HI was heated in a sealed tube at 440$°$C till the equilibrium was reached, HI was found to be 22 % decomposed. The equilibrium constant for dissociation is-

28 g N₂ and 6g H₂ were mixed. At equilibrium 17 g NH₃ was formed. the mass of N₂ and H₂ of equilibrium are respectively:

Which is the strongest acid in the following?          

pH for the solution of salt undergoing anionic hydrolysis (say CH₃COONa) is given by:

Which can act as an acidic buffer?

a. NH₄Cl + NH₄OH

b. CH₃COOH + CH₃COONa

c. 40 mL of 0.1 M NaCN + 20 mL of 0.1 M HCl

The following equilibrium exists in an aqueous solution 

CH₃COOH $\rightleftharpoons$H⁺ + CH₃COO^- . If dilute HCl is added to this solution:

The solubility product of CuS, CdS and HgS are 10^-31, 10^-44, 10^-54 respectively. The solubility of these sulphides are in the order

The hydroxide having the lowest value of K_sp at 25$°$C is:

For the reaction, A + B $\rightleftharpoons$C+D, the initial concentration of A and B are equal, but the equilibrium concentration of C is twice that of the equilibrium concentration of A. The equilibrium constant is:

Solubility of an aqueous solution of Mg(OH)₂ is X mol litre^-1, then its K_sp is:

At constant temperature, the equilibrium constant (K_p) for the decomposition reaction. N₂O₄ $\rightleftharpoons$2NO₂ is expressed by,

         K_p = (4x²P)/(1-x²)

where P= pressure, x = extent of decomposition. Which of the following statements is true?

An aqueous solution of ammonium acetate is:

The equilibrium constant for the reaction ${\mathrm{N}}_2\left(\mathrm{g}\right) + {\mathrm{O}}_2\left(\mathrm{g}\right) \stackrel{ }{\rightleftharpoons }2\mathrm{NO}\left(\mathrm{g}\right)$ is 4 X 10^-4 at 200K. In the presence of a catalyst, the equilibrium is attained 10 times faster. Therefore, the equilibrium constant in presence of the catalyst at 200K is

For the given reaction,

$2\mathrm{A}\left(\mathrm{s}\right) + \mathrm{B}\left(\mathrm{g}\right) \rightleftharpoons \mathrm{C}\left(\mathrm{g}\right) + 2\mathrm{D}\left(\mathrm{s}\right) + \mathrm{E}\left(\mathrm{s}\right)$

the degree of dissociation of B was found to be 20% at 300 K and 24% at 500K. The rate of backward reaction.

The pH of 0.1 M solution of anilium chloride is (K_a of ${\mathrm{C}}_6{\mathrm{H}}_5{\mathrm{NH}}_3^{+}$ = 10^-6)

In the following reaction

${\mathrm{HC}}_2{\mathrm{O}}_4^{-} + {\mathrm{PO}}_4^{3-} \rightleftharpoons {\mathrm{HPO}}_4^{2-} + {\mathrm{C}}_2{\mathrm{O}}_4^{2-}$ 

Which are the two Bronsted bases ?

Percentage ionisation of water at certain temperature is 3.6 X 10^-7%, Calculate K_w and pH of water.

A 50 ml solution of strong acid of pH = 1 is mixed with a 50 ml solution of strong acid of pH=2. The pH of the mixture will be nearly:                                                     

(log 5.5 = 0.74)

1 litre solution of pH =4 (solution of a strong acid) is added to the 7/3 litre of water. What is the pH of resulting solution. (Log 3 = 0.48)

The pH of a solution obtained by mixing 50ml of 0.4N HCl and 50ml of 0.2M NaOH is:

K_b for a monoacidic base whose 0.10 M solution has a pH of 10.48

In an acidic Buffer solution (CH₃COOH + CH₃COONa), the species mainly present in the solution is

(Ignore negligible amount)

When NH₄Cl is added in NH₄OH solution, then pH of the solution

The most hydrolyzed salt among the following is-

(Assume that K_b of all weak bases is the same)

The pH of 10^-6 M CH₃COOH (K_a = 1.8 X 10^-5) is:

60 ml 1M CH₃COOH is mixed with 20 ml 1 M NaOH then pH of resulting solution will be

(K_a = 1.8 X 10^-5, log1.8 = 0.25)

In which solvent, solubility of AgCl is maximum ?

