The pH of a solution obtained by mixing 100ml of 0.2 M CH₃COOH with 100ml of 0.2 M NaOH would be (given pKa for CH₃COOH = 4.74)

A 20 litre container at 400 K contains CO₂(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 the pressure of CO₂ attains its maximum value, when the pressure of C02 attains its maximum value, will be

(Given that: SrCO₃(s) $\rightleftharpoons$ SrO(s) + CO₂(g), (Kp =1.6 atm))

Concentration of the Ag⁺ ions in a saturated solution of Ag₂C₂O₄ is 2.2 x 10^-4 mol^-1 solubility product of Ag₂C₂O₄ is

The percentage of pyridine (C₅H₅N) that forms pyridinium ion (C₅H₅N⁺H) in a 0.10 M aqueous pyridine solution (K_b for C₅H₅N = 1.7 x 10^-9) is

The solubility of AgCl (s) with solubility product 1.6 x 10^-10 in 0.1 M NaCl solution would be

Boric acid is an  acid because its molecule

Which of the following fluoro-compounds is most likely to behave as a Lewis base?

Among the following, the correct order of acidity is

MY and NY₃ , two nearly insoluble salts, have the same Ksp values of 6.2 x 10^-13 at room

temperature. Which statement would be true in regard to MY and NY₃?

solubilities

The Ksp of Ag₂CrO₄, AgCl, AgBr and Agl are, respectively, 1.1x10^-12, 1.8x10^-10, 5.0x10^-13, and 8.3x10^-17. The salt precipitates that last if the AgNO₃ solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na₂CrO₄ is -

Which of the following statements is correct for a reversible process in a state of

equilibrium?

The pH of the resulting solution when equal volumes of 0.1 M NaOH and 0.01 M HCl are mixed is:

Among the following pairs of solution the one which is not an acidic buffer is 

For the reversible reaction, N₂(g) + 3H₂(g) — 2NH₃(g) + Heat the equilibrium shifts in

forward direction

PCl₅ is 50% dissociated at $20°\mathrm{C}$ and 1 atm pressure. The value of K_p is

For a given exothermic reaction, K_p and K'_p are the equilibrium constants at temperatures

T₁ and T₂ respectively. Assuming that heat of reaction is constant in a temperature range

between T₁ and T₂, it is readily observed that

Buffer solutions have constant acidity and alkalinity because

The molecule that is least likely to behave as Lewis base is: 

In which of the following equilibrium K_c and K_p are not equal?

Which one of the following molecular hydrides acts as a Lewis acid?

Which of the following molecules acts as a Lewis acid ?

The ionisation constant of ammonium hydroxide is 1.77 x 10^-5 at 298 K. Hydrolysis constant of ammonium chloride is

The oxide that is not expected to react with sodium hydroxide is : 

The dissociation constants for acetic acid and HCN at 25$°$C are 1.5 xl0^-5 and 4.5 xl0^-10,

respectively. The equilibrium constant for the equilibrium,

CN^- + CH₃COOH  =    HCN + CH₃COO^-   would be

the H⁺ ion concentration in the mixture?

1. 1.11 x 10^-4 M             

The value of equilibrium constant of the reaction HI (g) $\rightleftharpoons$ $\frac{1}{2}$ H₂(g) + $\frac{1}{2}$ I₂(g) is 8.0. The equilibrium constant of the reaction

H₂(g) + I₂(g) $\rightleftharpoons$2HI(g) will be

$$\begin{gathered} 1. \frac{1}{16} \\ 2. \frac{1}{64} \\ 3. 16 \\ 4. \frac{1}{8} \end{gathered}$$

Which one of the following ionic species has the greatest proton affinity to form stable compound?

For the reaction,

 CH₄(g) + 2O₂(g) $\rightleftharpoons$CO₂(g) + 2H₂O (l),

 $∆$_rH = -170.kJ mol-1

Which of the following statements is not true?

(a) At equilibrium, the concentrations of CO₂(g) and H₂O(l) are not equal

(b) The equilibrium constant for the reaction is given by K_p = [CO₂]/CH₄][O₂]

(c) Addition of CH₄(g) or O₂ (g) at equilibrium will cause a shift to the right

(d) The reaction is exothermic

The hydrogen ion concentration of a 10^-8 M HCl aqueous solution at 298 K (K_w = 10^-14) is:

The equilibrium constant for the reaction 

$N{H}_{4}N{O}_2\left(s\right)$$N_2\left(g\right) + 2H_{2}O\left(g\right)$ is given by

Two flasks A and B of equal volume containing 1 mole and 2 mole of O₃ respectively, are heated to the sametemperature. When the reaction 2O₃ $\underset{}{\overset{}{\leftrightharpoons }}$3O₂ practically stops, then both the flasks shall have

A 10L container at 300K contains CO₂ gas at pressure of 0.2 atm and an excess solid CaO (neglect thevolume of solid CaO). The volume of container is now decreased by moving the movable piston fitted in the container. What will be the maximum volume of container when pressure of CO₂ attains its maximum value given that CaCO₃ (s) $\underset{}{\overset{}{\leftrightharpoons }}$ CaO(s) + CO₂(g)K_ph = 0.800 atm

An equilibrium mixture at 700 K of 0.50 M N₂, 3.00 M H₂ and 2.00 M NH₃ is present in a container. Now if this equilibrium is disturbed by adding N₂ so that its concentration becomes 1.50 M just after addition then which of the following graphs represents the above situation more appropriately –

