Lithium Chloride Saturated Ethanol Solution - BioReagent

CAS: 7447-41-8 Cat. No.: L1528854 Fórmula: LiCl Peso molecular: 42.39 Número EC: 231-212-3

GRADE & PURITY BioReagent, Ready-to-use, Suitable for molecular biology

Storage

Room temperature

Shipped In

Normal

Application

1071

Descripción general

Saturated lithium chloride in ethanol is a commonly used laboratory reagent prepared by dissolving lithium chloride in absolute ethanol. Store sealed at room temperature.

Main applications:

Analytical chemistry: Used as filling solution for reference electrodes such as calomel electrodes, suitable for non-aqueous titration systems.

Molecular biology: Used for RNA precipitation.

Chromatography: Applied in ion chromatography for trace alkaline earth metal detection and size-exclusion chromatography analysis of cellulose.

Note: This solution is nearly saturated. White lithium chloride crystals may precipitate at the bottom of the bottle, which is normal and will not affect reagent performance.

Operating Procedures (For reference only):

Follow the specific requirements of your experiment.

Precautions:

1. For your safety and health, wear a lab coat and disposable gloves during operation.

2. This product is for research use only. Any other application is prohibited.

Specifications

Especificaciones y pureza

BioReagent, Ready-to-use, Suitable for molecular biology

Estabilidad y almacenamiento

Store at Room temperature long term (12 months).

Condiciones de almacenamiento de almacenamiento

Room temperature

Enviado en

Normal

Grado

BioReagent, Listo para usar, Suitable for molecular biology

Product Line

biological_products

Nombres e identificadores

Isómeros SMILES

[Li+].[Cl-]

WGK Alemania

3

RTECS

OJ5950000

Peso molecular

42.39

Propiedades químicas y físicas

• Punto de ebullición (°C): 1360℃
• Punto de fusión (°C): 605 °C (lit.)

Application Protocols

No assay‑specific, antibody, or kit protocols apply to this chemical reagent. For laboratory uses such as electrochemistry or synthetic transformations, follow method‑specific procedures from the primary literature and adapt to the LiCl concentration present in this saturated ethanol solution.

• For electrochemistry: Calibrate conductivity and reference electrode in ethanol; validate potential windows and background currents before substrate runs.
• For synthetic use: Run small‑scale trials to confirm rates/selectivity with this medium; compare against neat ethanol or alternative electrolyte systems as controls.

Biological Roles

This product is a laboratory reagent solution; it is not intended for biological administration. The following notes are general background on the components and are not product claims.

• Ethanol (literature/general): A small polar protic molecule; in biological systems, it is metabolized primarily by alcohol dehydrogenase to acetaldehyde and then to acetate. It perturbs membrane fluidity and protein stability at sufficient concentrations. In the lab, ethanol is commonly used for nucleic acid precipitation and protein precipitation, but those procedures typically use aqueous ethanol without added salts like LiCl.
• Lithium chloride (literature/general): Lithium ions can modulate signaling pathways (e.g., glycogen synthase kinase‑3 interactions) in biological research contexts, and LiCl is used in molecular biology for selective RNA precipitation from aqueous solutions at high ionic strength. In ethanol specifically, LiCl does not act as a buffer; it provides ionic strength and specific cation effects but little direct biological utility.

Applicability to this product:

• Because this is a nonaqueous ethanol solution, direct use in biochemical assays is uncommon unless protocols are explicitly designed for ethanol media (e.g., certain electrochemical biosensors or organic‑phase reactions). If biological workflows require LiCl, aqueous solutions at defined molarity are typically used instead.

Research Use Note: For research use only (per Product Data). No clinical or in vivo applications are implied.

Buffer Applications

Not typically applicable. This product is an ethanol solution saturated with LiCl and does not provide acid/base buffering capacity in aqueous systems.

• If buffering is required, prepare an appropriate aqueous buffer (e.g., phosphate, Tris, HEPES) and use ethanol only as a cosolvent at validated percentages.
• For nucleic acid precipitation workflows that use LiCl, standard protocols employ aqueous LiCl at defined molarity rather than ethanol‑based LiCl solutions.

Green Alternatives

Ethanol is comparatively favorable from a green chemistry standpoint versus many aprotic polar solvents, and adding LiCl does not significantly change its environmental profile aside from salinity in aqueous waste.

