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Chapter 16: Q22P (page 392)

Why is iodine almost always used in a solution containing excess l-?

Short Answer

Expert verified

Iodine is always used in a solution with excess l- because purel2 is not a polar substance and it cannot be dissolved in water.

Step by step solution

01

Properties of Iodine.

  • Iodine is a chemical element with atomic number 53 and the symbol l .
  • At typical conditions, it exists as a semi-lustrous, non-metallic solid that melts to produce a deep violet liquid at 114掳C and boils to form a violet gas at 184掳C
  • Iodine is found in a variety of oxidation states, including iodideI- , iodate IO3-, and periodate anions.
  • It is the heaviest nutrient in terms of necessary minerals.
02

To determine the iodine always used in solution containing  

  • lodine is always used in a solution with excessI-because pureI2is not a polar substance and it cannot be dissolved in water.
  • Because of that, iodide solution(for example, Kl) must be added to iodine to increase its solubility,
  • The following reactions occurs:
  • I2(s)+I-(aq)鈬�I3-(aq)
  • In this reaction triodide is formed by a complexation reaction between iodide and iodine and the solubility of I2 is increased.

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Most popular questions from this chapter

A titration of 50.0 mLof unknown Fe2+with 0.100MCeat 25掳C , monitored with Pt and calomel electrodes, gave data in the table. Prepare a Gran plot and decide which data lie on a straight line. Find the x-intercept of this line, which is the equivalence volume. Calculate the molarity of Fe2+in the unknown.

Write balanced reactions for the destruction ofS2O82鈥�,Ag3+andH2O2,by boiling.

Consider the titration of 25.0mLof 0.100M Sn2+ by 0.0500 MT3+in 1MHCI, using Pt and saturated calomel electrodes to find the end point.

(a) Write a balanced titration reaction.

(b) Write two different half-reactions for the indicator electrode.

(c) Write two different Nernst equations for the cell voltage.

(d) Calculate E at the following volumes ofTl3+:1.00,2.50,4.90,5.00,5.10and 10.0 mL. Sketch the titration curve.

Ascorbic acid (0.0100M)was added to 10.0mL of 0.0200MFe3+at pH 0.30, and the potential was monitored with Pt and saturated Ag | AgClelectrodes.

Dehydroascorbic acidrole="math" localid="1664865837362" +2H++2e-鈫�ascorbicacid+H2OE掳=0.390V

(a) Write a balanced equation for the titration reaction,

(b) Using E0=0.767V for the role="math" localid="1664865912877" Fe3+鈭�Fe2+ couple, calculate the cell voltage when 5.0,10.0 and 15.0 mL of ascorbic acid have been added. (Hint: Refer to the calculations in Demonstration 16 - 1.)

Why don'tCr3+and TiO2+interfere in the analysis of Fe3+when a Walden reductor, instead of a Jones reductor, is used for pre-reduction?
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