitate. Most alkali salts are soluble, but some lithium salts (e.g., Li₂CO₃, Li₃PO₄) have low solubility and must be checked separately. For phosphates, distinguish acid salts vs normal salts (different uses and pH ranges).
Hydroxides (OH⁻)	LiOH, NaOH, KOH, CsOH	Strong bases: pH adjustment, dissolution/etching, reaction driving (alkali treatment, precipitation formation, etc.)	Strongly reactive reagents, typically not used as background salts. Assess material compatibility and safety requirements.
Weakly coordinating fluorinated anions for electrolytes (PF₆⁻/TFSI⁻/FSI⁻/BF₄⁻, etc.)	LiPF₆, LiTFSI (expandable: LiFSI, LiBF₄; Na/K analogs)	Electrochemistry/device-grade conducting salts: influence ionic conductivity, interphase film/stability, temperature window, and solvent matching	The core is overall compatibility across salt–solvent–moisture/impurities–interfaces, plus regulatory/safety requirements. Compatibility differs greatly between anions; for fluorinated weakly coordinating anions in particular, moisture and impurity control is critical.

3.2 Three high-frequency application threads: the three most common roles of alkali metal salts in research

Application thread (scenario)	Real-world task / pain point	Common salt keywords	Why they’re commonly used	Selection notes (avoid misuse)
A. Solution chemistry & separation: using salts as the “ionic environment / precipitation tool”	Need a stable, reproducible ionic strength; or use precipitation to achieve separation / build controls	Background salts: NaCl/KCl, NaNO₃/KNO₃; Precipitation drivers: carbonates / phosphates / hydroxides	From empirical solubility rules: Group 1 salts and nitrates are usually soluble, making them suitable as background electrolytes and quantifiable ion sources; whereas CO₃²⁻ / PO₄³⁻ / OH⁻ are often used to drive precipitation or shift equilibria	For a “background salt,” prioritize counterions with minimal interference; CO₃²⁻ / PO₄³⁻ / OH⁻ will strongly alter pH, complexation, and precipitation equilibria, and are not suitable when you “only want to provide an ionic background.”
B. Energy electrochemistry: the conducting salt defines the electrolyte window and interfacial stability	Need high ionic conductivity, a stable interphase (SEI/CEI), temperature-range compatibility; and strict control of water/impurities	LiPF₆, LiTFSI (extensions: LiFSI, LiBF₄; corresponding Na/K analogs)	In Li-ion battery electrolytes, LiPF₆ has long been the mainstream/dominant conducting salt (despite issues such as moisture sensitivity and decomposition); the anion family directly links to conductivity and interfacial reaction pathways	The key is overall compatibility of salt–solvent–moisture–interface. Even with the same cation, changing the anion can produce completely different behavior. For fluorinated weakly coordinating anions, moisture and impurity control is especially critical.
C. Perovskites / optoelectronic devices: Cs⁺/Li⁺ salts as “composition and electronic-property tuning” components	Improve phase stability and defect/interfacial electronics; or increase transport-layer conductivity and device efficiency	A-site / mixed-cation: Cs salts (e.g., CsI/CsBr precursor salts); Device additives: LiTFSI, etc.	Commonly reported in papers and monographs: introducing Cs⁺ into mixed-cation perovskites can improve phase stability and photo/thermal stability; all-inorganic CsPbI₃ is also a major branch (many studies focus on black-phase stabilization and device performance). Meanwhile LiTFSI is a common dopant salt for hole-transport layers such as Spiro-OMeTAD	These uses are more sensitive to purity, water content, and metal impurities. The same salt can have very different specification requirements depending on whether it is used as a precursor or as a device additive.

