(D) As we know,$pH = -\log [H^+]$.Initial $pH = 2.0$,so initial $[H^+]_i = 10^{-2} \ M$.Final $pH = 5.0$,so final $[H^+]_f = 10^{-5} \ M$.The ratio of

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(D) As we know,$pH = -\log [H^+]$.Initial $pH = 2.0$,so initial $[H^+]_i = 10^{-2} \ M$.Final $pH = 5.0$,so final $[H^+]_f = 10^{-5} \ M$.The ratio of change is $\frac{[H^+]_f}{[H^+]_i} = \frac{10^{-5}}{10^{-2}} = 10^{-3}$.Thus,the hydrogen ion concentration decreases by a factor of $1000$ (thousand-fold).

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

Medium

An aqueous solution of $HCl$ has a $pH$ of $2.0$. When water is added to increase the $pH$ to $5.0$,the hydrogen ion concentration

KVPY 2010 All KVPY

A
remains the same
B
decreases three-fold
C
increases three-fold
D
decreases thousand-fold

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Class 11

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6-2.Equilibrium-II (Ionic Equilibrium)

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Water hydrolysis and pH scale

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KVPY 2010 Paper All KVPY years →

Explain the $pH$ scale and $pH$.

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

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If the $pH$ of an aqueous solution is $6$,then the concentration of $OH^{-}$ in the solution will be ...............

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The $pH$ of a sample of vinegar is $3.76$. Calculate the concentration of hydrogen ion in it.

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Calculate $[H^{+}]$ concentration for solutions with $pH = 12.0$ and $pH = 5.6$.

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An aqueous solution of $HCl$ has a $pH$ of $2.0$. When water is added to increase the $pH$ to $5.0$,the hydrogen ion concentration

Similar Questions

Explain the $pH$ scale and $pH$.

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

If the $pH$ of an aqueous solution is $6$,then the concentration of $OH^{-}$ in the solution will be ...............

The $pH$ of a sample of vinegar is $3.76$. Calculate the concentration of hydrogen ion in it.

Calculate $[H^{+}]$ concentration for solutions with $pH = 12.0$ and $pH = 5.6$.

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