What is an acid–base indicator? Define the equivalence (stoichiometric) point and the endpoint of a titration. Why should you choose an indicator so that the two points coincide? Do the pH values of the two points have to be within 60.01 pH unit of each other? Explain. Why does an indicator change from its acid color to its base color over a range of pH values? In general, when do color changes start to occur for indicators? Can the indicator thymol blue contain only a single — CO2H group and no other acidic or basic functional group? Explain.
Answer to relevant QuestionsTwo drops of indicator HIn (Ka = 1.0 × 10–9), where HIn is yellow and In- is blue, are placed in 100.0 mL of 0.10 M HCl. Which of the indicators in Fig. could be used for doing the titrations in Exercises 66 and 68? Fig Calculate the solubility of each of the following com-pounds in moles per liter. Ignore any acid– base properties. a. PbI2, Ksp = 1.4 × 10–8 b. CdCO3, Ksp = 5.2 × 10–12 c. Sr3(PO4)2, Ksp = 1 × 10-31 Explain the following phenomenon: a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 × 10-16. b. Calculate the molar solubility of AgI in 3.0 M NH3. The overall formation constant for Ag(NH3)2+ is 1.7 × 107. c. Compare the ...
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