1) Calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH

Question

1) Calculate the ratio of CH3NH2 to CH3NH3Cl required to create a buffer with pH=10.26

Part A: What is the pH of a buffer prepared by adding 0.405mol of the weak acid HA to 0.608mol of NaH in 2.00L of solution? The dissociation constant Ka of HA is 5.66e-7

Part B: What is the pH after 0.150mol of HCL is added to the buffer from part A? Assume no volume change on the addition of the acid.

Part C: What is the pH after 0.195mol of NaOH is added to the buffer form part A? Assume no volume change on the addition of the base

Explanation / Answer

1)

PH + pOH = 14

pOH = 3.88

We have to use hinderson equation

pOH = pKb + log[salt]/[base]

3.88 = 3.356 + log[salt]/[base]

0.524 = log[salt]/[base]

3.341 = [salt]/[base]

so [base]/[salt] = 0.39

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