When exactly of is slowly titrated with a solution at , which of the following statements precisely — Ionic Equilibrium Chemistry Question

💡 Solution & Explanation

The initial $[H^+]$ is $0.1 \text{ M}$, so $pH = 1.0$. Strong acid-strong base titrations always exhibit a massive vertical pH jump around the equivalence point. Since the resulting salt ($NaCl$) does not hydrolyze, the equivalence point pH is exactly 7.0 at $25^\circ C$. Statement D is entirely incorrect; at half-neutralization ($50 \text{ mL}$ NaOH added), the remaining HCl is $5 \text{ mmol}$ in $150 \text{ mL}$, so $[H^+] = 1/30 \text{ M}$, making the $pH \approx 1.48$, nowhere near 3.5.