Posted by Sharon on .
for a solution of the weak base, 0.075 M ethylamine C2H5NH2(aq), the hydroxide ion concentration (OH-) is 6.6x10^-3 M. Assume that temperature is constant and volumes are additive.
a. Write the equilibrium dissociation equation.
b. What's the pH of 0.075 M C2H5NH2(aq)?
c. What's the value of Kb?
Please show your work on how you calculate it so I can see how you figured it out. Thanks.
C2H5NH2 + HOH ==> C2H5NH3^+ + OH^-
You know OH^-; therefore,
pOH = -log(OH^-) and
pH + POH = pK2w = 14. Solve for pH.
Write the Kb expression
Substitute OH^- = 0.0066
(C2H5NH3^+) = 0.0066
(C2H5NH2) = 0.075-0.0066
Solve for Kb.
Thanks! This was very helpful.
corrn; type -
pH + pOH = pKw = 14 (and not pK2w)
(Kw has no K2).