Predict whether the Ph endpoint is =7 >7, or<7 for each of the following acid-base titrations. Justify you predictions

a) hydroiodic acid with sodium hydroxide.
b)boric acid with sodium hydroxide
c) hydrochloric acid with magnesium hydroxide
d) hydrochloric acid with aqueous ammonia

Here is the way you know.

acid + base ==> salt + water.
If the acid is strong and the base is weak, the salt will be acidic and the equivalence point will be <7.
If the base is strong and the acid is weak, the salt will be basic and the equivalence point will be >7. If the acid is strong and the base is strong, the pH at the equivalence point will be 7.
For a. HI + NaOH ==> NaI + H2O.
HI is strong. NaOH is strong. Equivalence point will be 7.0

To predict whether the pH endpoint is equal to 7, greater than 7, or less than 7 for each acid-base titration, we need to consider the nature of the reactants and products. Here are the predictions for each titration:

a) Hydroiodic acid with sodium hydroxide:
Hydroiodic acid (HI) is a strong acid, and sodium hydroxide (NaOH) is a strong base. In this titration, a strong acid reacts with a strong base, resulting in a neutral salt (sodium iodide) and water. Based on this, we predict that the pH endpoint will be equal to 7.

b) Boric acid with sodium hydroxide:
Boric acid (H3BO3) is a weak acid, and sodium hydroxide (NaOH) is a strong base. The reaction between a weak acid and a strong base results in the formation of a basic salt (sodium borate) and water. The pH endpoint is expected to be greater than 7, as the solution becomes basic due to the presence of the basic salt.

c) Hydrochloric acid with magnesium hydroxide:
Hydrochloric acid (HCl) is a strong acid, while magnesium hydroxide (Mg(OH)2) is a strong base. A strong acid reacting with a strong base leads to the formation of a neutral salt (magnesium chloride) and water. We predict that the pH endpoint will be equal to 7.

d) Hydrochloric acid with aqueous ammonia:
Hydrochloric acid (HCl) is a strong acid, and aqueous ammonia (NH3) is a weak base. The reaction between a strong acid and a weak base results in the formation of an acidic salt (ammonium chloride) and water. Therefore, we predict that the pH endpoint will be less than 7.

Note: Keep in mind that these predictions are based on the assumption that the titration is carried out under ideal conditions. In reality, other factors such as impurities or side reactions may influence the pH endpoint slightly.

To predict the pH endpoint for each of the mentioned acid-base titrations, we need to consider the reactants involved, their acid-base properties, and the resulting products. The pH endpoint is determined by the nature and strength of the acids and bases involved.

a) Hydroiodic acid with sodium hydroxide:
Hydroiodic acid (HI) is a strong acid, while sodium hydroxide (NaOH) is a strong base. A strong acid reacts with a strong base to form a neutral salt and water. In this case, the neutral salt formed is sodium iodide (NaI) and water (H2O). Since both the acid and base involved are strong, the pH endpoint of this titration is expected to be neutral, pH = 7.

b) Boric acid with sodium hydroxide:
Boric acid (H3BO3) is a weak acid, and sodium hydroxide (NaOH) is a strong base. In this titration, the boric acid will react with the sodium hydroxide to form a salt called sodium borate (Na3BO3) and water (H2O). As boric acid is a weak acid, it cannot fully ionize in solution, resulting in a slightly acidic solution. Therefore, the pH endpoint for this titration will be slightly acidic, pH < 7.

c) Hydrochloric acid with magnesium hydroxide:
Hydrochloric acid (HCl) is a strong acid, while magnesium hydroxide (Mg(OH)2) is a weak base. When these two react, they will form magnesium chloride (MgCl2) and water (H2O). As hydrochloric acid is a strong acid, it will completely dissociate in solution, resulting in a highly acidic environment. Therefore, the pH endpoint for this titration will be highly acidic, pH < 7.

d) Hydrochloric acid with aqueous ammonia:
Hydrochloric acid (HCl) is a strong acid, and aqueous ammonia (NH3 + H2O) is a weak base. In this reaction, hydrochloric acid will react with ammonia to form ammonium chloride (NH4Cl). The formation of the ammonium chloride salt will make the solution slightly acidic. However, due to the weak nature of ammonia as a base, the pH endpoint for this titration will still be slightly basic, pH > 7.

In summary:
a) pH endpoint = 7
b) pH endpoint < 7
c) pH endpoint < 7
d) pH endpoint > 7

These predictions are based on the acid-base properties of the reactants involved and the resulting products formed during the titration process.