(C) The formula for $pH$ is given by $pH = -\log [H^{+}]$.Given $[H^{+}] = 6 \times 10^{-4} \ M$.$pH = -\log (6 \times 10^{-4}) = -(\log 6 + \log 10^{

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(C) The formula for $pH$ is given by $pH = -\log [H^{+}]$.Given $[H^{+}] = 6 \times 10^{-4} \ M$.$pH = -\log (6 \times 10^{-4}) = -(\log 6 + \log 10^{-4})$.$pH = -(\log 2 + \log 3 - 4) = -(0.301 + 0.477 - 4) = -(-3.222) = 3.222$.Rounding to two decimal places,the $pH$ is $3.22$.

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

Medium

The hydrogen ion concentration in a given solution is $6 \times 10^{-4} \ M$. Its $pH$ will be

A
$6$
B
$4$
C
$3.22$
D
$2$

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2 Equilibrium: Ionic Equilibrium

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Water hydrolysis and pH scale

At $90\, ^\circ C$ pure water has $[H_3O^{+}] = 10^{-6}\, mol\, L^{-1}$. The value of $K_w$ at $90\, ^\circ C$ is

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

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What is the concentration of $OH^{-}$ ion in a solution containing $0.05 \ M \ H^{+}$ ions?

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When $NaCl$ is dissolved in water,the sodium ion becomes

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Which of the following does not make any change in $pH$ when added to $10 \ mL$ of dilute $HCl$?

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The hydrogen ion concentration in a given solution is $6 \times 10^{-4} \ M$. Its $pH$ will be

Similar Questions

At $90\, ^\circ C$ pure water has $[H_3O^{+}] = 10^{-6}\, mol\, L^{-1}$. The value of $K_w$ at $90\, ^\circ C$ is

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

What is the concentration of $OH^{-}$ ion in a solution containing $0.05 \ M \ H^{+}$ ions?

When $NaCl$ is dissolved in water,the sodium ion becomes

Which of the following does not make any change in $pH$ when added to $10 \ mL$ of dilute $HCl$?

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