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
One dm3 solution containing 10–5 moles each of Cl– ions and CrO4–2 ions is treated with 10–4 mole of silver nitrate. Which one of the following observations is made? [KSP of Ag2CrO4 = 4 × 10–12] [KSP of AgCl = 1 × 10–10] |
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The first and second dissociation constants of an acid H2A are 1.0 × 10–5 and 5.0 × 10–10 respectively.The overall dissociation constant of the acid will be |
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pH value of which one of the following is NOT equal to one? |
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Hydroxyl ion concentration of 1M HCl is |
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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 BaCO3 = 5.1 × 10–9) |
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If, in the reaction N2O4 ⇌ 2NO2, $x$ is that part of N2O4 which dissociates, then the number of molecules at equilibrium will be |
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The solubility of Ca3(PO4)2 in water is y moles/litre. Its solubility product is |
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Consider the following gaseous equilibria with equilibrium constants K1 and K2 respectively. SO2(g) + $\dfrac{1}{2}$O2(g) ⇌ SO3(g) 2SO3(g) ⇌ 2SO2(g) + O2(g) The equilibrium constants are related as ______. |
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Three reactions involving H2PO– (i) H3PO4 + H2O → H3O+ + H2PO– (ii) H2PO– (iii) H2PO– In which of the above does H2PO– |
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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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