314939
Assertion : \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). Reason : \(\mathrm{HCl}\) is a strong acid.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Pure \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). This is due to the common ion effect. The concentration of \(\mathrm{Cl}^{-}\)increases in the solution, due to which the reaction of dissociation of \(\mathrm{NaCl}\) moves in the backward direction leading to precipitation of \(\mathrm{NaCl}\). \(\mathrm{HCl}\) is strong acid in aq.solution but the strength of it has no relation with assertion.
AIIMS - 2007
CHXI07:EQUILIBRIUM
314940
Solubility of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) is decreased in the presence of
1 \(\mathrm{AgNO}_{3}\)
2 \(\mathrm{AgCl}\)
3 \(\mathrm{BaCrO}_{4}\)
4 \(\mathrm{PbCrO}_{4}\)
Explanation:
\(\mathrm {\mathrm{AgCl}, \mathrm{BaCrO}_{4}, \mathrm{PbCrO}_{4}}\) are sparingly soluble salts, and hence are not effective in decreasing solubility of \(\mathrm {\mathrm{Ag}_{2} \mathrm{CrO}_{4}}\).
CHXI07:EQUILIBRIUM
314941
The solubility of \({\text{AgI}}\) in \({\text{NaI}}\) solution is less than that in pure water, because
1 the temperature of the solution decreases
2 solubility product of \({\text{AgI}}\) is less than that of \({\text{NaI}}\)
3 of common ion effect
4 \({\text{AgI}}\) forms complex with \({\text{NaI}}\)
Explanation:
The solubility of \({{\rm{AgI}}}\) in NaI solution is less than that in pure water because of common ion effect of \({{{\rm{I}}^ - }}\) ions suppresses the dissociation of \({{\rm{AgI}}}\)
CHXI07:EQUILIBRIUM
314942
\({\text{MY}}\), and \({\text{N}}{{\text{Y}}_{\text{3}}}\) two nearly insoluble salts, have the same \({{\rm{K}}_{{\rm{SP}}}}\) values of \(6.2 \times 10^{-13}\) at room temperature. Which statement would be true in regard to \(\mathrm{MY}\) and \(\mathrm{NY}_{3}\) ?
1 The addition of the salt of \({\text{KY}}\) to solution of \(\mathrm{MY}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) will have no effect on their solubilities.
2 The molar solubilities of \({\text{MY}}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) in water are identical.
3 The molar solubility of \({\rm{MY}}\) in water is less than that of \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\)
4 The salts \({\rm{MY}}\) and \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\) are more soluble in \({\text{0}}{\text{.5M}}\) \({\text{KY}}\) than in pure water.
Explanation:
\({\text{MY}}{\mkern 1mu} {{\text{K}}_{{\text{SP}}}}{\text{ = S}}_{\text{1}}^{\text{2}}{\text{ = 6}}{\text{.2}} \times {\text{1}}{{\text{0}}^{{\text{ - 13}}}}{\text{ = 62}} \times {\text{1}}{{\text{0}}^{{\text{ - 14}}}}\) \(\mathrm {S_{1}=7.9 \times 10^{-7} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water \(\mathrm {M Y_{3} K_{S P}=27 S_{2}^{4}=6.2 \times 10^{-14}}\) \(\mathrm {S_{2}=10^{-3.5} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water Solubility of \(\mathrm {\mathrm{NY}_{3}>}\) solubility of \({\text{MY}}\) so \(\rm {{{\text{3}}^{{\text{rd}}}}}\) statement is true. Addition of KY will decrease the solubility due to common ion effect.
314939
Assertion : \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). Reason : \(\mathrm{HCl}\) is a strong acid.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Pure \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). This is due to the common ion effect. The concentration of \(\mathrm{Cl}^{-}\)increases in the solution, due to which the reaction of dissociation of \(\mathrm{NaCl}\) moves in the backward direction leading to precipitation of \(\mathrm{NaCl}\). \(\mathrm{HCl}\) is strong acid in aq.solution but the strength of it has no relation with assertion.
AIIMS - 2007
CHXI07:EQUILIBRIUM
314940
Solubility of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) is decreased in the presence of
1 \(\mathrm{AgNO}_{3}\)
2 \(\mathrm{AgCl}\)
3 \(\mathrm{BaCrO}_{4}\)
4 \(\mathrm{PbCrO}_{4}\)
Explanation:
\(\mathrm {\mathrm{AgCl}, \mathrm{BaCrO}_{4}, \mathrm{PbCrO}_{4}}\) are sparingly soluble salts, and hence are not effective in decreasing solubility of \(\mathrm {\mathrm{Ag}_{2} \mathrm{CrO}_{4}}\).
