Conductance of Electrolytic Solution

Q. Consider a sparingly soluble salt $AB$ having solubility as $smol{L}^{-1}$. What will be the value of $K_{sp}$ for $AB$ salt.

1. $smol{L}^{-1}$
2. $\sqrt[3]{3s}(mol{L}^{-1}{)}^{\frac{1}{3}}$
3. $\sqrt{s}(mol{L}^{-1}{)}^{0.5}$
4. $s^2(mol{L}^{-1}{)}^2$

Q. The solubility in water of a sparingly soluble salt $PbB{r}_2$ is $6.6\times {10}^{-6}$ mol $L^{-1}$. What is the concentration of $B{r}^{-}\left(aq\right)$ in a saturated solution of $PbB{r}_2\left(s\right)$?
$(1.65{)}^{\frac{1}{3}}=1.18$

1. $4\times {10}^{-10}$
2. $2.36\times {10}^{-2}$
3. $1.18\times {10}^{-2}$
4. $4\times {10}^{-15}$

Q. The molar conductance of a solution of a weak electrolyte with dilution.

1. increases
   
2. decreases
3. remains constant

Q.

The conductivity of strong electrolyte is

[CPMT 2003]

1. Increases on dilution slightly

2. Decreases on dilution

3. Does not change with dilution

4. Depends upon density of electrolytes itself

Q. $kg{m}^2{s}^{-3}{A}^{-2}$ is the SI unit of resistance

1. True
2. False

Q. An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these reactions is given in List II. Match List I with List II and select the correct option using the code given below the lists:
$\begin{array}{cc}\text{List I}& \text{List II}\\ \left(A\right)(C_2{H}_5{)}_{3}N+C{H}_{3}COOH& \text{(P) Initially conductivity decreases and then increases}\\ XY& \\ \left(B\right)KI\left(0.1M\right)+AgN{O}_3\left(0.01M\right)& \text{(Q) Initially conductivity decreases and then does not change much}\\ XY& \\ \left(C\right)C{H}_{3}COOH+KOH& \text{(R) Initially conductivity increases and then does not change much}\\ XY& \\ \left(D\right)NaOH+HI& \text{(S) Initially conductivity does not change much and then increases}\\ XY& \end{array}$
Which of the following is the only correct combination?

1. A-R; B-S; C-Q; D-P
2. A-S; B-R; C-Q; D-P
3. A-Q; B-R; C-S; D-P
4. A-P; B-S; C-R; D-Q

Q. In which of the following, dissociation of $N{H}_{4}OH$ will be minimised

1. $H_{2}O$
2. $NaOH$
3. $NaCl$
4. $N{H}_{4}Cl$

Q. The specific conductance of a saturated solution of $AgCl$ at ${25}^{\circ }C$ is $3.55\times {10}^{-6}{\Omega }^{-1}c{m}^{-1}$ and that of water used for preparing the solution is $1.60\times {10}^{-6}{\Omega }^{-1}c{m}^{-1}$. What is the solubility product of AgCl?
$\left({\Lambda }^{\infty }\right(AgCl)=150.0{\Omega }^{-1}c{m}^2{\text{eqv}}^{-1})$

1. $2.37\times {10}^{-5}$
2. $5.60\times {10}^{-10}$
3. $1.3\times {10}^{-5}$
4. $1.69\times {10}^{-10}$

Q. The conductivity of molten $L{i}^{+}$ salt is (than or to) the molten salt of $C{s}^{+}$.

1. greater
2. lesser
3. equal

Q. As the temperature increases, the current passed through the metal conductor but the current passed through the ionic solution .

1. increases
2. decreases
3. remains constant
4. becomes zero

Q.

The conductivity of strong electrolyte is

[CPMT 2003]

1. Increases on dilution slightly

2. Decreases on dilution

3. Does not change with dilution

4. Depends upon density of electrolytes itself

Q. It has been observed that gaseous hydrogen chloride is a very poor conductor of electricity but a solution of hydrogen chloride gas in water is a good conductor of electricity. This is due to the fact that

1. water is good conductor of electricity
2. hydrogen chloride gas dissociates in water
3. a gas is an electrolnic conductor but a liquid is always an electrolytic conductor
4. a gas does not obey Ohm's law whereas a solution does

Q. Which of the following statement is correct for a weak electrolytic solution?
${\Lambda }_m$ - Molar conductivity
${\Lambda }_m^0$ - Limiting molar conductivity
$C$ - concentration of electrolyte

Q. An aqueous solution of X is added slowly to an aqueous solution of Y as shown in List I. The variation in conductivity of these reactions is given in List II. Match List I with List II and select the correct option using the code given below the lists:
$\begin{array}{cc}\text{List I}& \text{List II}\\ \left(A\right)(C_2{H}_5{)}_{3}N+C{H}_{3}COOH& \text{(P) Initially conductivity decreases and then increases}\\ XY& \\ \left(B\right)KI\left(0.1M\right)+AgN{O}_3\left(0.01M\right)& \text{(Q) Initially conductivity decreases and then does not change much}\\ XY& \\ \left(C\right)C{H}_{3}COOH+KOH& \text{(R) Initially conductivity increases and then does not change much}\\ XY& \\ \left(D\right)NaOH+HI& \text{(S) Initially conductivity does not change much and then increases}\\ XY& \end{array}$
Which of the following is the only correct combination?

1. A-R; B-S; C-Q; D-P
2. A-S; B-R; C-Q; D-P
3. A-Q; B-R; C-S; D-P
4. A-P; B-S; C-R; D-Q

Q. During the electrolysis of an electrolyte, the number of ions produced is dependent on

1. Temperature
2. Nature of solvent
3. Nature of the electrolyte
4. All of the above

Q. Which of the following is/are true about an electrolyte solution at infinite dilution?

${\Lambda }_m$ is molar conductivity
${\Lambda }_m^0$ is limiting molar conductivity

1. All interionic effects of electrolyte disappears
2. All of the above.
3. $\text{Degree of dissociation of weak electrolyte,}\alpha =1$
4. ${\Lambda }_m^0$ of an electrolyte is the sum of the individual contributions of cation and anion of the electrolyte.