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For each of the following solutions, calculate the initial pH and the final pH after adding...

For each of the following solutions, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH. For 230.0 mL of a buffer solution that is 0.2763 M in CH3CH2NH2 and 0.2518 M in CH3CH2NH3Cl, calculate the initial pH and the final pH after adding 0.0150 mol of NaOH(Kb=5.6⋅10−4).

Solutions

Expert Solution

Since this is a buffer solution, we can use the Henderson Hasselbalch eqn. to calculate the pH
pKa = 10.636 for CH3CH2NH3Cl
pH = pKa + log([CH3CH2NH2] / [CH3CH2NH3Cl]) = 10.636 + log(0.2763/0.2518) = 10.676

Final pH:
moles CH3CH2NH2 = 0.230 L x 0.2763 M = 0.06355
moles CH3CH2NH3Cl = 0.230 L x 0.2518 M = 0.0579
CH3CH2NH3+ + OH- = CH3CH2NH2 + H2O
moles CH3CH2NH3+ = 0.0579 - 0.015 = 0.043
moles CH3CH2NH2 = 0.06355 + 0.015 = 0.07855
Can use the Henderson Hasselbalch eqn. since this is still a healthy buffer (still decent amount of base and acid present).
[CH3CH2NH3+] = 0.043/ 0.230 = 0.187 M
[CH3CH2NH2] = 0.07855/0.230 L = 0.3415 M
pH = 10.636 + log(.3415 / 0.187) = 10.897

queen_honey_blossom answered 2 years ago
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