IV. Alkaline Earth Metal Salts: quickly locate representative salts and common uses by anion type

4.1 Anion-type index: representative alkaline earth metal salts and selection pointers

Anion type	Representative alkaline earth metal salts	Common uses (typical roles)	Selection pointers (common risks / notes)
Halides Cl⁻/Br⁻/I⁻	MgCl₂, CaCl₂, SrCl₂, BaCl₂	Common M²⁺ ion sources and for constructing ionic environments in inorganic systems/interfaces; CaCl₂ is also widely used for dehumidification/drying	Some halides (especially CaCl₂) are strongly hygroscopic/deliquescent, making weighing, storage, and moisture control more demanding
Nitrates NO₃⁻	Mg(NO₃)₂, Ca(NO₃)₂, Sr(NO₃)₂, Ba(NO₃)₂	Frequently used soluble M²⁺ precursors (common in solution processing / sol–gel / impregnation routes)	Nitrates are generally highly soluble; however, in heating/thermal treatment routes, consider their thermal decomposition pathways and NOₓ release (process and safety assessment)
Sulfates SO₄²⁻	MgSO₄, CaSO₄, SrSO₄, BaSO₄	Used for precipitation separation / controlled precipitation / scale (fouling) controls; also common in inorganic materials and filler systems	Sulfates include classic low-solubility exceptions (e.g., BaSO₄, SrSO₄, CaSO₄). In the presence of other divalent ions, precipitation may be triggered. BaSO₄ is nearly insoluble in water and is a typical filler
Carbonates CO₃²⁻	MgCO₃, CaCO₃, SrCO₃, BaCO₃	High-frequency inorganic fillers/precursors (carbonate routes, thermal decomposition to oxides, etc.); also used for controlled precipitation and phase control	Carbonates tend to be poorly soluble (Group 1 and ammonium salts are common exceptions), so they are often used as an entry point for selective precipitation/precursors
Phosphates PO₄³⁻ (and related)	Ca₃(PO₄)₂ (hydroxyapatite, etc.)	Common in low-solubility phases, inorganic frameworks, biomineralization and ceramic routes	Most phosphates are poorly soluble or readily form sparingly soluble phases; in solution systems, pay attention to how pH and coordination environment affect precipitation and phase transformation
Hydroxides OH⁻	Mg(OH)₂, Ca(OH)₂, Ba(OH)₂	Used to set alkaline conditions, generate precipitates, and for inorganic reactions/material treatments	Hydroxides strongly reshape the system (pH/precipitation/complexation), so they are usually not used as “background salts.” Most M²⁺ hydroxides have limited solubility (sparingly soluble/insoluble category)

4.2 Four high-frequency application threads: typical “roles” of alkaline earth metal salts in research and processing

Application thread	Core pain point (real-world problem)	Representative salts / keywords	Key mechanism / advantage	Selection notes
A. Moisture removal and humidity control: reducing water content in a system	The system/sample is water-sensitive; need to reduce residual water in air or solutions	CaCl₂ (strongly hygroscopic/deliquescent), anhydrous MgSO₄ (drying organic phases)	CaCl₂ absorbs moisture and can deliquesce, so it is often used as a drying/dehumidifying material. Anhydrous MgSO₄ is a common drying agent in organic workups, removing trace water from organic layers by forming hydrates	The anhydrous vs hydrated form and actual water content directly determine drying capacity. Also, CaCl₂ can have poor compatibility with certain functional groups/solvents in some organic systems (choose a more suitable drying agent for the specific system)
B. Precipitation control and separation: selectively forming sparingly soluble salts	Need to selectively remove ions, build precipitation controls, or evaluate scaling risk	BaSO₄ (extremely low solubility), SrSO₄/CaSO₄ (low solubility); CaCO₃-related precipitation/scaling is also common	BaSO₄ has extremely low solubility and is a representative system for sulfate precipitation and scaling studies. Among alkaline earth sulfates, BaSO₄ and SrSO₄ are poorly soluble, while CaSO₄ is sparingly soluble, making them useful for selective precipitation separation and phase-control comparisons	With the same anion, solubility can differ greatly across M²⁺. Barium salts generally require stricter safety and compliance assessment (toxicity/disposal)
C. Inorganic materials precursors: providing a measurable M²⁺ element source	Need measurable, processable, phase-transformable sources of Mg/Ca/Sr/Ba (solution routes or solid-state routes)	Solution precursors: nitrates (Mg(NO₃)₂/Ca(NO₃)₂/Sr(NO₃)₂/Ba(NO₃)₂), some halides/acetates; Solid-state precursors: carbonates (CaCO₃/SrCO₃/BaCO₃, etc.)	Many oxide/carbonate/silicate/ceramic systems rely on M²⁺ supply. Choosing the anion is essentially choosing the pathway of dissolution → decomposition → residual impurities / gas release (e.g., nitrates often serve as an entry point for solution processing; carbonates are common in solid-state routes and as fillers/precursors)	Nitrates involve thermal decomposition and NOₓ during heat treatment—process and safety must be assessed. For solid-state routes, consider how particle size, purity, and hydration state affect phase transformation and sintering
D. Ionic bridging and crosslinking: using M²⁺ to “bridge” and stabilize structures	Hydrogels/interfacial layers/polyelectrolyte systems need higher mechanical strength or a more stable network	Ca²⁺–alginate (“egg-box”); Sr²⁺/Ba²⁺ and other divalent-ion crosslinking systems	In polysaccharide systems such as alginate, Ca²⁺-induced ionic crosslinking is often described by the classic egg-box model, a reproducible divalent-ion bridging mechanism	Crosslinking strength depends strongly on ion type, concentration, diffusion, and release rate (different salts differ in solubility and ion-release behavior). Distinguish whether you are choosing a salt to set an ionic environment or to trigger gelation via crosslinking

V. Product Navigation Table | Alkali Metal Salts & Alkaline Earth Metal Salts: quickly locate Tables 1–6 by “research task”

