A buffer solution is created from a weak acid, HA (pKa 6.0), and its conjugate
base, A-. To find the ratio of the base A- to the acid HA at pH 5.0, we can use
the Henderson-Hasselbalch equation:
**pH = pKa + log[A-]/[HA]**
Substituting the values, we have:
**5 = 6 + log[A-]/[HA]**
Rearranging gives:
**-1 = log[A-]/[HA]**
By converting from logarithmic form, we find:
**10^-1 = ratio**
Thus, the ratio is:
**ratio = 0.1**
, ---
Next, regarding the common elements in organic compounds within living cells,
which of the following is the least common?
a) C (Carbon)
b) F (Fluorine)
c) S (Sulfur)
d) N (Nitrogen)
**Answer: B - Fluorine**
---
If the hydrogen ion concentration in the blood increases ten-fold, the pH will
change as follows:
**Answer: The pH decreases by one unit.**
---
When the pH changes from 7.0 to 6.0, which amino acid R-group is most
affected? (Hint: The most affected R-group is the one with a pKa closest to pH
7.0):
base, A-. To find the ratio of the base A- to the acid HA at pH 5.0, we can use
the Henderson-Hasselbalch equation:
**pH = pKa + log[A-]/[HA]**
Substituting the values, we have:
**5 = 6 + log[A-]/[HA]**
Rearranging gives:
**-1 = log[A-]/[HA]**
By converting from logarithmic form, we find:
**10^-1 = ratio**
Thus, the ratio is:
**ratio = 0.1**
, ---
Next, regarding the common elements in organic compounds within living cells,
which of the following is the least common?
a) C (Carbon)
b) F (Fluorine)
c) S (Sulfur)
d) N (Nitrogen)
**Answer: B - Fluorine**
---
If the hydrogen ion concentration in the blood increases ten-fold, the pH will
change as follows:
**Answer: The pH decreases by one unit.**
---
When the pH changes from 7.0 to 6.0, which amino acid R-group is most
affected? (Hint: The most affected R-group is the one with a pKa closest to pH
7.0):
