JEE Questions for Chemistry Equilibrium Quiz 4 - MCQExams.com

At 30oC, the solubility of Ag2 CO3 (Ksp = 8 × 10-12) would be greatest in 1 L of
  • 0.05 M Na2 CO3
  • 0.05 M AgNO3
  • pure water
  • 0.05 M NH3
The Ksp of Ca3 (PO4)2 is
  • [Ca2+][PO43-]2
  • [Ca2+]3 [PO43-]
  • [Ca2+][PO43-]
  • [Ca2+]3 [PO43-]2
If solubility of calcium hydroxide is √3, then its solubility product will be
  • 27
  • 3
  • 9
  • 12√3
The molar solubility (in mol L-1) of a sparingly soluble salt MX4 is 's'. The corresponding solubility product is KSP. S is given in terms of KSP by the relation
  • S = (KSP 1/28)1/4
  • S = (128 KSP)1/4
  • S = (256 KSP)1/5
  • S = (KSP/256)1/5
Solubility of Al(OH)3 = s, Ksp will be
  • 108 S3
  • 27 S3
  • 4 S4
  • 27 S4
The solubility of AgI in NaI solution is less than that in pure water because
  • the temperature of the solution decreases
  • solubility product of AgI is less than that of NaI
  • of common ion effect
  • AgI forms complex with NaI
The solubility of Pb(OH)2 in water is 6.7 × 10-6 M. Its solubility in a buffer solution of pH = 8 would be
  • 1.2 × 10-2
  • 1.6 × 10-3
  • 1.6 × 10-2
  • 1.2 × 10-3
The solubility of Sb2 S3 in water is 1.0 ×10-5 mol / L at 298 K. What will be its solubility product ?
  • 108 × 10-25
  • 1.0 × 10-25
  • 144 × 10-25
  • 126 × 10-24
A precipitate of AgCl is formed when equal volumes of the following are mixed.
[KSP for AgCl = 10-10]
  • 10-4 M AgNO3 and 10-7 M HCl
  • 10-5 M AgNO3 and 10-6 M HCl
  • 10-5 M AgNO3 and 10-4 M HCl
  • 10-6 M AgNO3 and 10-6 M HCl
The correct expression for the solubility product of Ca3(PO4 )2 is
  • 108 s5
  • 27 s5
  • 16 s4
  • 81 s4
On adding 0.1 M solution each of [Ag+],[Ba2+], [Ca2+] in a Na2SO4 solution species first precipitated is (KSP BaSO4 = 10-11, KSP CaSO4 = 10-6, KSP AgSO4 = 10-5)
  • Ag2SO4
  • BaSO4
  • CaSO4
  • All of the above
In the titration of NaOH and HCl, which of the following indicator will be used ?
  • Methyl orange
  • Methyl red
  • Both (and (2)
  • None of these
A strong acid is titrated with weak base. At equivalence point, pH will be
  • < 7
  • > 7
  • = 0
  • cannot predict
For the titration of solution of oxalic acid and sodium hydroxide, the suitable indicator is
  • phenolphthalein
  • methyl orange
  • any of these
  • None of these
Which one of the following salts will produce an alkaline solution while dissolving in water?
  • NH4Cl
  • Na2CO3
  • NaNO3
  • Na2SO4
The aqueous solutions of HCOONa, C6H5NH3Cl and KCN are respectively
  • acidic, acidic, basic
  • acidic, basic, neutral
  • basic, neutral, neutral
  • basic, acidic, basic
In the titration of Na2CO3 and HCl, the indicator used is
  • methyl orange
  • methylene blue
  • phenolphthalein
  • litmus
Relation between hydrolysis constant and dissociation constant are given. Which is the correct formula for MgCl2?

