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Application Protocols
Not applicable. No vendor-validated bioassay protocols (e.g., WB, IHC, IF, FC) are associated with this materials-science reagent. For practical use, see Reaction Conditions for representative procedures in nanoparticle synthesis, halide scavenging, and film formation, and adapt to your system with appropriate controls.
Biological Roles
Item is for research use only; no clinical or in vivo use is implied.
General biochemical context (literature; not product-specific claims):
Citrate is a central metabolite in the tricarboxylic acid (TCA) cycle, coordinating metal ions via carboxylate and hydroxyl oxygens. In materials/biocolloid chemistry, citrate is widely used as a capping and stabilizing ligand for metal nanoparticles due to its multidentate binding and negative charge at neutral pH.
Silver(I) has no known essential biological role; Ag+ is a soft Lewis acid that binds thiol and imidazole donors in biomolecules. Its interactions underpin research into biointerfaces, antifouling surfaces, and protein–nanoparticle corona formation.
In aqueous systems, citrate can modulate Ag+ speciation, affecting solubility, reduction kinetics, and interaction with biomacromolecules—useful in designing experiments on protein adsorption or cell-surface interactions in materials research.
Notes:
Any discussion of antimicrobial performance should be restricted to controlled laboratory testing in materials science contexts. Regulatory and safety guidelines apply for environmental release and disposal.
For biological assays, confirm absence/presence of residual reductants or complexants that could confound results (e.g., ammonia, thiosulfate).
Buffer Applications
Not typically applicable. While citrate is a common buffering agent (pH ≈ 3–6, literature), the silver(I) citrate hydrate salt is not used to prepare citrate buffers due to silver’s low solubility and strong interactions/precipitation with common anions. For buffer preparation, use sodium or potassium citrate with citric acid instead. If your work involves silver speciation in buffered systems, prepare the buffer first and introduce silver under controlled, complexant-aware conditions.
Green Alternatives
When choosing a silver source, “green” considerations include oxidizing strength, corrosivity, waste toxicity, and solvent/ligand needs.
Comparison of common Ag(I) sources (general literature; not product specs):
Silver citrate vs. silver nitrate:
Pros: lower oxidizing power, potentially safer handling and reduced corrosion risk; citrate is a biogenic ligand with relatively benign fate compared to nitrate.
Cons: markedly lower solubility in water without complexants; may require ammonia or other ligands, complicating waste treatment.
Silver citrate vs. silver acetate/2-ethylhexanoate:
Pros: aqueous processing possible; citrate can serve dual role as complexant/capping agent; lower VOC profile when used in water-based systems.
Cons: organosilver carboxylates can be more soluble in organic media and better for low-temperature metallization; citrate may leave more inorganic/organic residue upon decomposition.
Greener process tips:
Prefer water as solvent where feasible; leverage citrate complexation to avoid chlorinated or high-VOC solvents.
Use ascorbate or glucose as mild, greener reductants for AgNP formation.
Optimize ligand loading to minimize excess complexants (e.g., ammonia, thiosulfate) and simplify wastewater treatment.
Implement closed-loop silver recovery from waste streams by controlled reduction/precipitation of Ag(0).
Pharmaceutical Uses
No pharmacopeial or excipient grade is specified for this item; it is provided for research use only.
Context (general, non-clinical):
Silver(I) citrate hydrate may be explored in R&D as a silver source for materials embedded in medical-device prototypes (e.g., coatings, polymer composites) under laboratory conditions; such investigations require extensive safety, regulatory, and biocompatibility evaluation and are outside the scope of this listing.
Compared with stronger oxidizing silver salts (e.g., AgNO3), silver citrate can offer milder handling and lower corrosivity in formulation studies; however, its low intrinsic solubility often necessitates complexing agents, which can complicate formulation and stability.
For any application approaching regulated use, sourcing must align with appropriate pharmacopeial standards, extractables/leachables profiles, and validated analytical controls—none of which are claimed here.
