The common-ion effect

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

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7

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

Tags

NGSS.HS-PS1-5

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

Tags

NGSS.HS-PS1-5

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

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7

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) + 2PO₄^3-(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