AP Chemistry - Solubility Unit Review Problems Worksheet #3

1. Write the ionic equation for these reactions

a) sodium cyanide and hydrochloric acid 

b) potassium carbonate with hydrobromic acid 

c) sulphuric acid and ammonium borate 

d) hydrofluoric acid and sodium phosphate (one product is NaH2PO4)

e) iron(II) sulphide and hydrochloric acid 

f) silver nitrate and hydrosulphuric acid 
2.  Which of these substances dissolves to an appreciable extent in 1.0 mol/L nitric acid? 

a) PbCO3

b) SrSO4

c) Mg(OH)2

d) AgCl 

e) CuCrO4

f) SrF2
3.  Calculate the [Ag+] needed to begin precipitation of each of these anions from solutions containing one mg of anions per mL of solution.

a) Br-       b) S2-       c) BrO3-       d) CrO42-        e) IO3-

Ksp of AgBrO3 = 6.0 x 10-5 and of AgIO3 = 3.1 x 10-18
4. Fifty mL of 0.10 mol/L AgNO3 is added to 150 mL of 0.10 mol/L CaCl2. What is the concentration of each ion in the resulting solution? 
5.   In which of these reactions does a precipitate form?

a) 10.0 mL of 0.01 AgNO3 and 10.0 mL of 0.10 mol/L Na2SO4

b) 1 mg of MgCl2 and 1 litre of 0.01 mol/L Na2C2O4

c) 1 mL of 0.10 mol/L Ca(NO3)2 and 1 L of 0.01 mol/L HF 

d) 1 mL of 0.1 mol/L Ca(NO3)2 and 1 L of 0.01 mol/L NaF 

e) 5 mL of 0.004 mol/L AgNO3 and 15 mL of a solution containing 1.5 mg of Br- ions. 
6.  How many mg of Pb2+ must be present in 10.0 mL of a 0.135 mol/L NaCl solution for PbCl2 to precipitate? 
7. Barium nitrate reacts with potassium sulphate solution and forms insoluble BaSO4. How many millilitres of 0.40 mol/L Ba(NO3)2 solution are required to precipitate effectively the sulphate ions in 25 mL of 0.80 mol/L K2SO4 solution? 

What mass of silver chloride can be precipitated from a silver nitrate solution by 200 mL of a solution of 0.50 mol/L CaCl2