Since pK_a = -log K_a, which of the following is a correct statement? A)acetic acid (pK_a = 4.7)is stronger than lactic acid, (pK_a = 3.9) B)lactic acid, (pK_a = 3.9)is weaker than all forms of phosphoric acid, (pK_a = 2.1, 6.9 and 12.4) C)since the pK_a for conversion of the ammonium ion to ammonia is 9.25, ammonia is a weaker base then the acetate ion D)for carbonic acid with pK_a values of 6.3 and 10.3, the bicarbonate ion is a stronger base than the carbonate ion E)none of the above

Question

Quizplus · Accepted Answer

The pK_a value (often referred to as pKa in the context of acids) is a measure of the strength of an acid; the lower the pKa, the stronger the acid. Therefore, the statements given are incorrect based on the pKa values provided. For example, a lower pKa value for lactic acid compared to acetic acid means lactic acid is actually stronger, not weaker. Similarly, the comparisons made in the other options are also based on misunderstandings of how pKa values reflect acid or base strength.

Since PKa = -Log Ka, Which of the Following Is

Since PK_a = -Log K_a, Which of the Following Is