Research context / experimental need	Which table to check first	Why start with this table	Representative “salt keywords” in the table
Build background electrolyte / ionic strength / osmolarity controls: want “stable, reproducible, and avoid introducing extra reactions”	Table 1. Basic background salts & ionic strength	Table 1 concentrates the most commonly used “ionic-environment scaffold salts” (Cl⁻/NO₃⁻/SO₄²⁻/CO₃²⁻ with Na⁺/K⁺/Mg²⁺/Ca²⁺), ideal for constructing reproducible ionic strength and control systems	NaCl, KCl, NaNO₃, KNO₃, MgCl₂·6H₂O, CaCl₂·2H₂O, Na₂SO₄, Na₂CO₃, K₂CO₃
Prepare media / buffer systems: need stable pH, controllable ionic environment, or need chelation/complexation to stabilize metals	Table 2. Buffering / chelating / coordinating anions	Table 2 groups anions that participate in acid–base, complexation, and buffering equilibria (phosphates, bicarbonate, acetates, citrates, EDTA, borates), best suited for formulation and ionic management in media/culture systems	PBS-related: NaH₂PO₄/Na₂HPO₄; phosphate pair: KH₂PO₄/K₂HPO₄; NaHCO₃; NaOAc/KOAc; sodium citrate; EDTA-2Na; borax
Control precipitation / phase / separation: want certain ions to “precipitate out,” study scaling or dissolution–precipitation equilibria; or run carbonate/sulfate/fluoride routes for inorganic materials as comparisons	Table 3. Precipitation / phase control & materials precursors	Table 3 gathers classic “low-solubility / controllable precipitation” families (carbonates, sulfates, fluorides) plus Ca–P (calcium phosphate) endpoints on the materials side—good for solubility, crystallization, filler/precursor and phase-comparison work	CaCO₃, SrCO₃, BaCO₃; CaSO₄·2H₂O, SrSO₄, BaSO₄; CaF₂, MgF₂; β-TCP, HA
Moisture-sensitive / trace-impurity-sensitive systems: need “anhydrous/ultra-dry/high-purity” halide salts as ion sources or controls (materials, coordination chemistry, electrolyte pretreatment, etc.)	Table 4. High-purity anhydrous/ultra-dry halides	Table 4 is dedicated to halide salts with reproducible moisture control (ultra-dry/anhydrous Li/Cs/Rb and Mg/Ca salts), ideal for systems with stricter requirements on water, metal impurities, and repeatability	LiCl (anhydrous, high purity), CsCl (anhydrous, high purity), LiBr, LiI (ultra-dry), CaBr₂ (ultra-dry), CsBr (ultra-dry), RbBr (ultra-dry), MgBr₂ (ultra-dry)
Electrochemistry / electrolytes: study ionic conduction, solvation, interphases (SEI/CEI), salt–solvent windows; need comparisons across PF₆⁻/TFSI⁻/FSI⁻/BF₄⁻/OTf⁻/borate systems (including multivalent Mg²⁺/Ca²⁺)	Table 5. Conducting salts for electrochemistry/electrolytes	Table 5 covers mainstream and comparison electrolyte anion systems, including cross-cation (Li⁺/Na⁺/K⁺) and cross-valence (Mg²⁺/Ca²⁺) controls—aligned with the electrochemistry logic that “salt chemistry sets the window and the interphase”	LiPF₆, KPF₆, NaPF₆; LiTFSI/NaTFSI; LiFSI/NaFSI; LiBF₄/NaBF₄; LiOTf; LiBOB, LiODFB; Ca(TFSI)₂, MgTFSI
Method development / reaction controls: need strong acid/base environments, redox conditions, deoxygenation/reduction, or analytical titration systems (not merely ionic strength)	Table 6. Common salts for reactions/analysis (acid–base / redox / deoxygenation / complexation)	Table 6 focuses on functional salts that significantly alter system chemistry (strong bases, oxidants, reducing/deoxygenating salts, nitrites, etc.), useful for mechanistic and methodological controls—different from the “as-inert-as-possible background salts” in Table 1	NaOH, KOH; Na₂SO₃, Na₂S₂O₃·5H₂O; NaNO₂; KMnO₄; NaBH₄; NaH

