3. In each of the following, the stronger acid is identified and an explanation

Question

3. 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? a. HCI> HF, because the HF bond energy is greater than the HCl bond energy b. HCO, >H,CO,, because the negative charge stabilizes the loss of a proton. c. CCl,CO,H CH,CO,H, because electronegative substituents stabilize the conjugate base. d. HBrO, HBrO2, because of the additional electronegative oxygen atom. e. CIOH >BrOH, because Cl is more electronegative than Br.

Explanation / Answer

All statments are true except statment b.

Because, The pKa for H2CO3 is 6.4, and the pKa for HCO3- is 10.3. This makes H2CO3 as a strong acid and HCO3- as a comparitively weaker acid. Lower the pKa stronger the acid.

Thus answer is answer is option b. HCO3- > H2CO3, because the negative charge stabilizes the loss of a proton.

Other statments:

HCl is a strong acid than HF. The size of the halogens changes more drastically than their electronegativities as you go down the group. The F- ion is small compared to the Cl- ion, so negative charge is concentrated on this small sphear. Big iodide with a negative charge is the most stable, because it can distribute the -1 charge over a larger surface.

CCl3COOH is stronger acid than CH3COOH because of -I effect of 3 Cl.

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