(C) For an acidic buffer,the Henderson-Hasselbalch equation is given by: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given $K_a = 10^{-5}$,so $pK_a = -\l

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(C) For an acidic buffer,the Henderson-Hasselbalch equation is given by: $pH = pK_a + \log \frac{[Salt]}{[Acid]}$ Given $K_a = 10^{-5}$,so $pK_a = -\log(10^{-5}) = 5$. Given $pH = 6$. Substituting these values into the equation: $6 = 5 + \log \frac{[Salt]}{[Acid]}$ $6 - 5 = \log \frac{[Salt]}{[Acid]}$ $1 = \log \frac{[Salt]}{[Acid]}$ Taking the antilog on both sides: $\frac{[Salt]}{[Acid]} = 10^1 = 10$ Therefore,the ratio of salt to acid concentration is $10: 1$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Buffer solution

Medium

Addition of sodium hydroxide solution to a weak acid $(HA)$ results in a buffer of $pH \ 6$. If ionisation constant of $HA$ is $10^{-5}$,the ratio of salt to acid concentration in the buffer solution will be

JEE MAIN 2017 All JEE MAIN

A
$4: 5$
B
$1: 10$
C
$10: 1$
D
$5: 4$

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2 Equilibrium: Ionic Equilibrium

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Buffer solution

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Which of the following will not function as a buffer solution?

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$A$ certain acidic solution contains equal concentrations of $X^-$ and $HX$. If $K_b$ for $X^-$ is $10^{-10}$,then the $pH$ of the buffer is equal to:

Medium

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Buffer Solution Volume of $0.1 \ M$ Weak Acid (mL) Volume of $0.1 \ M$ Sodium Salt (mL)

$I$ $4.0$ $4.0$

$II$ $4.0$ $40.0$

$III$ $40.0$ $4.0$

$IV$ $0.1$ $10.0$

Which of the two sets of buffer solutions have the least $pH$?

Buffer Solution	Volume of $0.1 \ M$ Weak Acid (mL)	Volume of $0.1 \ M$ Sodium Salt (mL)
$I$	$4.0$	$4.0$
$II$	$4.0$	$40.0$
$III$	$40.0$	$4.0$
$IV$	$0.1$	$10.0$

DifficultAP EAMCET 2004

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$A$ solution contains $0.1 \ mol$ of acetic acid and $0.1 \ mol$ of sodium acetate in $500 \ mL$ of solution. If the $pH$ of the solution is $4.74$,find the ionization constant $(K_a)$ of acetic acid.

Medium

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Buffer solutions have constant acidity and alkalinity because

DifficultAIPMT 2012

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Addition of sodium hydroxide solution to a weak acid $(HA)$ results in a buffer of $pH \ 6$. If ionisation constant of $HA$ is $10^{-5}$,the ratio of salt to acid concentration in the buffer solution will be

Similar Questions

Which of the following will not function as a buffer solution?

$A$ certain acidic solution contains equal concentrations of $X^-$ and $HX$. If $K_b$ for $X^-$ is $10^{-10}$,then the $pH$ of the buffer is equal to:

Buffer Solution Volume of $0.1 \ M$ Weak Acid (mL) Volume of $0.1 \ M$ Sodium Salt (mL) $I$ $4.0$ $4.0$ $II$ $4.0$ $40.0$ $III$ $40.0$ $4.0$ $IV$ $0.1$ $10.0$ Which of the two sets of buffer solutions have the least $pH$?

$A$ solution contains $0.1 \ mol$ of acetic acid and $0.1 \ mol$ of sodium acetate in $500 \ mL$ of solution. If the $pH$ of the solution is $4.74$,find the ionization constant $(K_a)$ of acetic acid.

Buffer solutions have constant acidity and alkalinity because

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Buffer Solution Volume of $0.1 \ M$ Weak Acid (mL) Volume of $0.1 \ M$ Sodium Salt (mL)

$I$ $4.0$ $4.0$

$II$ $4.0$ $40.0$

$III$ $40.0$ $4.0$

$IV$ $0.1$ $10.0$

Which of the two sets of buffer solutions have the least $pH$?