I | Background and Basic Definitions
1.1 Background: Why “precious metal salts” show up in research
1. In research and materials development, many “precious metals” do not enter a system as metal ingots or powders. Instead, they are introduced as salts or ionic coordination salts (ionic coordination salts) that serve as a measurable, soluble, and transformable metal source—often referred to as a “precursor.”
2. These precursors then undergo dissolution, ligand exchange, redox transformation, or deposition, ultimately becoming the active species or solid phase you actually need (e.g., catalytic active sites, thin films, nanoparticles). This explains why “the same metal” can behave very differently when supplied as different salts and/or with different coordinating counterions.
3. From an applications perspective, platinum-group metals (PGMs) have long been essential elements in catalysis and high-reliability material systems, widely used at scale in automotive exhaust catalytic converters, chemical/refining catalysis, electronics, and electrochemical fields. Therefore, in R&D, selecting and stably controlling an appropriate metal precursor (salt/complex) is often the foundation for reproducibility and scalability.
1.2 First, define the scope of “precious metals” here
1. In Chinese usage, “precious metals” typically refers to gold, silver, and platinum-group metals (PGMs: Pt, Pd, Rh, Ir, Ru, Os).
2. In English-language sources, two related but not identical terms are common:
a) noble metals (chemically inert/corrosion-resistant metals): emphasizes chemical properties such as oxidation and corrosion resistance; the exact set of elements included is not strictly consistent across disciplines.
b) precious metals: more of a set defined by scarcity and economic value/application; in commodities and investment contexts, gold, silver, platinum, and palladium are often treated as the main precious metals.
3. To avoid confusion, when this article says “precious metal salts,” it mainly focuses on salts/ionic coordination salt precursors commonly used in research and materials contexts: Au, Ag, Pt, Pd, and other PGMs.
1.3 What does “salt” mean here?
1. In chemical terminology, the core definition of a “salt” is clear: a compound assembled from cations and anions.
2. However, in precious-metal systems, the “anions/cations” in many “precious metal salts” are not simple small ions, but coordination ions (e.g., ions with coordination shells such as PtCl6PtCl₆PtCl6²⁻ and AuCl4AuCl₄AuCl4⁻). In notation, square brackets are commonly used to indicate the “coordination sphere/coordination scope,” which is a key convention in inorganic nomenclature.
3. A helpful way to think about it is:
Precious metal salts often carry two layers of information simultaneously: charge pairing (salt) + coordination environment (coordination chemistry). The coordination environment often determines solubility, stability, ease of reduction, and the real chemical species that form after entering the system.
Note: In this article, “precious metal salts” is a research-oriented umbrella term that includes ionic complex salts, acidic precursors, and commonly used neutral complexes (e.g., acac complexes). The core focus is how they behave as real species after being introduced into a system.
1.4 A key concept that is easy to miss — “real species in the system”
1. After a precious metal salt enters a specific solvent/ligand/acid–base/redox environment, the metal center typically does not persist as a single chemical substance. Instead, it distributes and evolves among a set of interconvertible species (e.g., different oxidation states, coordination structures, complexed/hydrolyzed forms). Under certain conditions, it may also form aggregates or be reduced to the metallic state (e.g., metal(0) species / nanoscale forms).
2. IUPAC defines speciation as: the distribution of an element among defined chemical species in a system. The definition of “chemical species” depends on the experimental timescale and detection method: if two forms interconvert slowly within your experimental time window and can be separately observed/distinguished, they can be treated as different species; if they interconvert rapidly within that window and behave as a single ensemble, they can be treated as the same species.
3. In this article, “real species in the system” means the set of metal forms that actually exist—on your experimental conditions and timescale—and that dominate reaction/deposition/nucleation behavior (usually more than one). This must be made explicit because solubility, stability, reducibility, and whether active sites or deposited phases form are often determined by the distribution and evolution of these real species, rather than solely by the “name of the purchased salt/complex.”
II | Core Logic for Selection & Troubleshooting: Turning a “precursor” into a reproducible system starting point
2.1 Compress the variables into three “control knobs”
Precious-metal systems can look complex, but the core variables that actually push speciation around usually fall into just three categories: metal center and oxidation state, coordination shell/counterion, and medium conditions. What you can read on the label generally maps to these three.