• Relative greenness (literature/general):

  • Ethanol: renewable feedstocks available, readily biodegradable, low acute aquatic toxicity, but flammable and volatile.
  • DMF/DMAc/DMSO systems: higher boiling, more persistent/toxic profiles; often superior for LiCl solubility but less green.
  • Methanol: higher LiCl solubility and conductivity, but greater human toxicity and similar flammability.

• Potential greener substitutions depending on task:

  • For higher salt solubility in a green alcohol: isopropanol has lower LiCl solubility than ethanol, so not advantageous; methanol improves performance but at a toxicity tradeoff.
  • For aprotic needs with improved sustainability: Cyrene or propylene carbonate as solvents are greener than DMF/DMAc, but LiCl solubility/supporting electrolyte behavior must be validated.

Comparison table (literature/general; not item specs):

• EtOH (this product): greener, protic, moderate LiCl solubility, easy removal, high flammability.
• MeOH + LiCl: higher ionic strength, easier low‑temp operation, worse toxicity.
• DMF/DMAc + LiCl: excellent LiCl solubility for challenging substrates, but worker/environmental hazards and difficult removal.

Waste minimization:

• Reuse/recirculate electrolyte solutions for electrochemistry when purity allows.
• Segregate saline organic waste; avoid unnecessary dilution with water to reduce treatment volume.

Pharmaceutical Uses

Not a pharmaceutical formulation. This product is supplied for laboratory research use only.

General/process‑oriented context (literature/general):

• Ethanol is a compendial solvent (e.g., Ph. Eur., USP) widely used in pharmaceutical manufacturing as a process solvent and in some dosage forms as an excipient; however, those uses require stringent quality controls (e.g., dehydrated alcohol, low UV absorbance) and do not include LiCl as an excipient in ethanol.
• Lithium chloride is not commonly used as an excipient; its presence in this reagent is to impart ionic strength/coordination effects for laboratory chemistry, not for formulation.

If a process requires ethanol with specific ionic strength or conductivity (e.g., for electrochemical synthesis of intermediates), a LiCl‑in‑ethanol system can be useful during R&D. For GMP or scale‑up, suitability, impurities, and extractables/leachables must be established independently.

Item‑specific pharmacopeial status: Not specified for this item; refer to CoA/Spec Sheet.

Physical Properties

For a saturated LiCl solution in ethanol, bulk properties are close to those of ethanol but are measurably shifted by dissolved salt. Values below are literature/general references for context and are not item specifications.

• Appearance: Not specified for this item; refer to CoA/Spec Sheet.
• Concentration of LiCl: Saturated (exact molarity depends on temperature and water content); Not specified for this item; refer to CoA/Spec Sheet.
• Boiling point (literature, ethanol): ~78.37 °C at 1 atm. Dissolved salts elevate BP slightly via ebullioscopy (magnitude depends on concentration).
• Melting/freezing point (literature, ethanol): −114.1 °C. Salt and water content may raise the freezing point and can cause salt precipitation on cooling.
• Density (literature, ethanol 20 °C): ~0.789 g/mL; salt increases density modestly proportional to molality.
• Viscosity (literature, ethanol 25 °C): ~1.2 mPa·s; LiCl increases viscosity with ionic strength.
• Dielectric constant (literature, ethanol 25 °C): ~24.3; effective polarity increases with Li+ coordination and ion pairing.
• Refractive index nD20 (literature, ethanol): ~1.361; increases slightly with dissolved salt.
• Solubility profile (general): Miscible with many organic solvents (ethanol component); water‑miscible. LiCl remains dissolved until dilution or temperature shift reduces solubility; water strongly increases LiCl solubility.
• Hygroscopicity: LiCl and ethanol both absorb moisture; water uptake alters concentration and properties.

Item‑specific numeric specs (e.g., exact density, refractive index, LiCl molarity): Not specified for this item; refer to CoA/Spec Sheet.

Quality and Grades

• Grade/Purity for this item: BioReagent (per Product Data).

