Effect on Conductance in Titration

Q.

The conductometric titration curve for $C{H}_{3}COOH$ against $NaOH$ can be given as

1. 
2. 
3. 
4. 

Q. Which of the following expressions correctly represents the equivalent conductance at infinite dilution of $A{l}_2(S{O}_4{)}_3$? Given that ${\Lambda }_{A{l}^{3+}}^o$ and ${\Lambda }_{S{O}_4^{2-}}^o$ are the equivalent conductances at infinite dilution of the respective ions.

1. $2{\Lambda }_{A{l}^{3+}}^o+3{\Lambda }_{S{O}_4^{2-}}^o$
2. ${\Lambda }_{A{l}^{3+}}^o+{\Lambda }_{S{O}_4^{2-}}^o$
3. $({\Lambda }_{A{l}^{3+}}^o+{\Lambda }_{S{O}_4^{2-}}^o)\times 6$
4. $\frac{1}{3}{\Lambda }_{A{l}^{3+}}^o+\frac{1}{2}{\Lambda }_{S{O}_4^{2-}}^o$

Q. The values of ${\Lambda }_{eq}^0$ for $N{H}_{4}Cl,NaOH$ and $NaCl$ are $149.74,248.1$ and $126.4oh{m}^{-1}c{m}^{2}e{q}^{-1}$ respectively. The value of ${\Lambda }_{eq}^0\left(N{H}_{4}OH\right)$ is :

1. 371.44
2. 271.44
3. 171.44
4. Cannot be calculated from the data given

Q. Choose the correct option(s) when conductometric titration of a strong acid vs. weak base (titrant) is carried out:

1. Conductance increases up to the equivalence point.
2. Conductance decreases up to the equivalence point.
3. Beyond equivalence point , conduction starts decreasing sharply.
4. Beyond equivalence point , conduction remains almost constant.

Q. Which of the following statement(s) is/are correct regarding the plot between ${\Lambda }_{m}vs\sqrt{C}$?

${\Lambda }_m$ - Molar conductivity
$C$ - concentration of electrolyte

1. ${\Lambda }_m$ increase slowly with increase in dilution for strong electrolyte
2. ${\Lambda }_m$ increase steeply as dilution is increased, for weak electrolyte
3. The plot curve is a straight line with negative slope for weak electrolyte
4. Both (a) and (b)

Q. Conductometric titration curve of an equimolar mixture of $HCl$ and $HCN$ with $NaOH\left(aq\right)$ can be given as

1. 
2. 
3. 
4. 

Q. Match the titration graphs
(1) NaOH + $N{H}_4$OH vs HCl
(2) $C{H}_3$ COOH vs NaOH
(3)HCl vs NaOH
(4)$C{H}_3$ COOH vs $N{H}_4$OH
a)

b)

c)

d)

1. 1-(c) 2-(a) 3-(d) 4-(b)
2. 1-(b) 2-(c) 3-(d) 4-(a)
3. 1-(c) 2-(b) 3-(a) 4-(d)
4. 1-(b) 2-(a) 3-(d) 4-(c)

Q. Assertion: when NaOH is added to the HCl solution, the conductance of the solution decreases right upto the equivalence point and then increases.
Reason: At starting, fast moving to ions replaced by relatively slower moving $N{a}^{\oplus }$ ions and after the equivalence point, as $O{H}^{-}$ start increases conductance increases.

1. Statement 1 & 2 are correct and statement 2 is correct explanation of statement 1
2. Statement 1 & 2 are correct but statement 2 is not correct explanation of statement 1
3. Statement 1 is true, statement 2 is false
4. Statement 1 is false and statement 2 is true

Q. Heat of neutralisation of weak acid and strong base is less than the heat of neutralisation of strong acid and strong base due to:

1. Incomplete dissociation of weak acid
2. Energy has to be spent for the total dissociation of weak acid
3. Salt of weak acid and strong base is not stable
4. Incomplete neutralisation of weak acid

Q. When SO₂ is passed through acidified K₂Cr₂O₇ solution.
(a) The solution turns green
(b) The solution is decolourized
(c) Reduction of SO₂ takes place
(d) Green ppt of Cr₂(SO₄)₃ is formed

Q. $AgN{O}_3(aq.)$ was added to an aqueous $KCI$ solution gradually and the conductivity of the solution was measured. The plot of conductance (A)versus the volume of $AgN{O}_3$ is.

1. P
2. Q
3. R
4. S

Q. Choose the correct option, when conductometric titration of a strong acid vs. weak base (titrant) is carried out:

1. Conductance increases up to the equivalence point.
2. Conductance remains constant up to the equivalence point.
3. Beyond equivalence point , conduction starts decreasing sharply.
4. Beyond equivalence point , conduction remains almost constant.

Q. A solution containing $C{u}^{2+}$ and $C_2{O}_4^{2-}$ ions is titrated with $20$ mL of $\frac{M}{4}$ $KMn{O}_4$ solution in acidic medium. The resulting solution is treated with excess of $KI$ after neutralization. The evolved $I_2$ is then absorbed is $25$ mL of $\frac{M}{10}$ hypo solution. Which of the following statements is/are correct?