Control knob | What you can often see on the label | What it typically affects |
Metal center & oxidation state | Au/Pd/Pt/Rh…; (I)/(II)/(III)/(IV) | Redox window and transformation pathways; propensity to form M(0)/nanophases; affinity to ligands/substrates |
Coordination shell / counterion | Cl⁻, NO₃⁻, OAc⁻; complex anions such as [MCl₄]²⁻/[MCl₆]²⁻; relatively weakly coordinating anions (BF₄⁻/PF₆⁻/OTf⁻, depending on the system) | Solubility and stability; ligand-exchange rate; tendency for side reactions (especially “hidden variables” introduced by halides or strongly coordinating anions) |
Medium conditions | Solvent/water content, pH, ligand identity and equivalents, reductants/oxidants, light/air exposure, etc. | How speciation evolves: whether hydrolysis/complexation/aggregation/precipitation/reduction occurs, to what extent, and how fast |
Key point:
The precursor name is only the “starting input.” What truly determines system behavior is the real-species starting point jointly defined by the three knobs.
2.2 Use “four questions” to turn selection into a decision order
Define the task → define the acceptable speciation window → choose precursor and counterion → finally, use the lowest-cost validation to lock in the starting point.
Four questions | Core information you must answer | Most common pitfall |
Q1 What is the target task? | Catalysis/deposition/nucleation/analytical standard/coordination synthesis… (different tasks require different speciation) | Treating “the same metal” as “the same use,” and ignoring task-specific requirements for species form and stability window |
Q2 What will the medium drive it into? (start from the system) | Whether solvent/water/pH/ligands/redox environment will cause hydrolysis, complexation, aggregation, reduction, or precipitation | Buying the reagent first and only then thinking about the system; when results deviate, blaming only “operation issues” instead of returning to speciation for troubleshooting |
Q3 Which metal center and oxidation state do you need as the starting point? | Whether the activation/reduction pathway you want is achievable (e.g., Pt(IV)→Pt(0) via impregnation–reduction vs Pt(II) via ligand exchange) | Looking only at the element and ignoring oxidation state, leading to entirely different pathways |
Q4 Will the coordination shell/counterion become a “hidden variable”? | Whether Cl⁻/OAc⁻/NO₃⁻/TFA⁻ etc. change solubility, exchange, corrosion/side reactions, or introduce strong-coordination interference | Treating the counterion as mere background; in practice it often determines “dissolves or not, stable or not, exchanges or not” |
Remark:
Q2 and Q4 are essentially asking the same thing: after the precursor is introduced, what form does it actually exist as? Differences in solubility, activity, deposition/nucleation, particle size, and reproducibility often start right here.
2.3 A universal “minimum validation” workflow: verify system stability first, then lock a reproducible starting point
Validation step (increasing evidence strength) | What you are confirming (mapped to the three knobs) | “Continue” signal (experience-based) | If abnormal, troubleshoot first (priority order) |
Step 1 Record solubility/clarity/color (same batch, same concentration, same solvent; label time points) | Impact of “shell/counterion + medium conditions” on the initial species ensemble | Clarity is reproducible; no persistent turbidity/flocs/obvious precipitation within the target time window | Change the medium first: water content, pH, ligand equivalents, whether halides/reductants/light are introduced; then consider hydrolysis/aggregation/reduction |
Step 2 Run a blank control (no substrate/support/electrode; keep only metal precursor + key ligands/acid–base/conducting salt) | Whether the medium alone can “push speciation away” | Blank remains stable within the target time window (appearance and key readout do not drift) | If the blank is unstable, first lock down the medium knobs (pH, ligand identity & equivalents, halides, redox environment, air/light) |
Step 3 Choose one task-matched fast readout (so changes have evidence) | Whether new species/secondary phases/new deposition pathways appear | Signal is repeatable and trends are interpretable | If signal drifts: first check whether new species/secondary phases form; then check formulation and operational consistency |
Step 4 Lock the reproducible experimental starting point | Whether key variables are pinned down to a “repeatably executable” level | You can explicitly write and execute: concentration, solvent/water content, pH, ligand equivalents, addition order, time window (and note stable appearance/readout) | If key parameters are missing or each run relies on “feel/experience” → return to the three knobs and pin them down one by one |
Reminder:
Color/clarity can only serve as an “early warning signal.” It cannot by itself identify oxidation state or structure. Its value is in quickly indicating that metal species in the system may be transforming (e.g., via hydrolysis, complexation, aggregation, or reduction).
