Equilibrium

In an equilibrium reaction, if temperature increases

For a reaction, 2NOCl(g) + Cl₂(g) , Kc at 427⁰C is 3 ˣ 10⁻⁶ L.mol⁻¹.The value of Kp is nearly

100 mL of HCl + 35 mL of NaOH, colour of methyl orange in the solution will be

Which of the following is a Lewis acid

Which of the following is a Lewis acid

The law of equilibrium was first given by

A buffer solution contains 0.1 M of acetic acid and 0.1 M of sodium acetate.What will be its pH? (pKa of acetic acid is 4.75)

In N₂ + 3H₂ → 2NH₃ reversible reaction ,increases in pressure will favour

In which of the following reaction Kp > Kc

If pH value of a solution is 3 and by adding water, it becomes 6,then the dilution is increased by

Which of the following is a characteristic of a reversible reaction

The pH of 0.001 N acetic acid solution, which is 10% dissociated, is

The equilibrium constant of a reaction is 300. If the volume of a reaction flask is trippled, the equilibrium constant will be

Which of the following is the strongest base

Which of the following indicator is known as metal indicator

If active mass of a 6% solution of a compound is 2, its molecular weight will be

The aqueous solution of which of the following salt will have the lowest pH

A solution with pH = 2 is more acidic then one with a pH = 6 , by a factor

In the reaction : I₂ + I⁻ → I₃⁻, the Lewis base is

In the gas phase reaction C₂H₂ + H₂ ⇌ C₂H₆, the equilibrium constant can be expressed in

The solubility of BaSO₄, in water, is 2.33 ˣ 10⁻³ g/L.Its solubility product will be (molecular weight of BaSO₄ = 233)

Which of the following does not acts as Lewis acid

The unit in which the solubility product of barium phosphate is expressed as

The pH value of 0.1 M NaOH solution is (when there is a given reaction [H⁺][OH⁻] = 10⁻¹⁴)

When the temperature of reactions will increases then the effect on pH value will

The pH of solution containing 0.10 M sodium acetate and 0.03 M acetic acid is (pKa for CH₃COOH = 4.57)

The solubility of CuBr is 2 ˣ 10⁻⁴ mol/L at 25⁰C. The Ksp value for CuBr is

In which one of the following is not a buffer solution

In which of the following acid – base titration,pH is greater than 8 at equivalence point

Dimethyl glyoxime gives a red precipitate with Ni²⁺ ,which is used for its detection .To get this precipitate readily the bast pH range is

For the equilibrium, H₂O(l) ⇌ H₂O(g) at 1 atm and 298 K,

What is the pH of 0.01 M glycine solution? For glycine, Ka₁ = 4.5 ˣ 10⁻³ and Ka₂ =1.7 ˣ 10⁻¹⁰ at 298 K

Of the following, which change will shift the reaction towards the product?
I₂(g) ⇌ 2 I(g) , ΔH°r (298 K) = 150 kJ

When 10 mL of 0.1 M acetic acid (pKa = 5.0 ) is titrated against 10mL of 0.1 M ammonia solution (pKb = 5.0),the equivalence point occurs at pH

For a reaction , 2NOCl(g) ⇌ 2NO(g) + Cl₂(g), Kc at 427⁰C is 3 ˣ 10⁻⁶ mol⁻¹ L. The value of Kp is nearly

40 mL of 0.1 M ammonia solution is mixed with 20 mL of 0.1 M HCl. What is the pH of the mixture? ( pKb of ammonia solution is 4.74)

The equilibrium constant for mutarotation α-D Glucose ⇌ β-D Glucose is 1.8. what percentage of a form remains at equilibrium

Ksp of CaSO₄.5H₂O is 9 ˣ 10⁻⁶, find the volume for 1g of CaSO₄ (M.wt, = 136)

Which of the following is not a characteristic of equilibrium

Which one of the following is most soluble

The pH value of blood does not appreciably change by a small addition of an acid or a base,because the blood

The pH value of a 10 M solution of HCl is

The solubility of AgCl will be minimum in

In liquid-gas equilibrium,the pressure of vapours above the liquid is constant at

If α is dissociation constant, then the total number of moles for the reaction 2HI ⇌ H₂ + I₂ will be

A physician wishes to prepare a buffer solution at pH = 3.85 that efficiently resists changes in pH yet contains only small concentration of the buffering agents. which of the following weak acids together with its sodium salt would be best to use

The strongest conjugate base is

The concentration of [H⁺] and [OH⁻] of a 0.1 M aqueous solution of 2% ionised weak acid is [ionic product of water = 1 ˣ 10⁻¹⁴]

The solubility of saturated solution of calcium fluoride is 2 ˣ 10⁻⁴ moles per litre.Its solubility product is

Correct relation between dissociation constant of a dibasic acid is

For a reversible reaction, if we increase concentration of the reactants, then effect on equilibrium constant

Which statements is wrong about pH and H⁺

In HS⁻, I⁻, R-NH₂, NH₃ order of proton accepting tendency will be

Ionisation constant of CH₃COOH is 1.7 ˣ 10⁻⁵ and concentration of H⁺ ions is 3.4 ˣ 10⁻⁴.Then find out initial concentration of CH₃COOH molecules

Solubility of M₂S salt is 3.5 ˣ 10⁻⁶ then find out solubility product

Reaction BaO₂(s) ⇌ BaO(s) + O₂(g) ; ΔH = +ve.In equilibrium condition, pressure of O₂ depends on

Solubility of MX₂ – type electrolytes is 0.5 ˣ 10⁻⁴ mol/L., then fine out Ksp of electrolytes

Which has highest pH

Solution of 0.1 N NH₄OH and 0.1 N NH₄Cl has pH 9.25 . Then fine out pKb of NH₄OH

IN Haber process 30 L of dihydrogen and 30 L of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end

The solubility product of AgI at 25⁰C is 1.0 ˣ 10⁻¹⁶ mol² L⁻². The solubility of AgI in 10⁻⁴ N solution of KI at 25⁰C is approximately (in mol L⁻¹)

The solubility product of a sparingly soluble salt AX₂ is 3.2 ˣ 10⁻¹¹.Its solubility (in mol/L)is

The rapid change of pH near the stoichiometric point of an acid-base titration is the basis of indicator detection.pH of the solution is related to ratio of the concentrations of the conjugate acid (HIn) and base (In⁻) forms of the indicator by the expression

At 25⁰C, the dissociation constant of a base, BOH, is 1.0 ˣ 10⁻¹². The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

What is the [OH⁻] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 M Ba(OH₂)

If pH of a saturated solution of Ba(OH)₂ is 12, the value of its Ksp is

In a buffer solution containing equal concentration of B⁻ and HB, the Kb for B⁻ is 10⁻¹⁰.The pH of buffer solution is