Final answer:
HBr and HCl are both strong acids that dissociate completely in water, making them comparable in strength with a slight edge to HBr in non-aqueous solutions. OH- is a strong base and not an acid. Cl-, being the conjugate base of HCl, has minimal basicity and is weaker as an acid.
Step-by-step explanation:
To rank the following compounds from strongest to weakest acid: HBr, HCl, OH-, and Cl-, we need to understand the relative strengths of acids and bases. Strong acids like HBr and HCl dissociate completely in water, which is a process influenced by the polarity and strength of the H-A bond, where 'A' is the halogen atom. In general, the acid strength increases with stronger H-A bonds and higher electronegativity of the corresponding halogen atom. Based on this, HBr and HCl are strong acids. OH- (hydroxide) is not an acid; it is actually a strong base. Cl- (chloride) is the conjugate base of HCl, and it has minimal basicity.
Therefore, the correct order from strongest to weakest acid, not considering OH- since it's a base, would be: HBr ≈ HCl > Cl-. The approximate equality sign between HBr and HCl represents their similar strengths in water due to the leveling effect, but showing a specific ranking, we can assume that HBr is slightly stronger than HCl in non-aqueous environments.
For compounds like OH- and Cl-, it's important to note that OH- is a strong base, not an acid, and Cl- is a very weak base, which would not typically fall under an acid strength ranking.