The pH of the aqueous solution containing 0.4 | vedclass

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(A) The molar mass of $H_2SO_4$ is $98 \ g/mol$. Moles of $H_2SO_4 = \frac{0.49 \ g}{98 \ g/mol} = 0.005 \ mol$. Since the volume of the solution is $

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$2$

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(A) The molar mass of $H_2SO_4$ is $98 \ g/mol$. Moles of $H_2SO_4 = \frac{0.49 \ g}{98 \ g/mol} = 0.005 \ mol$. Since the volume of the solution is $1 \ L$,the molarity of $H_2SO_4$ is $0.005 \ M$. $H_2SO_4$ is a strong diprotic acid,so it dissociates as: $H_2SO_4 ightarrow 2H^{+} + SO_4^{2-}$. Concentration of $[H^{+}] = 2 	imes [H_2SO_4] = 2 	imes 0.005 \ M = 0.01 \ M = 10^{-2} \ M$. $pH = -\log[H^{+}] = -\log(10^{-2}) = 2$.

The $pH$ of the aqueous solution containing $0.49 \ g$ of $H_2SO_4$ in one litre is

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