A buffer solution is made that is 0.498 M in H 2 C 2 O 4 and 0.498 M in NaHC 2 O
ID: 994947 • Letter: A
Question
A buffer solution is made that is 0.498 M in H2C2O4and 0.498 M in NaHC2O4.
(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 0.113 mol NaOH is added to 1.00 L of the buffer solution.
A buffer solution is made that is 0.458 M in HClO and0.458 M in NaClO.
(1) If Ka for HClO is 3.50×10-8, what is the pH of the buffer solution?
(2) Write the net ionic equation for the reaction that occurs when 0.129 mol KOH is added to 1.00 L of the buffer solution.
Explanation / Answer
1) pka = -logka = -log(5.9*10^-2) = 1.23
pH = pka + log(salt/acid)
= 1.23 + log(0.498/0.498)
= 1.23
2) net ionic equation : H2C2O4 + 2OH- ----> C2O4^2- + 2H2O
1)
pka = -logka = -log(3.5*10^-8) = 7.46
pH = pka + log(salt/acid)
= 7.46 + log(0.458/0.458)
= 7.46
2) net ionic equation : HClO + 2OH- ----> ClO- + H2O
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