The pH of a solution of H2O2 is 6.0, Some chlorine gas is bubbled into this solution. Which of the following is correct
A. The pH of resultant solution becomes 8.0
B. Hydrogen gas is liberated from resultant solution
C. The pH of resultant solution becomes less than 6.0 and oxygen gas is liberated
D. Cl2O is formed in the resultant solution
Study the following table: Buffer solution Volume(in ml) of 0.M weak Volume(in ml) of 0.1 M sodium salt of weak acid I 4.0 4.0 II 4.0 40.0 III 40.0 4.0 IV 0.1 10.0 Which of the two sets of buffer solutions have least pH?
A. I and II
B. I and III
C. II and III
D. II and IV
Assertion (A): The PH of a buffer solution containing equal moles of acetic acid and sodium acetate is 4.8 (pKa of acetic acid is 4.8)Reason (R): The ionic product of water at 250C is l0-14 mol2 .L-2. The correct answer is
A. Both (A) and (R) are true and (R) is the correct explanation of (A)
B. Both (A) and (R) are true and (R) is not the correct explanation of A
C. (A) is true but (R) is not true
D. (A) is not true but (R) is true
When 9.65 Coulombs of electricity is passed through a solution of AgN03 (atomic weight of silver 108), the amount of silver deposited is
A. 10.8mg
B. 5.4mg
C. 16.2mg
D. 21.2mg
If in a 100 mL of an aqueous HC1 of pH 1.00, 900 mL of more distilled water is added, the pH of the resultant solution will be :
A. 1.0
B. 2.0
C. 4.0
D. 7.0
The degree of dissociation of an acid HA in 0.1 M solution is 0.1%. Its dissociation constant is ;
A. 1 xl0-3
B. lx10-7
C. 1 x10-10
D. lx10-14
Which of the following is not a conjugate acid-base pair
A. HPO32- , PO33-
B. H2PO-4 ,HPO42-
C. H2PO-4 , H3PO4
D. H2PO-4 , PO33-
Which one of the following salts give an acidic solution in water
A. CH3COONa
B. NH4Cl
C. NaCl
D. CH3COONH4
The equilibrium constant for the reactionSO2(g) + (1/2) O2(g) <====> SO3(g) is 5 x 10-2 atm The equilibrium constant of the reaction2SO3(g) <====> 2SO2(g) + O2(g) would be
A. 100 atm
B. 200 atm
C. 4 x 102 atm
D. 6.25x 104 atm
The concentration of oxalic acid is 'x'mol L-1. 40 mL of this solution reacts with 16 mL of 0.05 M acidified KMn04. What is the pH of 'x' M oxalic acid solution ? (Assume that oxalic acid dissociates completely)
A. 1.3
B. 1.699
C. 1
D. 2
pH of a buffer solution decreases by 0.02 units when 0.12 g of acetic acid is added to 250 ml of a buffer solution of acetic acid and Potassium acetate at 270C. The buffer capacity of the solution is
A. 0.1
B. 10
C. 1
D. 0.4
The equilibrium constants for the reactions N2(g)+O2(g)⇔2NO(g) and NO(g)+1/2 O2(g) are K1 and K2 respectively .Then the equilibrium constant for the reaction N2(g)+O2(g)⇔2NO2(g) is
A. K1/K2
B. K12-K22
C. K1 x K22
D. K1 - K22
The solubility of LiOH in a solution of pH = 8 = is Ksp = 1.8 x 10-12
A. 1.8 x 10-18
B. 1.8 x 10-6
C. 1.3 x 10-5
D. 1.8 x 10-4
Assertion(A): A catalyst has no effect on the state of equilibrium Reason:A catalyst influences the rates of both forward and backward reactions to the same extent
A. Both A and R are true and R is not correct explanation of A
B. Both A and R are true and R is not correct explanation of A
C. A is true R is false
D. R is true A is false
The order of pH of 0.200 M solutions of NH4NO3, NaNO3 and Na2CO3 is
A. NH4NO3 < Na2CO3 < NaNO3
B. NH4NO3 < NaNO3 < Na2CO3
C. Na2CO3 < NaNO3 < NH4NO3
D. NaNO3 < NH4NO3 < Na2CO3
Which one of the following statements is correct
A. Bronsted - Lowry theory could not explain the acidic nature of BCl3
B. The pH of 0.01 M NaOH solution is 2
C. The ionic product of water at 250C is 10-10 mol2, L-2
D. The pH of a solution can be calculated using the equation pH = log [H+]
75 ml of 0.2 M HCl is mixed with 25 ml of 1 M HCl. To this solution, 300 ml of distilled water is added. What is the pH of the resultant solution
A. 1
B. 2
C. 4
D. 0.2