1.What concentration of carbonate ion is required to begin the precipitation of
ID: 828964 • Letter: 1
Question
1.What concentration of carbonate ion is required to begin the precipitation of strontium ion from a solution containing 0.050 M strontium ion?
2. What is the molar solubility of silver sulfate in 0.10 M silver nitrate?
3.If 100.0 ml of 0.10 M lead(II) nitrate is added to 300.0 ml of 0.010 M potassium fluoride, will a precipitate form? Show calculations to support your answer.
4. What pH is required to begin the precipitation of copper(II) hydroxide from a solution containing 0.10 M Cu2+?
5.How many grams of magnesium hydroxide will dissolve in 500.0 ml of a pH 9.0 buffer?
6.If 0.20 mole of copper(II) sulfate is added to a liter of 1.20 M ammonia solution, what is the copper(II) ion concentration at equilibrium?
7.If a solution contains 0.100 M each of calcium ions and strontium ions, what pH range will permit the selective precipitation of one ion but not the other?
8.How many grams of silver bromide will dissolve in 500.0 ml of 4.0 M ammonia solution?
Explanation / Answer
2.
Dissolving of 0.10 M AgNO3 produces 0.10 M Ag^+ ion.
AgNO3(s) ------> Ag^+(aq) + NO3^-(aq)
0.10 M -------------> 0.10 M + 0.10 M
Total [Ag^+] in solution: ( 0.10 + 2x ) M
But 2x M from the dissolving of Ag2SO4 is very small compared to the ion present in the solution, it can be neglected.
Ksp = (0.10)^2(x) = 1.2 x 10^-5
x = 1.2 x 10^-4 mol / L is the solubility of salt in 0.10 M AgNO3
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