Table 1 | Basic background salts & ionic strength (high-frequency general use: Cl⁻/SO₄²⁻/CO₃²⁻/NO₃⁻)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkali metal salts | Sodium salts (Na⁺) | Halide (Cl⁻)	7647-14-5	C111542	Sodium chloride	For plant cell culture, ≥99.5%	A benchmark salt for osmolarity/ionic strength: a common component in plant/cell culture media; also used as a control in salt effects, solubility/coordination studies, and protein stability experiments.
Alkali metal salts | Potassium salts (K⁺) | Halide (Cl⁻)	7447-40-7	P112144	Potassium chloride	For cell culture, ≥99.5%	A typical K⁺ supplement/osmolarity-adjusting salt: commonly used in cell culture; also a basic “background electrolyte” and ionic-strength control salt in electrochemistry and solution chemistry.
Alkali metal salts | Sodium salts (Na⁺) | Nitrate (NO₃⁻)	7631-99-4	S111648	Sodium nitrate (precursor/explosive-regulated)	Premium grade reagent, ≥99%	A common Na⁺/NO₃⁻ source and oxidizing inorganic salt: used in analytical chemistry, ionic-strength/background electrolyte controls, oxidizing systems, and formulation comparisons; note strong oxidizer/regulatory risk—handle, store, and ship in compliance.
Alkali metal salts | Potassium salts (K⁺) | Nitrate (NO₃⁻)	7757-79-1	P111633	Potassium nitrate (precursor/explosive-regulated)	Premium grade reagent, ≥99%	A common K⁺/NO₃⁻ source: used to construct solution ionic environments, formulation controls, analytical work, and salt-effect studies in materials/electrochemical systems; strong oxidizer/regulatory risk—observe safety and compliance.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Nitrate (NO₃⁻)	13477-34-4	C100078	Calcium nitrate tetrahydrate (precursor/explosive-regulated)	For plant cell culture, ≥99%	A typical Ca²⁺ supplement salt: a common calcium source in plant media; NO₃⁻ tends to be less prone to forming sparingly soluble salts/precipitates and is relatively mild in many systems—useful for anion-effect controls; oxidizing salt with labeled risk—ensure compliance.
Alkaline earth metal salts | Magnesium salts (Mg²⁺) | Halide (Cl⁻)	7791-18-6	M116335	Magnesium chloride hexahydrate	For cell culture; for insect cell culture; ≥99% (T)	A typical Mg²⁺ supplement salt: commonly used in cell/insect media, supporting enzyme activity and nucleic-acid-related processes while maintaining ionic balance; also used in inorganic precipitation/complexation and salt-effect controls.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Halide (Cl⁻)	10035-04-8	C118444	Calcium chloride dihydrate	For cell culture; for insect cell culture; for plant cell culture; ≥99%	A typical Ca²⁺ source: supports ionic balance and physiological processes in cell/insect/plant culture; also used to supply Ca²⁺ in inorganic reactions and to regulate precipitation/crosslinking (e.g., alginate crosslinking).
Alkali metal salts | Sodium salts (Na⁺) | Sulfate (SO₄²⁻)	7757-82-6	S112289	Sodium sulfate, anhydrous	For plant cell culture, ≥99%	A common SO₄²⁻/Na⁺ source and ionic-strength adjustment salt: used as an inorganic-salt component in media, formulation controls, and salt-effect studies; the anhydrous form is also common in baseline inorganic-salt control systems.
Alkali metal salts | Sodium salts (Na⁺) | Carbonate (CO₃²⁻)	497-19-8	S432764	Sodium carbonate	Anhydrous grade; premium grade reagent; suitable for analysis	A typical basic carbonate and alkalinity/carbonate source: used for alkalization, precipitation/carbonate-system studies, analytical and standardization controls; the anhydrous grade helps control water content and improve reproducibility.
Alkali metal salts | Potassium salts (K⁺) | Carbonate (CO₃²⁻)	584-08-7	P485463	Potassium carbonate	Anhydrous grade; high purity; reagent grade; ≥99%	A commonly used basic carbonate/carbonate source: used for alkalization, inorganic precipitation, and salt-effect controls; also used as a mild base in organic synthesis (relevant for K⁺ salt-environment comparisons).