  • Chemistry-Equilibrium-3522.png
  • 2)
    Chemistry-Equilibrium-3523.png

  • Chemistry-Equilibrium-3524.png

  • Chemistry-Equilibrium-3525.png
Which one of the following pair shows buffer's solution?
  • NaCl + NaOH
  • CH3COONa + CH3COOH
  • CH3 COOH + CH3 COONH4
  • H2SO4 + CuSO4
For a reversible reaction, if the concentration of the reactants are doubled, the equilibrium constant will be
  • The same
  • Halved
  • Doubled
  • One fourth
For the reaction SO2 (g) + 1/2 O2 (g) ⇌ SO3 (g)
if, Kp = Kc (RT)x
where, the symbols have usual meaning, then the value of x is (assuming ideality)
  • - 1
  • - (1/2)
  • 1/2
  • 1
The rate constant for forward reaction and backward reaction of hydrolysis of ester are 1.1 ×10-2 and 1.5 × 10-3 per minute, respectively. Equilibrium constant for the reaction
CH3COOC2H5 + H2O ⇌ CH3COOH + C2H5OH is
  • 33.7
  • 7.33
  • 5.33
  • 33.3
In reaction A + B ⇌ C + D, 40 % of B has reacted at equilibrium, when 1 mole of A was heated with 1 mole of B in a 10 L closed vessel.
The value of KC is
  • 0.44
  • 0.18
  • 0.22
  • 0.36
The mixture of reactants and products in the equilibrium state is called
  • chemical mixture
  • equilibrium mixture
  • chemical equilibrium
  • dynamic equilibrium
The equilibrium constant (KC) for the reaction
N2 (g) + O2 (g) → 2NO (g) at temperature T, is 4 × 10-4. The value of KC for the reaction NO (g) → 1/2 N2 (g) + 1/2 O2 (g) at the same temperature is
  • 0.02
  • 2.5 × 102
  • 4 × 10-4
  • 50.0
For 2NOBr (g) ⇌ 2NO (g) + Br2 (g), at equilibrium PBr2 = P/9 and p is the total pressure, the ratio KP/ P will be
  • 1/3
  • 1/9
  • 1/27
  • 1/81
A vessel at 1000 K contains CO2 with a pressure of 0.5 atm. Some of the CO2 is converted into CO on the addition of graphite. If the total pressure at equilibrium is 0.8 atm, then the value of KP is
  • 1.8 atm
  • 3 atm
  • 0.3 atm
  • 0.18 atm
4 moles of PC15 are heated in a closed 4 dm3 container to reach equilibrium at 400 K. At equilibrium, 50% of PCl5 is dissociated. What is the value of KC for the dissociation of PCl5 into PCl3 and Cl2 at 400 K?
  • 0.50
  • 1.00
  • 1.15
  • 0.05
  • 0.25
In aqueous solution, the ionisation constants for carbonic acid are
K1 = 4.2 × 10-7 and K2 = 4.8 × 10-11
Select the correct statement for a saturated 0.034M solution of the carbonic acid.
  • The concentration of CO2-3 is 0.034M
  • The concentration of CO2-3 is greater than that of HCO-3
  • The concentration of H+ and HCO-3 are approximately equal
  • The concentration of H+ is double that CO2-3
NH4 HS (s) ⇌ NH3 (g) + H2 S (g)
In the above reaction, if the pressure at equilibrium and at 300 K is 100 atm, then what will be the equilibrium constant KP ?
  • 2500 atm2
  • 50 atm2
  • 100 atm2
  • 200 atm2
For which one of the following reactions KP = KC ?
  • PCl5 ⇌ PCl3 + Cl2
  • N2 + O2 ⇌ 2NO
  • N2 + 3H2 ⇌ 2NH3
  • 2SO3 ⇌ 2SO2 + O2
The equilibrium constant KP1 and KP2 for the reactions
X ⇌ 2Y and Z ⇌ P + Q, respectively are in the ratio of 1 : 9. If the degree of dissociation of X and Z be equal, then the ratio of total pressure at these equilibria is
  • 1 : 36
  • 1 : 1
  • 1 : 3
  • 1 : 9
In a 500 mL flask, the degree of dissociation of PCl5 at equilibrium is 40% and the initial amount is 5 moles. The value of equilibrium constant (in mol L-1) for the decomposition of PCl5 is
  • 2.33
  • 2.66
  • 5.32
  • 4.66
1.6 moles of PCl5 (g) is placed in 4 dm3 closed vessel. When the temperature is raised to 500 K, it decomposes and at equilibrium, 1.2 moles of PCl5 (g) remains. What is the KC value for the decomposition of PCl5 (g) into PCl3 (g) and Cl2 (g) at 500 K ?
  • 0.013
  • 0.050
  • 0.033
  • 0.067
  • 0.045
CO (g) + 1/2 O2 (g) → CO2 (g) For the above reaction in gaseous phase, the value of KP/KC is
  • (RT)1/2
  • (RT)-1/2
  • (RT)
  • (RT)-1
Ammonium carbonate decomposes as
NH2COONH4 (s) ⇌ 2NH3 (g) + CO2 (g)
For the reaction, KP = 2.9 × 10-5 atm3 . If we start with 1 mole of compound, the total pressure at equilibrium would be
  • 0.766 atm
  • 0.0581 atm
  • 0.0388 atm
  • 0.0194 atm
The equilibrium constant (KP) for the decomposition of gaseous H2O as
H2O (g) ⇌ H2 (g) + 1/2 O2 (g)
is related to degree of dissociation (α) at a total pressure p is given by

