19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
Which of the following pairs constitutes a buffer?
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. The pKb of NH4OH is
A certain buffer solution contains equal concentration of X– and HX. the Ka for HX is 10–8. The pH of the buffer is
One litre of a buffer solution containing 0.01 M NH4Cl and 0.1 M NH4OH having pKb of 5 has pH of
A buffer solution of pH 9 can be prepared by mixing
The acidic buffer solution can be prepared by mixing solutions of
Buffer solution can be obtained by mixing aqueous solution of
A mixture of a weak acid (say acetic acid) and its salt with a strong base (say sodium acetate) is a buffer solution. Which other pair of substances from the following may have a similar property ?
A certain buffer solution contains equal concentration of Xand HX. The Kb for X is 10–10. The pH of the buffer is
Calculate the pH of a buffer prepared by mixing 0.10 mol of sodium formate and 0.05 mole of formic acid in 1.0 L of solution. [HCO2H : Ka =1.8 × 10–4]
What is the pH of a buffer solution which is 0.250 M in benzoic acid, C6H5COOH, and 0.150 M in sodium benzoate, C6H5COONa, if a K for benzoic acid is 6.5 × 10–5 ?
The principal buffer present in human blood is
For preparing a buffer solution of pH 6 by mixing sodium acetate and acetic acid, the ratio of the concentration of salt and acid should be (Ka = 10 –5)
The pKb of CNis 4.7. The pH of solution prepared by mixing 2.5 mol of KCN of 2.5 mol of HCN in water and making the total volume up to 500 mL is
10–6 M NaOH is diluted by 100 times. The pH of diluted base is
K C K /C x xx a H
The pH of 0.5 M aqueous solution of HF (Ka = 2 × 10–4) is
In decimolar solution, CH3COOH is ionised to the extent of 1.3%. If log 1.3 = 0.11, what is the pH of the solution ?
At a certain temperature the value of pKw is 13.4 and the measured pH of solution is 7. The solution is
What is the pH of a 0.015 M Ba(OH)2 solution ?
An acid solution of pH = 6 is diluted hundred times. The pH the solution becomes :
A is an aqueous acid; B is an aqueous base. They are diluted separately, then
The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation ?
What will be the pH of a solution formed by mixing 40 ml of 0.10 M HCl with 10 ml of 0.45 M NaOH
x x