(B) For a weak acid titrated with a strong base,the $pH$ is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.Give

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(B) For a weak acid titrated with a strong base,the $pH$ is given by the Henderson-Hasselbalch equation: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$.Given $K_a = 10^{-5}$,so $pK_a = -\log(10^{-5}) = 5$.At one-third neutralization,the concentration of salt (conjugate base) is $1/3$ and the remaining concentration of acid is $2/3$.Substituting these values: $pH = 5 + \log \frac{1/3}{2/3}$.$pH = 5 + \log(1/2) = 5 - \log 2$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium pH of weak Acids and weak Bases

Medium

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

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

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2 Equilibrium: Ionic Equilibrium

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pH of weak Acids and weak Bases

$pH$ value of a solution,whose hydronium ion concentration is $6.2 \times 10^{-9} \ mol/L$,is

MediumAIIMS 2000

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The percentage dissociation of a decinormal solution of a weak acid $HA$ is: $(K_a = 4.9 \times 10^{-8})$

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The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

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The dissociation constant of a monoacidic weak base $MOH$ is $1.8 \times 10^{-5}$. What is the concentration of $OH^{-}$ ions in its $0.1 \, M$ solution?

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At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?
$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$

MediumAP EAMCET 2025

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

Similar Questions

$pH$ value of a solution,whose hydronium ion concentration is $6.2 \times 10^{-9} \ mol/L$,is

The percentage dissociation of a decinormal solution of a weak acid $HA$ is: $(K_a = 4.9 \times 10^{-8})$

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

The dissociation constant of a monoacidic weak base $MOH$ is $1.8 \times 10^{-5}$. What is the concentration of $OH^{-}$ ions in its $0.1 \, M$ solution?

At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$

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At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?
$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$