2.4 Fast-readout reference table (for confirming whether the “system species starting point” is stable)
Experimental task (example scenario) | Fast readout (macroscopic observation + one simple measurement) | Decision point: did speciation transform / did a secondary phase appear (is the starting point reproducible)? |
Gold nanoparticles / colloids | Macroscopic: color/turbidity/precipitation/phase separation; Simple: UV–Vis (SPR peak position/intensity/width drift) | Whether Au(0) colloids have formed and whether aggregation occurs; whether trends are reproducible |
Electrochemical deposition / plating bath | Macroscopic: turbidity/precipitation/abnormal gassing; Simple: CV or polarization curve (is the window stable) | Whether the deposition window is stable; whether complexation/side reactions change speciation and deposition pathways |
Homogeneous catalysis precursor small trial | Macroscopic: whether the blank (precursor + key ligands/acid–base only) changes color/turbidity/precipitates; Simple: choose one “key reading” from a baseline trial (conversion/yield/selectivity/gas volume/color metric, etc.) | Whether new species/deactivated species form rapidly; whether anion/ligand differences change the pathway |
Impregnation for supported catalysts (Pt/Pd, etc.) | Macroscopic: whether the impregnation supernatant becomes turbid/precipitates, and whether the support changes color; Simple: compare halide trend in wash/supernatant (Cl⁻ for chloride complexes; for non-chloride systems use one of conductivity/metal residue) | Whether hydrolysis/precipitation or premature reduction occurs; whether key-component residue trends are controllable and reproducible (affecting loading and batch-to-batch consistency) |
III | Grouped by Research Task: Turning the “System Speciation Starting Point” into a Selection & Troubleshooting Checklist
3.1 Rapid precursor selection by research task: target outcome → speciation starting point → key variables → fast validation → common failure causes
Task type (scenario) | Target outcome that must be stable | Common in-system starting forms (examples) | Key variables (the three knobs) | Recommended fast validation readouts | Common failure causes |
A Homogeneous catalysis / organic synthesis precursors (mainly Pd/Pt/Rh/Ir/Ru) | The reaction runs; activity/selectivity are reproducible; condition screening is comparable | Metal precursors that can be converted into the intended active species under reaction conditions (common: Pd(II) carboxylates/halides/β-diketonates; certain reactions use Rh(II) dimers, etc.) | Metal & oxidation state (sets the pathway) + anion/shell (strongly coordinating? affects exchange) + solvent/ligand/redox environment (does it drive deactivation/precipitation/metalization?) | Blank control (precursor + key ligand/base/acid only) + baseline small trial under benchmark conditions (same time window) | Treating “same metal” as “same use”; ignoring anion/halide effects; the blank is already generating a secondary phase but it goes unnoticed |
B Supported catalysis / impregnation–reduction / nanomaterial preparation | Particle size/dispersity/loading are controllable and consistent across batches; nucleation pathway is reproducible | Typical chloroacids/complex salts (e.g., Pt(IV) chloroacids/salts; Au(III) chloroauric acid/salts) converted on reductant/stabilizer/support into M(0)/nanophases | Oxidation state & reducibility + shell (especially halide coordination) + pH/reductant/stabilizer/water content (controls hydrolysis/aggregation/reduction rate and nucleation mode) | Au: UV–Vis (SPR peak/drift) + appearance stability; Pt: before/after impregnation comparison (supernatant/color/support changes), and if needed a halide-trend comparison | Using a “salt as a stand-in for metal powder”; pH/water content cause hydrolysis/precipitation; tiny changes in reductant/stabilizer shift the nucleation pathway |
C Electrochemical deposition / thin films / surface metallization | Coating composition, density, deposition rate, and process window are stable | Stable complexed metal species in the bath (common: Au(III) or Au(I) complex systems; Pt/Pd chloro-complex systems, etc.) | Metal oxidation state & complex form + electrolyte/supporting salt & anions + acidity/pH and complexing agents (set the electrodeposition window and side reactions) | Bath appearance stability (turbidity/precipitation) + quick CV/polarization scan of the operating window | Overlooking corrosion/compatibility issues from “chloro-complex + strong acid”; the bath is actually slowly hydrolyzing/aggregating, causing window drift |
D Analytical chemistry / standards & methodological controls (mainly Ag) | Quantification is reliable; blanks and recoveries are interpretable; interferences are controlled | Ag⁺ as a controllable reactive ion (precipitation/complexation/redox); or insoluble silver salts as controls | Concentration & calibration + interfering ions & matrix + pH/indicator/complexant | Calibration/blank/spike-recovery (same matrix) | Treating “a precipitate appears” as the only conclusion; ignoring interferences such as Br⁻/I⁻/S²⁻ and matrix complexation effects |
Reminder:
Different task types mean you are not stabilizing the same thing—some require “reducible with controllable nucleation,” some require “a stable bath window,” and some require “quantification with explainable interferences.” Therefore, “the same metal” ≠ “the same selection logic.”
