Let's call saccharin BNH2.
pH = 12.34
pOH = 14-12.34 = 1.66
(OH^-) = about 0.022
......BNH2 + H2O ==> BNH3^+ + 2OH^-
I.......x..............0........0
C...-0.011..........0.011...0.022
E.....x-0.011.......0.011...0.022
Kb = 4.8E-3 = (BNH3^+)(OH^-)/(BNH2)
Subtitute the E line into the Kb expression and solve for x = M saccharin.
Then M = mols/L. You have M and L, solve for mols.
Then mols = grams/molar mass.
Repost ..
Saccharin is a weak organic base with a Kb of 4.8X10^-3. A 0.672-g sample of saccharin dissolved in 30.0mL of water had a pH of 12.34. What is the molar mass of saccharin?
3 answers
I did step by step but answer doesn't match any of the choices it gives me
Amine derivative Weak Bases do not give 1:2 ionization ratios. Balance your equation, then try your problem again.
1 answer