$\frac{{\mathrm{K}}_{\mathrm{p}}}{{\mathrm{K}}_{\mathrm{c}}}$ for the gaseous reaction:

$$\begin{gathered} \mathrm{I}. 2\mathrm{A} + 3\mathrm{B} \rightleftharpoons 2\mathrm{C} \\ \mathrm{II}. 2\mathrm{A}\rightleftharpoons 4\mathrm{B} \\ \mathrm{III}. \mathrm{A}+\mathrm{B}+2\mathrm{C} \rightleftharpoons 4\mathrm{D} \end{gathered}$$

Would be respectively:

N₂O₄ dissociates as ${\mathrm{N}}_2{\mathrm{O}}_4\left(\mathrm{g}\right)\rightleftharpoons 2{\mathrm{NO}}_2\left(\mathrm{g}\right)$ at 273 K and 2 atm pressure. The equilibrium mixture has a vapour density of 41. What will be the percentage degree of dissociation ?

On adding inert gas to the equilibrium ${\mathrm{PCl}}_5(\mathrm{g}) \rightleftharpoons {\mathrm{PCl}}_3(\mathrm{g}) + {\mathrm{Cl}}_2(\mathrm{g})$ at constant pressure. The degree of dissociation will :

Dissociation of phosphorus penta chloride is favoured by :

${\mathrm{N}}_2{\mathrm{O}}_4\rightleftharpoons 2{\mathrm{NO}}_2, {\mathrm{K}}_{\mathrm{c}}=4.$ This reversible reaction is studied graphically as shown in figure. Select the correct statement out of I, II and III.

I. Reaction quotient has maximum value at point A

II. Reaction proceeds left to right at a point when

     $\left[{\mathrm{N}}_2{\mathrm{O}}_4\right]=\left[{\mathrm{NO}}_2\right]=0.1M$

III. K_c=Q where point E or G is reached

The stability product constant K_sp of Mg(OH)₂ is 9.0 X 10^-12. If a solution is 0.010 M with respect to Mg²⁺ ion, what is the maximum hydroxide ion concentration which could be present without causing the precipitation of Mg(OH)₂ ?

How many grams of CaC₂O₄ (molecular weight =128) on dissolving in distilled water will give a 1 liter of a saturated solution

[K_sp (CaC₂O₄) = 2.5x10^-9 mol²l^-2

Which may be added to one litre of water to act as a buffer

Acoording to Bronsted-Lowry concept, the correct order of relative strength of bases follows the order

pOH of H₂O is 7.0 at 298K. If water is heated at 350K, which of the following statement should be true ?

In which case following equilibrium can't be established:

CaCO₃(s) $\rightleftharpoons$CaO(s) + CO₂(g)

Solubility product constant (K_sp) of salts of types MX, MX₂ and M₃X at temperature T are 4.0 X 10^-8, 3.2 X 10^-14 and 2.7 X 10^-15 respectively. Solublities(mol dm^-3) of the salts at temperature T are the order:

Ostwald dilution law for weak electrolyte HA can be given as

$$\begin{gathered} \left(1\right) {\mathrm{K}}_{\mathrm{a}}=\frac{{\mathrm{C\alpha }}^2}{(1-\mathrm{\alpha })} \\ \left(2\right) \mathrm{Ka} = {\mathrm{C\alpha }}^2 \mathrm{if} \mathrm{\alpha }\to 0 \\ \left(3\right) {\mathrm{K}}_{\mathrm{a}} = \frac{{\mathrm{C\lambda }}^2}{{\mathrm{\lambda }}^2({\mathrm{\lambda }}^2-\mathrm{\lambda })} \\ \left(4\right) \mathrm{All} \mathrm{of} \mathrm{the} \mathrm{above} \end{gathered}$$

In the reaction, N₂O₄ $\rightleftharpoons$ 2NO₂, $\mathrm{\alpha }$ is that part of N₂O₄ which dissociates, then the number of moles at equilibrium will be:

In which solution, AgCl has minimum solubility ?

50 ml of HCl (pH=1) is mixed with another 100 ml of HCl (pH=2) then pH of resulting solution will be approximately

In a nitrating mixture (HNO₃ + H₂SO₄), HNO₃ acts as

When a solution of acetic acid was titrated with NaOH, the pH of the solution when half of the acid, neutralised was 4.2. Dissociation constant of the acid is

Among the following, the strongest Lewis acid is

Calculate the molar solublity of Fe(OH)₂ at a pH of 8

[K_sp of Fe(OH)₂ = 1.6 X 10^-14]

To a 200 ml of 0.1 M weak acid HA solution 90 ml of 0.1 M solution of NaOH be added, Now, what volume of 0.1 M NaOH be added into above solution so that pH of resulting solution be 5.

[K_a(HA) = 10^-5]

If carbon dioxide is 2% dissociated at equilibrium 2CO₂ (g)$\rightleftharpoons$2CO(g) + O₂(g). The mole fraction of CO₂ at equuilibrium is

For N₂ + 3H₂ $\rightleftharpoons$2NH₃, one mole of N₂ and three moles of H₂ are at pressure of 4 atm. Equilibrium pressure is found to be 3 atm. Hence, K_p is