AP Chemistry - Solubility of Complex Ions Worksheet #2

1.    a) Write net ionic equation for any of these reaction which result in the formation of a precipitate.  If no reaction occurs write N.R. Assume equal volumes of 0.1 mol/L solutions are mixed. 

b) Write the Ksp expression for each precipitate.

      i) silver nitrate and sodium cyanide 

     ii) potassium chloride and ammonium sulphate 

    iii) mercury(I) nitrate and potassium bromide

    iv) iron(III) chloride and aqueous ammonia

     v) calcium nitrate and sodium oxalate 

    vi) lead nitrate and ammonium iodide 

   vii) bismuth nitrate and aqueous hydrogen sulphide
2.  Write net ionic equation for these acid-base reactions which result in the formation of a weakly dissociated species. 

a)  NaOH(aq) + HNO3(aq) 

b)  NaCN(s) + H2SO4(l) 

c)  K3BO3(s) + HClO4(aq) 

d)  CaSO3(s) + HCl(aq) 

e)  (NH4)2CO3(s) + HBr(aq) 

f)  FeS(s) + HI(aq) 

g)  NH4Cl(s) + KOH(s) 

h)  CuO(s) + HCl(aq) 

i)  MgCO3(s) + HI(aq) 

j)  NH4OH(aq) + H2SO4(l) 

k)  Cd(OH)2(s) + HNO3(aq) 

l)  Ca(HCO3)2(aq) + HCl(aq) 

m)  KOH(aq) + H3PO4(aq) 
3. Which of these substances dissolve to a significant extent in dilute, 1.0 M HNO3? Justify your answers. 

a) BaCO3       b) AgOH       c) AgI        d) PbCrO4      e) BaSO4        f) BaF2
4. Is CaCO3 more or less soluble in a 6 M Na2CO3 solution than in pure water? Explain in terms of Le Châtelier's Principle.
5. Explain why in terms of Le Châtelier's Principle why AgC2H3O2 (Ksp = 4.0 x 10-3), can be dissolved in an excess of each of these reagents.

a) H2O(l)         b) HNO3(aq)           c) NH3(aq) 
6. AgCl is appreciably soluble in 1 mol/L aqueous NH3, but AgI is not. Explain. 
7. Copy and complete the table below by writing the name and formula of the substance formed. If no reaction occurs, write N.R. 

Ion                      Excess NaOH                                             Excess NH3(aq) 
8.    A solution may contain Ba2+ and/or Al3+. Explain how you would prove the presence or absence of these ions.