IV | Product Navigation Table | Precious Metal Salts: Quickly Locate Tables 1–3 by “Research Task / Experimental Need”
Research task / experimental need (typical scenario) | Recommended table to check first | Table-selection logic (why start here) | Representative products in the table (examples) |
Silver salts for halide abstraction/activation: “pull X⁻ out” from metal chloro/bromo/iodo complexes to generate cationic metal species/cationic intermediates (catalytic activation, coordination chemistry, ion-pair effects) | Table 1 | Silver-salt systems (Ag) | The chemical essence is Ag⁺ binding halides to form AgX precipitates, coupled with weakly coordinating anions (BF₄⁻/PF₆⁻/OTf⁻) to stabilize/balance the resulting cationic species; Table 1 concentrates these “halide-abstraction” silver salts. | Silver tetrafluoroborate, silver hexafluorophosphate, silver trifluoromethanesulfonate (silver triflate) |
Analysis/titration/general Ag source: quantitative use or basic controls (analytical chemistry, surface modification, silver precursors) | Table 1 | Silver-salt systems (Ag) | The core need is “usable as a standard Ag source / controllable ionic strength / compatible with analytical readouts”: Table 1 includes AgNO₃ (common in analysis/titration) and inorganic controls such as Ag₂O/Ag₂SO₄ that better match analytical and baseline characterization tasks. | Silver nitrate, silver oxide, silver sulfate, silver acetate |
Heterogeneous Ag source / easy workup: prefer filterable silver reagents and lower solution residues (method/process friendly) | Table 1 | Silver-salt systems (Ag) | The key is “deliver Ag function in an immobilized/insoluble form,” then recover via solid–liquid separation after reaction; Table 1 provides supported silver salts, matching process needs for “easy separation / low residue.” | Supported silver carbonate |
Gold nanomaterials / gold surface modification / Au precursor reduction routes: need Au(III) reducible to Au(0) in aqueous media/system (nano-Au, surface gold plating/metallization) | Table 2 | Gold-salt systems (Au) | These tasks require “stable, soluble Au(III) chloroauric acid / chloroaurate salts” that can be reduced on a surface or by reductants to form Au(0); Table 2 focuses on typical Au(III) precursors such as HAuCl₄ and NaAuCl₄·xH₂O. | Chloroauric acid (HAuCl₄), sodium tetrachloroaurate (hydrate) |
Au(I)/Au(III) oxidation-state and halide-ligand effect controls: gold coordination chemistry / catalytic precursor routes (oxidation-state control, halide-ligand differences) | Table 2 | Gold-salt systems (Au) | The key is that starting oxidation state and halide ligation can alter ligand exchange and reaction channels; Table 2 includes both Au(I) halides and Au(III) halides/chloroauric systems, enabling direct oxidation-state/halide-ligand comparison. | Gold(I) chloride, gold(III) chloride, gold bromide |
Cyanide-complex gold systems (gold electroplating / strongly complexing environments): need Au(I)–CN complex as a stable Au source | Table 2 | Gold-salt systems (Au) | This relies on Au(I) cyanide complexes to provide stable gold species and a specific process window; Table 2 includes the corresponding products to match “cyanide-complex system” needs (with safety and waste-disposal compliance considered in parallel). | Potassium dicyanoaurate(I) |
General Pd catalysis precursors: cross-coupling / C–H activation / condition scouting and ligand screening (establish a working Pd system first) | Table 3 | PGMs and related transition precious-metal salts (Pt/Pd/Rh/Ir/Ru) | The core is selecting a commonly used Pd(II) precursor that can convert into active Pd species under reaction conditions; Table 3 concentrates Pd “entry points” such as carboxylates/halides/TFA salts/complexes for mechanism- and solubility-driven choice. | Palladium(II) acetate, palladium(II) chloride, palladium(II) trifluoroacetate, Pd(acac)₂ |
Pd/Pt chloro-complex salt systems: ligand exchange / solution equilibria / electroplating or deposition precursors (explicit chloro-complex anion forms) | Table 3 | The key variable is the metal existing as chloro-complex anions such as MCl4MCl₄MCl4²⁻ / MCl6MCl₆MCl6²⁻, which govern ligand exchange, reduction/deposition behavior, and ionic-strength effects; Table 3 concentrates K₂PdCl₄/Na₂PdCl₄/K₂PtCl₄/K₂PtCl₆, etc. | Potassium tetrachloropalladate(II), sodium tetrachloropalladate(II), potassium tetrachloroplatinate(II), potassium hexachloroplatinate(IV) |
