Buffer Solutions
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CHXI07:EQUILIBRIUM

314522 pH of an aqueous solution of \({\mathrm{0.6\, \mathrm{M}\, \mathrm{NH}_{3}}}\) and \({\mathrm{0.4 \, \mathrm{M} \, \mathrm{NH}_{4} \mathrm{Cl}}}\) is 9.4 \({\rm{(p}}{{\rm{K}}_{\rm{b}}}{\rm{ = }}\,{\rm{4}}.{\rm{74}})\). The new pH when \({\mathrm{0.1 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}}}\) solution is added to it is

1 9.86
2 3.75
3 7.25
4 10.5
CHXI07:EQUILIBRIUM

314523 Which one of the following mixture does not act as a buffer solution?

1 Boric acid an borax
2 Sodium acetate and sodium propionate
3 Sodium phosphate and disodium hydrogen phosphate
4 Sodium propionate and propionic acid
CHXI07:EQUILIBRIUM

314524 Read the Statement -A and Statement -B carefully to mark the correct options given below:
Statement A :
Mixture of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) is an example of acidic buffer.
Statement B :
Acidic buffer contains equimolar mixture of a weak acid and its salt with strong base.

1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
CHXI07:EQUILIBRIUM

314525 The \(\mathrm{pH}\) of an acid buffer can be raised by 2 units by

1 Increasing the concentration of both weak acid and salt by two moles
2 Increasing the concentration of both the acid and salt by 10 times
3 Diluting the solution by 10 times
4 Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times.
CHXI07:EQUILIBRIUM

314526 To a buffer solution of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\), some \(\mathrm{HCl}\) is added. The excess of \(\left[\mathrm{H}^{+}\right]\)ions are removed by the following equation

1 \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\)
3 \(\mathrm{Na}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{NaOH}\)
4 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{Na}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}\)
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CHXI07:EQUILIBRIUM

314522 pH of an aqueous solution of \({\mathrm{0.6\, \mathrm{M}\, \mathrm{NH}_{3}}}\) and \({\mathrm{0.4 \, \mathrm{M} \, \mathrm{NH}_{4} \mathrm{Cl}}}\) is 9.4 \({\rm{(p}}{{\rm{K}}_{\rm{b}}}{\rm{ = }}\,{\rm{4}}.{\rm{74}})\). The new pH when \({\mathrm{0.1 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}}}\) solution is added to it is

1 9.86
2 3.75
3 7.25
4 10.5
CHXI07:EQUILIBRIUM

314523 Which one of the following mixture does not act as a buffer solution?

1 Boric acid an borax
2 Sodium acetate and sodium propionate
3 Sodium phosphate and disodium hydrogen phosphate
4 Sodium propionate and propionic acid
CHXI07:EQUILIBRIUM

314524 Read the Statement -A and Statement -B carefully to mark the correct options given below:
Statement A :
Mixture of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) is an example of acidic buffer.
Statement B :
Acidic buffer contains equimolar mixture of a weak acid and its salt with strong base.

1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
CHXI07:EQUILIBRIUM

314525 The \(\mathrm{pH}\) of an acid buffer can be raised by 2 units by

1 Increasing the concentration of both weak acid and salt by two moles
2 Increasing the concentration of both the acid and salt by 10 times
3 Diluting the solution by 10 times
4 Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times.
CHXI07:EQUILIBRIUM

314526 To a buffer solution of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\), some \(\mathrm{HCl}\) is added. The excess of \(\left[\mathrm{H}^{+}\right]\)ions are removed by the following equation

1 \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\)
3 \(\mathrm{Na}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{NaOH}\)
4 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{Na}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}\)
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CHXI07:EQUILIBRIUM

314522 pH of an aqueous solution of \({\mathrm{0.6\, \mathrm{M}\, \mathrm{NH}_{3}}}\) and \({\mathrm{0.4 \, \mathrm{M} \, \mathrm{NH}_{4} \mathrm{Cl}}}\) is 9.4 \({\rm{(p}}{{\rm{K}}_{\rm{b}}}{\rm{ = }}\,{\rm{4}}.{\rm{74}})\). The new pH when \({\mathrm{0.1 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}}}\) solution is added to it is

1 9.86
2 3.75
3 7.25
4 10.5
CHXI07:EQUILIBRIUM

314523 Which one of the following mixture does not act as a buffer solution?

1 Boric acid an borax
2 Sodium acetate and sodium propionate
3 Sodium phosphate and disodium hydrogen phosphate
4 Sodium propionate and propionic acid
CHXI07:EQUILIBRIUM

314524 Read the Statement -A and Statement -B carefully to mark the correct options given below:
Statement A :
Mixture of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) is an example of acidic buffer.
Statement B :
Acidic buffer contains equimolar mixture of a weak acid and its salt with strong base.

