Of the following, which statement best explains why HF is a weak acid but HCl, H

Question

Of the following, which statement best explains why HF is a weak acid but HCl, HBr and HI are strong acids? (Question from MCAT Physical Sciences Review, 2008 Version, The Princeton Review.)

1. F has a larger radius than Cl, Br or I

2. F- has a smaller radius than Cl-, Br- or I-

3. F- has a larger radius than Cl-, Br- or I-

4. F has a greater ionization energy than Cl, Br or I

1. F has a larger radius than Cl, Br or I

2. F- has a smaller radius than Cl-, Br- or I-

3. F- has a larger radius than Cl-, Br- or I-

4. F has a greater ionization energy than Cl, Br or I

Explanation / Answer

2. F- has a smaller radius than Cl-, Br- or I-

Since F- has a smaller radius compared to other halide ions so the attraction between the H+ and F- ions is very high . Hence when HF is dissolved it does not dissociate into H+ and F- ions because og the strong attraction between them. THerefore HF is a weak acid compared to HCl , HBr and HI

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