(B) Given that $pOH = 12$ at $25\,^{\circ}C$. We know that $pH + pOH = 14$. Therefore,$pH = 14 - pOH = 14 - 12 = 2$. The concentration of $H^{+}$ ions

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(B) Given that $pOH = 12$ at $25\,^{\circ}C$. We know that $pH + pOH = 14$. Therefore,$pH = 14 - pOH = 14 - 12 = 2$. The concentration of $H^{+}$ ions is given by the formula $[H^{+}] = 10^{-pH}$. Substituting the value of $pH$,we get $[H^{+}] = 10^{-2} \ M$.

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

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If a solution has $pOH$ value $12$ at $25\,^{\circ}C$,$H^{+}$ concentration should be

A
$2$
B
$10^{-2}$
C
$10^{-12}$
D
$10^{-6}$

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6-2.Equilibrium-II (Ionic Equilibrium)

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Water hydrolysis and pH scale

For an acidic solution,the $[OH^{-}]$ will be .........

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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

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If the $pH$ of a solution is $4.0$ at $25\,^{\circ}C,$ its $pOH$ would be $(K_w = 10^{-14})$

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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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When sodium chloride is dissolved in water,the sodium ion undergoes ........

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If a solution has $pOH$ value $12$ at $25\,^{\circ}C$,$H^{+}$ concentration should be

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For an acidic solution,the $[OH^{-}]$ 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

If the $pH$ of a solution is $4.0$ at $25\,^{\circ}C,$ its $pOH$ would be $(K_w = 10^{-14})$

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

When sodium chloride is dissolved in water,the sodium ion undergoes ........

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