$25.0\mathrm{mL}$ of $0.100\mathrm{M}$ $\mathrm{CH}{}_3\mathrm{COOH}$ ($\mathrm{p}{K}_a=4.74$) is titrated with $0.100\mathrm{M}$ NaOH. The pH after $10.0\mathrm{mL}$ of NaOH has been added is

More questions on Acid-base titration curves and indicators

• 20 mL of benzoic acid (K_a = 6.3x 10^-5) is exactly half-neutralised by NaOH. The pH of the solution is NEET level
• 20 mL of 0.10 M HCl is titrated with 0.10 M NaOH. After 10 mL of NaOH have been added the pH of the mixture is NEET level
• 25 mL of 0.10 M acetic acid (K_a = 1.8x 10^-5) is titrated with 0.10 M NaOH. At the equivalence point the pH is closest to NEET level
• 20.0 mL of 0.100 M NH3 (K_b = 1.8x 10^-5) is titrated with 0.100 M HCl. The pH at the equivalence point is JEE Main level
• 20.0 mL of 0.100 M HCl is titrated with 0.100 M NaOH. The pH after 30.0 mL of NaOH has been added is JEE Main level
• NH3 (K_b = 1.8x 10^-5) at 0.10 M is titrated with 0.10 M HCl, and the equivalence-point pH is 5.28. Which indicator is best suited? JEE Main level