Physical Properties
Item-specific physico-chemical specifications (BP, MP, density, solubility limits, UV cutoff, refractive index, water content, peroxide content, metal impurities): Not specified for this item; refer to CoA/Spec Sheet.
General/literature-based properties for silver carboxylates and silver citrate (for context only; not product specifications):
Physical form: typically a white to off-white, light-sensitive solid that may darken upon light exposure (literature, common to Ag(I) salts with organic anions).
Solubility (qualitative): silver citrate is generally sparingly soluble in water, with improved dissolution in the presence of complexing agents (e.g., ammonia, amines, thiosulfate) due to Ag+ complexation (literature).
Thermal behavior: Ag–carboxylates often decompose on heating to form metallic silver and release CO2/organics rather than exhibiting a sharp boiling point (literature trend).
Hygroscopicity: hydrate content implies bound water; bulk hygroscopicity is typically low-to-moderate but material may lose or gain water depending on ambient humidity (literature expectation for hydrates).
Notes for use:
Because actual hydrate stoichiometry and surface area impact apparent solubility and handling, always verify with the batch CoA. Do not treat any value above as a product specification.
Quality and Grades
Item-specific grade/purity, appearance: Not specified for this item; refer to CoA/Spec Sheet.
Context and guidance for this material type:
Silver(I) citrate hydrate is a specialty silver salt frequently used as a silver source or precursor rather than as an analytical standard. When grade is unspecified, evaluate suitability by impurity profile (e.g., residual Ag0, chloride, nitrate, organics, water content) on the batch CoA.
“Materials science” use (per Category Path) often focuses on:
Consistent particle size and flow properties for reproducible processing.
Controlled hydrate level to minimize mass-balance and decomposition variability.
Low halide content to prevent unintended AgX precipitation during processing.
Stabilizers: None are listed for this item. If your method is sensitive to coordinating additives, confirm the absence of surfactants or anti-caking agents on the CoA.
Light sensitivity: Even trace photoreduction can affect apparent assay. Handle under subdued light and store in amber containers.
Recommendation: For quantitative applications (e.g., nanoparticle synthesis, thin-film precursors), request a current CoA and, if needed, a lot-specific Spec Sheet to confirm assay, loss on drying, and residual ions.
Reaction and Applications
This material serves primarily as a silver(I) source and precursor in materials chemistry and synthesis rather than as a classical homogeneous reagent.
Materials and nanochemistry (literature/good practice):
Silver nanoparticle (AgNP) precursor: reducible to Ag(0) using agents such as NaBH4, ascorbate, glucose, polyols, or photochemical methods. Citrate can contribute to particle stabilization/capping, complementing or replacing additional ligands.
Thin films/conductive features: thermal or photodecomposition pathways yield metallic silver for printed electronics or seed layers; decomposition typically occurs below the melting point of typical substrates when formulated with suitable binders.
Antifouling/antimicrobial coatings (materials context): incorporated into polymer matrices or coatings as a controlled Ag+ source; selection depends on release rate and leaching characteristics (no clinical claims; research and materials testing only).
Synthetic chemistry:
Halide scavenging/precipitation: Ag+ precipitates halides (AgCl/AgBr/AgI). Although AgNO3 or AgOTf are common, silver citrate can serve when lower oxidizing strength is desired and solubility constraints are acceptable.
Photochemistry: light-induced Ag+ → Ag(0) reduction enables patterning or seed generation on substrates.
Practical tips:
Control light exposure to avoid premature reduction.
Use complexing agents (e.g., NH3, thiosulfate, excess citrate) to prepare clear solutions; reduce under controlled conditions to tune nucleation/growth.
Remove organic residue post-decomposition by mild oxidative annealing if high-conductivity silver is required.
