How much would the concentration of CO2(aq) change due to a temperature change from 25°C to 26°C at 1atm?

Whoa! Back the boat up. While there seems to be a lot of work there, N3...'s solution makes no sense. He is calculating the moles of GAS in 1 L of CO2 at 298K and 1 atm. That isn't the amount that is dissolved in SOLUTION at 298K.

The amount of CO2 dissolved in water can be determined from Henry's law.

c = kH(p) ..... c is the concentration of the gas, kH is the Henry's law constant for the particular gas and p is the partial pressure of the gas above the solution.

c = 0.034 mol/Latm x 1.00 atm = 0.034 mol/L

The Henry's law constant varies with temperature, and must be calculated at the new temperature.

kH(T) = kH(T') x e^(C(1/T - 1/T')) .... where T is the new temperature, T' is 298K, C is a constant for each gas. For CO2, C = 2400

kH(T) = 0.034 mol/Latm x e^(2400(1/299 - 1/298))

kH(T) = 0.033 mol/Latm

Calculating the concentration at 26C....

c = kH(p)

c = 0.033 mol/Latm x 1.00 atm = 0.033 mol/L

The concentration will decrease by 0.001 mol/L as the CO2 solution goes from 25C to 26C.

PV = nRT

n = PV/RT

P = 1atm

R = 0.08205746 Latm/Kmol

T1 = 25C + 237.15K = 298.15K

T2 = 26C + 237.15K = 299.15K

n = PV/RT

n = 1atm(1L)/(0.08205746 Latm/Kmol)(298.15K)

n = 1/24.465mol

n = 0.0409mol CO2 --- initial mass of CO2

n = 1atm(1L)/(0.08205746 Latm/Kmol)(299.15K)

n = 1/24.547mol = 0.0407mol CO2 -- final mass of CO2

dm = mf - mi

where,

M = m/V

M = 0.0409mol/L = 0.0409M <--- Molarity of CO2 at 25C

M = 0.0407mol/L = 0.0407M <---- Molarity of CO2 at 26C

dM = Mf - Mi = 0.0407M - 0.0409M = -0.0002M <---- change of CO2 when T is increased by 1C

therefore,

----- The concentration of CO2 is decreased by about 0.0002M when the temperature is increased from 25C to 26C. The final concentration of CO2 at 26C is 0.0407M.