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Class XI Chemistry Equilibrium 4
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Question 1
50 ml of 0.6 M NaOH is added to 100 ml of 0.6 M acetic acid. What is the additional volume of 1.2 M NaOH required for making the solution of pH 4.74?
The ionization constant of acetic acid is 1.8 × 10–5
The ionization constant of acetic acid is 1.8 × 10–5
Question 2
The pH of a solution obtained by mixing 100 ml of 0.2 M CH3COOH with 100 ml of 0.2 M NaOH would be (
= 4.74)
= 4.74) Question 3
Calculate pH of 10–2M Ba(Lac)2.
(Given
= 10–4)
(Given
= 10–4)Question 4
In a reaction, 
, the concentration of N2, O2 and NO are 0.25 M, 0.2 M, 2.0 M at equilibrium. The initial concentration of N2 and O2 respectively are (assuming there are was no NO in the reaction mixture when the reaction started) -
, the concentration of N2, O2 and NO are 0.25 M, 0.2 M, 2.0 M at equilibrium. The initial concentration of N2 and O2 respectively are (assuming there are was no NO in the reaction mixture when the reaction started) -Question 5
What is the pH of 0.1M NaHCO3?
If K1 = 4.5 × 10–7, K2 = 4.5 × 10–11 for carbonic acids. (Given: log2 = 0.3, log3 = 0.48)
If K1 = 4.5 × 10–7, K2 = 4.5 × 10–11 for carbonic acids. (Given: log2 = 0.3, log3 = 0.48)
Question 6
From a weak acid of pKa = 6, the pH range of practically possible buffer solution is -
Question 7
If pH of an aqueous solution of Ca (OH)2 is 12. If the Ksp of Ca(OH)2 is 9 × 10–6 then the concentration of Ca2+ ions in the solution in
mole L–1 is -
mole L–1 is -
Question 8
10 ml of 0.2M acid is added to 250 ml of a buffer solution with pH = 6.34. The pH of the solution becomes 6.32. The buffer capacity of the solution is
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Aug 22JEE & BITSAT