Table 2 | Buffering / chelating / coordinating anions (phosphates / bicarbonate / acetates / citrate / EDTA / borates)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkali metal salts | Sodium salts (Na⁺) | Bicarbonate (HCO₃⁻)	144-55-8	S118660	Sodium bicarbonate	For cell culture; for insect cell culture; ≥99.5%	A typical HCO₃⁻ buffer salt: used with CO₂ systems in cell culture to maintain pH; also a benchmark salt for carbonate systems and gas–liquid equilibrium studies.
Alkali metal salts | Potassium salts (K⁺) | Phosphate (H₂PO₄⁻)	7778-77-0	P113042	Potassium dihydrogen phosphate	For plant cell culture, ≥99%	A common phosphorus source and buffer-pair component: forms a phosphate buffer system with K₂HPO₄; supplies P and K in media and is used for ionic-strength and pH-window controls.
Alkali metal salts | Potassium salts (K⁺) | Phosphate (HPO₄²⁻)	7758-11-4	D433945	Dipotassium hydrogen phosphate	Anhydrous grade; premium grade reagent; suitable for analysis	A common basic component of phosphate buffer pairs: forms a phosphate buffer with KH₂PO₄; used as a pH and ionic-environment control in analysis/media/formulations.
Alkali metal salts | Sodium salts (Na⁺) | Phosphate (H₂PO₄⁻)	7558-80-7	S108343	Sodium dihydrogen phosphate, anhydrous	For cell culture; for insect cell culture; ≥99% (T)	A common phosphorus source and acidic component of buffer pairs: forms PBS/phosphate-buffer systems with Na₂HPO₄; used for media and ionic-environment controls, pH-window studies, and phosphate effects.
Alkali metal salts | Sodium salts (Na⁺) | Phosphate (HPO₄²⁻)	7558-79-4	S118441	Disodium hydrogen phosphate, anhydrous	For cell culture; for insect cell culture	A common basic component of phosphate buffer pairs: paired with NaH₂PO₄ to form PBS; used to maintain pH, supply phosphate, and provide an ionic-strength background—suited for buffer systems and phosphate-effect controls.
Alkali metal salts | Sodium salts (Na⁺) | Acetate (AcO⁻)	127-09-3	S118648	Sodium acetate, anhydrous	For cell culture; for insect cell culture; ≥99%	A common acetate buffer/carbon-source control: used for formulation buffer systems, ionic-strength adjustment, and methodological controls; can serve as an acetate source in biological systems (set concentration based on the specific system design).
Alkali metal salts | Potassium salts (K⁺) | Acetate (AcO⁻)	127-08-2	P485461	Potassium acetate	Anhydrous grade; ACS; ≥99%	A common acetate buffer/mildly basic salt: used for formulations, ionic-strength and anion-effect controls; also used as an acetate and potassium source in synthesis.
Alkali metal salts | Sodium salts (Na⁺) | Citrate (Cit³⁻)	6132-04-3	S434901	Sodium citrate dihydrate	Pharmaceutical grade, PharmPure™	A common buffer/chelating/stabilizing agent: used in formulations and methods for pH buffering, metal-ion chelation, improved stability, and ionic-environment tuning; pharmaceutical grade is suitable for cleaner, impurity-controlled comparisons.
Alkali metal salts | Sodium salts (Na⁺) | Chelator salt (EDTA-2Na)	6381-92-6	E118596	Disodium EDTA dihydrate	For plant cell culture, ≥99%	A typical chelator salt (EDTA-2Na): chelates trace metals in media, stabilizes metal-ion activities, and reduces metal-induced precipitation/deactivation; commonly used in trace-element systems and metal-contamination control.
Alkali metal salts | Sodium salts (Na⁺) | Borate (tetraborate)	1303-96-4	S112464	Sodium tetraborate decahydrate (borax)	Chemical pure (CP), ≥99%	A typical borate buffer / glass and flux-system salt: used in borate buffers, glass/glaze and flux comparisons; also used in ionic-strength and complexation-effect studies.

Table 3 | Precipitation / phase control & materials precursors (carbonates / sulfates / fluorides / calcium–phosphate materials)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Carbonate (CO₃²⁻)	471-34-1	C432742	Calcium carbonate	Premium grade; precipitated; for silicate analysis	A common Ca²⁺/carbonate source: precipitated CaCO₃ is used for silicate analysis and as a benchmark control; also used as a filler/mineral-phase reference and for studies on carbonate–acid reactions and buffering systems.
Alkaline earth metal salts | Strontium salts (Sr²⁺) | Carbonate (CO₃²⁻)	1633-05-2	S759099	Strontium carbonate	For optical glass	A typical Sr²⁺ precursor for glass/ceramics: used in optical-glass and functional-ceramic formulations (as a control for refractive-index and structure tuning); also used for comparisons within alkaline earth carbonates.
Alkaline earth metal salts | Barium salts (Ba²⁺) | Carbonate (CO₃²⁻)	513-77-9	B759101	Barium carbonate	For optical glass	A typical Ba²⁺ glass raw material/flux and refractive-index modifier: used in optical-glass/ceramic formulations; also serves as a comparison material in carbonate systems and across alkaline earth metals.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Sulfate (SO₄²⁻)	10101-41-4	C431227	Calcium sulfate dihydrate	Suitable for analysis; premium grade; precipitated calcium sulfate	A representative sulfate precipitate phase: used for sulfate analysis and precipitation controls; also widely used in dissolution–precipitation equilibrium, ionic-strength effects, and polymorph/particle-size comparisons.
Alkaline earth metal salts | Strontium salts (Sr²⁺) | Sulfate (SO₄²⁻)	7759-02-6	S112897	Strontium sulfate	Chemical pure (CP)	A common Sr²⁺ sulfate precipitate/reference material: used for solubility, precipitation/crystallization, and materials-system comparisons; also used for homologous comparisons with CaSO₄ and BaSO₄.
Alkaline earth metal salts | Barium salts (Ba²⁺) | Sulfate (SO₄²⁻)	7727-43-7	B112376	Barium sulfate	PrimorTrace™, ≥99.99% metals basis	An ultra-pure sulfate precipitate phase / inert filler reference: used for sulfate precipitation and solubility studies, scattering/filler controls, and trace-metal-sensitive systems.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Fluoride (F⁻)	7789-75-5	C104253	Calcium fluoride	PrimorTrace™, ≥99.99% metals basis	An ultra-pure Ca²⁺/F⁻ material salt: a common optical/window material and a reference for inorganic fluoride systems; also used in fluoride precipitation/dissolution studies and trace-impurity-sensitive research.
Alkaline earth metal salts | Magnesium salts (Mg²⁺) | Fluoride (F⁻)	7783-40-6	M108388	Magnesium fluoride	PrimorTrace™, ≥99.99% metals basis	An ultra-pure inorganic fluoride material: commonly used for optical coatings/window materials and as a reference in fluoride systems; suitable for trace-impurity-sensitive optical/materials research.
Alkaline earth metal salt system | Calcium–phosphate (Ca–P) materials | β-tricalcium phosphate	7758-87-4	C139914	β-Tricalcium phosphate	Biomedical grade, ≥98%, β-phase basis, < 70 μm	A typical bioresorbable calcium-phosphate ceramic: used in bone-repair materials, tissue-engineering scaffolds, dissolution/mineralization kinetics, and biomineralization controls; the particle-size specification helps with sintering/forming and consistency in surface reactions.
Alkaline earth metal salt system | Calcium–phosphate (Ca–P) materials | Hydroxyapatite	1306-06-5	H306080	Hydroxyapatite (HAw)	Circular disks, diameter 11 ± 1 mm; thickness 3 ± 0.5 mm	A typical calcium-phosphate mineral phase (bone-/enamel-like): used for biomineralization, bone-repair material/coating controls, protein/ion adsorption and release-control studies; the disk format is convenient for evaluating surface reactions and film formation/deposition.

