Question
A weak base with a concentration of 1.3 mol/L has a percent ionization of 0.72%. What is the Kb of this weak base?
could someone help me with this question or how to get started?
could someone help me with this question or how to get started?
Answers
Call the weak base BOH.
BOH <==> B^+ + OH^-
Kb = (B^+)(OH^-)/(BOH)
If 0.72% ionized, that means(H^+) must be 1.3 M x 0.0072 = ??
Of course (OH^-) must be the same.
If BOH is 0.72% ionized, it must be 100% - 0.72% unionized.
Substitute into Kb expression and solve for Kb. Post your work if you get stuck.
BOH <==> B^+ + OH^-
Kb = (B^+)(OH^-)/(BOH)
If 0.72% ionized, that means(H^+) must be 1.3 M x 0.0072 = ??
Of course (OH^-) must be the same.
If BOH is 0.72% ionized, it must be 100% - 0.72% unionized.
Substitute into Kb expression and solve for Kb. Post your work if you get stuck.
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