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Chapter 12: Q29P (page 285)
Give an example of the use of a masking agent
The Mg2+ in a solution of Mg2+ and Fe3+ must be titrated by EDTA. If the Fe3+ is masked with to form which does not react with EDTA.
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A 50.0-mL sample containing Ni2+ was treated with 25.0 mL of 0.050 0 M EDTA to complex all the Ni2+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 5.00 mL of 0.050 0 M Zn2+. What was the concentration of Ni2+ in the original solution?
What is meant by water hardness? Explain the difference between temporary and permanent hardness.
According to Appendix I, Cu2+ forms two complexes with acetate:
(a) Referring to Box 6-2, find K2 for the reaction
(b) Consider 1.00 L of solution prepared by mixing 1.00 脳 10-4 mol Cu(ClO4)2 and 0.100 mol CH3CO2Na. Use Equation 12-16 to find the fraction of copper in the form Cu2+
Cyanide solution (12.73 mL) was treated with 25.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyano nickelate (II):
Excess Ni2+ was then titrated with 10.15 mL of 0.01307 M EDTA. does not react with EDTA. If 39.35 mL of EDTA were required to react with 30.10 mL of the original Ni2+ solution, calculate the molarity of CN- in the 12.73-mL sample.
A 1.000-mL sample of unknown containing Co2+ and Ni2+ was treated with 25.00 mL of 0.038 72 M EDTA. Back titration with 0.021 27 M Zn2+ at pH 5 required 23.54 mL to reach the xylenol orange end point. A 2.000-mL sample of unknown was passed through an ion-exchange column that retards Co2+ more than Ni2+. The Ni2+ that passed through the column was treated with 25.00 mL of 0.038 72 M EDTA and required 25.63 mL of 0.021 27 M Zn2+ for back titration. The Co2+ emerged from the column later. It, too, was treated with 25.00 mL of 0.038 72 M EDTA. How many milliliters of 0.021 27 M Zn2+ will be required for back titration?
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