Equilibrium

100 mL of 0.01 M solution of NaOH is diluted to 1 dm³. What is the pH of the diluted solution?

• 12

• 11

• 2

• 3

Consider the following reaction equilibrium:

${\mathrm{N}}_2\left(\mathrm{g}\right) +3{\mathrm{H}}_2\left(\mathrm{g}\right) \rightleftharpoons 2{\mathrm{NH}}_3\left(\mathrm{g}\right)$

Initially, 1 mole of N₂ and 3 moles of H₂ are taken in a 2 L flask. At equilibrium state if, the number of moles of N₂ is 0.6, what is the total number of moles of all gases present in the flask?

• 0.8

• 1.6

• 3.2

• 6.4

Assertion (A): The pH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8 (pK_a of acetic acid is 4.8).

Reason (R): The ionic product of water at 25°C is 10^-14mol².L^-2. The correct answer is

• Both (A) and (R) are true and (R) is the correct explanation of (A)

• Both (A) and (R) are true and (R) is not the correct explanation of (A)

• (A) is true but (R) is not true

• (A) is not true but (R) is true

The equilibrium constant for the reaction 

${\mathrm{SO}}_2\left(\mathrm{g}\right)\hspace{0.17em}+ \frac{1}{2}{\mathrm{O}}_2\left(\mathrm{g}\right) \rightleftharpoons {\mathrm{SO}}_3\left(\mathrm{g}\right) \mathrm{is}\hspace{0.17em}5\times {10}^{-2} \mathrm{atm}.$ The equilibnum constant of the reaction $2{\mathrm{SO}}_3\left(\mathrm{g}\right)\hspace{0.17em}\rightleftharpoons 2{\mathrm{SO}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \mathrm{would}\hspace{0.17em}\mathrm{be}.$

• 100 atm

• 200 atm

• 4 × 10² atm

• 6.25 × 10⁴ atm

The pH of 0.05 M acetic acid is K_a = 2 × 10^-5)

• 2

• 11

• 10^-3

• 3

The degree of ionization of 0.10 M lactic acid is 4.0%

The value of K_c is

• 1.66 × 10^-5

• 1.66 × 10^-4

• 1.66 × 10^-3

• 1.66 × 10^-2

pH of a solution is 4. The hydroxide ion concentration of the solution would be

• 10^-4

• 10^-10

• 10^-2

• 10^-12

In which solution/ solvent the solubility of AgCl is minimum?

• 0.01 M NaCl

• 0.01 M CaCl₂

• Pure water

• 0.001 M AgNO₃

1.0 L of 1.0 M solution of sodium hydroxide is neutralised by 1.0 L of 1.0 M of methanoic acid. If the heat of formation of water is X, the neutralisation energy of above reaction is

• less than X

• more than X

• equal to X

• None of the above

If the molar solubility of X₃B₃(AlF₆)₂ at 298 K is x, the solubility product K_sp is

• 18x³

• 27x⁴

• 27x⁸

• 2916x⁸