In each of the following, the stronger acid is identified and an explanation is given. All except one are correct statements. Which one is not correct?

Question

Quizplus · Accepted Answer

The correct statement is that the negative charge stabilizes the conjugate base, which makes HCO3- a weaker acid than H2CO3. The explanation given for option B is correct. Option A is correct because the larger bond energy in HF makes it less likely to donate a proton, making it a weaker acid than HCl. Option C is correct because electronegative substituents on a molecule stabilize the negative charge on the conjugate base, making the acid stronger. Option D is correct because the additional electronegative oxygen atom in HBrO2 stabilizes the negative charge on the conjugate base, making HBrO2 a stronger acid than HBrO. Option E is incorrect because the electronegativity of Cl and Br are not the deciding factor in determining acid strength. In fact, Cl is a stronger acid than Br due to its smaller atomic size and higher electronegativity.

In Each of the Following, the Stronger Acid Is Identified