A salt will dissolve in water completely, existing as the individual ions that make up the compound. These ions can be thought of as the conjugate bases and acids that result from the dissociation of the reactant acids and bases. If the conjugate acid of a weak base is present in the solution, then it will become deprotonated, releasing protons into the water and lowering the pH. To answer this question, we are looking for a salt in which one of the ions created is a conjugate acid of a weak base. Let's look at a few examples in order to find the right answer:

1.  will dissociate into sodium and fluoride ions. Sodium is the metal found on sodium hydroxide. Since sodium hydroxide is considered a strong base, the sodium ions will NOT attach to any hydroxide ions in solution. Fluoride ions, on the other hand, are the conjugate base of hydrofluoric acid, a weak acid. This means that some of the fluoride ions will attach to protons in solution, effectively raising the pH. This results in a basic solution.

2.  is an example of a salt that will result in a neutral solution. Because lithium ions come from the strong base lithium hydroxide, and bromide ions come from the strong acid hydrobromic acid, neither of these ions will be involved in an acid/base reaction. This results in a solution with a pH of 7.

 has two ions: ammonium ions and chloride ions. Chloride ions are the conjugate base of hydrochloric acid, a very strong acid. Ammonium ions, however, are the conjugate acid of ammonia, a weak base. This means that some of the ammonium ions will become deprotonated, and release protons into the solution. this results in an acidic solution.

A Brønsted-Lowry acid is an ionic compound that donates a proton, when the compound is placed in water.

HF and NaOH are the only ionic compounds of the given answer options; all the others are covalent compounds. When dissolved in water, only HF will donate protons.

Thus, HF is the only given Brønsted-Lowry acid.

An acid is classified as strong if it completely dissociates into ions in water. Some examples of common strong acids: 

 is not a strong acid because it doesn't ionize completely in solution.

By definition, and Arrhenius acid will dissociate in water to release .  will dissociate into  and  in solution. The increased concentration of  causes a drop in pH of the solution. In general, if a hydrogen atom is bound to a very electronegative atom, like in the case of , fluorine tends to take the electron away from hydrogen, resulting in ions.

 or ammonia is a complicated molecule. It's a kind of molecule that we call amphoteric, meaning that it can be an acid or a base. However, because ammonia plays the role of a very weak base, it's mostly thought of as having basic qualities. It has the ability to bind with acids to create an ammonium salt or act as a proton acceptor and become ammonium (acid). 

Also, commonly, acids have the  format, where  represents a halogen. In another construct, acids ideally have protons that they can donate - this can be observed in  and .

Commonly, bases have the  format, where  is any metallic element from the first two columns of the periodic table. This is seen with , , and . The remaining two options are essentially different "versions" of the same molecule - one just happens to be the protonated form ().  

While  is technically amphoteric, it's more so thought of in terms of its basic qualities. When it does act as an acid, it's a very weak acid. Ammonia can easily become ammonium, a proton donator, due to the lone pair of electrons that continue to orbit around the nitrogen center. 

The equation to use here is:

Here,  is the molarity of the acid,  is the volume of the acid,  is the molarity of the base, and  is the volume of the base. Don't forget to convert the volume to liters!

Below is a generic acid-base neutralization reaction:

The products are always water, and a salt. This salt is produced from the resulting ions  and . The  from the acid replaces the  from the base, and the  from the acid replaces the  from the base. Since there are two replacements, acid-base neutralizations are classified as double-replacement reactions.

Arrhenius acid/base theory was created by Swedish chemist Svante Arrhenius, and is the oldest acid/base classification. According to his classification, acids are compounds that increase the concentration of  ions in a solution, while bases are compounds or elements that either decrease the concentration of  ions in solution or increase the concentration of  ions in a solution. The other two answers describe the Brønsted–Lowry theory of acids and bases.

For every acidic or basic solution, the product of the hydroxide ion concentration and the hydronium ion concentration will be equal to , the dissociation constant for water. In other words:

Since we are given the hydroxide ion concentration, we can determine the hydronium ion concentration using this equation.