19,000+ solved questions for JEE Advanced, JEE Mains, NEET & IChO — with answers and expert explanations.
The pH of a solution is increased from 3 to 6; its H + ion concentration will be :
A solution contains 10ml of 0.1 N NaOH and 10 ml of 0.05 Na2SO4. pH of this solution is
A solution of an acid has pH = 4.70. Find out the concentration of OH– ions (pKw = 14)
2 1 [OH [O / 2 10 OH x x x x
The pH value of 0.1 M hydrochloric acid is approximately 1. The approximate pH value of 0.05 M sulphuric acid is most likely to be
What will be the pH of the solution obtained by mixing 10 cc of N/10 HCl and 10 cc of N/10 NaOH ?
x x
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
The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation ?
A is an aqueous acid; B is an aqueous base. They are diluted separately, then
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 ?
Buffer solution can be obtained by mixing aqueous solution of
The acidic buffer solution can be prepared by mixing solutions of
A buffer solution of pH 9 can be prepared by mixing
One litre of a buffer solution containing 0.01 M NH4Cl and 0.1 M NH4OH having pKb of 5 has pH of
A certain buffer solution contains equal concentration of X– and HX. the Ka for HX is 10–8. The pH of the buffer is
Solution of 0.1 N NH4OH and 0.1 N NH4Cl has pH 9.25. The pKb of NH4OH is
Which of the following pairs constitutes a buffer?
Consider the following solutions of equal concentrations. A = NH4Cl B = CH3COONa C = NH4OH D = CH3COOH A buffer solution can be obtained by mixing equal volumes of
The pKa value of NH3 is 5. Calculate the pH of the buffer solution, 1 L of which contains 0.01 M NH4Cl and 0.10 M NH4OH
The concentration of Ag+ ion in a given saturated solution of AgCl at 25ºC is 1.06 × 10–5g ion per litre. Thus the solubility product of AgCl is
The solubility product of barium sulphate is 1.5 × 10–9 at 18ºC. Its solubility in water at 18ºC is
The solubility of AgCl at 20ºC is 1.435 × 10–3gm/lit. The solubility product of AgCl is
How many grams of CaC2O4 will dissolve in distilled water to make one litre of saturated solution of it ? (Ksp for CaC2O4 = 2.5 × 10–9mol2 lit–2)
The solubility of BaSO4 in water is 2.33 × 10–3g L–1.Its solubility product will be (molecular weight of BaSO4 = 223)