(B) The $pH$ of a solution is defined as $pH = -\log[H^{+}]$.Given $pH = 0$,we have $0 = -\log[H^{+}]$,which implies $[H^{+}] = 10^0 = 1 \ M$.$A$ solu

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(B) The $pH$ of a solution is defined as $pH = -\log[H^{+}]$.Given $pH = 0$,we have $0 = -\log[H^{+}]$,which implies $[H^{+}] = 10^0 = 1 \ M$.$A$ solution with a high concentration of $H^{+}$ ions is strongly acidic.

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

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An aqueous solution whose $pH = 0$ is

A
Alkaline
B
Acidic
C
Neutral
D
Amphoteric

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Chapter

2 Equilibrium: Ionic Equilibrium

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Water hydrolysis and pH scale

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

Medium

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At $80\,^{\circ}C,$ distilled water has $[H_3O^{+}]$ concentration equal to $1 \times 10^{-6} \, mol/L.$ The value of $K_w$ at this temperature will be

MediumAIPMT 1994

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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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The hydrogen ion concentration of a solution is $3.98 \times 10^{-6} \text{ mole per liter}$. The $pH$ value of this solution will be

MediumMHT CET 2012

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The concentration of hydroxyl ions in a solution with a $pH$ value of $3$ is .......

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An aqueous solution whose $pH = 0$ is

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

At $80\,^{\circ}C,$ distilled water has $[H_3O^{+}]$ concentration equal to $1 \times 10^{-6} \, mol/L.$ The value of $K_w$ at this temperature will be

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

The hydrogen ion concentration of a solution is $3.98 \times 10^{-6} \text{ mole per liter}$. The $pH$ value of this solution will be

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