18 Questions
The Henderson-Hasselbalch equation is used to calculate the pH of basic/alkaline buffers.
True
Strong acids are used to prepare acidic buffers.
False
A buffer solution must contain equal concentrations of acid and base components.
False
The pKa of a weak acid is the negative log of its acid ionization constant.
True
Alkalosis is a condition where the blood pH drops.
False
A conjugate base is a strong acid.
False
A buffer solution can resist changes in pH upon the addition of large amounts of acid or base.
False
A weak acid and its conjugate base are required components of a buffer solution.
True
The pH of blood is maintained by a buffer solution that consists of only carbonic acid.
False
Hydrolysis of a salt can produce a neutral solution.
False
A buffer solution can completely neutralize the addition of acid or base.
False
The hydroxide ion produced in the reaction makes the solution acidic.
False
The pH of a buffer containing 0.1 M sodium acetate and 0.2 M acetic acid is 4.76.
False
A sodium acetate-acetic acid buffer with a pH of 5.76 has a molar ratio of salt to acid of 1:10.
False
Phosphoric acid is a strong acid.
False
The pH of a buffer prepared by mixing 100mL of 0.2 M phosphoric acid with 250 mL of 0.1 M sodium phosphate monobase is 2.125.
False
A conjugate base is the species that donates an electron pair.
False
A weak acid has a pH equal to its pKa.
False
Learn about the importance of buffer solutions in maintaining the body's acid-base balance, and how they work to regulate pH levels. Discover the conditions required for a buffer solution and the two main types of buffers.
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