(B) The relationship between $pH$ and hydrogen ion concentration is given by the formula: $pH = - \log [H^+]$.As the $pH$ value decreases,the term $-\

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(B) The relationship between $pH$ and hydrogen ion concentration is given by the formula: $pH = - \log [H^+]$.As the $pH$ value decreases,the term $-\log [H^+]$ decreases,which implies that the value of $[H^+]$ must increase.Therefore,the hydrogen ion concentration increases.

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

Medium

When $pH$ of a solution decreases,its hydrogen ion concentration

A
Decreases
B
Increases
C
Rapidly increases
D
Remains always constant

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Class 11 Questions

Class 11

Chemistry Questions

Chapter

2 Equilibrium: Ionic Equilibrium

Subtopic

Water hydrolysis and pH scale

The ionic product of water at $50^{\circ} C$ is $4 \times 10^{-14}$. The $pH$ and nature of water is :

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The hydrogen ion concentration in a given solution is $6 \times 10^{-4} \ M$. Its $pH$ will be

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An alcoholic drink has a $pH = 4.7$. What is the $OH^{-}$ ion concentration of this solution? (Given: $K_w = 10^{-14} \ mol^2/L^2$)

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At $25^{\circ}C$,if $[OH^{-}] = 10^{-9} \ M$,find the $pH$ value of the solution.

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

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When $pH$ of a solution decreases,its hydrogen ion concentration

Similar Questions

The ionic product of water at $50^{\circ} C$ is $4 \times 10^{-14}$. The $pH$ and nature of water is :

The hydrogen ion concentration in a given solution is $6 \times 10^{-4} \ M$. Its $pH$ will be

An alcoholic drink has a $pH = 4.7$. What is the $OH^{-}$ ion concentration of this solution? (Given: $K_w = 10^{-14} \ mol^2/L^2$)

At $25^{\circ}C$,if $[OH^{-}] = 10^{-9} \ M$,find the $pH$ value of the solution.

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

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