The concentration of $H C N$ and $N a C N$ in a solution is $0.01 M$ each. Calculate the concentration of hydroxyl ions if the dissociation constant of $H C N$ is $7.2 \times 10^{- 10}$ .

Q. What is the

H^{+}

ion concentration in ammonium acetate solution?

(K_{a} = 1.8 \times 10^{- 5}, K_{b} = 1.8 \times 10^{- 5}, K_{w} = 1.0 \times 10^{- 14})

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At 25oC the hydroxyl ion concentration of a basic solution is 6.75×10−3 M. Then Kw is:

The correct option is D 10−14As we know that,Kw=[H+][OH−]=10−14Since the value of Kw is constant and does not change w.r.t. the concentration of H+ ion and OH− ion.Hence the value of Kw will be 10−14.

At $25^{o} C$ the hydroxyl ion concentration of a basic solution is $6.75 \times 10^{- 3} M$ . Then $K_{w}$ is:

The correct option is D $10^{- 14}$
As we know that,
$K_{w} = [H^{+}] [{O H}^{-}] = 10^{- 14}$
Since the value of $K_{w}$ is constant and does not change w.r.t. the concentration of $H^{+}$ ion and ${O H}^{-}$ ion.
Hence the value of $K_{w}$ will be $10^{- 14}$ .