A monoprotic acid in a 0.1 M solution ionizes to 0.001%.Its ionisation constant is 

1. $1.0 \times {10}^{-3}$

2. $1.0 \times {10}^{-6}$

3.$1.0 \times {10}^{-8}$

4. $1.0 \times {10}^{-11}$

With increase in temperature, ionic product of water 

1. decreases 

2. increases 

3. remains same 

4. may increase or decrease 

pH of pure water at 25$°$C is 7 . If water is heated to 60 $°$C, the 

1. pH will decrease 

2. pH will increase 

3. pH will remain constant 

4. H${}^{+}$ions and OH${}^{-}$ions concentrations will become unequal. 

When a solution of acetic acid was titrated with NaOH, the pH of the solution when half of the acid, neutralised was 4.74 Dissociation constant of the acid is 

1. 1.8 $\times$ 10${}^{-5}$

2. 3.2 $\times$ 10${}^{-5}$

3. 8.7 $\times$ 10${}^{-5}$

4. 6.42 $\times$ 10${}^{-5}$

40 mg of pure sodium hydroxide is dissolved in 10 litres of distilled water. The pH of the

solution is 

1. 9.0

2. 10

3. 11

4. 12

In which of the following solvents will AgBr have the highest solubility 

1. 10${}^{-3}$ M NaBr

2. 10${}^{-3}$ M NH4OH 

3. Pure water 

4. 10${}^{-3}$ M HBr

The solubility product of CuS, Ag${}_2$S. HgS are 10${}^{-37},{10}^{-44}$ and 10${}^{-54}$ respectively. The solubilities of these sulphides are in the order of: 

1. Ag${}_2$S > CuS > HgS

2. Ag${}_2$S > HgS > CuS 

3. HgS > Ag${}_2$S > CuS

4. CuS > Ag${}_2$S > HgS 

The pH of 0.1 M solution of the following slats increases in the order 

1. NaCl < NH${}_4$Cl < NaCN < HCl 

2. HCl < NH${}_4$Cl < NaCl < NaCN

3. NaCN < NH${}_4$Cl < NaCl <HCl 

4. HCl < NaCl < NaCN < NH${}_4$Cl

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)

(1) 1.2

(2) 2.25

(3) 2.1

(4) 3.6

In the reaction HCN + H${}_2$O $\rightleftharpoons H_3{O}^{+}+ C{N}^{-}$ the conjugate acid- base pair is 

1. HCN,H${}_3$O${}^{+}$

2. HCN,CN${}^{-}$

3. $H_{2}O, C{N}^{-}$

4. $C{N}^{-},H_3{O}^{+}$