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(C) The titration involves a strong acid $(HCl)$ and a strong base $(NaOH)$.Initially,the beaker contains $HCl$,which is a strong acid,so the initial

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(C) The titration involves a strong acid $(HCl)$ and a strong base $(NaOH)$.Initially,the beaker contains $HCl$,which is a strong acid,so the initial $pH$ is low (around $1$).As $NaOH$ is added,the $H^+$ ions are neutralized by $OH^-$ ions,causing the $pH$ to increase gradually.Near the equivalence point,there is a very sharp or steep increase in $pH$ because the concentration of $H^+$ ions changes drastically.After the equivalence point,the solution becomes basic due to excess $NaOH$,and the $pH$ levels off at a high value.Graph $C$ correctly represents this characteristic sigmoidal curve for a strong acid-strong base titration,where the $pH$ rises sharply through $pH = 7$ at the equivalence point.

$100 \ mL$ of $0.1 \ M$ $HCl$ is taken in a beaker and to it $100 \ mL$ of $0.1 \ M$ $NaOH$ is added in steps of $2 \ mL$ and the $pH$ is continuously measured. Which of the following graphs correctly depicts the change in $pH$?

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