CHXI07:EQUILIBRIUM
314941
The solubility of \({\text{AgI}}\) in \({\text{NaI}}\) solution is less than that in pure water, because
1 the temperature of the solution decreases
2 solubility product of \({\text{AgI}}\) is less than that of \({\text{NaI}}\)
3 of common ion effect
4 \({\text{AgI}}\) forms complex with \({\text{NaI}}\)
Explanation:
The solubility of \({{\rm{AgI}}}\) in NaI solution is less than that in pure water because of common ion effect of \({{{\rm{I}}^ - }}\) ions suppresses the dissociation of \({{\rm{AgI}}}\)
CHXI07:EQUILIBRIUM
314942
\({\text{MY}}\), and \({\text{N}}{{\text{Y}}_{\text{3}}}\) two nearly insoluble salts, have the same \({{\rm{K}}_{{\rm{SP}}}}\) values of \(6.2 \times 10^{-13}\) at room temperature. Which statement would be true in regard to \(\mathrm{MY}\) and \(\mathrm{NY}_{3}\) ?
1 The addition of the salt of \({\text{KY}}\) to solution of \(\mathrm{MY}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) will have no effect on their solubilities.
2 The molar solubilities of \({\text{MY}}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) in water are identical.
3 The molar solubility of \({\rm{MY}}\) in water is less than that of \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\)
4 The salts \({\rm{MY}}\) and \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\) are more soluble in \({\text{0}}{\text{.5M}}\) \({\text{KY}}\) than in pure water.
Explanation:
\({\text{MY}}{\mkern 1mu} {{\text{K}}_{{\text{SP}}}}{\text{ = S}}_{\text{1}}^{\text{2}}{\text{ = 6}}{\text{.2}} \times {\text{1}}{{\text{0}}^{{\text{ - 13}}}}{\text{ = 62}} \times {\text{1}}{{\text{0}}^{{\text{ - 14}}}}\) \(\mathrm {S_{1}=7.9 \times 10^{-7} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water \(\mathrm {M Y_{3} K_{S P}=27 S_{2}^{4}=6.2 \times 10^{-14}}\) \(\mathrm {S_{2}=10^{-3.5} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water Solubility of \(\mathrm {\mathrm{NY}_{3}>}\) solubility of \({\text{MY}}\) so \(\rm {{{\text{3}}^{{\text{rd}}}}}\) statement is true. Addition of KY will decrease the solubility due to common ion effect.
314939
Assertion : \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). Reason : \(\mathrm{HCl}\) is a strong acid.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Pure \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). This is due to the common ion effect. The concentration of \(\mathrm{Cl}^{-}\)increases in the solution, due to which the reaction of dissociation of \(\mathrm{NaCl}\) moves in the backward direction leading to precipitation of \(\mathrm{NaCl}\). \(\mathrm{HCl}\) is strong acid in aq.solution but the strength of it has no relation with assertion.
AIIMS - 2007
CHXI07:EQUILIBRIUM
314940
Solubility of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) is decreased in the presence of
1 \(\mathrm{AgNO}_{3}\)
2 \(\mathrm{AgCl}\)
3 \(\mathrm{BaCrO}_{4}\)
4 \(\mathrm{PbCrO}_{4}\)
Explanation:
\(\mathrm {\mathrm{AgCl}, \mathrm{BaCrO}_{4}, \mathrm{PbCrO}_{4}}\) are sparingly soluble salts, and hence are not effective in decreasing solubility of \(\mathrm {\mathrm{Ag}_{2} \mathrm{CrO}_{4}}\).
CHXI07:EQUILIBRIUM
314941
The solubility of \({\text{AgI}}\) in \({\text{NaI}}\) solution is less than that in pure water, because
1 the temperature of the solution decreases
2 solubility product of \({\text{AgI}}\) is less than that of \({\text{NaI}}\)
3 of common ion effect
4 \({\text{AgI}}\) forms complex with \({\text{NaI}}\)
Explanation:
The solubility of \({{\rm{AgI}}}\) in NaI solution is less than that in pure water because of common ion effect of \({{{\rm{I}}^ - }}\) ions suppresses the dissociation of \({{\rm{AgI}}}\)
CHXI07:EQUILIBRIUM
314942
\({\text{MY}}\), and \({\text{N}}{{\text{Y}}_{\text{3}}}\) two nearly insoluble salts, have the same \({{\rm{K}}_{{\rm{SP}}}}\) values of \(6.2 \times 10^{-13}\) at room temperature. Which statement would be true in regard to \(\mathrm{MY}\) and \(\mathrm{NY}_{3}\) ?
1 The addition of the salt of \({\text{KY}}\) to solution of \(\mathrm{MY}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) will have no effect on their solubilities.
2 The molar solubilities of \({\text{MY}}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) in water are identical.
3 The molar solubility of \({\rm{MY}}\) in water is less than that of \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\)
4 The salts \({\rm{MY}}\) and \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\) are more soluble in \({\text{0}}{\text{.5M}}\) \({\text{KY}}\) than in pure water.
