| Name/Formula | Mass, g/mol | MP°C | BP°C | Density | Solubility g/100ml (°C) | |
|---|---|---|---|---|---|---|
| Silver Acetate AgCO2CH3 |
166.92 | d | – | 3.259 | 1.02(20) | 2.52(80) |
| white solid – Determination of Ksp experiment | ||||||
| Silver Bromide AgBr |
187.78 | 158 | >1026 | 6.437 | 8.4X10-6(20) | .00037(100) |
| bromyrite, pale yellow solid – light sensitive chemical in photography | ||||||
| Silver Carbonate Ag2CO3 |
275.75 | d 218 | – | 6.077 | .0032(20) | .05(100) |
| yellow solid | ||||||
| Silver Chloride AgCl |
143.32 | 455 | 1550 | 5.56 | .000089(10) | .0021(100) |
| White powder, Reagent, Stan-Gray Glass, Silver Plating, Titrations | ||||||
| Silver Fluoride AgF |
126.87 | 435 | 1150 | 5.852 | 182(15.5) | 205(108) |
| yellow solid, cubic | ||||||
| Silver Hydroxide AgOH |
124.87 | – | – | – | – | – |
| tan precipitate – used in anions experiment | ||||||
| Silver Iodide AgI |
234.77 | 558 | – | 5.683 | 2.8X10-7(25) | 2.5X10-6(80) |
| iodyrite, yellow hexagonal – photographic chemical | ||||||
| Silver Nitrate AgNO3 |
169.87 | 212 | d 444 | 4.352 | 122(0) | 952(190) |
| Analytical Reagent, Mirrors, Swimming Pool biocide, Catalysts, Photography | ||||||
| Silver Oxide Ag2O |
231.74 | 230 | – | 7.143 | .0013(20) | .0053(80) |
| Silver Tarnish, Batteries, Catalysts, Biocide, Water Purification, Electronics | ||||||
| Silver Phosphate Ag3PO4 |
418.58 | 849 | – | 6.37 | 2.8X10-18 | – |
| Used in Photography | ||||||
| Silver Sulfate Ag2SO4 |
311.80 | 652 | 1085 | 5.45 | 0.57(0) | 1.41(100) |
| white, rhombahedral – used in anions experiment | ||||||
| Silver Sulfide Ag2S |
247.8 | 845 | – | 7.326 | .00002 | – |
| acanthite, gray/black, rhombahedral | ||||||
Silver Reactions:
For each succeeding addition, a more stable silver compound or complex is formed:
- Start with 30 drops 0.1 M AgNO3 (1.70 g of AgNO3 in 100 ml water)
- Addition of a carbonate source leads to the formation of Silver Carbonate
Add 1 drop 1 M NaHCO3 (8.4 g Sodium Bicarbonate (NaHCO3) in 100 ml water)
2 Ag+ + HCO3– –> Ag2CO3 + H+- Silver Phosphate is less soluble than Silver Carbonate:
Add 5 drops 0.2 M Na3PO4 (3.3 g Sodium Phosphate (Na3PO4) in 100 ml water)
3 Ag2CO3 + 2 PO43– –> 2 Ag3PO4 + 3 CO32–- Silver Hydroxide is less soluble than Silver Phosphate:
Add 2 drops 1.0 M NaOH (33 mL 3 M Sodium Hydroxide (NaOH) in 100 ml water)
Ag3PO4 + 3 OH– –> 3 AgOH + PO43–- Silver Chloride is less soluble than Silver Hydroxide:
Add 5 drops 1 M NaCl (5.844 g Sodium Chloride (NaCl) in 100 ml water)
AgOH + Cl– –> AgCl + OH–- Silver Chloride dissolves in ammonia:
Add 25 drops 6.0 M NH3 (40.0 mL 15 M ammonia (NH3) in 100 ml water)
AgCl + 2 NH3 –> Ag(NH3)2+ + Cl–- Silver Bromide forms from Silver Ammine:
Add 5 drops 0.1 M KBr (1.19 g Potassium Bromide (KBr) in 100 ml water)
Ag(NH3)2+ + Br– –> AgBr + 2 NH3- Addition of a source of thiosulfate ions allows the formation of the Silver(I) Thiosulfate complex.
Add 4 drops 1.0 M Na2S2O3 (24.8 g Sodium Thiosulfate Pentahydrate (Na2S2O3ò5H2O) in 100 ml water)
AgBr + 2 S2O32– –> Ag(S2O3)23– + Br–- Addition of an iodide source forms Silver Iodide.
Add 2 drops 0.1 M KI (1.660 g Potassium Iodide (KI) in 100 ml water)
Ag(S2O3)23– + I– –> AgI + 2 S2O32–- Addition of a sulfide source allows the formation of Silver Sulfide.
Add 20 drops 0.1 M Na2S – (7.8 g Sodium Sulfide in 100 ml water)
2 AgI + S2– –> Ag2S + 2 I–If any of the reagents are added out of sequence, the compounds and complexes missed will never be formed as the predominant species.
From: One Pot Silver Reactions
Even a tiny amount is extremely dangerous! THEY WILL SERIOUSLY INJURE YOU.
Fulminating Silver:
Ag2O.(NH3)2 (black crystals) obtained by dissolving silver oxide in aqua ammonia.
When dry it explodes violently on the slightest percussion.
Silver Fulminate:
Ag2C2N2O2 (white crystals) obtained by adding alcohol to a solution of silver nitrate.
When dry it is violently explosive.