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 standard reduction potential for ${\mathrm{Cu}}^{2+}/\mathrm{Cu}$ is 0.34 V.
The reduction potential at pH =14 for the above couple given $\left({\mathrm{K}}_{\mathrm{sp}}\left[\mathrm{Cu}{\left(\mathrm{OH}\right)}_2\right]=1\times {10}^{-19}\right)$ is :

1.  -0.22 V

2.  +0.22 V

3.  -0.34 V

4.  +0.34 V

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

1. $5.3$ $\mathrm{x}$ ${10}^{-11}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$

2. $5.3$ $\mathrm{x}$ ${10}^{-8}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$

3. $5.3$ $\mathrm{x}$ ${10}^{-9}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$

4. $5.3$ $\mathrm{x}$ ${10}^{-10}$ $\mathrm{mol}$ ${\mathrm{L}}^{-1}$

The pH of a 0.01 M NaOH (aq) solution will be:

1. 7.01

2. 2

3. 12

4. 9

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 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)

If the pH of 0.1 M NaCN solution is 11, then the percentage hydrolysis will be:

1. 0.1%

2. 1%

3. 0.01%

4. 10%

How much water should be added to 400 mL of HCI solution in order to raise the pH by one unit?