Explanation:
\({\text{MY}}{\mkern 1mu} {{\text{K}}_{{\text{SP}}}}{\text{ = S}}_{\text{1}}^{\text{2}}{\text{ = 6}}{\text{.2}} \times {\text{1}}{{\text{0}}^{{\text{ - 13}}}}{\text{ = 62}} \times {\text{1}}{{\text{0}}^{{\text{ - 14}}}}\) \(\mathrm {S_{1}=7.9 \times 10^{-7} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water \(\mathrm {M Y_{3} K_{S P}=27 S_{2}^{4}=6.2 \times 10^{-14}}\) \(\mathrm {S_{2}=10^{-3.5} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water Solubility of \(\mathrm {\mathrm{NY}_{3}>}\) solubility of \({\text{MY}}\) so \(\rm {{{\text{3}}^{{\text{rd}}}}}\) statement is true. Addition of KY will decrease the solubility due to common ion effect.
314939
Assertion : \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). Reason : \(\mathrm{HCl}\) is a strong acid.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Pure \({\text{NaCl}}\) is precipitated when \(\mathrm{HCl}\) gas is passed in a saturated solution of \(\mathrm{NaCl}\). This is due to the common ion effect. The concentration of \(\mathrm{Cl}^{-}\)increases in the solution, due to which the reaction of dissociation of \(\mathrm{NaCl}\) moves in the backward direction leading to precipitation of \(\mathrm{NaCl}\). \(\mathrm{HCl}\) is strong acid in aq.solution but the strength of it has no relation with assertion.
AIIMS - 2007
CHXI07:EQUILIBRIUM
314940
Solubility of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\) is decreased in the presence of
1 \(\mathrm{AgNO}_{3}\)
2 \(\mathrm{AgCl}\)
3 \(\mathrm{BaCrO}_{4}\)
4 \(\mathrm{PbCrO}_{4}\)
Explanation:
\(\mathrm {\mathrm{AgCl}, \mathrm{BaCrO}_{4}, \mathrm{PbCrO}_{4}}\) are sparingly soluble salts, and hence are not effective in decreasing solubility of \(\mathrm {\mathrm{Ag}_{2} \mathrm{CrO}_{4}}\).
CHXI07:EQUILIBRIUM
314941
The solubility of \({\text{AgI}}\) in \({\text{NaI}}\) solution is less than that in pure water, because
1 the temperature of the solution decreases
2 solubility product of \({\text{AgI}}\) is less than that of \({\text{NaI}}\)
3 of common ion effect
4 \({\text{AgI}}\) forms complex with \({\text{NaI}}\)
Explanation:
The solubility of \({{\rm{AgI}}}\) in NaI solution is less than that in pure water because of common ion effect of \({{{\rm{I}}^ - }}\) ions suppresses the dissociation of \({{\rm{AgI}}}\)
CHXI07:EQUILIBRIUM
314942
\({\text{MY}}\), and \({\text{N}}{{\text{Y}}_{\text{3}}}\) two nearly insoluble salts, have the same \({{\rm{K}}_{{\rm{SP}}}}\) values of \(6.2 \times 10^{-13}\) at room temperature. Which statement would be true in regard to \(\mathrm{MY}\) and \(\mathrm{NY}_{3}\) ?
1 The addition of the salt of \({\text{KY}}\) to solution of \(\mathrm{MY}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) will have no effect on their solubilities.
2 The molar solubilities of \({\text{MY}}\) and \({\text{N}}{{\text{Y}}_{\text{3}}}\) in water are identical.
3 The molar solubility of \({\rm{MY}}\) in water is less than that of \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\)
4 The salts \({\rm{MY}}\) and \({\rm{N}}{{\rm{Y}}_{\rm{3}}}\) are more soluble in \({\text{0}}{\text{.5M}}\) \({\text{KY}}\) than in pure water.
Explanation:
\({\text{MY}}{\mkern 1mu} {{\text{K}}_{{\text{SP}}}}{\text{ = S}}_{\text{1}}^{\text{2}}{\text{ = 6}}{\text{.2}} \times {\text{1}}{{\text{0}}^{{\text{ - 13}}}}{\text{ = 62}} \times {\text{1}}{{\text{0}}^{{\text{ - 14}}}}\) \(\mathrm {S_{1}=7.9 \times 10^{-7} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water \(\mathrm {M Y_{3} K_{S P}=27 S_{2}^{4}=6.2 \times 10^{-14}}\) \(\mathrm {S_{2}=10^{-3.5} \mathrm{~mol} / \mathrm{L}=}\) Solubility in pure water Solubility of \(\mathrm {\mathrm{NY}_{3}>}\) solubility of \({\text{MY}}\) so \(\rm {{{\text{3}}^{{\text{rd}}}}}\) statement is true. Addition of KY will decrease the solubility due to common ion effect.
