Question

1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O.

2. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side of the simulation. Make sure to select the option "Concentration (mol/L)" above the graphic. Select on the Logarithmic scale below the graphic. Find the pOH of the solution.

3. A certain weak acid, HA, has a Ka value of 2.9×10⁻⁷. Calculate the percent ionization of HA in a 0.10 M solution.

4. A 0.153 M weak acid solution has a pH of 4.25. Find Ka for the acid.

5. The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10−14.

PART A: 0.50 g of hydrogen chloride (HCl) is dissolved in water to make 4.0 L  of solution. What is the pH of the resulting hydrochloric acid solution?.

PART B: 0.80 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 5.0 L of solution. What is the pH of this solution?

6. Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. What is the percent ionization of ammonia at this concentration?

7. Classify each anion as a weak base or pH neutral: HSO4-, HS-.

8. If the pH of a 1.00-in. rainfall over 1500 miles2 is 3.20, how many kilograms of sulfuric acid, H2SO4, are present, assuming that it is the only acid contributing to the pH?

For sulfuric acid, Ka1 is very large and Ka2 is 0.012.

Answer 1

Answer 2

1. Rank the solutions in order of decreasing [H3O+]: 0.10 M HF, 0.10 M HCl, 0.10 M HClO, 0.10 M HC6H5O.

To rank the solutions in order of decreasing [H3O+], we need to compare the acidity of the solutions. Acidity is determined by the concentration of hydronium ions, [H3O+].

[H3O+] is highest in the most acidic solution and lowest in the least acidic solution.

The order of decreasing [H3O+] is as follows:

1. 0.10 M HCl (Strong acid, completely ionizes in water)

2. 0.10 M HClO (Weak acid, partially ionizes in water)

3. 0.10 M HC6H5O (Weak acid, partially ionizes in water)

4. 0.10 M HF (Weak acid, partially ionizes in water)

5. The beaker will be filled to the 0.50 L mark with a neutral solution. Set the pH to 3.95 by using the green arrows adjacent to the pH value indicated on the probe in the solution. Once you adjust the pH, note the corresponding OH− ion concentration in M as given in the graphic on the left side of the simulation. Make sure to select the option "Concentration (mol/L)" above the graphic. Select on the Logarithmic scale below the graphic. Find the pOH of the solution.

Since the solution is neutral, the concentration of H3O+ ions is equal to the concentration of OH- ions.

From the information given, the OH- ion concentration can be found from the simulation. Once we have the OH- ion concentration, we can use the equation:

pOH = -log[OH-]

to calculate the pOH of the solution.

3. A certain weak acid, HA, has a Ka value of 2.9×10−7. Calculate the percent ionization of HA in a 0.10 M solution.

The percent ionization of a weak acid can be calculated using the formula:

% ionization = (concentration of ionized acid / initial concentration of acid) x 100

Given the Ka value and the initial concentration of the acid, we can determine the concentration of ionized acid using the equation for weak acid ionization.

4. A 0.153 M weak acid solution has a pH of 4.25. Find Ka for the acid.

To find Ka for the weak acid, we need to use the pH value and the concentration of the weak acid solution. By using the equation for the dissociation of a weak acid and the equilibrium expression for Ka, we can solve for Ka.

5. The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10−14.

This statement indicates that the temperature is constant and provides the value of Kw (the ion product of water). The information may be used to calculate concentrations of H+ or OH- ions in certain situations.

6. Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. What is the percent ionization of ammonia at this concentration?

To calculate the percent ionization of a weak base, we need to use the Kb value and the initial concentration of the base. The percent ionization can be determined by using the equation for weak base ionization.

7. Classify each anion as a weak base or pH neutral: HSO4-, HS-.

To classify each anion as a weak base or pH neutral, we need to analyze their behavior in water. Weak bases are capable of