Practice Questions Flashcards
What is the pH of the solution when 0.1 M of acetic acid and 0.05 M of sodium acetate are mixed, pKa=4.76?
pH=pKa+log[A-]/[HA]
∴pH=4.76+log[0.05]/[0.1]
∴pH=4.76+log0.5
∴pH=4.76|(-0.3)|
∴pH = 4.46
Calculate the pH of a buffer containing 0.05 M pyruvic acid and 0.06M sodium pyruvate, Ka of pyruvic acid = 3.2x10-3
The first step is to covert Ka to pKa:
pKa = -logKa
∴pKa = -log(3.2x10-3)
∴pKa = 2.49
→pH = pKa + log[A-]/[HA]
∴pH = 2.49 + log[0.06]/[0.05]
∴pH = 2.49 + log[1.2]
∴pH = 2.49 + 0.079
∴pH = 2.57
Prepare a buffer solution with a pH of 4.0
First step: Choose the buffer:
e.g. Lactic acid (pKa = 3.85)
Second step: Find ratio of buffer components:
pH = pKa + log[A-]/[HA]
[A-]/[HA] = 10(pH - pKa)
[A-]/[HA] = 10(4 - 3.85)
[A-]/[HA] = 1.41
→1.41 moles of sodium lactate: 1 mole of lactic acid
What is the pH of a solution of 0.04 M HNO3?
HNO3 is a strong acid
∴pH = -log[H+]
∴pH = -log(0.04)
∴pH = 1.40
What is the pH of a solution of 0.1 M HClO4?
HClO4 (perchloric acid) is a strong acid
∴pH = -log[H+]
∴pH = -log(0.1)
∴pH = 1
What is the pKa of C6H5CO2H if its Ka is 6.45x10-5?
pKa = -log(Ka)
∴pKa= -log(6.45x10-5)
∴pKa = 4.19
What is the Ka of triethylamine if its pKa is 11.01?
pKa = -log(Ka)
∴Ka = 10-pKa
∴Ka = 10-11.01
∴Ka = 9.77x10-12
What is the pH of a solution of 0.01 M C6H5CO2H, pKa(C6H5CO2H) = 4.05?
Ka=10-pKa
∴Ka=10-4.05
∴Ka=8.91x10-5
→[H+]=√(Ka x [HA])
∴[H+]=√(8.91x10-5x0.01)
∴[H+]=9.44x10-4
pH = -log[H+]
∴pH = -log(9.44x10-4)
∴pH = 3.03
What is the pH of a solution of 0.5 M trimethylamine, pKa(NMe3) = 9.81?
Ka = 10-pKa
∴Ka = 10-9.81
∴Ka = 1.55 x 10-10
→[H+] = √(Ka x [HA])
∴[H+] = √(1.55 x 10-10 x 0.5)
∴[H+] = 8.80 x 10-6
→pH = -log[H+]
∴pH = -log(8.80 x 10-6)
∴pH = 5.06
Prepare a 2 L buffer solution with a pH of 9.50
Buffer to be used: Phenol: pKa = 9. 89
Using the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
∴9.5 = 9.89 + log([A-]/[HA])
∴-0.39 = log([A-]/[HA])
∴0.41 = ([A-]/[HA])
∴dissolve 0.41 moles of sodium phenoxide and 1 mole of phenol in water
Prepare a 100 ml buffer solution with a pH of 7.5.
Buffer to be used: HEPES pKa = 7.66
Using the Henderson-Hasselbalch equation:
pH = pKa + log([A-]/[HA])
∴7.5 = 7.66 + log([A-]/[HA])
∴-0.16 = log([A-]/[HA])
∴0.69 = ([A-]/[HA])
∴Dissolve 0.69 moles of sodium salt of HEPES and 1 mole of HEPES in water
Does this structure exist? Why/Why Not?
This structure does not exist. As an amino acid consists of an acid and a base, it will always be protonated in one area, and thus cannot be uncharged.
The pKa of the amino acid carboxylic acid is very low compared with acetic acid (pKa = 4.75); why?
The amino group is electron-withdrawing due to its positive charge, enhancing the acidity of the carboxylic acid and hence reducing pKa
Explain why the amine pKa of proline differs significantly from glycine?
Locate the amide bond(s) in this molecule