Pt(II)/Pt(IV) oxidation-state routes and Pt nanoparticle/supported-catalyst precursors: need reducible/impregnable precursors or oxidation-state controls | Table 3 | The essence is choosing precursors around Pt oxidation state and coordination shell: Pt(IV) chloroplatinic acid/salts are often used for impregnation followed by reduction to Pt(0), while Pt(II) halides/ammine complexes are better for coordination chemistry and controlled transformations; these are centralized in Table 3. | Chloroplatinate salts (ammonium/potassium/hydrates), platinum(II) chloride, platinum(IV) chloride, tetraammineplatinum(II) salts, Pt(acac)₂ |
Organometallic precursors / film deposition / nanoparticle thermolysis routes: focus on solubility, thermal decomposition, and impurity control (acac route) | Table 3 | These tasks often need β-diketonate (acac) complexes as soluble metal sources suitable for thermolysis/deposition; Table 3 covers Pt/Pd/Rh/Ir/Ru acac precursors to enable horizontal comparisons under the same processing window. | Pt(acac)₂, Pd(acac)₂, Rh(acac)₃, Ir(acac)₃, Ru(acac)₃ |
Ultra-high purity / trace-metal background control: ICP/trace analysis controls, ultra-low contamination preparation, devices/materials sensitive to impurities | Table 3 | The key is minimizing metal impurity backgrounds; prioritize metals basis ultra-high purity or prepared high-purity metal-solution precursors; Table 3 includes PrimorTrace series and high-purity salts aligned with trace and contamination control. | Palladium(II) nitrate solution; tetraamminepalladium(II) nitrate solution (PrimorTrace); high-purity Rh/Pt(acac), etc. |
Rh(II) dirhodium dimers: specific catalysis types such as carbene/nitrene transfer (strong reaction-type dependence) | Table 3 | This is not “any rhodium source”: it requires a Rh(II) dirhodium carboxylate platform with characteristic reactivity; Table 3 includes representative catalytic salts directly matching these mechanisms and reaction scopes. | Dirhodium(II) acetate dimer |
Ir/Ru coordination and redox/electrochemical precursors: need defined Ir(III)/Ir(IV) and Ru(III) starting points or oxidation-state controls | Table 3 | The core is explicit oxidation state and chloro-ligation environment: e.g., Ir(IV) chloro-complex salts for redox/electrochemical controls; Ir(III)/Ru(III) halides for coordination chemistry and subsequent ligand functionalization; Table 3 groups these for oxidation-state-driven selection. | Iridium(III) chloride hydrate, potassium hexachloroiridate(IV), ruthenium(III) chloride hydrate, Ir/Ru(acac) |
Table 1 | Silver Salt Systems (Ag): Inorganic Salts / Weakly Coordinating Silver Salts / Supported Silver Sources
Category | CAS No. | Aladdin Cat. No. | Product name | Specification / Purity | Product features & applications (related to precious-metal salts) |
Silver salts | Silver oxide / oxidant & analytical silver source | 20667-12-3 | Silver oxide | For elemental analysis | A commonly used silver source / mild oxidant and an analytical silver compound: can serve as a halide scavenger and a silveration reagent source; also used as a silver precursor in materials and catalysis research; frequently used in elemental analysis contexts as well. | |
Silver salts | Nitrate / analytical reagent & general Ag source | 7761-88-8 | S433976 | Silver nitrate (explosive precursor) | European Pharmacopoeia (Ph.Eur), suitable for analysis, ACS, superior grade | Classic analytical-grade AgNO₃: used for titration/analysis, surface modification, and as a precursor for silver nanomaterials, etc.; strongly oxidizing and regulated (labeled as an “explosive precursor”), requiring strict safety and compliance management in research use. |
Silver salts | Sulfate / low-solubility Ag source | 10294-26-5 | Silver sulfate | puriss., ≥99% | A relatively low-solubility silver salt: can be used as an Ag source and control in specific solvents/systems (ionic strength, coordination/precipitation behavior), and is also used in some oxidation- and halide-scavenging-related studies. | |
Silver salts | Carboxylate Ag source / synthesis & surface chemistry | 563-63-3 | Silver acetate | AR, ≥99.5% | A commonly used soluble silver source: for halide scavenging, silveration/oxidation methodology, and studies of silver additives in metal catalysis (e.g., promoting halide departure / generating cationic species). | |
Silver salts | Cyanide silver salt / electroplating & complexation precursor | 506-64-9 | Silver cyanide | ≥99% | AgCN is a typical strongly coordinating silver salt: widely used in silver electroplating and silver complex chemistry; cyanide-containing systems require strict safety/compliance and waste-handling procedures (do not operate under non-professional conditions). | |
