Buffer Solutions
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CHXI07:EQUILIBRIUM

314527 Which of the following mixture acts as buffer solution?

1 \({\mkern 1mu} {\text{100 ml 0}}{\text{.2 M, C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
2 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.2 M NaOH}}\)
3 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
4 None of the above acts as buffer solution
CHXI07:EQUILIBRIUM

314528 0.1 mole of \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{N}}{{\rm{H}}_{\rm{2}}}\left( {\;{{\rm{K}}_{\rm{b}}}{\rm{ = 5 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}} \right)\) is mixed with 0.08 mole of \(\mathrm{HCl}\) and diluted to one litre. The \({{\rm{H}}^{\rm{ + }}}\) concentration in the solution is \({\text{x}} \times {\text{1}}{{\text{0}}^{{\text{ - y}}}}\) The value of x is

1 4
2 6
3 8
4 10
CHXI07:EQUILIBRIUM

314529 The \(\mathrm{pH}\) of a buffer containing equal molar concentrations of a weak base and its chloride ( \(\mathrm{K}_{\mathrm{b}}\) for weak base \(=2 \times\) \(10^{-5}, \log 2=0.3\) ) is ____.

1 0.3
2 9.3
3 11.5
4 6.3
CHXI07:EQUILIBRIUM

314530 Which of the following will produce a buffer solution when mixed in equal volumes?

1 \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
2 \({\text{0}}{\text{.05}}{\mkern 1mu} {\mkern 1mu} {\text{d}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1 mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
3 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.05}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
4 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ C}}{{\text{H}}_{\text{3}}}{\text{COONa}}\) and \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ NaOH}}\)
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CHXI07:EQUILIBRIUM

314527 Which of the following mixture acts as buffer solution?

1 \({\mkern 1mu} {\text{100 ml 0}}{\text{.2 M, C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
2 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.2 M NaOH}}\)
3 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
4 None of the above acts as buffer solution
CHXI07:EQUILIBRIUM

314528 0.1 mole of \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{N}}{{\rm{H}}_{\rm{2}}}\left( {\;{{\rm{K}}_{\rm{b}}}{\rm{ = 5 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}} \right)\) is mixed with 0.08 mole of \(\mathrm{HCl}\) and diluted to one litre. The \({{\rm{H}}^{\rm{ + }}}\) concentration in the solution is \({\text{x}} \times {\text{1}}{{\text{0}}^{{\text{ - y}}}}\) The value of x is

1 4
2 6
3 8
4 10
CHXI07:EQUILIBRIUM

314529 The \(\mathrm{pH}\) of a buffer containing equal molar concentrations of a weak base and its chloride ( \(\mathrm{K}_{\mathrm{b}}\) for weak base \(=2 \times\) \(10^{-5}, \log 2=0.3\) ) is ____.

1 0.3
2 9.3
3 11.5
4 6.3
CHXI07:EQUILIBRIUM

314530 Which of the following will produce a buffer solution when mixed in equal volumes?

1 \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
2 \({\text{0}}{\text{.05}}{\mkern 1mu} {\mkern 1mu} {\text{d}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1 mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
3 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.05}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
4 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ C}}{{\text{H}}_{\text{3}}}{\text{COONa}}\) and \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ NaOH}}\)
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CHXI07:EQUILIBRIUM

314527 Which of the following mixture acts as buffer solution?

1 \({\mkern 1mu} {\text{100 ml 0}}{\text{.2 M, C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
2 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.2 M NaOH}}\)
3 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
4 None of the above acts as buffer solution
CHXI07:EQUILIBRIUM

314528 0.1 mole of \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{N}}{{\rm{H}}_{\rm{2}}}\left( {\;{{\rm{K}}_{\rm{b}}}{\rm{ = 5 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}} \right)\) is mixed with 0.08 mole of \(\mathrm{HCl}\) and diluted to one litre. The \({{\rm{H}}^{\rm{ + }}}\) concentration in the solution is \({\text{x}} \times {\text{1}}{{\text{0}}^{{\text{ - y}}}}\) The value of x is

1 4
2 6
3 8
4 10
CHXI07:EQUILIBRIUM

314529 The \(\mathrm{pH}\) of a buffer containing equal molar concentrations of a weak base and its chloride ( \(\mathrm{K}_{\mathrm{b}}\) for weak base \(=2 \times\) \(10^{-5}, \log 2=0.3\) ) is ____.

1 0.3
2 9.3
3 11.5
4 6.3
CHXI07:EQUILIBRIUM

314530 Which of the following will produce a buffer solution when mixed in equal volumes?

1 \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
2 \({\text{0}}{\text{.05}}{\mkern 1mu} {\mkern 1mu} {\text{d}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1 mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
3 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.05}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
4 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ C}}{{\text{H}}_{\text{3}}}{\text{COONa}}\) and \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ NaOH}}\)
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CHXI07:EQUILIBRIUM

314527 Which of the following mixture acts as buffer solution?

1 \({\mkern 1mu} {\text{100 ml 0}}{\text{.2 M, C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
2 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.2 M NaOH}}\)
3 \({\text{100 ml 0}}{\text{.1 M C}}{{\text{H}}_{\text{3}}}{\text{COOH + 100 ml 0}}{\text{.1 M NaOH}}\)
4 None of the above acts as buffer solution
CHXI07:EQUILIBRIUM

314528 0.1 mole of \({\rm{C}}{{\rm{H}}_{\rm{3}}}{\rm{N}}{{\rm{H}}_{\rm{2}}}\left( {\;{{\rm{K}}_{\rm{b}}}{\rm{ = 5 \times 1}}{{\rm{0}}^{{\rm{ - 4}}}}} \right)\) is mixed with 0.08 mole of \(\mathrm{HCl}\) and diluted to one litre. The \({{\rm{H}}^{\rm{ + }}}\) concentration in the solution is \({\text{x}} \times {\text{1}}{{\text{0}}^{{\text{ - y}}}}\) The value of x is

1 4
2 6
3 8
4 10
CHXI07:EQUILIBRIUM

314529 The \(\mathrm{pH}\) of a buffer containing equal molar concentrations of a weak base and its chloride ( \(\mathrm{K}_{\mathrm{b}}\) for weak base \(=2 \times\) \(10^{-5}, \log 2=0.3\) ) is ____.

1 0.3
2 9.3
3 11.5
4 6.3
CHXI07:EQUILIBRIUM

314530 Which of the following will produce a buffer solution when mixed in equal volumes?

1 \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1}}\,{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
2 \({\text{0}}{\text{.05}}{\mkern 1mu} {\mkern 1mu} {\text{d}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.1 mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
3 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ N}}{{\text{H}}_{\text{4}}}{\text{OH}}\) and \({\text{0}}{\text{.05}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ HCl}}\)
4 \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ C}}{{\text{H}}_{\text{3}}}{\text{COONa}}\) and \({\text{0}}{\text{.1}}\;{\text{mold}}{{\text{m}}^{{\text{ - 3}}}}{\text{ NaOH}}\)
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