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$H_{2}SO_{4}$ (iii)50 mL of 0.01 M HCl (iv)Mixture of 50 mL of 0.02 M $H_{2}SO_{4}$ and 50 mL of 0.02 M $NaOH$

Question

Dr. Abubacker · Accepted Answer

(d)
Millieq. of 0.01 M $HCl = \frac{0.01 	imes 100}{1000} = 1 	imes 10^{- 3}$
$	herefore pH = 3$
Millieq. of 0.02 M $H_{2}SO_{4} = \frac{0.04 	imes 50}{1000} = 2 	imes 10^{- 3}$
Millieq. of 0.02 M $NaOH = \frac{0.02 	imes 50}{1000} = 1 	imes 10^{- 3}$
Left $\left\lbrack H^{+} ightbrack = 2 	imes 10^{- 3} - 1 	imes 10^{- 3};\ 	herefore pH = 3$

Q. 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$H_{2}SO_{4}$ (iii)50 mL of 0.01 M HCl (iv)Mixture of 50 mL of 0.02 M $H_{2}SO_{4}$ and 50 mL of 0.02 M $NaOH$

Explanation

Reviewed by Dr. Abubacker

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