Reaction Conditions
General literature guidance for using silver(I) citrate hydrate as an Ag source (not product specifications):
Preparation of Ag-containing solutions:
Dissolve under ligand-assisted conditions: aqueous ammonia (0.1–1.0 M NH3), excess citrate, or thiosulfate can yield clear solutions of Ag(I). Maintain controlled pH (typically pH 8–11 for ammonia complexes) and protect from light.
Reductants: NaBH4 (ice-cold, rapid nucleation), ascorbate or glucose (milder, larger particles). Add dropwise under vigorous stirring.
Temperature: 0–25 C for borohydride routes; 25–90 C for ascorbate/glucose. Monitor color change (yellow–brown to gray) and UV–vis plasmon band (≈390–420 nm; literature) for growth control.
Atmosphere: ambient or inert; exclude light to minimize uncontrolled nucleation.
Film/feature formation:
Prepare printable inks by forming a soluble Ag–ligand complex (ammonia/amine), mix with binder/solvent, print, and cure at 120–250 C depending on substrate to decompose ligands and sinter Ag (temperatures vary by formulation; literature).
Halide scavenging:
Add stoichiometric/slight excess relative to halide. Stir and filter off AgX precipitate under low light. Verify residual Ag+ to avoid contamination.
These ranges are representative literature conditions; optimize experimentally for your substrate, ligand system, and performance targets.
Safety and Handling
Item-specific hazard classification (GHS, signal word, H-statements, pictograms): Not specified for this item; refer to SDS.
General safety considerations for silver(I) salts and silver carboxylates (literature/good laboratory practice):
Photosensitivity: silver(I) compounds may darken on light exposure due to photoreduction to Ag(0). Store and handle protected from light (consistent with Product Data).
Sensitization/irritation: dusts of inorganic/organometallic salts can be irritating to eyes, skin, and respiratory tract. Avoid inhalation and contact; use in a fume hood.
Environmental hazard: silver ions are toxic to aquatic organisms; prevent release to the environment; collect waste as heavy-metal waste per institutional policy.
Incompatibilities: avoid contact with strong acids (may liberate citrate acid form and solubilize Ag+), halides (AgX precipitation), strong bases (may form oxo/hydroxo species), and reducing agents (can reduce Ag+ to metallic silver). Complexing reagents (ammonia, thiosulfate, cyanide) dramatically increase Ag+ solubility; handle with care. Do not mix with acetylene or alkynes under basic conditions due to risk of explosive silver acetylides (general hazard for silver salts).
PPE: lab coat, safety glasses, and nitrile gloves at minimum. Use respiratory protection if dusting risk exists and engineering controls are inadequate.
First aid (summary; defer to SDS): rinse skin/eyes with water for ≥15 minutes upon contact; move to fresh air if inhaled; seek medical attention for persistent symptoms.
Always consult the SDS for authoritative hazard, exposure limits, and emergency procedures.
Solvent Selection
Silver(I) citrate hydrate is an ionic/coordination solid with limited solubility in most common solvents; dissolution behavior is dominated by Ag+ complexation rather than bulk polarity.
Water: sparingly soluble; solubility increases with pH changes and in the presence of ligands that complex Ag+ (e.g., NH3, amines, thiosulfate, citrate excess).
Alcohols (MeOH, EtOH), acetone, acetonitrile: typically poor solubility without added ligands.
Coordinating media: aqueous ammonia, amine solutions, or thiosulfate can form soluble Ag complexes; citrate also self-complexes Ag+ in excess.
For homogeneous processing, use aqueous media with complexing agents to dissolve silver (careful control of ligand/Ag ratio to avoid unwanted precipitation).
For nanoparticle syntheses, water is preferred; citrate can act as an in situ stabilizer, but additional reductant is required.
For film deposition or inks, consider mixed aqueous–alcohol systems after forming a soluble Ag–ligand complex; remove ligand thermally during curing.
Comparison (general):
Silver nitrate: highly water-soluble, strong oxidizer; convenient but more reactive/oxidizing.
Silver acetate/propionate: more soluble in organics; different decomposition profiles.
