using your pH at half equivalence for acetic acid and ammonia and considering the Henderson-Hasselbalch equation, calculate their Ka and Kb values. Compare with the accepted values and explain sources of error.
using your pH at half equivalence for acetic acid and ammonia and considering the Henderson-Hasselbalch equation,...
Use the Henderson-Hasselbalch equation to calculate the Ka value of acetic acid. 20.50 mL of NaOH (0.95 M) was added to 20.00 mL of acetic acid (unknown molarity) pH at equivalence point was recorded as 8.67.
Use the Henderson-Hasselbalch equation to calculate the mass of solid sodium acetate required to mix with 50.0 mL of 0.10 M acetic acid to prepare a pH 4 buffer. Ka for acetic acid is 1.8 times 10^-5. Use the Henderson-Hasselbalch equation to calculate the mass of solid ammonium chloride required to mix with 50.0 mL of 0.10 M ammonia to prepare a pH 10 buffer. The Kb for ammonia is 1.8 times 10^-5. The purpose of this experiment is to...
Use the Henderson-Hasselbalch equation to perform the following calculations. The K a of acetic acid is 1.8 10 –5 . a. Buffer A: Calculate the mass of solid sodium acetate required to mix with 100.0 mL of 0.5 M acetic acid to prepare a pH 4 buffer. Record the mass in your data table. b. Buffer B: Calculate the mass of solid sodium acetate required to mix with 100.0 mL of 1.0 M acetic acid to prepare a pH...
Use the Henderson-Hasselbalch equation to perform the following calculations. The Ka of acetic acid is 1.8 x 10–5. Buffer A: Calculate the mass of solid sodium acetate required to mix with 100.0 mL of 0.5 M acetic acid to prepare a pH 4 buffer. Record the mass in your data table. Buffer B: Calculate the mass of solid sodium acetate required to mix with 100.0 mL of 1.0 M acetic acid to prepare a pH 4 buffer. Record the mass...
12. Using the Henderson-Hasselbalch equation, prove (mathematically and chemically) why pH equals pkat half-way to the equivalence point of the reaction. (6 pts) 13. You have a buffer that contains acetic acid and sodium acetate. Write the complete and balanced chemical reaction for what happens when sodium hydroxide is added to the buffer. Write a complete and balanced chemical reaction for what happens when hydrochloric acid is added to the buffer. (8 pts)
9. Use the Henderson Hasselbalch equation to find the pH of an acetic acid/acetate buffer in which: [HC H202] = L.OM [C:H:0:'] = 0.10M
Using the Henderson-Hasselbalch equation, calculate the pH when 0.5 mole of sodium hydroxide is added to 1 mole of acetic acid. (pKa of acetic acid is 4.76).
9. Use the Henderson-Hasselbalch equation to find the pH of an acetic acid/acetate buffer in which: [HC2H302] = 1.0M [C2H:02'] = 0.10M
use the henderson-hasselbalch equation to find the expected pH of a soltion that has 0.100 M Acetic Acid and 0.100 M Sodium Acetate Ka for acetic acid= 1.8x10^-5
1. (3) Using the Henderson-Hasselbalch Equation, calculate the pH of a buffer solution that is 0.065 M in benzoic acid (HC2H5O2) and 0.125 M is sodium benzoate (NaC7H5O2). For benzoic acid, Ka = 6.5 x 105.