At room temperature, MY and NY₃, two nearly insoluble salts, have the same K_sp values of 6.2 × 10^-13. The true statement regarding MY and NY₃ is:

1.	The molar solubility of MY in water is less than that of NY3.
2.	The salts MY and NY3 are more soluble in 0.5 M KY than in pure water.
3.	The addition of the salt of KY to a solution of MY and NY3 will have no effect on their solubilities.
4.	The molar solubilities of MY and NY3 in water are identical.

Consider the nitration of benzene using mixed conc. H₂SO₄ and HNO₃.
If a large amount of KHSO₄ is added to the mixture, the rate of nitration will be:

If the equilibrium constant for N₂(g) + O₂ (g) ⇄ 2NO(g) is K, the equilibrium constant for \(\frac{1}{2}\)N₂(g) + \(\frac{1}{2}\)O₂(g) ⇄ NO(g) will be?

1. $K^{\frac{1}{2}}$

2. $\frac{1}{2}K$

3. K

4. $K^2$

Aqueous solution of which of the following compounds is the best conductor of electric current?
1. Acetic acid, \(\mathrm{C_{2} H_{4} O_{2}}\)${\mathrm{}}_{}$
2. Hydrochloric acid, \(\mathrm{HCl}\)
3. Ammonia, \(\mathrm{N H_{3}}\)${\mathrm{}}_{}$
4. Fructose, \(\mathrm{C_{6} H_{12} O_{6}}\)${\mathrm{}}_{}$
 

The value of the equilibrium constant for a particular reaction is 1.6 × 10¹². When the system is in equilibrium, it will include:
1. All reactants
2. Mostly reactants
3. Mostly products
4. Similar amounts of reactants and products

For the reversible reaction:
N₂(g) + 3H₂(g) \(\rightleftharpoons\) 2NH₃(g) + heat 

The equilibrium shifts in a forward direction:

1. by increasing the concentration of $N{H}_3\left(g\right)$
2. by decreasing the pressure.
3. by decreasing the concentration of $N_2\left(g\right)$ $and$ $H_2\left(g\right)$
4. by increasing pressure and decreasing temperature.

For a given exothermic reaction, K_p and K_p^’ are the equilibrium constants at temperatures T₁ and T₂ respectively. Assuming that the heat of reaction is constant in temperatures range between T₁ and T₂, it is a readily observation that:
1. $K_p>K_p^{\text{'}}$
2. $K_p<K_p^{\text{'}}$
3. $K_p=K_p^{\text{'}}$
4. $K_p=\frac{1}{K_p^{\text{'}}}$

The strongest acid among the following compounds is:

Equimolar solutions of the following substances were prepared separately. Which one of these will record the highest pH value?

1. \(\mathrm{B a C l_{2}}\)
2. \(\mathrm{A l C l_{3}}\)
3. \(\mathrm{L i C l}\)
4. \(\mathrm{B e C l_{2}}\)${\mathrm{}}_{}$