(C) Given: $[OH^{-}] = 10^{-9} \ M$ at $25^{\circ}C$.We know that $K_w = [H^{+}] [OH^{-}] = 10^{-14}$.Therefore,$[H^{+}] = \frac{10^{-14}}{10^{-9}} =

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(C) Given: $[OH^{-}] = 10^{-9} \ M$ at $25^{\circ}C$.We know that $K_w = [H^{+}] [OH^{-}] = 10^{-14}$.Therefore,$[H^{+}] = \frac{10^{-14}}{10^{-9}} = 10^{-5} \ M$.The $pH$ is calculated as $pH = -\log[H^{+}]$.$pH = -\log(10^{-5}) = 5$.

Class 11 Chemistry 6-2.Equilibrium-II (Ionic Equilibrium)Water hydrolysis and pH scale

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

A
$9$
B
$10$
C
$5$
D
$11$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Water hydrolysis and pH scale

What is the $pH$ of a neutral solution at the normal temperature of the human body $(37^{\circ}C)$?

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At a certain temperature,if $pK_w = 12.60$,then which of the following is correct for an acidic solution?

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In a solution of acid,the $H^{+}$ concentration is $10^{-10} \ M$. The $pH$ of this solution will be:

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

Similar Questions

What is the $pH$ of a neutral solution at the normal temperature of the human body $(37^{\circ}C)$?

At a certain temperature,if $pK_w = 12.60$,then which of the following is correct for an acidic solution?

In a solution of acid,the $H^{+}$ concentration is $10^{-10} \ M$. The $pH$ of this solution will be:

When pure water is taken in a container and it absorbs $CO_2$ from the atmosphere,what will be the $pH$?

The $pH$ of a soft drink is $3.82$. Its hydrogen ion concentration will be

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