NET, IAS, State-SET (KSET, WBSET, MPSET, etc.), GATE, CUET, Olympiads etc.: Chemistry MCQs (Practice_Test 16 of 31)
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- Select the statement below that is correct
- All compounds of carbonate (CO32-) phosphate (PO43-) and sulfide (S2-) are soluble
- All compounds of nitrate (NO3-) and chlorate (ClO3-) are soluble
- All compounds of hydroxide (OH-) are soluble
- All compounds of the halogen ions (e. g. Cl-, Br-, I-) are insoluble
- No response above is correct
- Addition of sodium bromide, a very soluble salt, to a saturated solution of silver bromide, a slightly soluble salt, would cause:
- the concentrations of silver ion, bromide ion and silver bromide to increase.
- the concentration of bromide ion to increase and the concentration of silver ion to decrease.
- the concentration of bromide ion to decrease and the concentration of silver ion to increase.
- the concentration of bromide ion to decrease and the concentration of silver bromide to increase.
- Addition of hydrochloric acid to a saturated solution of cadmium hydroxide (Cd (OH) 2, Ksp = 2.5 × 10 − 14) in water would cause:
- the solubility of cadmium hydroxide to decrease.
- the OH-concentration to decrease and the Cd2 + concentration to increase.
- the concentrations of both Cd2 + and OH-to decrease.
- the concentrations of both Cd2 + and OH-to increase.
- no change in the solubility of Cd (OH) 2.
- Given the following slightly soluble salts and solubility-product constants, which salt would be most soluble in pure water?
- AgCl: Ksp = 1.8 × 10 − 10.
- AgBr: Ksp = 5.0 × 10 − 15.
- AgI: Ksp = 8.3 × 10 − 17.
- AuCl: Ksp = 2.0 × 10 − 13.
- The solubility of gold chloride (AuCl3) in pure water is 1.0 × 10 − 6 moles per liter. Calculate the solubility product constant of gold chloride in water.
- N⟋A
- N⟋A
- N⟋A
- N⟋A
- Calculate the molar solubility of cadmium hydroxide (Cd (OH) 2) in pure water. For cadmium hydroxide, Ksp = 2.5 × 10 − 14
- N⟋A
- N⟋A
- N⟋A
- N⟋A
- Calculate the molar solubility of cupric hydroxide (Cu (OH) 2, Ksp = 2.2 × 10 − 20) in a solution buffered at pH 8
- N⟋A
- N⟋A
- N⟋A
- N⟋A
- Assume a solution containing 0.01 M stannous sulfide (SnS, Ksp = 1.0 × 10 − 25) and 0.01 M manganese sulfide (MnS, Ksp = 3.0 × 10 − 15) . If sulfide ion (S2-) concentration is increased gradually without dilution of the solution, what will be the molar concentration of Sn2 + ion when manganese sulfide first starts to precipitate?
- N⟋A
- N⟋A
- N⟋A
- N⟋A
- Which of the following statements is correct?
- Most salts of alkali metal ions (K + , Na +) , most nitrates, most sulfides and most hydroxides are soluble in water.
- Most salts of alkali metal ions (K + , Na +) and most nitrates are insoluble in water and most sulfides and most hydroxides are soluble in water.
- Most salts of alkali metal ions (K + , Na +) and most nitrates are soluble in water and most sulfides and most hydroxides are insoluble in water.
- Most salts of alkali metal ions (K + , Na +) and most sulfides are insoluble in water and and most nitrates and most hydroxides are soluble in water.
- Most salts of alkali metal ions (K + , Na +) , most nitrates, most sulfides and most hydroxides are insoluble in water.
- Which of the following salts is least soluble in otherwise pure water?
- AgCl, Ksp = 1.8 × 10 − 10
- AuCl, Ksp = 2.0 × 10 − 13
- AgI, Ksp = 8.3 × 10 − 17
- AgBr, Ksp = 5.0 × 10 − 15
- CuBr, Ksp = 5.3 × 10 − 9
- Addition of silver nitrate (AgNO3) to a saturated solution of silver chloride (Ksp = 1.8 × 10 − 10) would cause:
- the chloride ion concentration to be larger than that in the saturated solution.
- the chloride ion concentration to be smaller than that in the saturated solution.
- the chloride ion and silver ion concentrations to be larger than that in the saturated solution.
- the chloride ion and silver ion concentrations to be smaller than that in the saturated solution.
- no change in the chloride ion concentration.
- Addition of solid silver chloride to a saturated solution of silver chloride (Ksp = 1.8 × 10 − 10) would cause:
- the chloride ion concentration to be larger than that in the saturated solution.
- no change in the chloride ion concentration.
- the chloride ion and silver ion concentrations to be larger than that in the saturated solution.
- the chloride ion and silver ion concentrations to be smaller than that in the saturated solution.
- the chloride ion concentration to be smaller than that in the saturated solution.
- The solubility of gold chloride (AuCl3 ⟺ Au3 ++ 3Cl-) in water is 1.04 × 10 − 6 mol⟋L. Calculate the value of the solubility-product constant, Ksp, for gold chloride.
- The solubility-product constant for lead iodide (PbI2 ⟺ Pb2 ++ 2I-) is Ksp = 7.1 × 10 − 9. Calculate the molar solubility of lead iodide in otherwise pure water.
- Calculate the molar solubility of lead iodide (PbI2 ⟺ Pb2 ++ 2I-, Ksp = 7.1 × 10 − 9) in a solution containing 0.10 M potassium iodide (KI) , a very soluble salt.
- What mimimum hydronium ion concentration (M) would be needed to prevent precipitation of cupric hydroxide (Cu (OH) 2 ⟺ Cu2 ++ 2OH-, Ksp = 2.2 × 10 − 20) from a solution containing 0.010 M Cu2 + ion?