So we prepared 100mL of .1M solutions of these solutions, and found the pH and H+ contents:

pH H+
HCl: .57 .270
HNO3: .58 .260
H2SO4: 1.29 .051
HC2H3O2: 2.44 .0036
H2C2O4: .84 .145
HKC6H4(CO2)2: 4.13 7.41

Now I'm stuck on this question. What conclusions can be drawn from this data? (Hnt: Write a chemical equation expressing the reaction that occurs when the acids are dissolved in water. COnsidering that all the solutions were about .1M what would the expected pH be for each solution? Which solutions attained this value and which didn't? What might be the reason for some solutions not attaining this value?)

Please help!

To draw conclusions from the given data, we need to analyze the pH and H+ contents of each acid solution and compare them to the expected values.

First, let's write the chemical equation expressing the reaction that occurs when the acids are dissolved in water:

HCl + H2O -> Cl- + H3O+
HNO3 + H2O -> NO3- + H3O+
H2SO4 + 2H2O -> 2H+ + SO4^2-

Next, let's consider that all the solutions were approximately 0.1M in concentration. In a solution of a strong acid, where complete ionization occurs, the concentration of H+ (H3O+) will be equal to the concentration of the acid. So, for the HCl and HNO3 solutions, the expected H+ concentration would be 0.1M.

Now let's determine the expected pH for each solution. The pH is defined as the negative logarithm (base 10) of the H+ concentration. So, for a 0.1M H+ concentration, the pH is:

pH = -log[H+]
pH = -log[0.1]
pH ≈ 1

Based on this, we would expect the pH of the HCl and HNO3 solutions to be around 1.

Now let's compare the expected pH with the measured pH values from the data:

HCl: Expected pH ≈ 1 Measured pH = 0.57
HNO3: Expected pH ≈ 1 Measured pH = 0.58
H2SO4: Expected pH ≈ 1 Measured pH = 1.29
HC2H3O2: Expected pH > 1 Measured pH = 2.44
H2C2O4: Expected pH > 1 Measured pH = 0.84
HKC6H4(CO2)2: Expected pH > 1 Measured pH = 4.13

From the data, we can see that HCl, HNO3, and H2SO4 have pH values close to the expected pH of 1 for a 0.1M H+ concentration. However, HC2H3O2, H2C2O4, and HKC6H4(CO2)2 have higher pH values than expected.

The reason for some solutions not attaining the expected pH value could be related to the acid's strength and the ability to fully ionize in water. HCl, HNO3, and H2SO4 are strong acids and completely dissociate in water, resulting in a higher concentration of H+ and a lower pH. On the other hand, HC2H3O2, H2C2O4, and HKC6H4(CO2)2 are weaker acids and do not fully dissociate in water, resulting in a lower concentration of H+ and a higher pH.

Therefore, the data suggests that HCl, HNO3, and H2SO4 are strong acids, while HC2H3O2, H2C2O4, and HKC6H4(CO2)2 are weak acids or partially dissociate in water.

From the given data, we can draw the following conclusions:

1. Chemical equation for the reaction when acids are dissolved in water:
HX + H2O ↔ H3O+ + X-, where HX represents the acid.

2. Considering that all the solutions were about 0.1 M in concentration, the expected pH for each solution would be as follows:

- HCl: Strong acid, so it should completely dissociate in water, resulting in a high concentration of H3O+. Therefore, the expected pH should be low (acidic).
- HNO3: Strong acid, similar to HCl, so the expected pH should also be low.
- H2SO4: Sulfuric acid is a strong acid and should fully dissociate, resulting in a high concentration of H3O+. The expected pH should be low.
- HC2H3O2: Acetic acid is a weak acid and does not dissociate completely. The expected pH should be slightly acidic, but higher than the previous strong acids.
- H2C2O4: Oxalic acid is a weak acid and will not dissociate completely. The expected pH should be acidic, but higher than the strong acids.
- HKC6H4(CO2)2: This is the potassium salt of benzoic acid, which is not an acid itself. Therefore, it will not release H+ ions and will not contribute to the acidity of the solution. The expected pH would be neutral or close to neutral.

3. Comparing the expected pH values with the given pH values, we can see that:
- HCl, HNO3, H2SO4, and HKC6H4(CO2)2 have pH values in line with the expected pH for their acidic or neutral nature.
- HC2H3O2 and H2C2O4 have pH values that are higher than the expected pH for their weak acidic nature.

4. The reason for HC2H3O2 and H2C2O4 not attaining the expected pH value could be due to their weak acidic nature. Weak acids do not completely dissociate in water, resulting in a lower concentration of H3O+ ions compared to strong acids. This leads to a higher pH value than expected for weak acids.

In summary, the data shows that strong acids such as HCl, HNO3, H2SO4, and the neutral salt HKC6H4(CO2)2 have pH values in line with their expected acidic or neutral nature. However, weak acids like HC2H3O2 and H2C2O4 have higher pH values than expected due to their incomplete dissociation in water.