(B) The relationship between $pH$ and hydrogen ion concentration is given by the formula: $pH = -\log[H^{+}]$ Given that $pH = 4$,we have: $4 = -\log[

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(B) The relationship between $pH$ and hydrogen ion concentration is given by the formula: $pH = -\log[H^{+}]$ Given that $pH = 4$,we have: $4 = -\log[H^{+}]$ $\log[H^{+}] = -4$ $[H^{+}] = 10^{-4} \ mol/L$ Therefore,the correct option is $B$.

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

Medium

The $pH$ of the solution is $4$. The hydrogen ion concentration of the solution in $mol/L$ is

A
$9.5$
B
$10^{-4}$
C
$10^{4}$
D
$10^{-2}$

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Class 11

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Chapter

6-2.Equilibrium-II (Ionic Equilibrium)

Subtopic

Water hydrolysis and pH scale

At $298 \ K$,the $pH$ of a $NaCl$ solution is $7$. If the solution is heated to $320 \ K$,which of the following statements is correct?

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When the $pH$ of a solution is $2$,the hydrogen ion concentration in moles per litre is

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Calculate the $[H_3O^+]$ concentration if the $pH$ of the solution is $4.25$.

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At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

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

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The $pH$ of the solution is $4$. The hydrogen ion concentration of the solution in $mol/L$ is

Similar Questions

At $298 \ K$,the $pH$ of a $NaCl$ solution is $7$. If the solution is heated to $320 \ K$,which of the following statements is correct?

When the $pH$ of a solution is $2$,the hydrogen ion concentration in moles per litre is

Calculate the $[H_3O^+]$ concentration if the $pH$ of the solution is $4.25$.

At $25\,^oC$,the $pH$ of a solution is $2$. If the $pH$ is doubled,the concentration of hydronium ions in the solution will ............

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

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