H2O + CO2 <--> HCO3- + H+ K1 = 4.4 x 10-7 HCO3- <--> CO3-2 + H+ K2 = 4.7 x 10-11 A buffer solution is made by putting

[answerhappygod]

H2O + CO2 <-->
HCO3- + H+
K1 = 4.4 x 10-7
HCO3- <-->
CO3-2 + H+ K2 = 4.7 x
10-11
A buffer solution is made by putting 0.30 mol
CO3-2 and 0.50 mol
HCO3- in water to create a 1.00 L solution.
Half the solution is poured into a flask labeled "A", and the
other half is placed in flask "B".
a) What is the effect on [HCO3-] and
[CO3-2] when 0.10 mol
KHSO4(s) is added to the solution in flask A?
In your answer, be in terms of moles of protons transferred. Has
the capacity of the buffer been exceeded? Show work.
b) In another experiment, 0.10 mol NaOH(s) is added
to the solution in flash B. What are the new equilibrium values for
[HCO3-] and [CO3-2]?
Show work.
FRQ Help, thanks!