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Chapter 4: Q4.12P (page 178)

Question:State whether an aqueous solution of each of the following substances conducts an electric current. Explain your reasoning.

(a) Caesium bromide (b) Hydrogen iodide

Short Answer

Expert verified

Answer

a) Yes, an aqueous solution of Caesium bromide conducts electric current.

b) Yes, an aqueous solution of Hydrogen iodide conducts electric current.

Step by step solution

01

Explain the solubility of ionic compounds in water

All the ionic compounds which dissociate into ions on dissolving in water conduct electricity because they contain charge and are free to move in the solution.

02

Determine the aqueous solution of given compounds conduct electricity or not

An aqueous solution of both the given compounds i.e.,

(a) Caesium bromide and (b) Hydrogen iodide can conduct electricity

Because both produce free moving charged ions on dissolving in water and conduct electric current.

In the case of Caesium bromide, it dissociates into CS+and Br-ions and conducts electricity.

In the case of Hydrogen iodide, it is a strong acid and dissociates completely in the water into H+and I_ ions through which it conducts electricity.

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Most popular questions from this chapter

A mixture of CaCO3 and CaO weighing 0.693 g was heated to produce gaseous CO2. After heating, the remaining solid weighed 0.508g. Assuming all the CaCO3 broke down to CaO and CO2, calculate the mass percent of CaCO3 in the original mixture.

In a titration of HNO3, you add a few drops of phenolphthalein indicator to 50.00 mL of acid in a flask. You quickly add 20.00 mL of 0.0502 MNaOH but overshoot the end point, and the solution turns deep pink. Instead of starting over, you add 30.00 mL of the acid, and the solution turns colorless. Then, it takes 3.22 mL of the NaOH to reach the end point. (a) What is the concentration of the HNO3solution? (b) How many moles of NaOH were in excess after the first addition?

Identify the oxidizing and reducing agents in the following:

a8H+aq+Cr2O72-aq+3SO32-aq→2Cr3+aq+3SO42-aq+4H2OlbNO3-aq+4Zns+7OH-aq+6H2Ol→4ZnOH42-aq+NH3aq

Thyroxine (C15H11I4NO4) is a hormone synthesized by the thyroid gland and used to control many metabolic functions in the body. A physiologist determines the mass percent of thyroxine in a thyroid extract by igniting 0.4332 g of extract with sodium carbonate, which converts the iodine to iodide. The iodide is dissolved in water, and bromine and hydrochloric acid are added, which convert the iodide to iodate.

(a) How many moles of iodate form per mole of thyroxine?

(b) Excess bromine is boiled off and more iodide is added, which reacts as shown in the following unbalancedequation:

IO3-(aq)+H+(aq)+I-(aq)→I2(aq)+H2O(I)

How many moles of iodine are produced per mole of thyroxine?

(Hint:Be sure to balance the charges as well as the atoms.) What are the oxidizing and reducing agents in the reaction?

(c) The iodine reacts completely with 17.23 mL of 0.1000 Mthiosulfate as shown in the following unbalancedequation:

I2(aq)+S2O32-(aq)→I-(aq)+S4O62-(aq)

What is the mass percent of thyroxine in the thyroid extract?

Do either of the following reactions go to completion? If so, what factor(s) cause(s) each to do so?

  1. MgSO3s+2HCIaq→MgCI2aq+SO2g+H2O
  2. 3BaOH2aq+2H3PO4aq→Ba3PO42s+6H2OI
See all solutions

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