100 mL of 0.1 M HCl is taken in a beaker an | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

Vedclass · Answer

(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 $pH$?

Similar Questions

When a $10^{-6} \ M \ NaOH$ solution is diluted $100$ times,the $pH$ of the diluted solution will be ............ .

What is the concentration of hydrogen $[H^{+}]$ ions in $0.01 \, M \, HCl$?

The $pH$ of $1 \ L$ of an aqueous solution of $HCl$ is $1$. How many liters of water must be added to make the $pH$ of this solution $2$ (in $L$)?

What is the pH of $10^{-8} \ M \ HCl$ solution?

Aqueous solution of $HCl$ has the $pH = 4$. Its molarity would be (in $, M$)

Vedclass Test Series

Exam Paper Generator

Online Exam Module