The solubility product constant K_sp of Mg(OH)₂ is 9.0 X 10^-12. If a solution is 0.010 M with respect to Mg²⁺ ion, what is the maximum hydroxide ion concentration that could be present without causing the precipitation of Mg(OH)₂?

1. 1.5 X 10^-7 M

2. 3.0 X 10^-7 M

3. 1.5 X 10^-5 M

4. 3.0 X 10^-5 M

The amount of CaC₂O₄ (molecular weight =128) will dissolve in distilled water to make 1 liter of a saturated solution is: 

[K_sp (CaC₂O₄) = 2.5 x 10^-9 ]

1. 0.0064 g             
2. 0.1280 g
3. 0.0128 g           
4. 1.2800 g

What substance could be added to one liter of water to serve as a buffer?

1. One mole of \(CH_ 3 COO H\) and 0.5 moles of \(NaOH\)

2. One mole of \(NH_4Cl\) and one mole of \(HCl\)

3. One mole of \(NH_4OH\) and one mole of \(NaOH\)

4. One mole of \(CH_ 3 COO H\) and one mole of \(HCl\)

Acoording to Bronsted-Lowry concept, the correct order of relative strength of bases follows the order

1. CH₃COO^- > Cl^- > OH^-

2. CH₃COO^- > OH^- > Cl^-

3. OH^- > CH₃COO^- > Cl^-

4. OH^- > Cl^-> CH₃COO^-

pOH of H₂O is 7.0 at 298K. If water is heated at 350K, which of the following statement should be true ?

(1) pOH will decrease

(2) pOH will increase

(3) pOH will remain 7.0

(4) Concentration of H⁺ ions will increase but that of OH^- will decrease.

An aqueous solution of NaHSO₃ is-

1. Acidic                 
2. Slightly alkaline
3. Alkaline             
4. Slightly Acidic

The solubility product constant (K_sp) of salts of type MX, MX₂ and M₃X at temperature T are 4.0 X 10^-8, 3.2 X 10^-14 and
2.7 X 10^-15 respectively. The order of solubilities (mol dm^-3) of the salts at temperature T is:

1. MX > MX₂ > M₃X

2. M₃X > MX₂ > MX

3. MX₂ >M₃X >MX > 

4.  MX >M₃X > MX₂

Ostwald dilution law for weak electrolyte HA can be given as

$\left(1\right)<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })}$
$\left(2\right)<mspace\; width="1em"></mspace>\mathrm{Ka}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>{\mathrm{C\alpha }}^2<mspace\; width="1em"></mspace>\mathrm{if}<mspace\; width="1em"></mspace>\mathrm{\alpha }\to 0$
$\left(3\right)<mspace\; width="1em"></mspace>{\mathrm{K}}_{\mathrm{a}}<mspace\; width="1em"></mspace>=<mspace\; width="1em"></mspace>\frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })}$
$\left(4\right)<mspace\; width="1em"></mspace>\mathrm{All}<mspace\; width="1em"></mspace>\mathrm{of}<mspace\; width="1em"></mspace>\mathrm{the}<mspace\; width="1em"></mspace>\mathrm{above}$

In the reaction, N₂O₄(g) $\rightleftharpoons$ 2NO₂(g), $\mathrm{\alpha }$ is that part of N₂O₄ which dissociates. The number of moles at equilibrium will be:

1. ${\left(1-\mathrm{\alpha }\right)}^2$

2. $3\mathrm{\alpha }$

3. $\mathrm{\alpha }$

4. $1+\mathrm{\alpha }$

In which solution, AgCl has minimum solubility ?

1. 0.05 M AgNO₃

2. 0.01 M NaCl

3. Pure Water

4. 0.01 M NH₄OH