Silver salts | Supported silver reagent / heterogeneous Ag source | 534-16-7 | Supported silver carbonate | extent of labeling: ~50 wt. % loading | An immobilized silver salt: facilitates solid–liquid separation and reduces handling complexity; useful for synthesis and methodology studies requiring a “heterogeneous Ag source / halide scavenging / mild silveration environment.” | |
Silver salts | Weakly coordinating silver salt (BF₄⁻) / halide abstraction activation | 14104-20-2 | Silver tetrafluoroborate | Suitable for synthesis | A classic weakly coordinating anion silver salt: commonly used to “abstract Cl⁻/Br⁻/I⁻” to generate cationic intermediates or cationic metal complexes, for catalyst activation, coordination chemistry, and halide-abstraction in organic synthesis. | |
Silver salts | Weakly coordinating silver salt (PF₆⁻) / halide abstraction activation | 26042-63-7 | Silver hexafluorophosphate | PrimorTrace™, ≥99.99% metals basis | A high-purity weakly coordinating silver salt: for halide abstraction, construction of cationic metal complexes, catalyst activation, and ion-pair effect studies; well suited to fine coordination/catalysis systems. | |
Silver salts | Weakly coordinating silver salt (OTf⁻) / strongly activating Ag source | 2923-28-6 | Silver trifluoromethanesulfonate | ≥99.98% metals basis | AgOTf is a widely used strongly activating silver salt: for halide abstraction, generation of cationic intermediates/metal complexes, and promoting certain electrophilic activations and coordination-chemistry constructions; higher purity benefits mechanistic work and reproducibility. |
Table 2 | Gold Salt Systems (Au): Chloroauric Acid / Gold Halides / Cyanide Gold Complexes
Category | CAS No. | Aladdin Cat. No. | Product name | Specification / Purity | Product features & applications (related to precious-metal salts) |
Gold salts | Chloroaurate salt (Au(III)) / electroplating & nano-Au precursor | 13874-02-7 | Sodium tetrachloroaurate dihydrate | Au 48–50% | A typical Au(III) chloro-complex salt: used for electroplating/surface gold plating, preparation of Au nanomaterials (reduction route), and coordination chemistry; the sodium salt form is convenient for aqueous formulation and system-to-system comparisons. | |
Gold salts | Chloroauric acid (Au(III)) hydrate / nano-Au & surface-chemistry precursor | 16961-25-4 | Chloroauric acid trihydrate | ≥99.9% metals basis | HAuCl₄·xH₂O is among the most widely used Au(III) precursors: for Au nanomaterial synthesis (reduction route), surface functionalization, and coordination chemistry; higher purity supports reproducibility in optical/catalysis studies. | |
Gold salts | Gold(I) halide / coordination precursor | 10294-29-8 | Gold(I) chloride | ≥99.9% metals basis | A commonly used Au(I) halide precursor: for building Au(I) complexes (e.g., linear coordination systems), as a Au(I) source in catalysis/materials research, and for oxidation-state controls. | |
Gold salts | Gold(III) halide / Lewis acid & precursor | 13453-07-1 | Gold(III) chloride | ≥99.9% metals basis | An Au(III) halide precursor: for Au(III) complex synthesis, Lewis-acid/halogenation studies, and materials-precursor routes; condition controls are needed for systems sensitive to water/ligands. | |
Gold salts | Gold halide (bromide) / coordination precursor | 10294-28-7 | Gold bromide (AuBr₃) | ≥99% | A gold bromide precursor: for gold complex chemistry, halide-system comparisons, and materials-precursor research; compared with chlorides, often used to probe halide-ligand effects and reactivity differences. | |
Gold salts | Gold(I) cyanide salt / gold electroplating & coordination chemistry | 13967-50-5 | Potassium dicyanoaurate(I) | ≥99.95% metals basis, Au ≥67.6% | A classic Au(I) cyanide complex salt: widely used in gold electroplating and Au(I) coordination chemistry; contains cyanide ligands—research use requires strict safety and waste-handling compliance (not recommended for non-professional environments). |
Table 3 | Platinum-Group and Related Transition Precious-Metal Salts (Pt/Pd/Rh/Ir/Ru): Inorganic Halides / Chloro-complex Salts / β-Diketonate (acac) / High-Purity Solutions
Category | CAS No. | Aladdin Cat. No. | Product name | Specification / Purity | Product features & applications (related to precious-metal salts) |
