Auto Protolysis of Water

Q.

What is a Ionic reaction?

Q. $K_{w}for{H}_{2}Ois9.62\times {10}^{-14}at{60}^{\circ }C$
The pH of water at this temperature is :

1. 6.5
2. 7.5
3. 7
4. 6

Q.

Find out the solubility of $Ni{\left(OH\right)}_2$ in$0.1\mathrm{M}$ $\mathrm{NaOH}.$

The ionic product of $Ni{\left(OH\right)}_2$ is $2\times {10}^{-15}$

1. $1\times {10}^{-13}M$

2. $1\times {10}^{-8}M$

3. $2\times {10}^{-13}M$

4. $1\times {10}^{8}M$

Q.

Theory of ionization was given by

1. Rutherford

2. Graham

3. Faraday

4. Arrhenius

Q.

A salt is formed from a weak acid and weak base. If $p{K}_b$ > $p{K}_a$, then the pH of that salt solution is

1. < 7

2. > 7

3. = 14

4. = 7

Q. Which of the following can be classified as autoprotolysis reactions?

1. $H_{2}O\left(l\right)+H_{2}O\left(l\right)\rightleftharpoons H_3{O}^{+}\left(aq\right)+O{H}^{-}\left(aq\right)$
2. $2N{H}_3\left(l\right)\rightleftharpoons N{H}_4^{+}\left(aq\right)+N{H}_2^{-}\left(aq\right)$
3. $C{H}_{3}COOH\left(aq\right)\rightleftharpoons C{H}_{3}CO{O}^{-}\left(aq\right)+H^{+}\left(aq\right)$
4. $2C{H}_{3}COOH\left(l\right)\rightleftharpoons C{H}_{3}CO{O}^{-}\left(aq\right)+C{H}_{3}COO{H}_2^{+}\left(aq\right)$

Q. Consider the following cases A and B in Ostwald-Walker Method:
Case A : Dry air is passed through a pure solvent and then, a dehydrating agent.

Case B: Dry air is passed through a pure solvent and then a solution with non-volatile solute and then, a dehydrating agent

Here,
\(p^\circ \text{ is the vapour pressure of the pure solvent}\)
\(p_s \text{ is the vapour pressure of the solution}\)

Choose the correct option(s) :

Q. Which of the following expression is not true

1. $\left[H^{+}\right]=\left[O{H}^{-}\right]=\sqrt{K_w}$ for a neutral solution at all temperatures.
2. $\left[H^{+}\right]>\sqrt{K_w}$ & $\left[O{H}^{-}\right]<\sqrt{K_w}$ for an acidic solution
3. $\left[H^{+}\right]<\sqrt{K_w}$ & $\left[O{H}^{-}\right]>\sqrt{K_w}$ for an alkaline solution
4. $\left[H^{+}\right]=\left[O{H}^{-}\right]={10}^{-7}M$ for a neutral solution at all temperatures.

Q. At ${25}^{\circ }C$ disociation constant of acid $HA$ and base $BOH$ in aqueous solution are same. The $pH$ of $0.01M$ solution of $HA$ is $5$. The $pOH$ of ${10}^{-4}$ M solution of $BOH$ at the same temperature is:

1. $3.5$
2. $4$
3. $6$
4. None of these

Q. When $HN{O}_3\left(aq\right)$ is titrated with NaOH (aq) conductometrically, the graphical representation of this titration can be shown as

1. 
2. 
3. 
4. 

Q.

The ionic product of water does not change with the temperature - True or false?

1. False

2. True

Q. The degree of dissociation of pure water at $25{}^{o}C$ is found to be $1.8\times {10}^{-9}$. Find $K_{w}and{K}_d$ at $25{}^{o}C$ ?

1. $3.24\times {10}^{-18}$ ; $5.83\times {10}^{-20}$
2. $1.00\times {10}^{-14}$ ; $1.80\times {10}^{-16}$
3. $1.80\times {10}^{-16}$ ; $1.00\times {10}^{-14}$
4. $1.00\times {10}^{-14}$ ; $1.00\times {10}^{-14}$

Q.

The ionic product of water will increase if

1. temperature is reduced

2. temperature is increased

3. pressure is decreased

4. pressure is increased

Q. On reaction with dihydrogen, the alkali metals:

1. form hydrides which are ionic solids with high melting points
2. form hydrides which are molecular solids with low melting points
3. form hydrides which are ionic solids with low melting points
4. form hydrides which are non-stoichiometric

Q.

Theory of ionization was given by

1. Rutherford

2. Graham

3. Faraday

4. Arrhenius

Q. Which of the following condition(s) is/are valid for an ideal solution?

1. No change in volume on mixing. $\Delta V_{mix}=0$
   
2. No change in enthalpy on mixing. $\Delta H_{mix}=0$
3. Entropy on mixing $\Delta S_{mix}>0$
4. All of the above.

Q. Which of the following condition(s) is/are valid for an ideal solution?

1. No change in entropy on mixing $\Delta S_{mix}=0$
2. No change in enthalpy on mixing. $\Delta H_{mix}=0$
3. Ionisation of solute occurs to a small extent.
4. No change in volume on mixing. $\Delta V_{mix}=0$
   

Q. Dry air was passed through a beaker solution containing $15\text{g}$ of solute and $120\text{g}$ of water. Then, it passed through a beaker containing pure water solvent. Loss in weight of the solution beaker was $2\text{g}$ and loss in weight of solvent beaker was $0.05\text{g}$. What is the molecular weight of the solute ?

1. $90\text{g/mol}$
2. $100\text{g/mol}$
3. $85\text{g/mol}$
4. $95\text{g/mol}$

Q. The $pH$ of neutral water at ${25}^{\circ }\text{C}$ is $7.0$. What will be the nature of pure water at ${60}^{\circ }\text{C}$?

1. Acidic
2. Basic
3. Neutral
4. Cannot predict

Q. 40. How to find a cosucated acid base? What is equilibrium of ionic compound o water?