In: Chemistry
What is the pH of a solution created by combining 1.22 mole of HOBr and 0.49 mole NaOH in a 1.00L solution? Ka HOBr = 2.5 x 10-9
HOBr + NaOH -----------> NaOBr + H2O
I 1.22 0.49 0
C -0.49 -0.49 0.49
E 0.73 0 0.49
PKa = -logka
= -log2.5*10-9
= 8.6
PH = Pka + log[NaOBr]/[HOBr]
= 8.6 + log0.49/0.73
= 8.6-0.173 = 8.427