Question

1. 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.

2. 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.

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

4. 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?

5. 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?

6. 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

1)

Given that the pH of the solution is 3.95.

From equation (2), calculate the value of pOH as follows:

3.95+ pOH= 14

pOH= 14-3.95 = 10.05

For a neutral solution, the sum of pH and pOH is 14. As pH is given, the pOH is calculated by subtracting the pHfrom 14.

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