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Chapter 16: Problem 9

The failure of Ostwald's dilution law in case of strong electrolytes is due to (a) strong electrolytes are almost completely dissociated at all dilutions and \(\lambda_{v} / \lambda_{\infty}\) do not give accurate value of \(a\) (b) the law of mass action in its simple form cannot be applied when the concentration of the ions is very high (c) the ions get hydrolysed and affect the concentration terms (d) all of the above

Short Answer

Expert verified
(d) all of the above

Step by step solution

01

Understanding Ostwald's Dilution Law

Ostwald's dilution law describes the relationship between the degree of dissociation (α) of a weak electrolyte and the molar concentration of the electrolyte (C) in an ideally dilute solution. It's important to recognise that this law applies mainly to weak electrolytes, indicating their incomplete dissociation.
02

Analyzing Each Option

The following option analysis is done: (a) Strong electrolytes are almost completely dissociated at all dilutions, hence do not follow the Ostwald's Dilution law because it is applicable for weak electrolytes having partial dissociation.(b) The law of mass action in its simple form operates within the premise of low concentration of ions. Therefore, for high ion concentrations, the prediction of the law of mass action becomes inaccurate.(c) The hydrolysis of ions can indeed influence concentration terms, thus affecting the efficacy of Ostwald's law.
03

Final Answer Determination

With the above points, it is clear that all the options (a, b, and c) are correct reasons for the failure of Ostwald's dilution law in the context of strong electrolytes.

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Most popular questions from this chapter

Kohlrasch's law can be expressed as (a) \(\lambda_{\infty}=\lambda_{a}-\lambda_{c}\) (b) \(\lambda_{\infty}=\lambda_{c}-\lambda_{a}\) (c) \(\lambda_{\infty}=\lambda_{a}+\lambda_{c}\) (d) \(\lambda_{\infty}=\lambda_{c}+\lambda_{a}\)

The statement of Kohlrausch's law is (a) the equivalent conductance of an electrolyte at infinite dilution is equal to the product of equivalent conductance of the component ions (b) the equivalent conductance of an electrolyte at infinite dilution is equal to the difference of equivalent conductances of the component ions (c) the equivalent conductance of an electrolyte at infinite dilution is equal to the sum of the equivalent conductances of the component ions (d) none of the above

The Hittorf's rule states that (a) the loss of concentration around any electrode is proportional to the speed of the ions moving towards it (b) the loss of concentration around any electrode is proportional to the speed of the ions moving away from it (c) the loss of concentrations around both the electrodes is proportional to the sum of speed of cations and anions (d) none of the above

If \(\lambda_{\infty}\) and \(\lambda_{v}\) are the equivalent conductances at infinite dilution and at \(V\) dilution, the degree of dissociation, \(\alpha\) is given by (a) \(\alpha=\frac{\lambda_{\infty}}{\lambda_{v}}\) (b) \(\alpha=\frac{\lambda_{c 0}}{\lambda_{v}^{2}}\) (c) \(\alpha=\frac{\lambda_{v}}{\lambda_{\mathrm{cos}}}\) (d) None of these

The effect that trends to retard the mobilities of ions in solution is (a) asymmetry effect (b) relaxation effect (c) electrophoretic effect (d) all of these
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