pH of a buffer solution: Mass of NaC2H3O2 * 3H2O (FW=136g/mol): 3.540g
Calculate the Theoretical pH of these buffer solutions:
A. pH of original buffer solution (with 8.8 mL of 3.0 M acetic acid and 55.6 mL of water) : 4.7
B. pH of buffer + 1.0 mL of 6.0 M HCl: 3.8
C. pH of buffer + 1.0 mL of 6.0 M NaOH: 4.9
3.540 g NaC2H3O2 * 3H2O (salt) = mass / molar mass = 3.540 g / 136 g / mole = 0.026 mole.
8.8 mL of 3.0 M acetic acid = 0.0088 L * 3.0 mole / L = 0.0264 mole.
a) Using Henderson equation,
pH = pKa + log [salt] / [acid]
or
pH = 4.74 + log (0.026 / 0.0264)
or
pH = 4.73
b) 1.0 mL of 6.0 M HCl = 0.001 L * 6.0 mole / L = 0.006 mole.
pH = pKa + log [salt] / [acid]
or
pH = 4.74 + log [(0.026 - 0.006) / (0.0264 + 0.006)]
or
pH = 4.53
c) 1.0 mL of 6.0 M NaOH = 0.001 L * 6.0 mole / L = 0.006 mole.
pH = pKa + log [salt] / [acid]
or
pH = 4.74 + log [(0.026 + 0.006) / (0.0264 - 0.006)]
or
pH = 4.93
PH of a buffer solution: Mass of NaC2H3O2 * 3H2O (FW=136g/mol): 3.540g Calculate the Theoretical ...
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Part A. Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.171 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.230 M in HC2H3O2 and 0.170 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH.
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