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What is the pH of 1L of buffer made from 0.6M HF and 0.54M NaF (pKa...

What is the pH of 1L of buffer made from 0.6M HF and 0.54M NaF (pKa of HF = 3.45)? If 0.01M HCl is added (disregard change in volume), what is the new pH? If 0.01M NaOH had been added instead?

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Answer #1

HF = 1.0L of 0.6M

number of moles of HF = 0.6M x 1.0L = 0.6 moles

NaF = 1.0L of 0.54M

number of moles of NaF = 0.54M x 1.0L = 0.54 moles

Pka = 3.45

PH = Pka + log[salt]/[acid]

PH = 3.45 + log(0.54/0.6)

PH = 3.40

a)

concentration of HCl = 0.01M = 0.01 mol/L

number of moles of HCl = 0.01 mole

number of moles of HF = 0.6M x 1.0L = 0.6 moles

number of moles of NaF = 0.54M x 1.0L = 0.54 moles

after addition of HCl

number of moles of HF = 0.6 + 0.01 = 0.61 moles

number of moles of NaF = 0.54 - 0.01 = 0.53 moles

PH = 3.45 + log(0.53/0.61)

PH = 3.39

b) NaOH = 0.01M = 0.01 mol/L

mnumber of moles of NaOH = 0.01 mole

after addition of NaOH

number of moles of HF = 0.6- 0.01 = 0.59 moles

number of moles of NaF = 0.54 + 0.01 = 0.55moles

PH = 3.45 + log(0.55/0.59)

PH = 3.42.

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