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, $\underset{\left(g\right)}{PQ}<mspace\; width="1em"></mspace>\rightleftharpoons <mspace\; width="1em"></mspace>\underset{\left(g\right)}{P}+\underset{\left(g\right)}{Q}$ 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

$K_c<mspace\; width="1em"></mspace>for<mspace\; width="1em"></mspace>PC{l}_5\left(g\right)\rightleftharpoons PC{l}_3\left(g\right)+C{l}_2\left(g\right)<mspace\; width="1em"></mspace>is<mspace\; width="1em"></mspace>0.04<mspace\; width="1em"></mspace>at<mspace\; width="1em"></mspace>25°.$ 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)

If solubility product of Ca${\left(\mathrm{OH}\right)}_2<mspace\; width="1em"></mspace>\mathrm{is}<mspace\; width="1em"></mspace>{10}^{-11}$, the pH at which $\mathrm{Ca}{\left(\mathrm{OH}\right)}_2$ precipitate from a solution containing decimolar concentration of ${\mathrm{Ca}}^{2+}$ is

1. <5

2. 9<pH<5

3. >9

4. 9<pH>7

For the reaction,

${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)\rightleftharpoons {\mathrm{CuSO}}_4.3{\mathrm{H}}_2\mathrm{O}\left(\mathrm{s}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

choose the correct representation:

1. ${\mathrm{K}}_{\mathrm{P}}={\mathrm{P}}_{{\mathrm{H}}_2\mathrm{O}}^2$

2. K_c = [H₂O]²

3. ${\mathrm{K}}_{\mathrm{P}}={\mathrm{K}}_{\mathrm{C}}{\left(\mathrm{RT}\right)}^2$

4. All of the above

The solubility of PbCI₂  in water is  0.01 M  at  25 °C. The maximum concentration of Pb²⁺ in 0.1 M NaCI will be:

1. 2×10^-3 M

2. 1×10^-4 M

3. 1.6×10^-2 M

4. 4×10^-4 M

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?