Solution Found!
a. At what pH will the concentration of a compound with a
Chapter 2, Problem 40P(choose chapter or problem)
Problem 40P
a. At what pH will the concentration of a compound with a pKa = 8.4 be 100 times greater in its basic form than in its acidic form?
b. At what pH will the concentration of a compound with a pKa = 3.7 be 10 times greater in its acidic form than in its basic form?
c. At what pH will the concentration of a compound with a pKa = 8.4 be 100 times greater in its acidic form than in its basic form?
d. At what pH will 50% of a compound with a pKa = 7.3 be in its basic form?
e. At what pH will the concentration of a compound with a pKa = 4.6 be 10 times greater in its basic form than in its acidic form?
Questions & Answers
QUESTION:
Problem 40P
a. At what pH will the concentration of a compound with a pKa = 8.4 be 100 times greater in its basic form than in its acidic form?
b. At what pH will the concentration of a compound with a pKa = 3.7 be 10 times greater in its acidic form than in its basic form?
c. At what pH will the concentration of a compound with a pKa = 8.4 be 100 times greater in its acidic form than in its basic form?
d. At what pH will 50% of a compound with a pKa = 7.3 be in its basic form?
e. At what pH will the concentration of a compound with a pKa = 4.6 be 10 times greater in its basic form than in its acidic form?
ANSWER:
Solution 40P :
Step 1 of 6:
Here, the given questions can be answered using the Henderson–Hasselbalch equation. It is the equation that relates pKa of the acid and the pH of the solution, which is derived to calculate precisely how much of the compound will be in its acidic form and how much will be in its basic form at a particular pH. The equation is as follows :
pKa = pH +
Where, HA is acidic form and A- is basic form.