Since hydrofluoric acid is a weak acid, an ICE table needs to be set up in order to determine the hydronium ion concentration. Since both fluoride ion and hydronium ion concentrations will increase by , while the acid concentration will decrease by , the equilibrium expression comes out to be:

Note that the  in the denominator will have a negligible effect and can be ignored.

Since  is equal to the hydronium ion concentration, we can calculate the pH by taking the negative log of the concentration:

At the equivalence point, there are equimolar amounts of acid and base. This means that all weak acid has been neutralized, and only the conjugate base remains. Since the conjugate base of a weak acid will affect the pH, we need to use an ICE table in order to find the pH. First, we start by finding the base dissociation constant of the conjugate base, using the equation:

The balanced equation for the conjugate base dissociation is:

As the hydroxide ion and acid concentrations increase by , the fluoride ion concentration will decrease by . This makes the equilibrium expression:

Since this is the hydroxide concentration, we can find the pH by taking the negative log of this value, then subtracting from 14:

Since the product of the cation and anion is , the only true statement is that the concentration of the cation  is the square root of this number:

Each of these compounds requires one equivalent of H⁺ is added to 100mL of 5N NH₃ mol, so for HClO₄, 2N = 2M, and for NH₃, 5N = 5M.

Using the concentrations and volumes, we can find the moles, finding  HClO₄ and  NH₃.

In this case, equivalents of acid are equal to the equivalents of base, meaning that we are at the equivalence point in a titration. HClO₄ is a strong acid, and NH₃ is a weak base.

Thus, the acid will fully dissociate, while the base will not, resulting in a greater concentration of H⁺ than OH^– in the solution. This means the resulting solution will be acidic. We know that the indicator changes from yellow to green at 8.3, which is a basic pH. Our initial solution is basic, and we must pass through the pH of 8.3 to reach our final acidic solution, with pH < 8.3, meaning that the indicator must change from yellow to green during the reaction. This gives out final answer that the solution will be acidic and green.

NaOH is a strong base, so if the acid were a strong acid, the pH at equivalence would be 7. The graph, however, shows that the pH at equivalence is greater than 7, which means the acid being titrated is a weak acid.

We can also find the approximate pK_a value from the half equivalence point. In the graph, the equivalence point occurs at a pH around 8.9, corresponding to the addition of about 22mL of NaOH. The half equivalence point will thus be after the addition of approximately 11mL of NaOH, giving a pH of 5.0. The pH at the half equivalence is equal to the pK_a, meaning that the K_a value must be around 10^-5.

This leads to our answer, .

For a strong acids and strong base, the equivalence pH will be 7.0. We can see that our equivalence pH is less than 7.0, meaning that the acidic component is prevailing. Hence, we must be working with an acid that is stronger than our base. HNO₃ is a strong acid, and NH₃ is a weak base, meaning that the acid will prevail, and the pH will be acidic (<7.0).

The other answer choices show a strong acid and strong base (HCl and NaOH), a weak acid and strong base (HF and KOH, HCN and LiOH), and a weak acid and weak base (H₂S and C₅H₈O₂). Though the equivalence pH of a weak acid and weak base may not be 7.0, we do not have enough information to choose this answer. The best answer choice is HNO₃ and NH₃

The equivalence point is the point during a titration when there are equal equivalents of acid and base in the solution. Since a strong acid will have more effect on the pH than the same amount of a weak base, we predict that the solution's pH will be acidic at the equivalence point. 5.2 and 1.3 are both acidic, but 1.3 is remarkably acidic considering that there is an equal amount of base in the solution. As a result, 5.2 is a more appropriate answer.

The equivalence point for a strong acid and strong base will be 7.0. When one of the compounds is weak, however, it will dissociate less than its strong counterpart. In our case, the base will dissociate less than the acid. The acid, thus, contributes more to the pH character of the solution.

At the half equivalence point, the concentration of acid in the solution is equal to the concentration of the conjugate base in solution. At this point, the graph shows a line that is near horizontal. This means that base or acid could be added and the pH of the solution would change very slowly.

Remember that pH is on the y-axis of the titration curve; thus a near-horizontal line will signify a region where pH is most stable. At the half equivalence point, pH = pK_a.

Since we are adding acid to a base, the pH must decrease. The initial base will have a high pH, while the final acid will have a low pH; the right of the curve must be lower than the left. In addition, the pH does not change very rapidly until the equivalence point is reached, hence the curve must show little initial change followed by a rapid change.

A titrant is added to a solution being studied. In this scenario, the base is the titrant and the equivalence point is reached when all of the acid has been neutralized by the base. The equivalence point is defined as the point at which moles of added titrant equal the moles of initial solute in solution.

The equimolar concentration of acid and conjugate base happens at a point known as the half-equivalence point, which can be confusing.