1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
CHXI07:EQUILIBRIUM

314525 The \(\mathrm{pH}\) of an acid buffer can be raised by 2 units by

1 Increasing the concentration of both weak acid and salt by two moles
2 Increasing the concentration of both the acid and salt by 10 times
3 Diluting the solution by 10 times
4 Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times.
CHXI07:EQUILIBRIUM

314526 To a buffer solution of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\), some \(\mathrm{HCl}\) is added. The excess of \(\left[\mathrm{H}^{+}\right]\)ions are removed by the following equation

1 \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\)
3 \(\mathrm{Na}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{NaOH}\)
4 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{Na}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}\)
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CHXI07:EQUILIBRIUM

314522 pH of an aqueous solution of \({\mathrm{0.6\, \mathrm{M}\, \mathrm{NH}_{3}}}\) and \({\mathrm{0.4 \, \mathrm{M} \, \mathrm{NH}_{4} \mathrm{Cl}}}\) is 9.4 \({\rm{(p}}{{\rm{K}}_{\rm{b}}}{\rm{ = }}\,{\rm{4}}.{\rm{74}})\). The new pH when \({\mathrm{0.1 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}}}\) solution is added to it is

1 9.86
2 3.75
3 7.25
4 10.5
CHXI07:EQUILIBRIUM

314523 Which one of the following mixture does not act as a buffer solution?

1 Boric acid an borax
2 Sodium acetate and sodium propionate
3 Sodium phosphate and disodium hydrogen phosphate
4 Sodium propionate and propionic acid
CHXI07:EQUILIBRIUM

314524 Read the Statement -A and Statement -B carefully to mark the correct options given below:
Statement A :
Mixture of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) is an example of acidic buffer.
Statement B :
Acidic buffer contains equimolar mixture of a weak acid and its salt with strong base.

1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
CHXI07:EQUILIBRIUM

314525 The \(\mathrm{pH}\) of an acid buffer can be raised by 2 units by

1 Increasing the concentration of both weak acid and salt by two moles
2 Increasing the concentration of both the acid and salt by 10 times
3 Diluting the solution by 10 times
4 Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times.
CHXI07:EQUILIBRIUM

314526 To a buffer solution of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\), some \(\mathrm{HCl}\) is added. The excess of \(\left[\mathrm{H}^{+}\right]\)ions are removed by the following equation

1 \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\)
3 \(\mathrm{Na}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{NaOH}\)
4 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{Na}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}\)
NEET DIGITAL LIBRARY
CHXI07:EQUILIBRIUM

314522 pH of an aqueous solution of \({\mathrm{0.6\, \mathrm{M}\, \mathrm{NH}_{3}}}\) and \({\mathrm{0.4 \, \mathrm{M} \, \mathrm{NH}_{4} \mathrm{Cl}}}\) is 9.4 \({\rm{(p}}{{\rm{K}}_{\rm{b}}}{\rm{ = }}\,{\rm{4}}.{\rm{74}})\). The new pH when \({\mathrm{0.1 \mathrm{M} \mathrm{Ca}(\mathrm{OH})_{2}}}\) solution is added to it is

1 9.86
2 3.75
3 7.25
4 10.5
CHXI07:EQUILIBRIUM

314523 Which one of the following mixture does not act as a buffer solution?

1 Boric acid an borax
2 Sodium acetate and sodium propionate
3 Sodium phosphate and disodium hydrogen phosphate
4 Sodium propionate and propionic acid
CHXI07:EQUILIBRIUM

314524 Read the Statement -A and Statement -B carefully to mark the correct options given below:
Statement A :
Mixture of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONH}_{4}\) is an example of acidic buffer.
Statement B :
Acidic buffer contains equimolar mixture of a weak acid and its salt with strong base.

1 Statement A is correct but Statement B is incorrect.
2 Statement A is incorrect but Statement B is correct.
3 Both statements are correct.
4 Both Statements are incorrect.
CHXI07:EQUILIBRIUM

314525 The \(\mathrm{pH}\) of an acid buffer can be raised by 2 units by

1 Increasing the concentration of both weak acid and salt by two moles
2 Increasing the concentration of both the acid and salt by 10 times
3 Diluting the solution by 10 times
4 Increasing the concentration of the salt by 10 times and decreasing concentration of the acid by 10 times.
CHXI07:EQUILIBRIUM

314526 To a buffer solution of \(\mathrm{CH}_{3} \mathrm{COOH}\) and \(\mathrm{CH}_{3} \mathrm{COONa}\), some \(\mathrm{HCl}\) is added. The excess of \(\left[\mathrm{H}^{+}\right]\)ions are removed by the following equation

1 \(\mathrm{CH}_{3} \mathrm{COOH}+\mathrm{OH}^{-} \rightarrow \mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}_{2} \mathrm{O}\)
2 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{H}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COOH}\)
3 \(\mathrm{Na}^{+}+\mathrm{OH}^{-} \rightarrow \mathrm{NaOH}\)
4 \(\mathrm{CH}_{3} \mathrm{COO}^{-}+\mathrm{Na}^{+} \rightarrow \mathrm{CH}_{3} \mathrm{COONa}\)