What BioReagent typically implies (general guidance):

• Prepared and packaged to meet common requirements for biochemical and molecular biology workflows (e.g., controlled trace contaminants, consistent performance), though not necessarily meeting HPLC/LC‑MS low‑UV or mass‑spec solvent criteria unless separately stated.
• Emphasis on batch‑to‑batch consistency and low bioreactive impurities (e.g., low aldehydes/acids for some enzyme‑sensitive applications). For salt‑in‑solvent reagents, this often includes control of moisture and inorganic contamination.

What is and is not specified for this item:

• Stabilizers/inhibitors: Not specified for this item; refer to CoA/Spec Sheet.
• Water content, LiCl assay, conductivity, UV cutoff, metals/peroxides: Not specified for this item; refer to CoA/Spec Sheet.
• Storage: Room temperature (per Product Data). Shipped under normal conditions.

Practical quality notes for LiCl‑in‑ethanol solutions (general):

• Water content critically impacts LiCl solubility and effective molarity; BioReagent‑grade control reduces variability. Confirm lot‑specific concentration if your protocol is concentration‑sensitive (e.g., electrochemistry).
• Visual clarity should be checked before use; if crystals are present, warm gently and mix to re‑dissolve or filter through a dry, inert membrane if a particle‑free solution is required.
• For analytical or chromatographic work, verify background UV absorbance and nonvolatile residue on your instrument prior to routine use.

Reaction and Applications

Lithium chloride in ethanol combines a polar protic solvent with a coordinating lithium salt, which can meaningfully alter reactivity and selectivity in several laboratory contexts.

• Electrochemistry (literature/general): LiCl serves as a supporting electrolyte to increase solution conductivity in ethanol. Useful for potential‑controlled oxidations/reductions of species soluble in ethanol. Saturation provides near‑maximal ionic strength for this solvent; verify conductivity for your cell geometry.
• Solvolysis/ethanolysis: Li+ coordination to leaving groups and/or carbonyl oxygens can accelerate certain substitution and acylation reactions where ethanol is the nucleophile/solvent. Elevated ionic strength may stabilize carbocationic transition states in SN1‑leaning systems (substrate‑dependent).
• Nucleophilic substitutions (general): In some SN2 reactions, LiCl can act as a halide source or as an ion‑pairing modulator. The protic environment favors ethanol as nucleophile; consider temperature control to balance rate vs. elimination.
• Workup/processing: High ionic strength ethanol can aid phase disengagement or precipitation of nonpolar by‑products and can displace coordinating solvents (e.g., THF) from metal complexes during isolation (user‑optimized).
• Polymer and materials handling: As a protic, hydrogen‑bonding medium with Li+, this solution can modify solvation of polar polymers or oligomers; salt presence may screen charges and influence aggregation (method development recommended).

Practical tips:

• Mix before dispensing; if crystals are observed, warm gently (ambient to ~30–40 °C) with stirring to re‑dissolve.
• Water content has an outsized effect on both LiCl solubility and reaction outcomes; use dry techniques when water‑sensitive chemistry is intended.
• For electrochemistry, pre‑degass by sparging with inert gas to remove dissolved oxygen if needed, and verify reference electrode compatibility with ethanol.

Reaction Conditions

General guidance for using LiCl‑saturated ethanol (literature/general). Adjust to your substrate and scale; these are not product specifications.

• Electrochemistry:

  • Supporting electrolyte: Use the solution as supplied; verify conductivity by cell calibration. Typical supporting electrolyte levels in organic electrochemistry are 0.05–0.2 M; the effective concentration here will be governed by LiCl solubility at your temperature and water content.
  • Atmosphere: Inert gas blanket (N2/Ar) to limit oxygen; sparge 10–20 min for O2‑sensitive reductions.
  • Electrodes: Glassy carbon/platinum working electrodes are broadly compatible with ethanol/LiCl; Ag/AgCl (ethanol‑compatible) or nonaqueous reference electrodes can be used with salt bridge precautions.
  • Temperature: 0–40 °C commonly; monitor for salt precipitation at low temperatures.

• Ethanolysis/solvolysis and substitutions:

  • Base: A mild base (e.g., Et3N, NaOEt generated in situ) may be added when converting activated acyl derivatives to ethyl esters; Li+ can assist carbonyl activation. Start at 0–25 °C and titrate conditions.
  • Nucleophilic substitutions: For benzylic/allylic substrates, begin at ambient temperature; for less reactive systems, gentle heating (40–60 °C) may be explored, watching for elimination.
  • Workup: Evaporate ethanol under reduced pressure; residue can be partitioned between water and organic solvent, removing LiCl to the aqueous phase.

• Handling tips:

  • Mix before sampling; warm gently to re‑dissolve any precipitated LiCl.
  • Minimize water ingress to keep concentration constant; use septa and dry needles for transfers when needed.

Safety and Handling

• GHS classification, signal word, pictograms, H‑statements: Not specified for this item; consult the product SDS for authoritative classification.
• Typical hazards (literature/general):
  • Ethanol solutions are Highly flammable liquids and vapors (commonly Flam. Liq. 2, H225). Keep away from heat/sparks/open flames/hot surfaces. No smoking.
  • May cause eye irritation and transient CNS effects at high vapor concentrations; avoid inhalation of vapors/mists.
  • Lithium salts may cause irritation if contacted or ingested; avoid skin/eye contact.
• PPE (best practice): Safety glasses or splash goggles, lab coat, and suitable chemical‑resistant gloves (e.g., nitrile). Use in a fume hood to control vapors.
• Incompatibilities (general): Strong oxidizers; strong acids/bases (may affect corrosion and salt stability); reactive metals; ignition sources. Avoid contact with water if a defined anhydrous concentration is critical (water alters LiCl solubility and solution properties).
• Special risks/practices:
  • Static ignition risk: Ground/bond containers and equipment during transfer. Use only non‑sparking tools.
  • Salt precipitation: Cooling or solvent evaporation can precipitate LiCl; mix before use and filter if a clear solution is required.
  • Hygroscopic uptake: Minimize headspace and exposure time; promptly re‑cap.
• First aid (overview; see SDS):
  • Inhalation: Move to fresh air; seek medical attention if symptoms persist.
  • Skin/eyes: Rinse with water for at least 15 minutes; remove contaminated clothing; obtain medical advice for persistent irritation.
  • Ingestion: Rinse mouth; do not induce vomiting; seek medical attention.

Solvent Selection

This product functions as a polar protic solvent system (ethanol) with an added lithium salt to provide high ionic strength and specific Li+ coordination effects.

• Polarity/miscibility (literature/general):
  • Ethanol is miscible with water and many organics (THF, acetone, acetonitrile) and partly miscible with nonpolars depending on ratio. LiCl remains soluble in ethanol up to a limited concentration that depends strongly on water content; dilution into less polar solvents can precipitate salt.
• When to choose LiCl‑saturated ethanol:
  • As a convenient, ready‑to‑use supporting electrolyte for electrochemical experiments conducted in ethanol, where high conductivity and a protic medium are desired.
  • To modulate solvation and ion‑pairing in ethanolysis/solvolysis, nucleophilic substitutions with ethanol as nucleophile, or reactions benefiting from Li+ Lewis acid coordination to oxygen or halides.
  • For workups where ionic strength and a protic environment aid phase behavior or precipitate separation (method‑dependent).
• When to consider alternatives:
  • Need for higher salt concentration/electrolyte strength in an alcohol: methanol often dissolves substantially more LiCl (literature) but at the cost of higher toxicity.
  • Water‑sensitive substrates: switch to an aprotic system (e.g., LiCl in DMAc, DMSO, or DMF) to avoid protic reactivity while retaining lithium salt effects.
  • Chromatographic compatibility: use HPLC‑grade solvent systems if low UV background or MS compatibility is required.
• Small comparison (literature/general):
  • EtOH/LiCl: protic, greener, moderate conductivity.
  • MeOH/LiCl: protic, higher LiCl solubility, more toxic, more volatile.
  • DMF/DMAc + LiCl: aprotic, very high LiCl solubility, less green, higher boiling.

