Question

$100mL$ of $0.1MHCl$ is titrated against the $0.1MNaOH$ solution. What will be the $pH$ of the solution when $100mLNaOH$ is added ?

• A. 1
• B. 7
• C. 1.3
• D. 2

Answer 1

The correct option is B 7

mmol of $HCl=100\times 0.1=10$
mmol of $NaOH\text{added}=100\times 0.1=10$

$HCl\left(aq\right)+NaOH\left(aq\right)\to NaCl\left(aq\right)+H_{2}O\left(l\right)Initial:101000Final:001010$

After titration , no acid or base is remaining as both will completely neutralizes each other and salt $NaCl$ is formed which does not hydrolyzed infact it rather hydrated in water.

So , the resultant solution will be neutral and the pH of the solution will be equal to 7.