Which one of the following salts give an acidic solution in water?

• CH₃COONa

• NH₄Cl

• NaCl

• CH₃COONH₄

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

If the equilibrium constant for the reaction,

${\mathrm{H}}_2\left(\mathrm{g}\right)\hspace{0.17em}+ {\mathrm{I}}_2\left(\mathrm{g}\right) \rightleftharpoons 2\mathrm{HI} \left(\mathrm{g}\right) \mathrm{is} \mathrm{K}$. what is the equilibrium constant of $\mathrm{HI}\left(\mathrm{g}\right) \rightleftharpoons \frac{1}{2}{\mathrm{H}}_2\left(\mathrm{g}\right) +\hspace{0.17em}\frac{1}{2}{\mathrm{I}}_2\left(\mathrm{g}\right) ?$

• 1/K

• √K

• K

• 1/√K

The pH of 0.01 M solution of acetic acid is 5.0. What are the values of [H⁺] and K_a respectively?

• 1 × 10^-5M, 1× 10^-8

• 1 × 10^-5M, 1× 10^-9

• 1 × 10^-4M, 1 × 10^-8

• 1 × 10^-3M, 1 × 10^-8

pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic acid is added to 250 mL of a buffer solution of acetic acid and potassium acetate at 27°C. The buffer capacity of the solution is

• 0.1

• 10

• 1

• 0.4

The equilibnum constant for the given reaction is 100.

N₂ (g) + 2O₂ (g) $\rightleftharpoons$ 2NO₂ (g)

What is the equilibrium constant for the reaction given below?

NO₂ (g) $\rightleftharpoons \frac{1}{2}{\mathrm{N}}_2$ (g) + O₂ (g)

• 10

• 1

• 0.1

• 0.01

207.

20 mL of 0.1 M acetic acid is mixed with 50 mL of potassium acetate. K_a of acetic acid = 1.8 × 10^-5 at 27°C. Calculate concentration of potassium acetate if pH of the mixture is 4.8.

• 0.1 M

• 0.04 M

• 0.4 M

• 0.02 M

If the equilibrium constant for the reaction,

2AB  A₂ + B₂ 

is 49, what is the equilibrium constant for AB $$ \rightleftharpoons \frac{1}{2}{\mathrm{A}}_1 + \frac{1}{2}{\mathrm{A}}_2${\mathrm{}}_{}$ ? 

• 7

• $\frac{1}{7}$

• 24.5

• 49

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