(C) The $pH$ is defined as $pH = -\log[H^{+}]$.For $pH_1 = 3$,$[H^{+}]_1 = 10^{-3} \ M$.For $pH_2 = 6$,$[H^{+}]_2 = 10^{-6} \ M$.The ratio of concentr

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(C) The $pH$ is defined as $pH = -\log[H^{+}]$.For $pH_1 = 3$,$[H^{+}]_1 = 10^{-3} \ M$.For $pH_2 = 6$,$[H^{+}]_2 = 10^{-6} \ M$.The ratio of concentrations is $\frac{[H^{+}]_1}{[H^{+}]_2} = \frac{10^{-3}}{10^{-6}} = 10^{3} = 1000$.Therefore,the $H^{+}$ ion concentration decreases by $1000$ times.

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

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If the $pH$ of a solution increases from $3$ to $6$,then its $H^{+}$ ion concentration:

A
decreases by half.
B
doubles.
C
decreases by $1000$ times.
D
increases by $1000$ times.

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6-2.Equilibrium-II (Ionic Equilibrium)

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Water hydrolysis and pH scale

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If the $pH$ of a solution increases from $3$ to $6$,then its $H^{+}$ ion concentration:

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When $KBr$ is dissolved in water,$K^{+}$ ions are

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