In: Chemistry
Calculate the pH and the concentrations of all species present in 0.18 M H 2 SO 3 . ( K a1 = 1.5× 10 −2 , K a2 = 6.3× 10 −8 ) Express your answer to three significant figures and include the appropriate units
H2SO3(aq) <-----> HSO3^-(aq) +
H^+(aq)
initial 0.18 M 0 M 0 M
change x x x
at equil 0.18 - x x x
Ka1 = [HSO3^-][H^+]/[H2SO3]
1.5*10^-2 = x*x/(0.18-x)
x = 0.045 M
At equilibrium [H2SO3] = 0.18 - 0.045 = 0.135 M
[ HSO3^-] = 0.045 M
[H+] = 0.045 M
HSO3^- (aq) <----->
SO3^2-(aq) + H^+(aq)
initial 0.045 M 0 M
0.045 M
change x x x
at equili 0.045-x x 0.045+x = 0.045 M
Ka2 = [SO3^2-][H^+]/[HSO3^-]
6.3*10^-8 = x*(0.045)/(0.045-x)
x = 6.29*10^-8
[SO3^2-] = x = 6.29*10^-8 M
[HSO3^-] = 0.045 - 6.29*10^-8 = 0.045 M
[ H^+] = 0.045 M