  • Chemistry-Equilibrium-3528.png
  • 2)
    Chemistry-Equilibrium-3529.png

  • Chemistry-Equilibrium-3530.png

  • Chemistry-Equilibrium-3531.png
1 mole of H2 and 2 moles of I2 are taken initially in 2 L vessel. The number of moles of H2 at equilibrium is 0.2. Then, the number of moles of I2 and HI at equilibrium respectively are
  • 1.2, 1.6
  • 1.8, 1.0
  • 0.4, 2.4
  • 0.8, 2.0
4 moles of SO2 and O2 gases are allowed to react to form SO3 is closed vessel. At equilibrium, 25% of O2 is used up. The total number of moles of all the gases at equilibrium is
  • 6.5
  • 7.0
  • 8.0
  • 2.0
For an equilibrium reaction, N2O4 (g) ⇌ 2NO2 (g), the concentrations of N2O4 and NO2 at equilibrium are 4.8 × 10-2 and 1.2 × 10-2 mol/L, respectively. The value of KC for the reaction is
  • 3 × 10-3 mol/L
  • 3.3 × 10-3 mol/L
  • 3 × 10-1 mol/L
  • 3.3 × 10-1 mol/L
If 200 mL of a 0.031 molar solution of H2SO4 are added to 84 mL of a 0.150 M KOH solution, what is the value of pH of the resulting solution?
  • 12.4
  • 1.7
  • 2.2
  • 10.9
What will be the pH of a solution formed by mixing 10 mL of 0.1 M H2SO4 and 10 mL of N/10 KOH ?
  • 11.40
  • 8.64
  • 1.00
  • 7.00
How much is the pH of human blood ?
  • 5.2
  • 8.3
  • 6.3
  • 7.4
The concentration of hydrogen ion in a sample of soft drink is 3.8 × 10-3 M. What is its pH ?
  • 3.84
  • 2.42
  • 4.44
  • 1.42
The equilibrium constant for the reaction.
2NO2 (g) ⇌ 2NO (g) + O2 (g) is 2 × 10-6 at 185oC
Then the equilibrium constant for the reaction,
4NO (g) + 2O2 (g) ⇌ 4NO2 (g) at the same temperature would be
  • 2.5 × 10-5
  • 4 × 10-12
  • 2.5 × 10-11
  • 2 × 106
  • 5 × 105
How many litres of water must be added to 1 L of an aqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?
  • 0.1 L
  • 0.9 L
  • 2.0 L
  • 9.0 L
By adding 20 mL of 0.1 N HCl to 20 mL of 0.001 N KOH, the pH of the obtained solution will be
  • 2
  • 1.3
  • 0
  • 7
The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionisation constant, Ka of the acid is
  • 3 × 10-1
  • 1 × 10-3
  • 1 × 10-5
  • 1 × 10-7
If Ka of HCN= 4 x 10-10, then the pH of 2.5 x 10-1 molar HCN (aq) is
  • 1
  • 2.5
  • 4
  • 5
On adding which of the following, the pH of 20 mL of 0.1 N HCl will not alter ?
  • 20 mL of distilled water
  • 1 mL of 0.1 N NaOH
  • 500 mL of HCL of pH = 1
  • 1 mL of 1 N HCL
0:0:1


Answered Not Answered Not Visited Correct : 0 Incorrect : 0

Practice Chemistry Quiz Questions and Answers