Equal volumes of three acid solutions with pH | vedclass

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(B) Let the volume of each solution be $V \ L$. The total volume of the mixture is $3V \ L$. The concentration of $H^+$ ions in the solutions are: $[H

Vedclass · Accepted Answer

$3.7 	imes 10^{-4} \ M$

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(B) Let the volume of each solution be $V \ L$. The total volume of the mixture is $3V \ L$. The concentration of $H^+$ ions in the solutions are: $[H^+]_1 = 10^{-3} \ M$,$[H^+]_2 = 10^{-4} \ M$,$[H^+]_3 = 10^{-5} \ M$. The total number of moles of $H^+$ ions is $n_{total} = (10^{-3} 	imes V) + (10^{-4} 	imes V) + (10^{-5} 	imes V) = V(10^{-3} + 0.1 	imes 10^{-3} + 0.01 	imes 10^{-3}) = 1.11 	imes 10^{-3} 	imes V$. The final concentration $[H^+]_{mix} = \frac{n_{total}}{V_{total}} = \frac{1.11 	imes 10^{-3} 	imes V}{3V} = 0.37 	imes 10^{-3} \ M = 3.7 	imes 10^{-4} \ M$.

List-$I$	List-$II$
$A$. $Aq.$ solution of $AlCl_3$	$I$. Basic
$B$. $Aq.$ solution of $CH_3COONa$	$II$. Acidic
$C$. $Aq.$ solution of $KCl$	$III$. Highly conductive
$D$. $Al_2O_3$	$IV$. Strongly basic
	$V$. Amphoteric

Equal volumes of three acid solutions with $pH$ values of $3, 4,$ and $5$ are mixed. What will be the concentration of $H^+$ ions in the resulting mixture?

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The plot of $pH$-metric titration of weak base $NH_4OH$ vs strong acid $HCl$ looks like:

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Match the following:
List-$I$ List-$II$
$A$. $Aq.$ solution of $AlCl_3$ $I$. Basic
$B$. $Aq.$ solution of $CH_3COONa$ $II$. Acidic
$C$. $Aq.$ solution of $KCl$ $III$. Highly conductive
$D$. $Al_2O_3$ $IV$. Strongly basic
$V$. Amphoteric

The correct match is:

$100 \ cm^3$ of $0.1 \ N \ HCl$ solution is mixed with $100 \ cm^3$ of $0.2 \ N \ NaOH$ solution. The resulting solution is

In which of the following acid-base titrations is the $pH$ at the equivalence point greater than $8$?

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