Answer:
Pyruvic acid: conjugate base
Lactic acid: conjugate base
Explanation:
The ratio of conjugate base to conjugate acid can be found using the Henderson-Hasselbalch equation when the pH and pKa are known.
pH = pKa + log([A⁻]/[HA])
The equation can be rearranged to solve for the ratio:
pH - pKa = log([A⁻]/[HA])
[A⁻]/[HA] = 10^(pH-pKa)
Now we can calculate the ratio for the pyruvic acid:
[A⁻]/[HA] = 10^(pH-pKa) = 10^(7.4 - 2.50) = 79433
[A⁻] = 79433[HA]
There is a much higher concentration of the conjugate base.
Similarly for lactic acid:
[A⁻]/[HA] = 10^(pH-pKa) = 10^(7.4 - 3.86) = 3467
[A⁻] = 3467[HA]
For lactic acid the conjugate base also dominates at pH 7.4
Remark
The balance numbers in front of the chemicals tell you how to set up the proportion to solve your question
For every 2 moles Na only 1 mole of Cl2 is required.
Equation
2 moles Na:1 mole Cl2 :: x moles Na:4 moles Cl2
Solution
2/1 = x/4 Cross multiply
2*4 = x*1
8 = x
Conclusion
8 moles of Na will be used. <<< Answer
Answer: The answer is an ionic bond