At 1400 K, K_c= 2.5x10^-3 for the reaction CH₄(g) + 2H₂S(g) $\underset{}{\overset{}{\rightleftharpoons }}$ CS₂(g) + 4H₂(g). A 10.0L reaction vesselat 1400 K contains 2.00 mole of CH₄, 3.0 mol of CS₂, 3.0 mole of H₂ and 4.0 mole of H₂S. Then

The graph which will be representing all the equilibrium concentrations for the reaction N₂O₄(g) $\underset{}{\overset{}{\rightleftharpoons }}$ 2NO2 (g) will be : (the concentrations of N₂O₄ (g) and of NO (g) for which the following reaction will be at equilibrium will lie:

For the chemical equilibrium, CaCO₃(s) $\stackrel{}{\rightleftharpoons }$ CaO(s) + CO₂ (g) ΔH_f° can be determined from which one of the following plots ?

At a certain temperature the following equilibrium is established, CO(g) + N0₂(g) $\stackrel{}{\rightleftharpoons }$ CO₂(g)+ NO(g)One mole of each of the four gas is mixed in one litre container and the reaction is allowed to reach equilibrium state. When excess of baryta water (Ba(OH)₂) is added to the equilibrium mixture, the weight of white ppt (BaCO₃) obtained is 236.4 gm. The equilibrium constant K_c of the reaction is (Ba = 137)

At temperature T^, the compound AB₂ (g) dissociates according to the reaction, 2AB₂ (g) $\stackrel{}{\rightleftharpoons }$ 2 AB(g) + B₂(g). With a degree of dissociation x^, which is small compared with unity. Deduce the expression for x in terms of the equilibrium constant, K_p and the total pressure, P.

Equilibrium constant for the given reaction is kc = 10²⁰ at temperature 300 K,A(s) + 2B (aq.) $\stackrel{}{\rightleftharpoons }$ 2C (s) + D (aq.)K = 10²⁰ The equilibrium conc. of B starting with mixture of 1 mole of A and 1/3 mole/litre of B at 300 K is

10L box contain O₃ and O₂ at equilibrium at 2000 K. The ΔG° = –534.52 kJ at 8 atm equilibrium pressure.The following equilibrium is present in the container. 2O₃(g) $\stackrel{}{\rightleftharpoons }$ 3O₂(g). The partial pressure of O₃ will be (ln 10 = 2.3, R = 8.3 Jmole^–1K^–1):

Solid ammonium carbamate dissociates to give ammonia and carbon dioxide as follows:

NH₂COONH₄(s) $\stackrel{}{\rightleftharpoons }$ 2 NH3(g) + CO₂(g) At equilibrium, ammonia is added such that partial pressures of NH3 now equals the original total pressure. Calculate the ratio of the total pressures now to the original total pressure.

The reactions, PCl₅ (g) $\stackrel{}{\rightleftharpoons }$ PCl₃(g) + Cl₂(g) and COCl₂(g) $\stackrel{}{\rightleftharpoons }$ CO(g) + Cl₂(g) are simultaneously in equilibrium in an equilibrium box at constant volume. A few moles of CO(g) are later introduced into the vessel. After some time, the new equilibrium concentration of

In the Haber process for the industrial manufacture of ammonia involving the reaction, N₂ + 3H₂ $\stackrel{}{\rightleftharpoons }$ 2NH₃ at 200 atm pressure in the presence of a catalyst, temperature of about 500°C. This is considered as optimum temperature for the process because

What is the minimum mass of CaCO3 (s), below which it decomposes completely, required to establish equilibrium in a 6.50 litre container for the reaction : [ K_C = 0.05 mole/litre]

CaCO₃ (s) $\stackrel{}{\rightleftharpoons }$ CaO(s) + CO₂(g)

The value of k_p for the reaction at 27°C Br₂(l) + Cl₂(g) $\stackrel{}{\rightleftharpoons }$ 2BrCl(g) is '1 atom'. At equilibrium in a closed container partial pressure of BrCI gas is 0.1 atm and at this temperature the vapour pressure of Br₂(l) is also 0.1 atm. Then what will be minimum moles of Br₂(l) to be added to 1 mole of Cl₂ , initially, to get above equilibrium situation :

5 mol PCI₅(g) and one mole N₂ gas is placed in a closed vessel. At equilibrium PCI₅(g) decomposes 20% and total pressure in to the container is found to be 1 atm. The k_P for equilibrium

PCl5(g) $\stackrel{}{\rightleftharpoons }$ PCl₃(g) + Cl₂(g)

Which one is the correct expression below for the solution containing 'n' number of weak acids?

The pH of glycine at the first half equivalence point is 2.34 and that at second half equivalence point is 9.60.At the equivalence point (The first inflection point) The pH is :

A 1.458 g of Mg reacts with 80.0 ml of a HCI solution whose pH is –0.477. The change in pH after all Mg has reacted. (Assume constant volume. Mg = 24.3 g/mol.)(log 3 = 0.477)

Find the $∆$pH (initial pH –final pH) when 100 ml 0.01 M HCl is added in a solution containig 0.1 m molesof NaHCO₃ solution (pH = 9 ) of negligible volume ( K_ai =10^–7, K_a, =10^–11 for H₂CO₃) :