Silver citrate: lower solubility, milder oxidizing character; useful where controlled Ag release or lower corrosivity is desired.
Storage and Reconstitution
Item-specific storage and shipping (Product Data):
Storage Conditions: Protected from light, Room temperature
Shipped In: Normal
Handling guidance (good practice):
Store in tightly sealed, amber containers to minimize photoreduction. Minimize exposure to ambient light during weighing and transfers.
Avoid humid environments that could alter hydrate content. Reseal promptly after use.
Reconstitution/solution preparation (general, not item-specific specs):
To prepare solutions, use high-purity water and, if needed, introduce a complexing agent (e.g., aqueous ammonia, excess citrate, or thiosulfate) to achieve dissolution. Adjust pH carefully and filter through 0.2 µm PTFE/PES if particulates persist.
For nanoparticle syntheses, prepare fresh solutions immediately prior to reduction and work under subdued light.
Stability notes:
Silver(I) solutions can slowly reduce to Ag(0), especially under light or in the presence of contaminants. Prepare small volumes and use promptly.
Always consult the product CoA/SDS for lot-specific stability, incompatibilities, and safe handling directions.
Structure and Identity
Silver(I) citrate hydrate is the silver(I) salt of the tricarboxylate anion derived from citric acid, isolated with bound water of hydration. It functions as a coordination polymer/ionic solid where Ag+ centers are coordinated by carboxylate and hydroxy groups from citrate.
Item-specific identifiers (Product Data):
SKU: S358203
Product Name: Silver(I) citrate hydrate
CAS: 206986-90-5
CID: 16212313
InChIKey: 121228 (as provided)
SMILES: Not specified for this item; refer to CoA/Spec Sheet.
Molecular Formula: Not specified for this item; refer to CoA/Spec Sheet.
Molecular Weight: Not specified for this item; refer to CoA/Spec Sheet.
Structural features (general chemistry description):
Composed of Ag(I) cations coordinated by the citrate3− ligand (C6H5O7 3−), a polyfunctional anion bearing three carboxylates and one alcohol.
Expected extended structure through bridging carboxylate O-donors, potentially forming polymeric Ag–O networks (literature, common for Ag–carboxylates).
No defined stereogenic centers at silver; citrate originates from chiral citric acid but is present as an achiral trianion in the solid.
2D description: central tertiary carbon with hydroxyl substituent, three pendant carboxylate groups; Ag+ ions coordinate oxygen atoms from these carboxylates in a network; water of hydration is present but stoichiometry may vary (hydrate).
Synthetic Utility
As a functional material, silver(I) citrate hydrate provides a convenient route to silver under controlled conditions and a platform for ligand-mediated solubilization.
Functional groups/coordination:
Ag(I) center: soft Lewis acid, accepts electron density from O-donor citrate; readily reduced to Ag(0).
Citrate3− ligand: tricarboxylate with β-hydroxy; multidentate binding enables polymeric lattices and stabilizes Ag+ in solution under appropriate conditions.
Typical transformations (literature):
Reduction to Ag(0) using chemical (NaBH4, ascorbate, glucose), thermal, or photochemical methods to yield nanoparticles, films, or seed layers.
Ligand exchange to generate alternative Ag(I) complexes (e.g., with amines, phosphines, thiols) in situ for catalysis or materials assembly.
Halide capture by Ag+ to remove trace halides in solution (precipitation as AgX), with citrate serving as spectator/complexing ligand.
Retrosynthetic value:
Serves as a non-nitrate silver source when avoiding nitrate/oxidizer contamination is important (e.g., in redox-sensitive substrates or polymer matrices).
Citrate’s coordinating ability allows tuning of nucleation/growth kinetics in nanoparticle syntheses by adjusting pH, ionic strength, and citrate:Ag ratios.
Target Specificity
Not applicable. This product is not an antibody, enzyme, or affinity reagent, and no target specificity information applies. For materials and synthesis uses, refer to Reaction & Applications and Synthetic Utility.
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