A). A buffer solution is made that is 0.337 M in H 2 CO 3 and 0.337 M in KHCO 3
ID: 1066439 • Letter: A
Question
A). A buffer solution is made that is 0.337 M in H2CO3 and 0.337 M in KHCO3.
(1) If Ka for H2CO3 is 4.20×10-7, what is the pH of the buffer solution?
(2) Write the net ionic equation for the reaction that occurs when 0.075 mol NaOH is added to 1.00 L of the buffer solution
B). A buffer solution is made that is 0.317 M in H2C2O4 and 0.317 M in KHC2O4.
(1) If Ka for H2C2O4 is 5.90×10-2, what is the pH of the buffer solution?
(2) Write the net ionic equation for the reaction that occurs when 0.071 mol HBr is added to 1.00 L of the buffer solution.
Use H3O+ instead of H+.
Explanation / Answer
Pka = -logKa
= -log4.2*10-7
= 6.3767
PH = Pka + log[KHCO3]/[H2CO3]
= 6.3767 + log0.337/0.337
= 6.3767
2. naOH -------> Na+ + OH-
no of moles of H2C2O4 = 0.317
no of moles of KHC2O4 = 0.317
Ka = 5.9*10-2
PKa = -logka
= -log0.059 = 1.229
PH = Pka + log[KHC2O4]/[H2C2O4]
PH = 1.229 + log0.317/0.317
PH = 1.229
HBr +H2O ------> H3O+ + Br-
0.071 M 0.071M
= 1.229 + log
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