Storage and Reconstitution

• Storage conditions: Room temperature (per Product Data). Store tightly closed in a well‑ventilated area away from heat, sparks, open flames, and hot surfaces.
• Shipping: Shipped under normal conditions (per Product Data).
• Stability considerations (general):
  • Evaporation of ethanol will concentrate the solution and can lead to LiCl precipitation or compositional drift; keep containers tightly sealed.
  • Hygroscopic uptake alters LiCl solubility and effective concentration; limit headspace and exposure to ambient humidity. If moisture control is critical, store under inert gas and use septum caps.
  • Precipitation on cooling: If crystals form, warm gently (e.g., to 30–40 °C) with swirling to re‑dissolve before use, or filter through a dry 0.2–0.45 µm membrane to obtain a clear solution.
• Reconstitution: Not applicable—supplied as a ready‑to‑use solution. If dilution or blending is required, use dry ethanol to maintain defined water content; document final composition for reproducibility.
• Container/material compatibility: Store in compatible solvent‑resistant containers (e.g., amber glass with PTFE‑lined cap). Avoid reactive metals and elastomers that may swell in ethanol.
• Freeze–thaw: Avoid freezing; salt may crystallize and require redissolution. If accidental freezing occurs, thaw to ambient temperature and mix thoroughly until homogeneous.
• For research use only (per Product Data). Refer to the SDS and CoA/Spec Sheet for authoritative guidance on handling and specifications.

Structure and Identity

Lithium Chloride Saturated Ethanol Solution is a defined mixture consisting of anhydrous ethanol containing dissolved lithium chloride at its solubility limit (saturation) at the stated storage temperature.

• Item identity: Ethanol solution saturated with LiCl (no single CAS/InChIKey applies to the mixture)
• Components (literature/general):
  • Ethanol (EtOH): CH3CH2OH; polar protic solvent with one primary alcohol functional group; 2D structure is a two‑carbon chain terminating in a hydroxyl group.
  • Lithium chloride (LiCl): ionic inorganic salt; Li+ (small, hard cation) and Cl− (halide anion); in solution, forms strongly solvated ion pairs and clusters in alcohols depending on water content.
• Molecular formula, Molecular weight, SMILES, InChIKey: Not specified for this item; refer to CoA/Spec Sheet. (Note: these identifiers are not typically assigned to multi‑component solutions.)
• Structural features (general):
  • Ethanol supplies hydrogen‑bond donors/acceptors; Li+ coordinates to ethanol oxygen lone pairs, modifying the solvent’s effective polarity and ion‑pairing behavior.
  • At saturation, undissolved LiCl may be present as a small solid phase if temperature decreases or if ethanol becomes drier/wetter than at preparation.
• Category: Polar protic solvent system with added supporting electrolyte/ Lewis acidic lithium salt.

Practical identity note: The exact LiCl molarity of a “saturated” ethanol solution depends on temperature and water content; consult the product CoA for the empirical concentration determined for this lot.

Synthetic Utility

Lithium chloride is a versatile, hard Lewis acid/halide source that exerts notable effects on organic reactivity; pairing it with ethanol leverages these effects in a polar protic medium.

• Coordinative effects (literature/general): Li+ coordinates to heteroatoms (O, N, halides), influencing rates and selectivity. In ethanol, such coordination can activate carbonyls toward nucleophilic attack by ethoxide/ethanol and stabilize ionic transition states.
• Ion‑pairing and medium effects: Elevated ionic strength can shift equilibria in solvolysis and transesterification. LiCl can modulate anion availability by forming contact ion pairs with nucleophiles or leaving groups.
• Ethanolysis and acyl chemistry: Ethanol as nucleophile can convert acyl derivatives (e.g., acid chlorides/anhydrides) to ethyl esters; Li+ may enhance rates in some systems (substrate‑dependent). Control of temperature and acid scavenging/base is often necessary.
• Electroorganic synthesis: As a supporting electrolyte, LiCl enables controlled potential/current reactions in ethanol without introducing strongly coordinating anions that complicate workup; evaporation of ethanol followed by aqueous wash can remove LiCl efficiently.
• Halide exchange and substitution (general): LiCl can participate in halide exchange equilibria or promote substitution by shifting ion pairing; in ethanol the protic environment must be balanced against elimination.

Limitations:

• Limited LiCl solubility in ethanol relative to methanol or polar aprotic media may cap achievable ionic strength.
• Water content strongly influences performance; dry handling is advised for water‑sensitive transformations.

Target Specificity

Not applicable. This product is a chemical reagent solution (LiCl in ethanol) and does not have biological target specificity, antigen binding, clone information, or isotype characteristics.