The ionization constants for the diprotic acid H 2S
are 1.0 x 10 -7 and 1.3 x 10 -13.
H2S
(aq) +
H2O (l) <=> HS
-(aq) +
H3O
+(aq) Ka
= 1.0 x 10 -7
HS -(aq) +
H2O (l) <=> S-2
(aq) + H3O
+(aq) Ka
= 1.3 x 10 -13
What is the equilibrium concentration of HS - in a 0.300
M solution of H2S?
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3...
The ionization constants for the diprotic acid H 2S are 1.0 x 10 -7 and 1.3 x 10 -13. H2S (aq) + H2O (l) <=> HS -(aq) + H3O +(aq) Ka = 1.0 x 10 -7 HS -(aq) + H2O (l) <=> S-2 (aq) + H3O +(aq) Ka = 1.3 x 10 -13 What is the equilibrium concentration of HS - in a 0.300 M solution of H2S?
Write the acid ionization constants ( also referred to as the equilibrium constant for a weak acid) for the following reactions: a. H2CO3(aq) + H2O(l) H3O+(aq) + HCO3-(aq) b. H2S(aq) + H2O(l) H3O+ (aq) + HS-(aq) c. HC3H5O3 + H2O(l) H3O+(aq) + C3H5O3(aq)
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