Table 4 | High-purity anhydrous / ultra-dry halides (moisture control & reproducibility: common in materials/coordination/moisture-sensitive systems)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkali metal salts | Lithium salts (Li⁺) | Halide (Cl⁻)	7447-41-8	L130112	Lithium chloride	Anhydrous grade, 99.99% metals basis	A high-purity Li⁺ source: used in electrochemistry/materials (including lithium-containing systems) and as a high-purity inorganic-salt reference; the anhydrous, high-purity grade is suitable for moisture-sensitive and trace-impurity-sensitive formulations and mechanistic studies.
Alkali metal salts | Cesium salts (Cs⁺) | Halide (Cl⁻)	7647-17-8	C433762	Cesium chloride	Anhydrous grade; high purity; reagent grade; ≥99.9% metals basis	A high-purity Cs⁺ source: used in materials chemistry (e.g., halide/perovskite additives and controls), high-ionic-strength systems, and density-gradient methods; anhydrous high purity suits moisture-sensitive and trace-impurity-sensitive research.
Alkali metal salts | Lithium salts (Li⁺) | Halide (Br⁻)	7550-35-8	L433600	Lithium bromide	Anhydrous grade; high purity; reagent grade; ≥99%	A high-purity Li⁺/Br⁻ source: used for inorganic/materials and electrochemical salt-effect controls; LiBr is also common as a strongly hydrophilic salt in high-ionic-strength systems (sensitive to moisture and formulation windows—moisture control is required).
Alkali metal salts | Lithium salts (Li⁺) | Halide (I⁻)	10377-51-2	L753625	Lithium iodide	Ultra-dry grade, PrimorTrace™, ≥99.99% metals basis	An ultra-dry, high-purity Li⁺/I⁻ source: used as a control in moisture-sensitive and trace-metal-sensitive systems (electrochemistry, electrolytes, coordination chemistry, and materials precursors). I⁻ is prone to oxidation (iodine release); store sealed and protect from light.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | Halide (Br⁻)	7789-41-5	C283864	Calcium bromide	PrimorTrace™, ultra-dry grade, ≥99.99% metals basis	An ultra-dry, high-purity Ca²⁺/Br⁻ source: used in moisture-sensitive systems and for electrochemistry/materials and halide-ion-effect controls; suitable for trace-metal-sensitive experiments (trace metals basis).
Alkali metal salts | Cesium salts (Cs⁺) | Halide (Br⁻)	7787-69-1	C292202	Cesium bromide	PrimorTrace™, ultra-dry grade, ≥99.99% metals basis	An ultra-dry, high-purity Cs⁺/Br⁻ source: used for materials doping/halide-ion controls and high-ionic-strength systems; suited for reproducible studies sensitive to moisture and impurities.
Alkali metal salts | Rubidium salts (Rb⁺) | Halide (Br⁻)	7789-39-1	R290979	Rubidium bromide	PrimorTrace™, ultra-dry grade, ≥99.99% metals basis	An ultra-dry, high-purity Rb⁺/Br⁻ source: used for within-group alkali-metal comparisons, ionic-radius effects, lattice/phase stability, and halide-ion-effect studies.
Alkaline earth metal salts | Magnesium salts (Mg²⁺) | Halide (Br⁻)	7789-48-2	M290956	Magnesium bromide	PrimorTrace™, ultra-dry grade, ≥99.99% metals basis	An ultra-dry, high-purity Mg²⁺/Br⁻ source: used for coordination chemistry/solvation and electrochemical salt-effect controls; especially important for moisture-sensitive systems.

