Determine the [OH^-] of a solution that is 0.145 M in CO3^2-.
Write the hydrolysis of CO3^-2.
CO3^-2 + HOH ==> HCO3^- + OH^-
Now set up an ICE chart and solve for the Kb expression which is
Kb = (Kw/k2) = (HCO3^-)(OH^-)/(CO3^-2)
To determine the concentration of hydroxide ions ([OH^-]) in a solution that is 0.145 M in carbonate ions (CO3^2-), we need to consider the dissociation reaction of the carbonate ion with water:
CO3^2- + H2O ⇌ HCO3^- + OH^-
From this reaction, we can see that for every carbonate ion that reacts, one hydroxide ion is produced.
Therefore, the concentration of hydroxide ions is equal to the concentration of carbonate ions. In this case, the concentration of hydroxide ions ([OH^-]) is 0.145 M.
To determine the [OH^-] (hydroxide ion concentration) of a solution that is 0.145 M in CO3^2- (carbonate ion), we need to consider the reaction that occurs between CO3^2- and water (H2O).
The CO3^2- ion can combine with water to form bicarbonate (HCO3^-) and hydroxide (OH^-) ions. The balanced reaction equation is as follows:
CO3^2- + H2O → HCO3^- + OH^-
In this equation, one CO3^2- ion produces one OH^- ion. Therefore, the concentration of OH^- ions in the solution will be equal to the concentration of CO3^2- ions.
Therefore, in this case, [OH^-] = 0.145 M.