17 Questions
In a strong monobase, the hydroxide ion is completely dissociated in solution.
True
The pH of a solution can be calculated only using the Henderson-Hasselbalch equation.
False
The equivalence point in an acid-base titration is the point where the pH of the solution is exactly 7.
False
Buffer solutions are used to maintain a constant pH in pharmaceutical applications.
True
Polyacids and polybases are always strong acids and bases, respectively.
False
PH indicators are used to determine the equivalence point in an acid-base titration.
True
A weak acid and its conjugate base have the same colour.
False
The pH at the equivalence point of a strong acid and strong base titration is always 7.
True
PH indicators are used in large quantities during titration to detect the equivalence point.
False
The derivative of the curve is used to calculate the equivalent point in potentiometry.
True
The volume of titrant poured at the equivalence point is used to determine the inactive substance content.
False
A weak acid/strong base titration has a pH at the equivalence point that is greater than 7.
True
The pH of a buffer solution can be calculated using the formula pH = pKa + log [acidT] [baseT].
False
Buffer systems in the blood can maintain a pH of exactly 7.4.
False
The addition of a large quantity of acid or base to a buffer solution will not cause a significant change in pH.
False
Acid-base titration is used to measure the strength of strong acids or bases in pharmacy.
False
The equivalence point of an acid-base titration is the point where the pH of the solution is equal to 7.
False
Test your knowledge of acid-base equilibrium in solution, covering topics such as strong and weak acids and bases, pH calculations, buffer solutions, neutralizations, and titrations. Ideal for 1st-year pharmacy students.
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