2. Consider the following substances: HC4H2O2, C5HsN, NaCIO3, C6H5COOH, C3HgN. For each compound
a. Decide whether the compound behaves as an acid or base in solution
b. Write the equation for the dissociation of the compound in water
c. Write the equilibrium equation for the dissociation in water
3. The compound CsOH is highly reactive and powerful enough to corrode through glass. Determine the [H*], the [OH`], the pH and the poh for a solution of CsOH prepared by adding 0.42 grams of this compound to 250 ml of solution.
4. Calculate the [H*], the [OH`], the pH and the pOH for a solution prepared by diluting 20.0 ml of 0.075 M HCIO4 to a new volume of 50 ml in a volumetric flask.
5. Phenylpropionic acid, (C9H10O2) also known as hydrocinnamic acid, is a white, crystalline solid with a sweet, floral scent at room temperature. It has a wide variety of uses including cosmetics, food additives, and pharmaceuticals. Determine the [H*], the [OH`], the pH and the poh for a solution prepared by adding 0.82 grams of this compound to 150 ml of solution if the Ka of this acid is 2.3 x 10âˆ’âµ
6. Pyridine,C5H is a flammable, colorless liquid with a disagreeable odor and it is a good solvent for many organic substances. It was formerly used in the treatment of asthma, but it can cause depression of the central nervous system as well as irritation to the skin and respiratory tract. If a 0.65 M solution of this substance has a pH of 9.67, determine the value of the equilibrium constant for this substance.
7. Butanoic acid, also called butyric acid, is an oily liquid with an unpleasant, rancid odor. It is present in butter as an ester to the extent of 4-5%. If a solution of 0.59M butanoic acid, (HC4H7O2) is found to be 3.1% ionized, determine the pH of the solution and the pKa for this acid.
8. All parts of the hemlock plant contain the alkaloid coniine. Coniine (CgH17N) is an alkaline liquid with a pKb of 3.1, and a density of 0.844 g/ml. Ingestion of this substance may cause weakness, drowsiness, nausea, vomiting, labored respiration, paralysis and death. Explain how you would prepare a 500 ml solution of coniine that has a pH of 12.0.
9. Calculate the pH of a buffer system made by dissolving 3.4 grams of sodium nitrite (NaNO2 ) in 100 ml of solution and mixing that with 100 ml of a 0.25 M HNO2 solution if the Ka of nitrous acid is 3.98 x 10-â´

10. Salicylic acid occurs in the forms of esters in several plants, notably in wintergreen leaves and the bark of sweet birch. It is used in the manufacture of aspirin and in a number of medications related to the skin. Its sodium salt is used as an anti-inflammatory and as an analgesic and antipyretic.
a. What is the ratio of sodium salicylate, C7H5NaO3, to salicyclic acid, C7H6O3, in a buffer solution that has a pH of 3.2 if the Ka of salicylic acid is 1.05 x 10âˆ’Â³.
b. IF both substances are solids at room temperature, explain how you would prepare exactly 1 liter of this buffer solution.
11. What is the pH of a buffer system that is prepared with 0.025 moles of lactic acid and 0.050 moles of sodium lactate in 500 ml of solution, if the Ka for lactic acid is 1.38 X 104? What is the new pH of this buffer if exactly 10 ml of 0.01 M HCI is added to the system?
12. A 0.092 M solution of the potassium salt of a weak acid has a pH of 8.72. Determine the hydrolysis constant for the potassium salt and then find the Ka for weak acid from this data.
13. Sodium propionate is used as a food preservative and also as a fungicide and mold inhibitor. Determine the pH for a solution prepared by adding of 0.38 g of sodium propionate, C3H5NaO2, to 100 ml of solution, if the pKa of propionic acid is 4.85
14. Exactly 20.00 ml of 0.085 M HCIO4 solution is placed in a flask and titrated with 0.050M NaOH. Determine the pH after addition of the following amounts of the NaOH solution.
a. ) 0.00 ml NaOH
b.) 5.00 ml NaOH
c.) 15.00 ml NaOH
d.) 20.00 ml NaOH
e.) 28.00 ml NaOH
f.) 32.00 ml NaOH
g.) 33.80 ml NaOH
h.) 34.00 ml NaOH
i.) 34.20 ml NaOH
j.) 38.00 ml NaOH
k.) 40.00 ml NaOH
I.) 50.00 ml NaOH
15. Exactly 20.00 ml of 0.085 M butyric acid solution which has a pKa of 4.83, is placed in a flask and titrated with standardized 0.050 M NaOH. Determine the pH after addition of the following amounts of the NaOH :
a. ) 0.00 ml NaOH
b.) 5.00 ml NaOH
c.) 15.00 ml NaOH
d.) 20.00 ml NaOH
e.) 28.00 ml NaOH
f.) 32.00 ml NaOH
g.) 33.80 ml NaOH
h.) 34.00 ml NaOH
i.) 34.20 ml NaOH
j.) 38.00 ml NaOH
k.) 40.00 ml NaOH
I.) 50.00 ml NaOH

2. Consider the following substances: HC4H2O2, C5HsN, NaCIO3, C6H5C...