Calculate the pH of a solution at the equivalence point when 200.0 mL of a 0.20 M solution of Lactic acid (HC;H;O3), which has a K value of 1.4 x 104, is titrated with a 6. 0.10 M LIOH solution.

a An analytical chemist is titrating 86.1 mL of a 1.100M solution of hydrazoic acid (HN3) with a 0.7600M solution of KOH. The p K of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 74.4 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.

When 25.00 mL of 0.467 M NaOH was added to 50.00 mL of a 0.467 M solution of a weak acid, HX, the pH of the mixture reached a value of 3.49. What is the Ka of the weak acid? Ka=

An analytical chemist is titrating 234.0 mL of a 0.4400M solution of butanoic acid (HC,H,CO,) with a 0.3900M solution of NaOH. The p K, of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 63.61 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places.

An analytical chemist is titrating 103.5 mL of a 0.3300M solution of acetic acid (HCH₂CO₂) with a 0.3600M solution of KOH. The p K of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 22.84 mL of the KOH solution to it. a Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of? KOH solution added. Round your answer to 2 decimal places. pH = Ś 000 18 Ar

An analytical chemist is titrating 240.2 mL of a 1.000M solution of acetic acid (HCH,CO, with a 0.2300M solution of KOH. The p K, of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 306.7 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH =|

An analytical chemist is titrating 145.0 mL of a 0.7900M solution of dimethylamine ((CH) NH) with a 0.8700M solution of HNO3. The p K, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 93.9 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =