Only the alkali metal and ammonium bicarbonates are obtainable as solids; group 2 bicarbonates exist only in solution.
I found this on a site and it seems to explain why there is no direct answer to this question. When speaking of solubility we take something that is out of solution and make one, but in the case of bicarbonates only the Alkali metals and ammonium types exist out of solution. In other words AgHCO3 is always 100% soluble and always in solution. If you can see it it is not Silver bicarbonate.
AgHCO3
Ksp= [Ag]^2 [CrO4] / [Ag2CrO4]
due to the solubility product constant(ksp)
Sodium bicarbonate
222g/100g H2O at 20 degrees Celsius
Bicarbonate of soda is sodium bicarbonate or NaHCO3. Ammonium bicarbonate is NH4HCO3 and is less alkaline.
Temperature is proportional to solubility for sodium bicarbonate in water. Generally, adding heat increases solubility, as this input of energy helps break bonds.
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7.8g/100g water @ 18C
yes Solubility: 7.8g/100g water @ 18 °C (64 °F).
The solubility of sodium bicarbonate is 96 g/L at 20 0C.
solubility of an ionic compound decreases in the presence of a common ion. A common ion in the solution, that is common to the ionic compound being dissolved. for example the silver ion in silver nitrate solution is common to the silver in silver chloride. the presence of a common ion must be taken into accounts when determining the solubility of an ionic compounds.
Silver Nitrate
Silver carbonate (AgCO3), a white precipitate is formed.
Silver bicarbonate or Silver Hydrogen Carbonate.
Rubbing it gently with sodium bicarbonate.
The solubility of silver chloride in water is almost negligible. So it could be separated from water by filtration or evaporation.
Ionic. BUT because of Fajans rules silver salts have significant covalent character which expalins the low solubility of silver chloride.