1. The difference in the number of mmol of $C{u}^{2+}$ and $C_2{O}_4^{2-}$ ions in the solution is $10$ mmol
2. The difference in the number of mmol of $C{u}^{2+}$ and $C_2{O}_4^{2-}$ ions in the solution is $22.5$ mmol
3. The equivalent weight of $C{u}^{2+}$ ions in the titration with $KI$ is equal to the atomic weight of $C{u}^{2+}$
4. The equivalent weight of $KI$ in the titration is $\frac{M}{2}$ where $M$ is the molecular weight of $KI$

Q.

What is meant by ‘demineralised’ water and how can it be obtained?

Q.

$AgN{O}_3\left(aq\right)$ was added to an aqueous KCl solution gradually and the conductivity of the solution was measured. The plot of conductance (A) versus the volume of $AgN{O}_3$ is

(IIT-JEE, 2011)

1. P

2. Q

3. R

4. S

Q. Which of the following orders regarding the acidic strength of phenols is correct?

1. p-nitrophenol > p-amino phenol > p-chloro phenol
2. p-amino phenol > p-nitro phenol > p-chloro phenol
3. p-amino phenol > p-chloro phenol > p-nitro phenol
4. p-amino phenol < p-chloro phenol < p-nitro phenol

Q. The value of molar conductivity of HCl is greater than that of NaCl at a particular temperature because:

1. NaCl is a salt
2. velocity of $H^{\oplus }$ ions is more than that of $N{a}^{\oplus }$ ions
3. HCl is strongly acidic
4. ionization of HCl is larger than that of NaCl

Q. Match the titration graphs
(1) NaOH + $N{H}_4$OH vs HCl
(2) $C{H}_3$ COOH vs NaOH
(3)HCl vs NaOH
(4)$C{H}_3$ COOH vs $N{H}_4$OH
a)

b)

c)

d)

1. 1-(c) 2-(a) 3-(d) 4-(b)
2. 1-(b) 2-(c) 3-(d) 4-(a)
3. 1-(c) 2-(b) 3-(a) 4-(d)
4. 1-(b) 2-(a) 3-(d) 4-(c)

Q.

The increase in the molar conductivity of $HCl$ with dilution is due to:

1. decrease in the self ionization of water
2. decrease in the interionic forces
3. increase in the self ionization of water
4. hydrolysis of $HCl$

Q. $AgN{O}_3(aq.)$ was added to an aqueous $KCI$ solution gradually and the conductivity of the solution was measured. The plot of conductance (A)versus the volume of $AgN{O}_3$ is.

1. P
2. Q
3. R
4. S

Q. The nature of an aqueous solution of sodium acetate $\left(C{H}_{3}COONa\right)$ is _______.

1. Acidic
2. Neutral
3. Alkaline
4. Amphoteric

Q. How is the titration curve of mixture of weak and strong acids against a strong base looks like?

1. 
2. 
3. 
4. 

Q. According to Bronsted-Lowry concept, the relative strengths of the bases $C{H}_{3}CO{O}^{-},O{H}^{-}$ and $C{l}^{-}$ are in the order:

1. $O{H}^{-}>C{H}_{3}CO{O}^{-}>C{l}^{-}$
2. $C{l}^{-}>O{H}^{-}>C{H}_{3}O{O}^{-}$
3. $C{H}_{3}CO{O}^{-}>O{H}^{-}>C{l}^{-}$
4. $O{H}^{-}>C{l}^{-}>C{H}_{3}CO{O}^{-}$

Q. When mercuric iodide is added to an aqueous solution of potassium iodide the:

1. freezing point is lowered
2. freezing point is raised
3. freezing point does not change
4. boiling point does not change

Q. Which technique would be applied to determine the concentration of an unknown sample of an acid?

1. Chromatography
2. Distillation
3. Titration
4. Filtration

Q. Which has least molar solubility in $H_{2}O$?

1. $LiCl$
2. $NaCl$
3. $KCl$
4. $CsCl$

Q. Which of the following compounds will react with sodium hydroxide solution in water ?

1. $(C{H}_3{)}_{3}COH$
2. $C_6{H}_{5}C{H}_{2}OH$
3. $C_2{H}_{5}OH$
4. $C_6{H}_{5}OH$

Q. If true enter 1, else enter 0.
$HCHO$ disproportionates in presence of ${OH}^{-}$.

1. 1

Q. Assertion: when NaOH is added to the HCl solution, the conductance of the solution decreases right upto the equivalence point and then increases.
Reason: At starting, fast moving to ions replaced by relatively slower moving $N{a}^{\oplus }$ ions and after the equivalence point, as $O{H}^{-}$ start increases conductance increases.

1. Statement 1 & 2 are correct and statement 2 is correct explanation of statement 1
2. Statement 1 is true, statement 2 is false
3. Statement 1 & 2 are correct but statement 2 is not correct explanation of statement 1
4. Statement 1 is false and statement 2 is true

Q. Thiosulphate on reaction with ferrous ions gives :

1. a violet complex.(soluble)
2. a reddish brown precipitate.
3. a green complex compound
4. none of the above