In an acid-base titration,0.1 M HCl solutio | vedclass

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(A) In this titration,a strong acid $(HCl)$ is added to a strong base $(NaOH)$.Initially,the solution contains $NaOH$,so the $pH$ is high (basic).As $

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Graph $(a)$

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(A) In this titration,a strong acid $(HCl)$ is added to a strong base $(NaOH)$.Initially,the solution contains $NaOH$,so the $pH$ is high (basic).As $HCl$ is added,the $pH$ decreases gradually.Near the equivalence point,there is a sharp drop in $pH$ because the concentration of $OH^-$ ions decreases rapidly.After the equivalence point,the solution becomes acidic due to excess $HCl$,and the $pH$ levels off at a low value.Graph $(a)$ correctly represents this sigmoidal decrease in $pH$ as the volume of the acid titrant increases.

In an acid-base titration,$0.1 \ M \ HCl$ solution was added to the $NaOH$ solution of unknown strength. Which of the following correctly shows the change of $pH$ of the titration mixture in this experiment?

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