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.
Answer to relevant QuestionsCalculate the pH at the halfway point and at the equiva-lence point for each of the following titrations. a. 100.0 mL of 0.10 M HC7H5O2 (Ka = 6.4 × 10–5) titrated with 0.10 M NaOH b. 100.0 mL of 0.10 M C2H5NH2 (Kb = 5.6 ...Which of the indicators in Fig. could be used for doing the titrations in Exercises 61 and 63? Fig For which of the following is the Ksp value of the ionic compound the largest? The smallest? Explain your answer. Calculate the solubility (in mol/ L) of Fe(OH) × (Ksp = 4 × 10-38) in each of the following. a. water (assume pH is 7.0 and constant) Kf for the complex ion Ag(NH3)2+ is 1.7 × 107. Ksp for AgCl is 1.6 × 10-10. Calculate the molar solubility of AgCl in 1.0 M NH3.
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