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Chapter 21: Q21.145 CP (page 979)

Use Appendix D to calculate theKspof AgCl.

Short Answer

Expert verified

The value is obtained as: Ksp=1.90×10- 4

Step by step solution

01

Define chemical reaction

Chemical synthesis or, alternatively, chemical breakdown into two or more separate chemicals occurs when one component interacts with another to generate new material. These processes are known as chemical reactions, and they are generally irreversible until followed by other chemical reactions.

02

Evaluate the value of  Ksp

Silver is oxidized during the production of AgCl.

Reaction: Ag(s)+ Cl(aq)-→AgCl(s)+e-Ehalf - cell0= - 0.22∆Go= - nFECell0= - 1e-×96,500Cmole-×-0.22V=21,230J

∆Go= - RTlnKin Action theKspfor AgCl may be calculated as:

21,230J = - RTlnKlnK =- 21,230JRTKsp= e- 21,230RT= e- 21,230298 K×8.314Jmol K= 1.90×10- 4

Therefore, the value is:Ksp= 1.90××10- 4

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Most popular questions from this chapter

A voltaic cell is constructed with anAg/Ag+half-cell and aPb/Pb2 +half-cell. The zinc electrode is negative.

(a) Write balanced half-reactions and the overall reaction.

(b) Diagram the cell, labeling electrodes with their charges and showing the directions of electron flow in the circuit and of cation and anion flow in the salt bridge.

Consider the following voltaic cell:

(a) In which direction do electrons flow in the external circuit?

(b) In which half-cell does reduction occur?

(c) In which half-cell do electrons leave the cell?

(d) At which electrode are electrons generated?

(e) Which electrode is positively charged?

(f) Which electrode increases in mass during cell operation?

(g) Suggest a solution for the anode electrolyte.

(h) Suggest a pair of ions for the salt bridge.

(i) For which electrode could you use an inactive material?

(j) In which direction do cations within the salt bridge move to maintain charge neutrality?

(k) Write balanced half-reactions and an overall cell reaction.

How does over voltage influence the products in the electrolysis of aqueous salts?

Compare and contrast a voltaic cell and an electrolytic cell with respect to each of the following:

(a) Sign of the free energy change

(b) Nature of the half-reaction at the anode

(c) Nature of the half-reaction at the cathode

(d) Charge on the electrode labelled “anode”

(e) Electrode from which electrons leave the cell

Bubbles of H2 form when metal D is placed in hot . No reaction occurs when D is placed in a solution of a salt of metal E, but D is discoloured and coated immediately when placed in a solution of a salt of metal F. What happens if E is placed in a solution of a salt of metal ? Rank metals, E, and F in order of increasing reducing strength.
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