Assuming complete dissociation which of the following aqueous solutions will have the same pH value? (i)100 mL of 0.01 M HCl (ii)100 mL of 0.01 M ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}$ (iii)50 mL of 0.01 M HCl (iv)Mixture of 50 mL of 0.02 M ${{\rm{H}}_2}{\rm{S}}{{\rm{O}}_4}$ and 50 mL of 0.02 M ${\rm{NaOH}}$

NEET UG CHEMISTRY MCQ: Equilibrium

1 Medium

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Analyzing +4 | -1

Assuming complete dissociation which of the following aqueous solutions will have the same pH value?

(i)100 mL of 0.01 M HCl
(ii)100 mL of 0.01 M

{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}

(iii)50 mL of 0.01 M HCl
(iv)Mixture of 50 mL of 0.02 M

{\mathrm{H}_2}\mathrm{S}{\mathrm{O}_4}

and 50 mL of 0.02 M

\mathrm{NaOH}

View answer and explanation

Correct option: D

(i), (iv)

Option D ((i), (iv)) is correct because both solutions have the same final concentration of

H^+

ions after considering neutralization in (iv).

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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}