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Question

Chemistry Question on Equilibrium

Which of the following equations give ionic product of water? (i) NH3(aq)+H2O<=>NH4(aq)++OH(aq) { NH_{3(aq)} + H_2 O <=> NH^+_{4(aq)} + OH^{-}_{(aq)}} (ii) NH4(aq)++H2O<=>H3O++NH3(aq) { NH^+_{4(aq)} + H_2 O <=> H_3O^+ + NH_{3(aq)}} (iii) NH2(aq)+H2O<=>NH3(aq)+OH { NH^{-}_{2(aq)} + H_2 O <=> NH_{3(aq)} + OH^-} (iv) NH3(aq)+OH(aq)<=>NH2(aq)+H2O { NH_{3(aq)} + OH^{-}_{(aq)} <=> NH^{-}_{2(aq)} + H_2O}

A

ii and iii

B

iii and iv

C

i and ii

D

iii and i

Answer

i and ii

Explanation

Solution

option i) and ii) are the correct ones.

So, the very first two equations

NH3 (aq) + H2o → NH4+ (aq) + OH-

And

NH4+ (aq) + H2o → H3o+ + NH3 (aq)

Give the ionization form of water as a product.

The result of the ion concentrations in water is represented by the constant known as the ionic product. Water's ionic byproduct is referred to as Kw.

As the temperature rises, the value climbs, suggesting that the concentration of H+ and OH- ions grows as well.

The amount of hydronium and hydroxide ions present in water at any one time is almost unaffected by this minute ionization.

As a result, the concentration of undissociated water molecules is essentially constant at all times and can be referred to as a constant.