Table 5 | Conducting salts for electrochemistry/electrolytes (PF₆⁻/TFSI⁻/FSI⁻/BF₄⁻/OTf⁻/BOB/ODFB + multivalent controls)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkali metal salts | Lithium salts (Li⁺) | PF₆⁻ electrolyte salt	21324-40-3	L777368	Lithium hexafluorophosphate	Electronic grade, ≥99.99% trace metals basis	A typical Li-battery electrolyte salt: used for ionic-conduction studies in non-aqueous electrolytes; electronic grade/low trace metals are critical for electrochemical stability windows and side-reaction control (strict moisture control required).
Alkali metal salts | Potassium salts (K⁺) | PF₆⁻ electrolyte salt	17084-13-8	P104056	Potassium hexafluorophosphate	≥99.98% metals basis	A high-purity PF₆⁻ electrolyte salt: used for electrochemistry/electrolyte and ionic-conduction studies; PF₆⁻ is often used as a weakly coordinating anion control (strict moisture control required).
Alkali metal salts | Sodium salts (Na⁺) | PF₆⁻ electrolyte salt	21324-39-0	S759713	Sodium hexafluorophosphate (SHFP)	≥99.9% metals basis	A high-purity PF₆⁻ salt: used for electrolyte and ionic-conduction controls; enables comparisons of Na⁺ vs K⁺/Li⁺ in electrolyte solvation and transport.
Alkali metal salts | Lithium salts (Li⁺) | TFSI⁻ electrolyte salt	90076-65-6	B398978	Lithium bis(trifluoromethanesulfonyl)imide (LiTFSI)	≥99.9%	A classic lithium salt with a large weakly coordinating anion: used in electrolytes/polymer electrolytes and ion-transport studies; often used as an alternative/control vs LiPF₆ (consider moisture and corrosive side reactions in system design).
Alkali metal salts | Sodium salts (Na⁺) | TFSI⁻ electrolyte salt	91742-21-1	S161091	Sodium bis(trifluoromethylsulfonyl)imide (NaTFSI)	≥98% (T)	A commonly used sodium salt with a large weakly coordinating anion: used for sodium-battery electrolytes/ion transport and anion-effect controls; can be paired with LiTFSI for same-anion cross-cation comparisons.
Alkali metal salts | Lithium salts (Li⁺) | FSI⁻ electrolyte salt	171611-11-3	L157764	Lithium bis(fluorosulfonyl)imide	≥98% (T)	A commonly used high-conductivity electrolyte salt: used in electrolytes and ion-transport studies; compared with TFSI, the anion structure differs—useful for interface/solvation comparisons (moisture control is important).
Alkali metal salts | Sodium salts (Na⁺) | FSI⁻ electrolyte salt	100669-96-3	S161088	Sodium bis(fluorosulfonyl)imide (NaFSI)	≥98%	A commonly used sodium-battery electrolyte salt: used for Na⁺ transport and electrochemical-window studies; comparison with NaTFSI helps evaluate how anion structure affects interphases/stability.
Alkali metal salts | Lithium salts (Li⁺) | BF₄⁻ electrolyte salt	14283-07-9	L432081	Lithium tetrafluoroborate	Anhydrous grade, ≥98%, acid < 200 ppm	A commonly used electrolyte salt/weakly coordinating anion system: used in electrochemistry and non-aqueous ion conduction; low-acidity specification helps reduce side reactions (more friendly to acid-sensitive systems).
Alkali metal salts | Sodium salts (Na⁺) | BF₄⁻ weakly coordinating salt	13755-29-8	S118606	Sodium tetrafluoroborate	PrimorTrace™, ≥99.99% metals basis	An ultra-pure BF₄⁻ salt: BF₄⁻ is relatively weakly coordinating and is often used in coordination/electrochemistry and ionic-strength background controls; suitable for trace-metal-sensitive systems.
Alkali metal salts | Lithium salts (Li⁺) | OTf⁻ weakly coordinating salt	33454-82-9	L398970	Lithium trifluoromethanesulfonate	≥99.5%	A commonly used lithium salt with a weakly coordinating anion: used for electrochemistry, electrolytes, and Lewis-acid/coordination-system controls; relatively stable and convenient for studying anion effects.
Alkali metal salts | Lithium salts (Li⁺) | Borate electrolyte (BOB⁻)	244761-29-3	L120347	Lithium bis(oxalato)borate (LiBOB)	≥99% metals basis	A commonly used electrolyte additive / SEI-film-forming salt and control: used in battery electrolyte research and interphase stability evaluation; also useful for comparing how anion structure affects solvation and interfacial reactions.
Alkali metal salts | Lithium salts (Li⁺) | F-containing borate electrolyte (ODFB⁻)	409071-16-5	L303675	Lithium difluoro(oxalato)borate (LiODFB)	≥99%	A common electrolyte “hookup”/interphase-film-forming comparison salt: used to study how F-containing borate anions influence interphase chemistry and stability; suitable for comparisons with LiBOB/LiPF₆.
Alkaline earth metal salts | Calcium salts (Ca²⁺) | TFSI⁻ electrolyte salt	165324-09-4	C153286	Calcium bis(trifluoromethylsulfonyl)imide (Ca(TFSI)₂)	≥98%	A representative divalent-metal TFSI salt: used for multivalent (Ca²⁺) electrolytes and solvation/coordination studies; suitable for comparing divalent vs monovalent cations under the same anion in transport and coordination behavior.
Alkaline earth metal salts | Magnesium salts (Mg²⁺) | TFSI⁻ electrolyte salt	133395-16-1	M157949	Magnesium bis(trifluoromethylsulfonyl)imide (Mg(TFSI)₂)	≥97% (T)	A representative Mg²⁺ electrolyte salt: used for magnesium-battery/multivalent-ion transport and solvation–coordination studies; easy to run cross-valence comparisons alongside Li/Na/Ca TFSI salt systems.

