Draw the general titration curve for a strong acid titrated with a strong base. At the various points in the titration, list the major species present before any reaction takes place and the major species present after any reaction takes place. What reaction takes place in a strong acid– strong base titration? How do you calculate the pH at the various points along the curve? What is the pH at the equivalence point for a strong acid– strong base titration? Why? Answer the same questions for a strong base– strong acid titration. Compare and contrast a strong acid– strong base titration with a strong base– strong acid titration.
Answer to relevant QuestionsConsider the following four titrations: i. 100.0 mL of 0.10 M HCl titrated with 0.10 M NaOH ii. 100.0 mL of 0.10 M NaOH titrated with 0.10 M HCl iii. 100.0 mL of 0.10 M CH3NH2 titrated with 0.10 M HCl iv. 100.0 mL of 0.10 M ...Repeat the procedure in Exercise 65 for the titration of 25.0 mL of 0.100 M pyridine (Kb = 1.7 × 10–9) with 0.100 M hydrochloric acid. Do not do the points at 24.9 mL and 25.1 mL. Which of the indicators in Fig could be used for doing the titrations in Exercises 62 and 64? Fig Calculate the solubility of each of the following compounds in moles per liter and grams per liter. (Ignore any acid–base properties.) a. Ag3PO4, Ksp = 1.8 × 10-18 b. CaCO3, Ksp = 8.7 × 10-9 Explain the following phenomenon:
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