Platinum salts | Inorganic halide precursor (Pt(II)) | 10025-65-7 | Platinum(II) chloride | Pt basis ≥73% | A typical Pt(II) halide precursor: used to synthesize Pt complexes and catalytic systems (subsequent ligation/reduction to active species), and also as a starting point for thin-film/material precursor studies. | |
Platinum salts | Ammine complex (Pt(II)) / coordination chemistry & precursor | 13933-32-9 | Tetraammineplatinum(II) chloride (anhydrous) | Pt 58.0% | A classic Pt(II) ammine complex salt: used in coordination chemistry, ligand-exchange reactions, and Pt complex construction; often chosen when a “stable, controllable Pt(II) coordination starting point” is needed. | |
Platinum salts | Inorganic halide precursor (Pt(IV)) | 13454-96-1 | Platinum(IV) chloride | Pt ≥57% | A Pt(IV) halide precursor: used for Pt(IV)/Pt(II) complex synthesis, redox chemistry controls, and materials-precursor routes (reducible to Pt species). | |
Platinum salts | Chloroplatinate salt (Pt(IV)) / recovery precipitation & catalytic precursor | 16919-58-7 | Ammonium chloroplatinate | Pt ≥43.4% | A common chloroplatinate salt: used for Pt recovery/separation (precipitation/salt conversion) and as an intermediate for preparing H₂PtCl₆, K₂PtCl₆ and related chloroplatinate systems; also used for catalyst-precursor preparation. | |
Platinum salts | Chloroplatinic acid (Pt(IV)) hydrate / bio & materials precursor | 18497-13-7 | Chloroplatinic acid hexahydrate | BioReagent | H₂PtCl₆·6H₂O is among the most widely used Pt(IV) chloroacids: commonly used for Pt catalyst impregnation/loading (reduction to Pt nanoparticles) and as an electrochemical materials precursor; the BioReagent grade suits studies more sensitive to biological context/impurities. | |
Platinum salts | High-purity ammine complex (Pt(II)) / precursor & control | 20634-12-2 | Tetraammineplatinum(II) nitrate | ≥99.995% metals basis | A high-purity Pt(II) ammine complex: for coordination chemistry and subsequent ligand-exchange synthesis; better suited when a low-impurity, controllable Pt(II) starting point is needed (device/material precursors). | |
Platinum salts | β-Diketonate (acac) precursor | 15170-57-7 | Platinum(II) acetylacetonate | PrimorTrace™, ≥99.99% metals basis | High-purity Pt(acac)₂: commonly used as a precursor for Pt thin films/nanoparticles, thermolysis/deposition studies, and coordination chemistry; helps reduce impurity introduction in device/material research. | |
Platinum salts | Potassium chloroplatinite (Pt(II)) / coordination & electroplating precursor | 10025-99-7 | Potassium tetrachloroplatinate(II) | ≥99.9% metals basis, Pt ≥46% | A Pt(II) chloro-complex salt (K₂PtCl₄ type): used for Pt(II) coordination chemistry and synthetic precursors; also used for electroplating/deposition and as a control in materials systems. | |
Platinum salts | Potassium chloroplatinate (Pt(IV)) / high-valent precursor | 16921-30-5 | Potassium hexachloroplatinate(IV) | ≥99.9% metals basis | A Pt(IV) chloroplatinate salt (K₂PtCl₆ type): used for high-valent Pt coordination chemistry, precursor routes reducible to Pt(II)/Pt(0), and controls in electrochemical materials studies. | |
Palladium salts | Catalytic precursor (carboxylate) | 3375-31-3 | Palladium(II) acetate (47% Pd) | Suitable for synthesis | One of the most commonly used Pd(II) catalytic precursors for cross-coupling/C–H activation, etc.; readily generates active Pd species in situ—useful as a general Pd source to “get a reaction working” and as a baseline for ligand screening. | |
Palladium salts | Inorganic halide precursor (Pd(II)) | 7647-10-1 | Palladium(II) chloride | Reagent grade, high purity, ≥99% | A classic Pd(II) salt: used to synthesize Pd complexes for cross-coupling/coordination chemistry, and also for electroplating/deposition and materials-precursor studies; suitable as an inorganic Pd control. | |
Palladium salts | Ultra-high-purity solution precursor / trace analysis & contamination control | 10102-05-3 | Palladium(II) nitrate solution | PrimorTrace™, ≥99.999% metals basis, 10 wt.% in 10 wt% nitric acid | An ultra-high-purity Pd solution precursor: suitable for ICP/trace-metal background control, doping/deposition precursors, and high-purity formulation; “metals basis” supports comparable controls in trace-level systems. | |
Palladium salts | Ultra-high-purity ammine complex solution / trace & deposition precursor | 13601-08-6 | Tetraamminepalladium nitrate solution | PrimorTrace™, ≥99.99% metals basis, 10 wt.% in H₂O | A high-purity Pd(II) ammine-complex solution: a more “coordination-stabilized” Pd(II) solution precursor, convenient for thin-film/deposition, analytical controls, and low-contamination formulation research. | |