Table 6 | Common salts for reactions/analysis (acid–base / redox / deoxygenation / complexation: for controls & methodology)

Category	CAS No.	Aladdin Cat. No.	Name	Grade / purity	Product features & applications
Alkali metal salts | Sodium salts (Na⁺) | Hydroxide (OH⁻)	1310-73-2	S111498	Sodium hydroxide	Premium grade reagent, ≥96%	A typical strong base/alkalinity adjuster: used for pH adjustment, saponification/hydrolysis, inorganic precipitation, and surface cleaning; in salt-system studies, often used to control how “alkaline conditions” affect speciation and precipitation pathways.
Alkali metal salts | Potassium salts (K⁺) | Hydroxide (OH⁻)	1310-58-3	P431767	Potassium hydroxide	Anhydrous grade, ≥99.95% metals basis	A high-purity strong base: used for pH/alkalinity adjustment, hydrolysis/saponification, and inorganic precipitation; anhydrous high purity suits moisture-sensitive systems and trace-impurity-sensitive alkalization controls.
Alkali metal salts | Sodium salts (Na⁺) | Sulfite (SO₃²⁻)	7757-83-7	S433921	Sodium sulfite	Anhydrous grade, reagent grade, ≥98%	A common reducing salt / deoxygenation and antioxidant control: used to remove dissolved oxygen, scavenge oxidizing impurities, and in analysis and formulation stability research; also used as a control for how “reducing environments” affect speciation in salt systems.
Alkali metal salts | Sodium salts (Na⁺) | Thiosulfate (S₂O₃²⁻)	10102-17-7	S431245	Sodium thiosulfate pentahydrate	European Pharmacopoeia (Ph.Eur); suitable for analysis; ACS; premium grade	A typical reducing/complexing salt: widely used for iodometric titrations, dechlorination/reduction controls, and complexing metal ions such as Ag⁺; used to assess how a “reducing environment / complexing anion” affects system behavior.
Alkali metal salts | Sodium salts (Na⁺) | Nitrite (NO₂⁻)	7632-00-0	S433708	Sodium nitrite	Anhydrous grade; high purity; reagent grade; ≥99%	A common NO₂⁻ source: used for diazotization/nitrosation reactions, analytical work, and corrosion/passivation system controls; note reactivity and safety practices (avoid improper mixing with strong acids/amines).
Alkali metal salts | Potassium salts (K⁺) | Permanganate (MnO₄⁻)	7722-64-7	P485670	Potassium permanganate (precursor/explosive-regulated; precursor/drug-control flagged)	For analysis (max 0.000005% mercury column); premium grade reagent; ACS	A typical strong oxidant and benchmark reagent for redox titration/analysis: used in redox titrations, digestion/oxidation, and methodological controls; high-risk/regulatory-related chemical—ensure compliance and strict safety handling.
Alkali metal salts | Sodium salts (Na⁺) | Borohydride (BH₄⁻)	16940-66-2	S432207	Sodium borohydride (precursor/explosive-regulated)	purum p.a., ≥96% (gas-volumetric)	A typical hydride reducing agent: used to reduce metal salts/organic functional groups; in salt-system studies, often used to control how a “reducing environment” affects true species and side reactions; strict safety and compliance required.
Alkali metal salts | Sodium salts (Na⁺) | Hydride (H⁻)	7646-69-7	S110860	Sodium hydride	60% dispersion in mineral oil	A strong base/strong reducing reagent: used for deprotonation and anhydrous synthesis; in the “salt/metal-precursor” context, can be used to create strongly basic conditions or reduction controls; mineral-oil dispersion lowers pyrophoric risk but strict moisture/oxygen control is still essential.

Note: The above are representative Aladdin products. For more specifications, please refer to the product list at the end of the article or search the Aladdin website using the “product name / CAS / catalog number.”

Aladdin: https://www.aladdinsci.com/

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