Sodium carbonate (2.4134 g) is dissolved in enough deionized water to give a solution with a total volume of 250.0 mL. What is the pH of the resulting solution? For carbonic acid, pKa1 = 6.351 and pKa2 = 10.329.
Also:
What is the equilibrium concentration of H2CO3 in the solution
calculate the value of aHCO3−.
Write a mass balance and charge balance equation
please show all work!
concentration of Na2CO3 solution = 2.4134 g/106 g/mol x 0.250 L = 0.091 M
Na2CO3 + H2O <==> HCO3- + OH-
Ka1 = 4.45 x 10^-7 = x^2/0.091
x = [OH-] = 2.01 x 10^-4 M
pH = -log[OH-] = 3.70
pH = 14 - pOH = 10.3
[H+] = 5.01 x 10^-11 M
aHCO3- = [H+]Ka1/([H+]^2 + [H+]Ka1 + Ka1.Ka2)
= (2.23 x 10^-17)/(2.51 x 10^-21 + 2.23 x 10^-17 + 2.08 x 10^-17)
= 0.517 M
charge balance equation,
[CO3^2-] + [OH-] = 2[Na+] + [H+]
mass balance equation,
[CO3^2-] = 2[Na+]
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