(C) The $pH$ is defined as $pH = -\log[H^{+}]$.For $pH_1 = 3$,$[H^{+}]_1 = 10^{-3} \ M$.For $pH_2 = 6$,$[H^{+}]_2 = 10^{-6} \ M$.The ratio of concentr

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(C) The $pH$ is defined as $pH = -\log[H^{+}]$.For $pH_1 = 3$,$[H^{+}]_1 = 10^{-3} \ M$.For $pH_2 = 6$,$[H^{+}]_2 = 10^{-6} \ M$.The ratio of concentrations is $\frac{[H^{+}]_1}{[H^{+}]_2} = \frac{10^{-3}}{10^{-6}} = 10^{3} = 1000$.Therefore,the $H^{+}$ ion concentration decreases by $1000$ times.

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

Easy

If the $pH$ of a solution increases from $3$ to $6$,then its $H^{+}$ ion concentration:

A
decreases by half.
B
doubles.
C
decreases by $1000$ times.
D
increases by $1000$ times.

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Chapter

2 Equilibrium: Ionic Equilibrium

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Water hydrolysis and pH scale

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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The $pH$ of $1 \ N \ H_2O$ is

Medium

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Which equation represents the $pH$ of a solution?

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What will be the hydrogen ion concentration in moles $L^{-1}$ of a solution whose $pH$ is $4.58$?

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The number of $H^{+}$ ions present in $10 \ mL$ of a solution with $pH = 12$ is ........

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If the $pH$ of a solution increases from $3$ to $6$,then its $H^{+}$ ion concentration:

Similar Questions

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

The $pH$ of $1 \ N \ H_2O$ is

Which equation represents the $pH$ of a solution?

What will be the hydrogen ion concentration in moles $L^{-1}$ of a solution whose $pH$ is $4.58$?

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