A .) Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.167 M in

Question

A.) Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.167 M in KCN. For HCN, Ka = 4.9×1010 (pKa = 9.31).

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.)

C.)A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×105.

Calculate the

pH of the solution, upon addition of 0.085 mol of NaOH to the original buffer.

D.) Consider a buffer solution that is 0.50 M in NH3and 0.20 M in NH4Cl. For ammonia,

Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH.pKb=4.75

Explanation / Answer

a)

apply pH equation

pH = pKa + log(CN-/HCN)

pKa = -log(Ka) = -log(4.9*10^-10) = 9.3098

pH = 9.3098+ log(0.167/0.247)

pH = 9.139819

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