(B) Given $K_a = 10^{-5}$,so $pK_a = -\log(10^{-5}) = 5$. At one-third neutralization,the amount of salt formed is $1/3$ and the amount of acid remain

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(B) Given $K_a = 10^{-5}$,so $pK_a = -\log(10^{-5}) = 5$. At one-third neutralization,the amount of salt formed is $1/3$ and the amount of acid remaining is $2/3$ of the initial concentration. According to the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[\text{Salt}]}{[\text{Acid}]}$ $pH = 5 + \log \frac{1/3}{2/3}$ $pH = 5 + \log \frac{1}{2}$ $pH = 5 - \log 2$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Buffer solution

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$A$ weak acid with a dissociation constant of $10^{-5}$ is being titrated with an aqueous $NaOH$ solution. The $pH$ at the point of one-third neutralization of the acid will be:

WBJEE 2010 All WBJEE

A
$5 + \log 2 - \log 3$
B
$5 - \log 2$
C
$5 - \log 3$
D
$5 - \log 6$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Buffer solution

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$A$ buffer solution contains $100 \ mL$ of $0.01 \ M \ CH_3COOH$ and $200 \ mL$ of $0.02 \ M \ CH_3COONa$. If $700 \ mL$ of $1 \ M \ NaCl$ is added,what are the $pH$ values before and after the addition? $(pK_a = 4.74)$

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The $pH$ of the blood buffer $CO_2-HCO_3^-$ is $7.4$. The ratio of conjugate base to acid is ....... $(K_a (H_2CO_3) = 4.5 \times 10^{-7})$

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For a weak acid $(HA)$,$pK_a = 4.5$. The $pOH$ of a buffer solution of $HA$ in which $50\%$ of the acid is ionized is:

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

MediumAP EAMCET 2001

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$A$ solution of $0.1 \ mol$ of $CH_3NH_2$ $(K_b = 5 \times 10^{-4})$ and $0.08 \ mol$ of $HCl$ is diluted to $1 \ L$. The $pOH$ of the resulting solution is $(\log 1.25 = 0.1)$.

MediumTS EAMCET 2019

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$A$ weak acid with a dissociation constant of $10^{-5}$ is being titrated with an aqueous $NaOH$ solution. The $pH$ at the point of one-third neutralization of the acid will be:

Similar Questions

$A$ buffer solution contains $100 \ mL$ of $0.01 \ M \ CH_3COOH$ and $200 \ mL$ of $0.02 \ M \ CH_3COONa$. If $700 \ mL$ of $1 \ M \ NaCl$ is added,what are the $pH$ values before and after the addition? $(pK_a = 4.74)$

The $pH$ of the blood buffer $CO_2-HCO_3^-$ is $7.4$. The ratio of conjugate base to acid is ....... $(K_a (H_2CO_3) = 4.5 \times 10^{-7})$

For a weak acid $(HA)$,$pK_a = 4.5$. The $pOH$ of a buffer solution of $HA$ in which $50\%$ of the acid is ionized is:

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

$A$ solution of $0.1 \ mol$ of $CH_3NH_2$ $(K_b = 5 \times 10^{-4})$ and $0.08 \ mol$ of $HCl$ is diluted to $1 \ L$. The $pOH$ of the resulting solution is $(\log 1.25 = 0.1)$.

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