WorksheetsThe common-ion effect
Total questions: 10
Worksheet time: 2hrs 40mins
Which of the following statements is held true about the common-ion effect on the equilibrium of solubility of salt ?
(you may choose more than one answer)
Adding common-ion to the solution containing dissolved salt cause the solubility equilibrium shifts to the formation of undissolved salt
Adding common-ion to the solution containing dissolved salt cause the numerical value of Ksp of corresponding salt changes
Solubility of salt in solution containing common-ion is greater than that of pure water.
Consider a beaker containing 100 ml of water, with solid AgCl on the bottom.
Which of the following statements is held true if NaCl is added to the solution?
(you may choose more than one answer)
The amount of AgCl solid at the bottom of the beaker increases
The amount of AgCl solid at the bottom of the beaker decreases
The concentration of dissolved Ag+ ion in the solution stays the same
The concentration of dissolved Ag+ ion in the solution changes
Consider a beaker containing 200 ml of saturated solution of PbSO4 salt.
Which of the following statements is held true if the solution is acidified by addition of H2SO4 solution?
(you may choose more than one answer)
concentration of dissolved Pb2+ ion in solution increase
concentration of dissolved Pb2+ ion in solution decrease
pH of the solution drops followed by an increase iof amount of PbSO4 solid at the bottom of the beaker
pH of the solution rises followed by decrease of amount of PbSO4 solid at the bottom of the beaker
Which of the following effect increase the solubility of Ca(OH)2 ?
Ca(OH)2(s) ↔ Ca2+(aq) + 2OH-(aq)
(you may choose more than one answer)
Adding solid NaOH
Adding an acid solution
The pH of solution is adjusted to be below 7
Adding solid CaCl2
Which of the following effect decrease the solubility of Mn(OH)2 ?
Mn(OH)2(s) ↔ Mn2+(aq) + 2OH-(aq)
(you may choose more than one answer)
adding pure water to the solution
adding a NH3 solution
adding a acid buffer
adding a basic buffer
At which solution will AgBr have the lowest molar solubility ?
(Ksp AgBr =5 x 10-13)
AgBr(s) ↔ Ag+(aq) + Br-(aq)
0.5 M AgNO3 solution
0.5 M NaBr solution
0.5 M AgClO4 solution
0.5 M MgBr2 solution
At which solution will PbI2 have the lowest molar solubility ?
(Ksp PbI2 = 7.1 x 10-9)
PbI2(s) ↔ Pb2+(aq) + 2I-(aq)
0.02 M Pb(NO3)2 solution
0.02 M CaI2 solution
0.02 M Pb(ClO4)2 solution
0.02 M KI solution
At which solution will Ca3(PO4)2 have the highest molar solubility ?
(Ksp Ca3(PO4)2 =2 x 10-29)
Ca3(PO4)2(s) ↔ 3Ca2+(aq) + 2PO43-(aq)
0.01 M CaCl2 solution
0.01 M K3PO4 solution
0.05 M Ca(NO3)2 solution
0.05 M Na3PO4 solution
At which solution will Al(OH)3 have the highest molar solubility ?
(Ksp Al(OH)3 =1.3 x 10-33)
Al(OH)3(s) ↔ Al3+(aq) + 3OH-(aq)
buffered solution of pH 9
0.01 M NaOH solution
0.01 M Sr(OH)2 solution
0.01 M AlCl3 solution
At which solution will Zn(OH)2 have the lowest molar solubility ?
(Ksp Zn(OH)2 =1.2 x 10-27)
Al(OH)3(s) ↔ Al3+(aq) + 3OH-(aq)
buffered solution of pH 12
10-3 M KOH solution
10-3 M ZnCl2 solution
10-2 M ZnSO4 solution
