1) it is found that .30 M solutions of the three shots Na3X, Na2Y and NaZ have pH's of 8.5, 7.0 and 10.5 not necessarily in order. (X,Y, and Z AE anions. Na is sodium ion)

A) explain how anions can act as bases in aqueous solution. Write a chemical equation to explain your answer.
B) which pH most likely goes with which salt. Explain.
C) what is the approximate pH of a .010M solution of HZL explain your reasoning.
D)Calculate the acid dissociation constants, Ka for each of the acids, HX-2, HY-, and HZ, and rank them in order of increasing strength, the weakest first. Justify your answer.

a. X^- + HOH ==> HX + OH^-

The anion hydrolyzes with water producing OH^- ions which is why they are basic.

b.
.....X^- + HOH ==> HX + OH^-. For 0.3M
I...0.3.............0.....0
C....-y.............y.....y
E...0.3-y...........y.....y
Kb for X,Y, or Z = (Kw/Ka for HX, k2 for H2X and k3 for H3X)
Therefore, smaller Ka, k2, or k3 values lead to larger Kb values.
Kb = (y)(y)/(0.3-y)
Thus smaller k1, k2, k3 values lead to larger Kb values and that leads to higher values of y when the above equation is solved. y = OH^- in this case, so larger OH^- values means more OH which is smaller H^+ and larger pH values.

c.
I have no idea what HZL is.
d. Go through the calculation I show for part B, then Kb = Kw/Ka where Ka = Ka for HZ, k2 for H2Y and k3 for H3X,

A) Anions can act as bases in aqueous solutions because they can accept a proton (H+ ion) from the water molecule. This leads to the formation of hydroxide ions (OH-) in the solution. The chemical equation for this process can be represented as follows:

Anion (X-) + H2O → OH- + HX

B) Based on the given information, we can match the pH values with the respective salts as follows:

- pH 8.5 corresponds to Na2Y (since Y- serves as a weaker base compared to others)
- pH 7.0 corresponds to NaX (since X- does not readily accept protons and yields a neutral pH)
- pH 10.5 corresponds to NaZ (since Z- acts as a stronger base, resulting in a higher pH)

C) To determine the approximate pH of a 0.010 M solution of HZL, we need additional information about the dissociation of HZL. Without that information, it is not possible to approximate the pH accurately.

D) To calculate the acid dissociation constants (Ka) for HX-2, HY-, and HZ, we need additional information about their dissociation equilibria. Without that information, we cannot rank them in order of increasing strength. However, we can assume that as the pH increases, the acid strength decreases. So, based on the pH values given, we can deduce that the ranking is as follows:

HX-2 > HY- > HZ

A) Anions can act as bases in aqueous solutions by accepting protons (H+) from the solvent or other substances present in the solution. This process is known as hydrolysis. When an anion interacts with water, it can gain a proton to form a hydronium ion (H3O+). This can be represented by the following chemical equation:

A- (aq) + H2O (l) ⇌ HA (aq) + OH- (aq)

In this equation, A- represents the anion, H2O represents water, HA represents the conjugate acid formed by the anion, and OH- represents the hydroxide ion. This equilibrium reaction illustrates how an anion can act as a base by accepting a proton from water.

B) Based on the pH values provided, we can make some inferences regarding which pH most likely goes with which salt.

Water has a pH of 7, which is considered neutral. Solutions with a pH greater than 7 are basic, while solutions with a pH less than 7 are acidic.

Given that Na3X has a pH of 8.5, it is likely that X is a weak base, resulting in a basic solution.

Since Na2Y has a pH of 7.0, it can be assumed that Y is neutral or a spectator ion, which does not affect the pH of the solution.

Finally, NaZ has a pH of 10.5, indicating that Z is a strong base, resulting in a highly basic solution.

Therefore, the most likely pairing is Na3X with Z, Na2Y with Y, and NaZ with X.

C) To determine the approximate pH of a 0.010 M solution of HZL, we need to consider the ionization of HZL. Assuming HZL is a weak acid, it will undergo partial ionization in water:

HZL (aq) + H2O (l) ⇌ H3O+ (aq) + ZL- (aq)

Since the concentration of HZL is low (0.010 M), it can be assumed that the ionization is incomplete. Therefore, the concentration of H3O+ ions will be low, resulting in a slightly acidic pH. The exact pH value will depend on the specific acid dissociation constant (Ka) of HZL.

D) To calculate the acid dissociation constants (Ka) for HX-2, HY-, and HZ, we need more information such as the concentrations of the acids and the corresponding conjugate bases. Unfortunately, this information is not provided in the question. Without the concentrations, it is not possible to calculate the Ka values. However, we can rank the acids in terms of strength by comparing the pH values provided.

Based on the given pH values, the salt with the highest pH (10.5) is likely the strongest base, meaning the corresponding acid (HZ) is the weakest acid. Therefore, the ranking from weakest to strongest acid would be: HZ, HY-, HX-2.

A) Anions can act as bases in aqueous solution because they can accept protons (H+) from water molecules. This can happen when the anion has lone pairs of electrons that can readily accept a proton. The chemical equation for this process can be represented as:

A- + H2O <=> HA + OH-

Here, A- is the anion acting as a base, H2O is water, HA is the corresponding acid formed, and OH- is the hydroxide ion.

B) To determine which pH most likely goes with each salt, we can analyze the pH values given.

Since a higher pH value indicates a more alkaline or basic solution, the salt with a pH of 10.5 is most likely NaZ. This is because Z- is likely to be the anion that reacts with water to produce OH- ions, resulting in a higher concentration of hydroxide ions, therefore increasing the pH.

Similarly, the salt with a pH of 7.0 is likely NaY. This suggests that Y- is the anion that has a weaker tendency to interact with water compared to Z-. Hence, it would result in a lower concentration of hydroxide ions, leading to a lower pH.

The remaining salt, NaX, must have a pH of 8.5. This indicates that X- has an intermediate tendency to act as a base compared to Y- and Z-. Hence, it will result in a slightly higher concentration of hydroxide ions and a higher pH compared to NaY.

C) To estimate the pH of a 0.010 M solution of HZL, we need to consider how the HZ molecule will interact with water. Assuming HZ fully dissociates into H+ and ZL-, we can write the chemical equation:

HZL -> H+ + ZL-

Since H+ is an acid and ZL- is the corresponding conjugate base, H+ can react with water to form hydronium ions (H3O+). This results in a decrease in pH. Therefore, the pH of the solution will be lower than that of a pH-neutral solution (pH 7). However, without further information about the strength of HZ as an acid, we cannot determine its exact pH value.

D) To rank the acid dissociation constants (Ka) for HX-2, HY-, and HZ, we need to consider their relative strengths. The acid strength is determined by the tendency to donate protons (H+). A higher Ka value indicates a stronger acid.

However, since we do not have the Ka values directly, we can make some assumptions based on their pH values:

- The salt with a pH of 7.0 is likely to have a weaker acid (higher pH). Therefore, HY- is the weakest acid among the three, with the lowest Ka value.
- The salt with a pH of 8.5 is slightly more acidic than the pH-neutral solution. Thus, HX-2 can be considered as having intermediate acid strength.
- The salt with a pH of 10.5 corresponds to the strongest acid among the three, HZ. Consequently, HZ must have the highest Ka value.

Therefore, ranking the acids in order of increasing strength (weakest first) would be HY- < HX-2 < HZ.