(D) The ionic product of water is defined as $K_w = [H^+][OH^-]$.By definition,$pK_w = -\log(K_w)$.Given $K_w = 10^{-13} \ M^2$,we have $pK_w = -\log(

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(D) The ionic product of water is defined as $K_w = [H^+][OH^-]$.By definition,$pK_w = -\log(K_w)$.Given $K_w = 10^{-13} \ M^2$,we have $pK_w = -\log(10^{-13}) = 13$.Since $pH = -\log[H^+]$ and $pOH = -\log[OH^-]$,the relationship between $pH$,$pOH$,and $pK_w$ is given by $pH + pOH = pK_w$.Therefore,at $62 \ ^\circ C$,the sum $pH + pOH = 13$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium Water hydrolysis and pH scale

Medium

Given that $K_w$ for water is $10^{-13} \ M^2$ at $62 \ ^\circ C$,compute the sum of $pOH$ and $pH$ for a neutral aqueous solution at $62 \ ^\circ C$.

A
$7$
B
$13.30$
C
$14$
D
$13$

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Chapter

2 Equilibrium: Ionic Equilibrium

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Water hydrolysis and pH scale

The concentration of hydrogen ion in pure water at $298 \ K$ is:

Medium

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$A$ is an aqueous acid; $B$ is an aqueous base. They are diluted separately,then:

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Statement-$I$ :- $pH$ of pure water increases with increase in temperature.
Statement-$II$ :- Degree of ionisation increases with increase in temperature.

Medium

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What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?
$(\log 1.342 = 0.1277)$

MediumMHT CET 2022

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Explain the $pH$ scale and $pH$.

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Given that $K_w$ for water is $10^{-13} \ M^2$ at $62 \ ^\circ C$,compute the sum of $pOH$ and $pH$ for a neutral aqueous solution at $62 \ ^\circ C$.

Similar Questions

The concentration of hydrogen ion in pure water at $298 \ K$ is:

$A$ is an aqueous acid; $B$ is an aqueous base. They are diluted separately,then:

Statement-$I$ :- $pH$ of pure water increases with increase in temperature.Statement-$II$ :- Degree of ionisation increases with increase in temperature.

What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?$(\log 1.342 = 0.1277)$

Explain the $pH$ scale and $pH$.

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Statement-$I$ :- $pH$ of pure water increases with increase in temperature.
Statement-$II$ :- Degree of ionisation increases with increase in temperature.

What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?
$(\log 1.342 = 0.1277)$