Equilibrium

Phosphoric acid ionizes in three steps with ionization constant values \(K_{a_1}\), \(K_{a_2}\) and \(K_{a_3}\), respectively, while K is the overall ionization constant. Which of the following statements are true?

A. \(\log K = \log K_{a_1} + \log K_{a_2} + \log K_{a_3}\)

B. \(\mathrm{H_3PO_4}\) is a stronger acid than \(\mathrm{H_2PO_4^-}\) and \(\mathrm{HPO_4^{2-}}\).

C. \(K_{a_1} > K_{a_2} > K_{a_3}\)

D. \(K_{a_1} = \frac{K_{a_3}+K_{a_2}}{2}\)

Choose the correct answer from the options given below:

For the reaction \(\mathrm{A(g) \rightleftharpoons 2B(g)}\), the backward reaction rate constant is higher than the forward reaction rate constant by a factor of 2500, at 1000 K.

[Given : R = 0.0831 L atm \(\mathrm{mol^{-1}\,K^{-1}}\)]

\(K_p\) for the reaction at 1000 K is

Higher yield of NO in \(\mathrm{N_2(g) + O_2(g) \rightleftharpoons 2NO(g)}\) can be obtained at

[\(\Delta H\) of the reaction = + 180.7 kJ \(\mathrm{mol^{-1}}\)]

A. higher temperature

B. lower temperature

C. higher concentration of \(\mathrm{N_2}\)

D. higher concentration of \(\mathrm{O_2}\)

Choose the correct answer from the options given below:

For the reaction \(2A \rightleftharpoons B + C\), \(K_c = 4\times10^{-3}\). At a given time, the composition of reaction mixture is : \([A]=[B]=[C]=2\times10^{-3}\) M.

Then, which of the following is correct?

In which of the following equilibria, \(K_p\) and \(K_c\) are NOT equal?

The Henry's law constant (\(K_H\)) values of three gases (A, B, C) in water are 145, \(2\times10^{-5}\) and 35 kbar, respectively. The solubility of these gases in water follow the order:

Consider the following reaction in a sealed vessel at equilibrium with concentrations of \(N_2 = 3.0\times10^{-3}\) M, \(O_2 = 4.2\times10^{-3}\) M and \(NO = 2.8\times10^{-3}\) M.

\(2NO_{(g)} \rightleftharpoons N_{2(g)} + O_{2(g)}\)

If 0.1 mol \(L^{-1}\) of \(NO_{(g)}\) is taken in a closed vessel, what will be degree of dissociation (\(\alpha\)) of \(NO_{(g)}\) at equilibrium?

Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R :

Assertion A : Helium is used to dilute oxygen in diving apparatus.

Reasons R : Helium has high solubility in O\(_2\).

In the light of the above statements, choose the correct answer from the options given below :

Amongst the given options which of the following molecules / ion acts as a Lewis acid?

The pH of the solution containing 50 mL each of 0.10 M sodium acetate and 0.01 M acetic acid is

[Given \(pK_a\) of \(CH_3COOH\) = 4.57]

\(3O_2(g) \rightleftharpoons 2O_3(g)\)

for the above reaction at 298 K, \(K_c\) is found to be \(3.0 \times 10^{-59}\). If the concentration of \(O_2\) at equilibrium is 0.040 M then concentration of \(O_3\) in M is

The \(pK_b\) of dimethylamine and \(pK_a\) of acetic acid are 3.27 and 4.77 respectively at T (K). The correct option for the pH of dimethylammonium acetate solution is :

Find out the solubility of Ni(OH)\(_2\) in 0.1 M NaOH. Given that the ionic product of Ni(OH)\(_2\) is \(2\times10^{-15}\).

HCl was passed through a solution of CaCl\(_2\), MgCl\(_2\) and NaCl. Which of the following compound(s) crystallise(s) ?

pH of a saturated solution of Ca(OH)\(_2\) is 9. The solubility product (\(K_{sp}\)) of Ca(OH)\(_2\) is :

Conjugate base for Brönsted acids H\(_2\)O and HF are :

Which will make basic buffer ?

Given van der Waals constant for NH\(_3\), H\(_2\), O\(_2\) and CO\(_2\) are respectively 4.17, 0.244, 1.36 and 3.59, which one of the following gases is most easily liquefied ?

Following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations :

a. 60 mL \(\frac{M}{10}\) HCl + 40 mL \(\frac{M}{10}\) NaOH

b. 55 mL \(\frac{M}{10}\) HCl + 45 mL \(\frac{M}{10}\) NaOH

c. 75 mL \(\frac{M}{5}\) HCl + 25 mL \(\frac{M}{5}\) NaOH

d. 100 mL \(\frac{M}{10}\) HCl + 100 mL \(\frac{M}{10}\) NaOH

pH of which one of them will be equal to 1 ?

The solubility of BaSO\(_4\) in water is \(2.42\times10^{-3}\) gL\(^{-1}\) at 298 K. The value of its solubility product (K\(_{sp}\)) will be

(Given molar mass of BaSO\(_4\) = 233 g mol\(^{-1}\))

Which one of the following conditions will favour maximum formation of the product in the reaction,

A\(_2\)(g) + B\(_2\)(g) \(\rightleftharpoons\) X\(_2\)(g) \(\Delta_r\)H = \(-\)X kJ ?

The correction factor 'a' to the ideal gas equation corresponds to

The equilibrium constants of the following are :

\(N_2 + 3H_2 \rightleftharpoons 2NH_3\) \(K_1\)

\(N_2 + O_2 \rightleftharpoons 2NO\) \(K_2\)

\(H_2 + \frac{1}{2}O_2 \rightarrow H_2O\) \(K_3\)

The equilibrium constant (K) of the reaction : \(2NH_3 + \frac{5}{2}O_2 \overset{K}{\rightleftharpoons} 2NO + 3H_2O\), will be :

Which one of the following statements is not correct ?

A 20 litre container at 400 K contains \(CO_2\)(g) at pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the container is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of \(CO_2\) attains its maximum value, will be :

(Given that : \(SrCO_3(s) \rightleftharpoons SrO(s) + CO_2(g)\), \(K_p = 1.6\) atm)

Concentration of the \(Ag^+\) ions in a saturated solution of \(Ag_2C_2O_4\) is \(2.2 \times 10^{-4}\) mol \(L^{-1}\). Solubility product of \(Ag_2C_2O_4\) is :

MY and \(NY_3\), two nearly insoluble salts, have the same \(K_{sp}\) values of \(6.2\times10^{-13}\) at room temperature. Which statement would be true in regard to MY and \(NY_3\) ?

The solubility of AgCl (s) with solubility product \(1.6\times10^{-10}\) in \(0.1\,M\) NaCl solution would be

The percentage of pyridine (\(C_5H_5N\)) that forms pyridinium ion (\(C_5H_5N^+H\)) in a \(0.10\,M\) aqueous pyridine solution (\(K_b\) for \(C_5H_5N = 1.7\times10^{-9}\)) is