Think ammonia, NH3.
NH3 + HOH ==> NH4^+ + OH^-
Kb = (NH4^+)(OH^-)/(NH3). You've probably solved 100 problem where you know pH of a NH3 solution and you calculate (NH3).
(CH3)3N does EXACTLY the same thing.
(CH3)3N + HOH ==> (CH3)3NH^+ + OH^-
Write Kb expression, look up Kb, calculate OH from pH and solve for (CH3)3N.
Post your work if you get stuck.
1.) What must be the molarity of an aqueous solution of trimethylamine (CH3)3N
if it has a Ph of 11.04? Kb = 6.3*10^-5
if someone can show the mechanics of doing this, will be appreciated much.
1 answer