A.)Consider a buffer solution that is 0.50 M in NH3and 0.20 M in NH4Cl. For ammo

Question

A.)Consider a buffer solution that is 0.50 M in NH3and 0.20 M in NH4Cl. For ammonia, pKb=4.75.

Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid

NaOH

B.)Calculate the

pH of a buffer solution that is 0.240 M in HC2H3O2 and 0.200 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×105.)

Express your answer to two decimal places.C.)

D.) What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.10 M HCl? K a = 3.0 × 10-8 for HOCl.

What is the pH at the equivalence point of a weak base-strong acid titration if 20.00 mL of NaOCl requires 28.30 mL of 0.10 M HCl? K a = 3.0 × 10-8 for HOCl.

Explanation / Answer

A.)Consider a buffer solution that is 0.50 M in NH3and 0.20 M in NH4Cl. For ammonia, pKb=4.75.

Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH

This will be a buffer so:

pOH = pKb + log(NH4+/NH3)

NH4+ = 0.2*1 - 0.11 = 0.09 mmol left

NH3 = 0.5*1 +0.11 = 0.61

then

pOH = pKb + log(NH4+/NH3) = 4.75 + log(0.09/0.61)

pOH= 3.9189

pH = 14-3.9189 = 10.0811

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