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Calculating Ka and Kb Worksheet 1. The hydronium ion concentration of a 0.500 M solution of HF at 25°C is found to be 0.0185 M. Calculate the ionization constant. 2. At 25°C, a 0.025 M solution of formic acid, HCOOH, is found to have a hydronium ion concentration of 2.03 x 10-3 M. Calculate the ionization constant. 3. At 25°C, a 0.050 M solution of sodium hydroxide is found to have a hydroxide on concentration of 1.04 x 10-9 M. Calculate the ionization constant. 4. At 25°C, the pH of a 0.315 M solution of nitrous acid is 1.93. Calculate the Ka. 5. At 25°C, the pOH of a 0.62 M solution of ammonium hydroxide is 5.02. Calculate the Kb. 6. The pH of a 0.400 M solution of iodic acid, HIO3, is 0.726 at 25°C. What is the Ka? 7. The pH of a 1.5 M solution of calcium hydroxide is 12.5 at 25°C. What is the Kb? Calculating Ka and Kb Worksheet 1. The hydronium ion concentration of a 0.500 M solution of HF at 25°C is found to be 0.0185 M. Calculate the ionization constant. 2. At 25°C, a 0.025 M solution of formic acid, HCOOH, is found to have a hydronium ion concentration of 2.03 x 10-3 M. Calculate the ionization constant. 3. At 25°C, a 0.050 M solution of sodium hydroxide is found to have a hydroxide ion concentration of 1.04 x 10-9 M. Calculate the ionization constant. 4. At 25°C, the pH of a 0.315 M solution of nitrous acid is 1.93. Calculate the Ka. 5. At 25°C, the pOH of a 0.62 M solution of ammonium hydroxide is 5.02. Calculate the Kb. 6. The pH of a 0.400 M solution of iodic acid, HIO3, is 0.726 at 25°C. What is the Ka? 7. The pH of a 1.5 M solution of calcium hydroxide is 12.5 at 25°C. What is the Kb? Titration WS 1. A titration of 25.00mL sample of hydrochloric acid solution of unknown molarity reaches the equivalence point when 38.28mL of 0.4370M sodium hydroxide solution has been added. What is the molarity of the HCl solution? 2. A 50.00mL sample of sodium hydroxide solution is titrated with a 1.605M solution of sulfuric acid. The titration requires 24.09mL of the acid solution to reach the equivalence point. What is the molarity of the base solution? 3. A 50.00mL sample of potassium hydroxide is titrated with a 0.8186M HCl solution. The titration requires 27.87mL of HCl solution to reach the equivalence point. What is the molarity of the KOH solution? 4. A H2SO4 solution of unknown molarity is titrated with 1.209M NaOH solution. The titration requires 42.27mL of NaOH solution to reach the equivalent point with 25.00mL of H2SO4 solution. What is the molarity of the acid solution? 5. A 12.00mL sample of ammonia solution is titrated with 1.499M HNO3 solution. A total of 19.48mL of acid is required to reach the equivalence point. What is the molarity of the ammonia solution? Titration WS 1. A titration of 25.00mL sample of hydrochloric acid solution of unknown molarity reaches the equivalence point when 38.28mL of 0.4370M sodium hydroxide solution has been added. What is the molarity of the HCl solution? 2. A 50.00mL sample of sodium hydroxide solution is titrated with a 1.605M solution of sulfuric acid. The titration requires 24.09mL of the acid solution to reach the equivalence point. What is the molarity of the base solution? 3. A 50.00mL sample of potassium hydroxide is titrated with a 0.8186M HCl solution. The titration requires 27.87mL of HCl solution to reach the equivalence point. What is the molarity of the KOH solution? 4. A H2SO4 solution of unknown molarity is titrated with 1.209M NaOH solution. The titration requires 42.27mL of NaOH solution to reach the equivalent point with 25.00mL of H2SO4 solution. What is the molarity of the acid solution? 5. A 12.00mL sample of ammonia solution is titrated with 1.499M HNO3 solution. A total of 19.48mL of acid is required to reach the equivalence point. What is the molarity of the ammonia solution?

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posted: | 11/30/2011 |

language: | English |

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