$100\;{\rm{ }}mL\;{\rm{ }}of\;{\rm{ }}0.01{\rm{ }}M$ solution of ${\rm{NaOH}}$ is diluted to $1\;{\rm{d}}{{\rm{m}}^3}$. What is the pH of the diluted solution?

NEET UG CHEMISTRY MCQ: Equilibrium

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100\;\mathrm{ }mL\;\mathrm{ }of\;\mathrm{ }0.01\mathrm{ }M

solution of

\mathrm{NaOH}

is diluted to

1\;\mathrm{d}{\mathrm{m}^3}

. What is the pH of the diluted solution?

View answer and explanation

Correct option: B

Option B (11) is correct because diluting the NaOH solution decreases the hydroxide concentration, leading to a pOH of 3 and therefore a pH of 11.

Practice All Chapter MCQs →

Mg{(HC{O_3})_2}

MgC{O_3}

Mg{(OH)_2}

MgC{O_3}

K_{\mathrm{P}}

\mathrm{CaCO}_3

4.5 \times 10^{-2}

\mathrm{C}(\mathrm{s})+\mathrm{CO}_2(\mathrm{g}) \rightleftharpoons 2 \mathrm{CO}(\mathrm{g}),

K_{\mathrm{P}}

2.0 \mathrm{~atm}.

\mathrm{CaO}

\mathrm{CaCO}_3

+

\leftrightharpoons

\mathrm{PC}{\mathrm{l}_5}\leftrightharpoons\mathrm{PC}{\mathrm{l}_3} + \mathrm{C}{\mathrm{l}_2}

{K_{\mathrm{eq}}} = 0.41

\mathrm{p}{K_a}