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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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Important Questions on Equilibrium

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The pKa of a weak acid (HA) is 4.5. The pOH of an aqueous buffered solution of HA in which 50% of the acid is ionized is
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In a saturated solution of the sparingly soluble strong electrolyte AgIO3 (Molecular mass= 283), the equilibrium which sets in is

AgIO3 (s)  Ag+ (aq) + IO3- (aq)

If the solubility product constant Ksp of AgIO3 at a given temperature is 1.0×10-8, what is the mass of AgIO3 contained in 100 ml of its saturated solution?

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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? KsfoBaCO3=5.1×10-9
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Three reactions involving H2PO4- are given below:
i H3PO4+H2OH3O++H2PO4-
ii H2PO4-+H2OHPO42-+H3O+
iii H2PO-4+OH-H3PO4+O2-
In which of the above, does H2PO4 -act as an acid?
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In aqueous solution, the ionization constants for carbonic acid are K1=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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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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At 25oC, the solubility product of MgOH2 is 1.0×1011. At what pH, will Mg2+ ions start precipitating in the form of MgOH2 from a solution of 0.001MMg2+ ions?
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What is the best description of the change that occurs when Na2O(s) is dissolved in water?