14 mL of 0.0100 M NaOH are added to 25.0 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
7 A 25.00 ml acetic acid solution is trated with 0.110 M NaOH. The end point is reached after 18.55 mL NaOH has been added. a. What was the original concentration of acetic acid? 5 pts bWhat is the initial pH of the acetic acid solution? 5 pts was the plh after the adition of 5.00 mL NaOH to the original solution? 5 pts d. What is the pH at the equivalence point? 5 pts e. What is the pH...
when 10.00 ml of .200 M NaOH is added to 25.00 ml of .200 M acetic acid solution, what is the pH of the solution? pKa of acetic acid =4.76
A 25.0 mL sample of 0.125 M acetic acid is titrated with 0.125 M NaOH. Calculate the pHs after each of the following volumes of base have been added: 12.5 mL 15 mL
A 25.0 mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of acetic acid is 4.5E-4
6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added, the pH of the resulting solution was 6.70. After 50.0 mL of NaOH was added, the pH of the solution was 8.00. What are the values of Ka1 and Ka2? 6. A student titrated 50.0 mL of the 0.10 M unknown diprotic H2A with 0. 10 M NAOH. After 25.0 mL of NaOH was added,...
40.0 ml of an acetic acid of unknown concentration is titrated with 0.100 M NaOH. After 20.0 mL of the base solution has been added, the pH in the titration flask is 5.10. What was the concentration of the original acetic acid solution? [Ka(CH3COOH) = 1.8 × 10–5]
A solution of 100. ml of .500 M Acetic Acid is titrated with .500 M sodium hydroxide. The Ka of acetic acid is 1.8*10^-5. Find the pH values at the given stages: a) before the addition of any NaOH. B) After 25.0 mL of NaOH added. C) At the equivalence point.
A 25.0 mL sample of 0.293 M acetic acid solution is titrated with 37.5 mL of 0.195 M NaOH solution. What is the pH of this solution if K = 1.8 x 10-5? Final Answer: _______
A 25.00 mL sample of 0.310 M NaOH is titrated with 0.750 M HCl at 25 °C. Calculate the initial pH before any titrant is added. Calculate the pH of the solution after 5.00 mL of the titrant is added.