Asked by Anonymous
What is the pH of a 0.2 M solution of pyridinium
chloride (C5H5NHCl)? Kb for pyridine
(C5H5N) is 1.5 × 10−9
.
1. 8.824
2. 2.788
3. 4.761
4. 3.068
5. 3.308
6. 2.698
7. 2.938
8. 5.176
9. 9.239
chloride (C5H5NHCl)? Kb for pyridine
(C5H5N) is 1.5 × 10−9
.
1. 8.824
2. 2.788
3. 4.761
4. 3.068
5. 3.308
6. 2.698
7. 2.938
8. 5.176
9. 9.239
Answers
Answered by
DrBob222
Let's call pyridinium chloride just BNHCl so it's the BNH^+ that is hydrolyzed.
...........BNH^+ + H2O ==> BN + H3O^+
I..........0.2..............0.....0
C...........-x..............x.....x
E.........0.2-x.............x.....x
Ka for BNH^+ = (Kw/Kb for pyridine) = (x)(x)/(0.2-x)
Solve for x = (H3O^+) and convert to pH. Looking at the answers, you may need to solve the quadratic but I should point out that the answers are given to 4 significant figures and Kb is known only to 2 s.f. so all of that precision in the answer choices is not warranted.
...........BNH^+ + H2O ==> BN + H3O^+
I..........0.2..............0.....0
C...........-x..............x.....x
E.........0.2-x.............x.....x
Ka for BNH^+ = (Kw/Kb for pyridine) = (x)(x)/(0.2-x)
Solve for x = (H3O^+) and convert to pH. Looking at the answers, you may need to solve the quadratic but I should point out that the answers are given to 4 significant figures and Kb is known only to 2 s.f. so all of that precision in the answer choices is not warranted.
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