The correct option is C 1.8×10−16mol/litre
Suppose water contains X mol/litre or X eq/litre of H+ ions or OH− ions.
∵ Equivalent of H+= Eq. of H2
∴ Volume of H2O in mL having 1 Eq. H+=1000X
∴ Equivalent conductivity of water, A∞eq.H2O=k×1000N
=5.8×10−8×1000X
Since, water dissociated feebly, i.e., water may be considered to be a dilute solution of H+ and OH− ions.
∴A∞eq.H2O=λ∞H++λ∞OH−
∴5.8×10−8×1000X=350+198=548
∴X=1.0×10−7
∴[H+]=[OH−]=1×10−7
For the equilibrium
H2O⇌H++OH−
Equilibrium constant (K)=[H+][OH−][H2O]
Kw=K×[H2O]=[H+][OH−]
=1.0×10−7×1.0×10−7=1×10−14
∴K=Kw[H2O]=1×10−1455.5 [[H2O]=100018=55.5mol/litre]
=1.8×10−16mol/litre