I have no idea what the term "two concentration tables" means. However, I assume the problem wants you to calculate concn HBrO, H3O^+, etc.
First, CsBrO is the salt of a strong base (CsOH) and a weak acid (HBrO). The BrO^- is a strong base and hydrolyzes in aqueous solution as follows:
......BrO^- + HOH ==> HBrO + OH^-
I...0.0400.............0......0
C......-x..............x......x
E..0.0400-x............x......x
Kb for BrO^- = (Kw/Ka for HBrO) = (x)(x)/(0.0400-x).
Solve for x = (HBrO) = (OH^-). Convert (OH^-) to (H3O^_) to get c. The final (BrO^-) = 0.0400-x = ?
Use two concentration tables to calculate the concentrations of the species present in a 0.0400 M solution of CsBrO.
a.[HBrO]
b.[BrO-] = 0.0400M
c. [H3O+]
d.[OH-]
hi. how would I attempt this problem. can you walk me through it or give me a hint.
1 answer
1 answer