How many litres of water must be added to 1 litre anaqueous solution of HCl with a pH of 1 to create an aqueous solution with pH of 2?
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Solubility product constant (Ksp) of salts of types MX, MX2 and M3X at temperature T are 4.0 × 10-8, 3.2 × 10-14 and 2.7 × 10-15, respectively. Solubilities (mol dm-3) of the salts at temperature ‘T’ are in the order–
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2.5 ml of (2/5) M weak monoacidic base (Kb = 1 × 10-12 at 25°) is titrated with (2/15) M HCl in water at 25°C. The concentration of H+ at equivalence point is (Kw = 1 × 10-14 at 25°C)
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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, the value of K is :
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An acid HA ionises as HA ⇌ H+ + A– .The pH of 1.0 M solution is 5. Its dissociation constant would be :
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At 25°C, the solubility product of Mg(OH)2 is 1.0 × 10–11.At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001 M Mg2+ ions?
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Solubility product of silver bromide is 5.0 × 10-13. The quantity of potassium bromide (molar mass taken as 120 g mol-1) to be added to 1 litre of 0.05 M solution of silver nitrate to start the precipitation of AgBr is
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In aqueous solution the ionization constants for carbonic acid ar eK1 = 4.2 × 10-7 and K2 = 4.8× 10-11.Select the correct statement for a saturated 0.034 M solution of the carbonic acid.
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Solid Ba(NO3)2 is gradually dissolved in a 1.0 × 10-4 M Na2CO3 solution. At what concentration of Ba2+ will a precipitate begin to form? (Ksp for Ba2CO3 = 5.1 × 10-9)
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The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionization constant, Ka of the acid is :
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