Question

The pkb of a weak base is 3.22. determine the initial concentration of a solution of this weak base with a ph of 10.6. give the answer to 3 significant figures in the form of 0.000xxx. assume unit is mol dm⁻³ and is not required in the answer.

Answer 1

To determine the initial concentration of a solution of a weak base with a pH of 10.6, we can calculate Kb using the formula Kb = 10^(-pKb) and solve for [base] using the equation [OH-] = sqrt(Kb * [base]).

Step-by-step explanation:

To determine the initial concentration of a solution of a weak base with a pH of 10.6, we need to use the concept of pKb. Given that pKb is equal to 3.22, we can calculate Kb using the formula Kb = 10^(-pKb). Once we have Kb, we can use the equation [OH-] = sqrt(Kb * [base]). Since the solution is basic (pH greater than 7), we can assume that [OH-] is equal to the concentration of the base, [base]. Therefore, we can solve for [base] by substituting the known values into the equation.