<p>Chemistry II- Acid Base Titrations</p><p>1. A 15.5 mL sample of 0.215 M KOH solution required 21.2 mL of aqueous acetic acid solution in a titration experiment. Calculate the molarity of the acetic acid solution (0.157M)</p><p>2. By titration, 17.6 mL of aqueous H2SO4 just neutralized 27.4 mL of 0.0165 M LiOH solution. What was the molarity of the aqueous acid solution (0.0128 M)</p><p>3. For each of the following acid-base titration combinations, determine the number of moles of the first substance listed that would be required to react with given quantity of the second: a. NaOH with 1.0 mole HCl b. HNO3 with 0.75 mole KOH c. Ba(OH)2 with 0.20 mole HF d. H2SO4 with 0.60 mole Al(OH)3</p><p>4. If 15.0 mL of 0.0250 M aqueous H2SO4 is required to neutralize 10.0 mL of an aqueous solution of KOH, what is the molarity of the KOH solution? (0.0750 M)</p><p>5. In a titration experiment, a 12.5 mL sample of 0.0175 M Ba(OH)2 just neutralized 14.5 mL of HNO3 solution. Calculate the molarity of the HNO3. (0.0302 M)</p><p>6. If 13.4 mL of 0.0230 M H3PO4 is required to neutralize 22.5 mL of Ba(OH)2 in a titration experiment, determine the molarity of the Ba(OH)2 solution. (0.0205 M)</p><p>7. How many milliliters of 0.250 M H3PO4 solution would be required to neutralize 40.0 mL of 0.280 M Ba(OH)2? (29.9 mL)</p><p>8. What is the molarity of 3.50 L of solution that contains 90.0 g of sodium chloride? (0.440 M)</p><p>9. What volume of 0.196 M LiOH is required to neutralize 27.3 cm3 of 0.413 M HBr? (57.5 cm3)</p><p>10. How many milliliters of 0.54 M AgNO3 would contain 0.34 g of pure AgNO3? (3.7 mL)</p><p>11. What is the concentration of a solution of NaOH if 21.2 cm3 of a 0.0800 M solution of HCl is needed to neutralize 30.0 cm3 of the base? (0.0565 M)</p><p>12. How many cm3 of 0.0200 M KOH will exactly neutralize 15.0 cm3 of 0.400 M 3 H2SO4? (600 cm )</p>