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In this lesson, we will learn how to describe iodometry, iodimetry, and other redox titration methods and troubleshoot common errors.
Which of the following would not improve the accuracy of an iodometric titration?
A 0.357 g sample contains only lead(II) iodide and sodium iodide in 100 mL of
distilled water. Titration to the Fajan’s end point requires 22.37 mL of 0.050 M
silver nitrate. What is the mass percent (w/w
) of lead(II) iodide in the sample?
Which of the following is an accurate description of iodometry?
and potassium permanganate
react according to the net ionic equation:
Titration of a 20.0 mL aqueous solution of oxalic acid required 23.24 mL of 0.09113 M
aqueous potassium permanganate. Calculate to 3 significant figures the concentration of the oxalic acid solution.
A 58.3 mg
is dissolved in 1.0 M
. If 23.6 mL
of 0.010 M
is required to reach the end-point of the titration, what is the mass percent (w/w%) of tin in the original sample?
Adding aqueous sodium chloride to aqueous silver
nitrate results in the precipitation of silver
Calculate the concentration of silver
nitrate in a 23.00 mL aqueous sample if 32.10 mL of 0.203 M aqueous sodium chloride is required for the end point to be reached.
Copper(II) nitrate reacts with potassium iodide in water to produce solid copper(I) iodide and elemental iodine:
A copper(II) nitrate solution has a volume of 43.88 mL and concentration of 0.3842 M. Calculate the volume of a 0.2089 M potassium
iodide solution needed to convert all of the copper(II) nitrate to copper(I) iodide.
Triiodide ions are produced by the reaction of iodine with iodide ions. Why should iodine solutions contain an additional iodide salt if used as a titrant?
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