Rank the given compounds based on their relative Brønsted acidities.

H-CH3

H-OH

H-Cl

H-F

H-NH2

Here is a table that lists the pKa for organic and inorganic compounds.

http://www.cup.uni-muenchen.de/oc/trauner/files/evans_pKa_table.pdf

For example, H2O is 15.7 and HF is 3.17. That means HF is a stronger acid than H2O. I couldn't find NH3 in that list but it is 9.25. Be sure you look in the water column and not the DMSO (dimethylsulfoxide) column for the right solvent.

To rank the given compounds based on their relative Brønsted acidities, we need to consider their ability to donate a proton (H+). The stronger the acid, the more readily it donates a proton. Here is the ranking from strongest to weakest Brønsted acid:

1. H-Cl
2. H-F
3. H-OH
4. H-NH2
5. H-CH3

Explanation:

1. H-Cl: Hydrochloric acid (H-Cl) is a strong acid. It readily donates a proton, making it the strongest Brønsted acid among the given compounds.

2. H-F: Hydrofluoric acid (H-F) is a relatively strong acid. While it is not as strong as H-Cl, it still readily donates a proton, making it the second strongest Brønsted acid.

3. H-OH: Water (H-OH) is a weak acid. It can donate a proton but not as readily as H-Cl or H-F. There is a decreased ability to donate a proton due to the electronegative oxygen atom that stabilizes the negative charge.

4. H-NH2: Ammonia (H-NH2) is a weak base but can still act as a weak acid by donating a proton. However, it is weaker than H-OH due to the stabilizing effect of the lone pair on the nitrogen atom.

5. H-CH3: Methane (H-CH3) is the weakest Brønsted acid among the given compounds. It is very weakly acidic as the carbon-hydrogen bonds are non-polar and do not readily dissociate to donate a proton.

Remember that this ranking is based on the relative acidities of the compounds and their ability to donate a proton.

To rank the given compounds based on their relative Brønsted acidities, we need to consider the strength of the acid in terms of its ability to donate a proton (H+). A stronger acid will easily donate a proton, while a weaker acid will not.

In general, there are several factors that affect the acidity of a compound. These include:

1. Electronegativity: Acidity generally increases with increasing electronegativity of the atom to which the acidic proton is attached.

2. Size: Acidity generally increases with increasing size of the atom to which the acidic proton is attached.

Now, let's analyze the given compounds in order to rank them based on their relative acidities:

1. H-CH3: This compound consists of a hydrogen atom bonded to a methyl group. The acidic proton is attached to a carbon atom, which has a relatively low electronegativity and larger size. Therefore, H-CH3 is the weakest acid among the given compounds.

2. H-OH: This compound consists of a hydrogen atom bonded to a hydroxyl group. Oxygen is more electronegative than carbon, making H-OH a stronger acid compared to H-CH3.

3. H-Cl: This compound consists of a hydrogen atom bonded to a chlorine atom. Chlorine is more electronegative than oxygen, making H-Cl a stronger acid compared to H-OH.

4. H-F: This compound consists of a hydrogen atom bonded to a fluorine atom. Fluorine is the most electronegative element in the periodic table. As a result, H-F is the strongest acid among the given compounds.

5. H-NH2: This compound consists of a hydrogen atom bonded to an amino (NH2) group. Nitrogen is less electronegative than oxygen, but it is larger in size compared to oxygen. Therefore, H-NH2 is stronger acid compared to H-OH but weaker than H-Cl and H-F.

Based on the analysis, the compounds can be ranked from weakest to strongest acid as follows:

H-CH3 < H-OH < H-NH2 < H-Cl < H-F

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