When 10 ml of 0.1 M acetic acid (pK_a=5.0) is titrated against 10 ml of 0.1 M
ammonia solution (pK_b=5.0), the pH at equivalence point will be:

1.	9.0	2.	6.0
3.	5.0	4.	7.0

For the reaction 2NOCl_(g)⇔2NO_(g)+Cl_2(g), K_C at 427$°$C is \(3\times 10^{-6} \ mol\ L^{-1}\). The value of K_p will be :

1. $1.72\times {10}^{-4}$

2. $7.50\times {10}^5$

3. $2.50\times {10}^{-5}$

4. $2.50\times {10}^{-4}$

The molar solubility of ${\mathrm{CaF}}_2$ $({\mathrm{K}}_{\mathrm{sp}}=5.3$ $\mathrm{\times }$ ${10}^{-11})$ in 0.1 M solution of NaF will be:

Which of the following cannot act both as a Bronsted acid and as a Bronsted base?

1. \(\mathrm{H C O_{3}^{-}}\)

2. \(\mathrm{NH_3}\)

3. \(\mathrm{HCl}\)

4. \(\mathrm{H S O_{4}^{-}}\)

The oxoacid that has the highest K_a value is: t

1 HClO₃

2 HBrO₃

3 HlO₃

4 All have equal K_a

For the equilibrium, $\underset{\left(g\right)}{PQ} \rightleftharpoons \underset{\left(g\right)}{P}+\underset{\left(g\right)}{Q}$ at 300 K. The pressure at which 50% of PQ is dissociated is numerically equal to 

1. 3 $K_p$

2. 4$K_p$

3. $K_p$

4. Can't be predicted

$K_c for PC{I}_5\left(g\right)\rightleftharpoons PC{I}_3\left(g\right)+C{I}_2\left(g\right) is 0.04 at 25°.$ The number of moles of $PC{I}_5$ required to a 3.0 liter flask to obtain $C{I}_2$ of concentration 0.15 M is

1. 1.5 mole

2. 2.1 mole

3. 6.0 mole

4. 0.45 mole

For the following reaction, 
 H$$₂(g)+I₂(g)⇌2HI(g) $at$ $250°C,$

The effect on the state of equilibrium on doubling the volume of the system will be:

Which of the following cannot act as a buffer? 
1. NaH₂PO₄ + H₃PO₄
2. NH₄OH + NH₄CI
3. NaOH + CH₃COONa
4. Both (1) & (3)