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To obeserve the effect of concentration ...

To obeserve the effect of concentration on the conductivity, electrolytes of different natures are taken in two vessels `A` and `B,` A contains weak electrolyte, `e.g., NH_(4)OH` and `B` contains strong electrolyte, `e.g., NaCl`. In both containers, the concentration of respective electrolyte is increased and the conductivity observed`:`

A

in `'A'` conductivity increased , in `'B'` conductivity decreases

B

in `'A'` conductivity decreases while in `'B'` conductivity increases

C

in both `'A'` and `'B'` conductivity increases

D

in both `'A'` and `'B'` conductivity decreases

Text Solution

Verified by Experts

The correct Answer is:
4
Weak electrolyte is weakly ionizing substance, dilution promotes ionization thus conductivity.
For strong electrolyte, as concentration increases interionic attraction increases and conduct on decreases.
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A solution which remains in equilibrium with undissolved solute , in contact , is said to be saturated . The concentration of a saturated solution at a given temperature is a called solubility . The product of concentration of ions in a saturated solution of an electrolyte at a given temperature is called solubility product (K_(sp)) . For the electrolyte A_(x),B_(y) with solubility S. The solubility product (K_(sp)) is given as K_(sp) = x^(x) xx y^(y) xx S^(x-y) . While calculating the solubility of a sparingly . soluable salt in the presence of some strong electrolyte containing a common ion , the common ion concentration is practically equal to that of strong electrolyte containing a common ion . the common ion soncentration is practically equal to that of strong electrolyte . If in a solution , the ionic product of an electroylte exceeds its K_(sp) value at a particular temperature , then precipitation occurs . If two or more electrolyte are presentt in the solution , then by the addition of some suitable reagent , precipitation generally occurs in increasing order of their k_(sp) values . Solubility of some sparingly soluable salts , is sometimes enhanced through complexation . While we are calculating the solubility of some sparingly or pH of an electrolyte , the nature of cation of anion should be checked carefully whether there ion (s) are capable of undergoing hydrolysis or not . If either or both of the ions are capable of undergoing hydrolysis , it should be taken into account in calculating the solubility . While calculating the pH of an amphiprotic species , it should be checked whether or not cation can undergo hydrolysis . Total a_(H^(-)) = sqrt(K_(a_(1)xxK_(a_(2)))) (if cation do not undergo hydrolysis ) a_(H^(+)) = sqrt(K_(a_(1))((K_(w))/(K_(b)) - K_(a_(2)))) (if cation also undergoes hydrolysis ) where symbols have usual meaning . Solubility of solids into liquids is a function of temperature alone but solubility of gases into liquids is a function of temperature as well as pressure . The effect of pressure on solubility of gases into liquids is governed by Henry's law . The solubility of PbSO_(4) in water is 0.0303 g/l at 25^(@)C , its solubility product at that temperature is

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