When equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed, the pH of the resulting solution will be:

1.	12.65	2.	2.0
3.	7.0	4.	1.04

Which one of the following pairs of solutions is not an acidic buffer?

1. ${\mathrm{HClO}}_4$ $\mathrm{and}$ ${\mathrm{NaClO}}_4$
2. ${\mathrm{CH}}_3\mathrm{COOH}$ $\mathrm{and}$ ${\mathrm{CH}}_3\mathrm{COONa}$
3. ${\mathrm{H}}_2{\mathrm{CO}}_3$ $\mathrm{and}$ ${\mathrm{Na}}_2{\mathrm{CO}}_3$
4. ${\mathrm{H}}_3{\mathrm{PO}}_4$ $\mathrm{and}$ ${\mathrm{Na}}_3{\mathrm{PO}}_4$

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

The strongest acid among the following compounds is:

Find the equilibrium constant K for the reaction:

NO₂(g) ⇌ ½N₂(g) + O₂(g)

Given:

N₂(g) + O₂(g) ⇌ 2NO(g), K₁

2NO(g) + O₂(g) ⇌ 2NO₂(g), K₂

A saturated solution of Ba(OH)₂ has a pH of 12. The value of its K_sp will be:
1. $4.00\times {10}^{-6}$ $M^3$
2. $4.00\times {10}^{-7}$ $M^3$
3. $5.00\times {10}^{-6}$ $M^3$
4. $5.00\times {10}^{-7}$ $M^3$

The equilibrium reaction that doesn't have equal values for K_c and K_p is: 

1. \(2NO(g) \rightleftharpoons N_2(g) + O_2(g)\)
2. \(SO_2(g) + NO_2(g) \rightleftharpoons SO_3(g) + NO(g)\)
3. \(H_2(g) + I_2(g) \rightleftharpoons 2HI (g)\)
4. \(2C(s) + O_2(g) \rightleftharpoons 2CO_2(g)\)

In a buffer solution containing an equal concentration of B^- and HB, the K_b for B^- is 10^-10. pH of the buffer solution is:

Find the equilibrium constant for the reaction:

H₂(g) + I₂(g) ⇌ 2HI(g)

Given that:

HI(g) ⇌ ½H₂(g) + ½I₂(g)  K = 8

The pOH of a solution at 25 °C that contains 1×10^-10 M of hydronium ions is: