Quiz
1. How does Gibbs' free energy affect the solubility of a substance?
a. It determines whether a process is spontaneous or non-spontaneous.
b. It has no impact on solubility.
c. It directly correlates with the volume of the solute.
d. It affects only the solubility of gases.
2. What happens to the water organization of oil and water when you mix it?
a. Oil and water mix evenly
b. Water sinks below the oil
c. Oil and water form separate layers
d. Oil dissolves into the water
3. Which of the following is the formula for Gibbs free energy?
a. ΔG = ΔH - TΔS
b. ΔG = ΔH + TΔS
c. ΔG = ΔH / TΔS
d. ΔG = ΔH TΔS
4. Which of the following conditions will favor lowered ΔG values according to the
equation?
a. Increase enthalpy and decrease entropy
b. Decrease enthalpy and increase entropy
c. Both enthalpy and entropy will increase
d. Both enthalpy and entropy will decrease
5. In what way do weak acids act as “Uninterruptible Proton Suppliers”?
a. They continuously release protons into the solution
b. They absorb protons from the solution
c. They release or absorb protons as needed
d. They do not interact with protons
6. What are the key characteristics of amphiphilic molecules?
a. Hydrophilic head and hydrophobic tail
b. Polar head and polar tail
c. Hydrophobic head and hydrophilic tail
d. Nonpolar head and nonpolar tail
7. What types of groups are found in the hydrophilic head of an amphiphilic molecule?
a. Hydrocarbon chains
b. Polar groups
c. Ionic bonds
d. Nonpolar groups
8. What do hydrophobic tails of amphiphilic molecules prefer to interact with?
a. Water
b. Nonpolar substances
c. Ionic substances
d. Polar substances
9. The pH of a 0.01 M solution of HCL is
a. 2
b. 8
c. 4
d. 3
10. The pOH of the solution is 4.5. Calculate the pH of the solution
a. 9.8
b. 9.5
c. 8.5
d. 7.5
11. Find the pH of a 0.03 M solution of hydrochloric acid
a. 2.523
b. 3.523
c. 1.523
d. 4.523
12. What is the hydrogen ion concentration of a solution that has a pH of 7.40?
a. 4.97 x 10 -7 M
b. 3.98 x 10 -6 M
c. 2.93 x 10 -8 M
d. 3.98 x 10 -8 M
13. What is the hydroxide ion concentration of a solution that has a pOH of 4.60?
a. 2.51 x 10 -5 M
b. 2.52 x 10 -4 M
c. 2.50 x 10 -3 M
d. 2.50 x 10 -5 M
Modified True or False
14. Surfactants are amphiphilic molecules that increase surface tension between two
substances. FALSE
15. Lipid bilayers are the structural basis of cell membranes, providing a selectively
permeable barrier. TRUE
16. What does the Henderson-Hasselbalch equation describe?
a. The relationship between pH and pKa of a weak acid
b. The relationship between pH and concentration of a weak acid or base in a buffer
solution
c. The relationship between concentration of a weak acid and its conjugate base
d. The relationship between concentration of a strong acid and its conjugate base
17. In the Henderson-Hasselbalch equation, what does [A-] represent?
a. Concentration of the weak acid
b. Concentration of the conjugate base
c. pKa of the weak acid
d. pH of the solution
18. Which of the following represents the Henderson-Hasselbalch equation?
a. pH = pKa + log [A-]/[HA]
b. pH = pKa - log [A-]/[HA]
c. pH = -log [A-]/[HA]
d. pH = -log [A-] + log [HA]
19. What is a weak acid?
a. An acid that completely dissociates into ions in water
b. An acid that partially dissociates into ions in water
c. An acid that does not react with water
d. An acid that forms strong covalent bonds in water
20. What happens to a weak acid when it is dissolved in water?
a. It completely dissociates into ions
b. It partially dissociates into ions
c. It remains unchanged
d. It reacts with water to form a strong acid
COMPLETE ME (5 POINTS)
Type of intermolecular forces that occurs when a hydrogen atom is covalently bonded in highly
electronegativity atom such as oxygen, nitrogen and fluorine. _ _ _ r _ _ e _ b _ _ d _
P_ _tial _ _ _ _tive c_ _ _ge occurs on more electronegative atoms, indicating a partial excess of
electrons.
_a_ _ _ _ l _ _ a _ _ _ _ a rise due to unequal sharing of electrons in a covalent bond that creates
a positive and negative charge.
P_ _tial _ _ _ _tive c_ _ _ge on less electronegative atoms.
Hydrogen bonds are D_ _ _ _e - d_ _ _ _e interactions.
HYDROGEN BONDS
PARTIAL NEGATIVE CHARGE
PARTIAL CHARGES
PARTIAL POSITIVE CHARGE
DIPOLE-DIPOLE
