1. The pH of a solution is a measure of the concentration of hydrogen ions present. (True/False) - True. The pH scale is a measure of the concentration of hydrogen ions in a solution. 2. A buffer solution resists changes in pH when small amounts of acid or base are added. (True/False) - True. A buffer solution contains a weak acid and its conjugate base, or a weak base and its conjugate acid, which can neutralize small amounts of added acid or base. 3. The pKa of an acid is a measure of its strength as a proton donor. (True/False) - True. The lower the pKa of an acid, the stronger the acid and the more readily it donates a proton. 4. The dissociation constant (Ka) for a weak acid is a measure of its ability to donate protons. (True/False) - True. The dissociation constant Ka measures the extent to which a weak acid donates protons in solution. 5. In a titration, the equivalence point is reached when the moles of acid are equal to the moles of base added. (True/False) - True. The equivalence point in a titration is when the moles of acid are equal to the moles of base added, indicating neutralization. 6. A pH of 7 is considered neutral, while a pH below 7 is acidic and above 7 is basic. (True/False) - True. A pH of 7 is considered neutral, with lower values indicating acidity and higher values indicating basicity. 7. The Henderson-Hasselbalch equation relates the pH of a buffer