Palladium salts | Chloropalladate salt (Pd(II)) / complexes & electroplating precursor | 13820-53-6 | Sodium tetrachloropalladate(II) | PrimorTrace™, ≥99.99% metals basis | High-purity Na₂PdCl₄: commonly used for preparing Pd(II) complexes, solution-chemistry controls, and electroplating/deposition precursor studies; the chloro-complex anion system is well suited for coordination/exchange studies. | |
Palladium salts | β-Diketonate (acac) precursor | 14024-61-4 | Bis(acetylacetonato)palladium(II) | ≥99.95% metals basis | Pd(acac)₂ is a widely used Pd precursor compatible with organic solvents: for catalysis and materials routes (thermolysis/deposition/nano-Pd); suitable as an “organometallic Pd source” control. | |
Palladium salts | Potassium chloropalladite (Pd(II)) / coordination & electroplating precursor | 10025-98-6 | Potassium tetrachloropalladate(II) | ≥99.95% metals basis | A Pd(II) chloro-complex salt (K₂PdCl₄ type): used for Pd complex synthesis, mechanistic/equilibrium studies of chloro-complex systems, and commonly as a precursor in electroplating/deposition and surface chemistry. | |
Palladium salts | Strongly electron-withdrawing ligand precursor (TFA salt) | 42196-31-6 | Palladium(II) trifluoroacetate | ≥98% | Pd(TFA)₂ is often used when stronger electronic tuning and/or easier formation of active species is desired (e.g., certain C–H activation, oxidative coupling, and coordination-chemistry screening); can serve as a “stronger precursor” control relative to Pd(OAc)₂. | |
Rhodium salts | Dirhodium(II) carboxylate dimer catalyst | 15956-28-2 | Dirhodium(II) acetate dimer | RH: 43.0%–46.6% | A representative Rh(II) dirhodium catalyst: widely used for carbene/nitrene transfer (e.g., cyclopropanation, C–H insertion) and selective transformations; a high-frequency catalyst salt in mechanism and reaction screening. | |
Rhodium salts | Inorganic halide precursor (Rh(III)) | 20765-98-4 | Rhodium(III) chloride hydrate | Rh 38.5%–42.5% | A general Rh(III) precursor: used to prepare Rh catalysts/complexes for hydrogenation/isomerization, etc.; also commonly used as a rhodium-source control in materials and surface chemistry. | |
Rhodium salts | β-Diketonate (acac) precursor | 14284-92-5 | Rhodium(III) acetylacetonate | PrimorTrace™, ≥99.99% metals basis | High-purity Rh(acac)₃: used in organometallic precursor routes (nanoparticles/thin-film deposition/thermolysis) and in catalysis/coordination chemistry; suitable for materials systems extremely sensitive to impurities. | |
Iridium salts | Inorganic halide precursor (Ir(III)) | 14996-61-3 | Iridium(III) chloride hydrate | Reagent grade, Ir ≥52% | A commonly used Ir precursor: for preparing Ir catalysts and complexes (coordination chemistry, electrocatalysis/redox systems); also a frequent starting point for luminescent/functional complexes (requires further ligand installation). | |
Iridium salts | Chloroiridate salt (Ir(IV)) / redox & coordination precursor | 16920-56-2 | Potassium hexachloroiridate(IV) | PrimorTrace™, ≥99.99% metals basis | An Ir(IV) salt (K₂IrCl₆ type): commonly used as a precursor for redox/electrochemistry and coordination chemistry; especially suitable when a well-defined high-valent Ir starting point is required. | |
Iridium salts | β-Diketonate (acac) precursor | 15635-87-7 | Iridium(III) acetylacetonate | ≥99.95% metals basis | Ir(acac)₃ as an organometallic Ir precursor: used as a starting point for functional Ir complex synthesis, thin-film/nanomaterial precursors, and luminescent/electrochemical materials research. | |
Ruthenium salts | Inorganic halide precursor (Ru(III)) | 14898-67-0 | Ruthenium(III) chloride hydrate | Suitable for analysis, superior grade | A general Ru precursor: for preparing many Ru catalysts/complexes (redox, hydrogenation/transfer hydrogenation, etc.), and for electrochemical and materials deposition/precursor studies. | |
Ruthenium salts | β-Diketonate (acac) precursor | 14284-93-6 | Ruthenium acetylacetonate | ≥99.95% metals basis | Ru(acac)-type organometallic precursor: commonly used for thin-film/nanomaterial preparation (thermolysis/deposition routes) and catalyst-complex synthesis; high purity benefits device-grade materials research. |
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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