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Lesson 2: Ionic Equilibrium, pH Scale, Hydrolysis and Solubility Product (Ksp) — Picture questions (exam style)

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  • Questions count: 10
  • Passing grade: 60%
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1.
In the equilibrium shown, which option gives two compounds each of which lowers the solubility of PbBr₂?
In the equilibrium shown, which option gives two compounds each of which lowers the solubility of PbBr₂?
NaNO₃ ، KNO₃
Pb(NO₃)₂ ، NaNO₃
NaNO₃ ، NaBr
Pb(NO₃)₂ ، NaBr
2.
40 mL of 0.1 M HCl is mixed with 20 mL of 0.2 M NaOH as shown. Which option is correct?
40 mL of 0.1 M HCl is mixed with 20 mL of 0.2 M NaOH as shown. Which option is correct?
pH = 7.00, the solution is basic
pH = 7.00, the solution is neutral
pH = 13.30, the solution is basic
pH = 13.30, the solution is neutral
3.
Equal-concentration aqueous solutions of the salts shown. Arrange them in increasing pH.
Equal-concentration aqueous solutions of the salts shown. Arrange them in increasing pH.
CuSO₄ < K₂CO₃ < NaCl
CuSO₄ < NaCl < K₂CO₃
K₂CO₃ < NaCl < CuSO₄
K₂CO₃ < CuSO₄ < NaCl
4.
Ksp of Mg(OH)₂ is 4.00×10−18 (Mr = 58). Find its solubility in g L−1.
Ksp of Mg(OH)₂ is 4.00×10⁻¹⁸ (Mr = 58). Find its solubility in g L⁻¹.
5.80×10−5 g/L
1.00×10−6 g/L
5.80×10−8 g/L
2.32×10−16 g/L
5.
100 mL of 1.00×10−5 M cation solution is mixed with 100 mL of 1.00×10−4 M anion solution to form AgBr (Ksp = 5.00×10−9). What happens?
100 mL of 1.00×10⁻⁵ M cation solution is mixed with 100 mL of 1.00×10⁻⁴ M anion solution to form AgBr (Ksp = 5.00×10⁻⁹). What happens?
a precipitate forms because Q < Ksp
no precipitate because Q < Ksp
cannot tell without the temperature
a precipitate forms because Q > Ksp
6.
Find [H+] in a 0.2 M weak acid with Ka = 2.50×10−6.
Find [H⁺] in a 0.2 M weak acid with Ka = 2.50×10⁻⁶.
2.50×10−7 mol/L
3.54×10−3 mol/L
5.00×10−7 mol/L
7.07×10−4 mol/L
7.
Ksp of CaCO₃ is 2.50×10−5 (Mr = 100). Find its solubility in g L−1.
Ksp of CaCO₃ is 2.50×10⁻⁵ (Mr = 100). Find its solubility in g L⁻¹.
5.00×10−3 g/L
2.50×10−3 g/L
0.500 g/L
5.00×10−4 g/L
8.
In the equilibrium shown, which option gives two compounds each of which lowers the solubility of Ag₂CrO₄?
In the equilibrium shown, which option gives two compounds each of which lowers the solubility of Ag₂CrO₄?
NaNO₃ ، KNO₃
AgNO₃ ، NaNO₃
NaNO₃ ، K₂CrO₄
AgNO₃ ، K₂CrO₄
9.
Equal-concentration aqueous solutions of the salts shown. Arrange them in increasing pH.
Equal-concentration aqueous solutions of the salts shown. Arrange them in increasing pH.
NaHCO₃ < NH₄Cl < Na₂CO₃
Na₂CO₃ < NH₄Cl < NaHCO₃
NH₄Cl < NaHCO₃ < Na₂CO₃
NaHCO₃ < Na₂CO₃ < NH₄Cl
10.
Find [H+] in a 1.0 M weak acid with Ka = 1.40×10−3.
Find [H⁺] in a 1.0 M weak acid with Ka = 1.40×10⁻³.
0.0651 mol/L
0.0374 mol/L
7.00×10−4 mol/L
1.40×10−3 mol/L
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