The ph of a 0.1 m mcl (m is an unknown cation) was found to be 4.7. write the net ionic equation for the hydrolysis of m and its corresponding equilibrium expression kb. calculate the value of kb

6.25 X10^{-9} = Ka

Explanation:

The ionic equation for the hydrolysis of the cation of the given salt will be:

The expression for Ka will be:

Ka =

As given that the concentration of the salt is 0.1 M and pH of solution = 4.7, we can determine the concentration of Hydrogen ions from the pH

pH = -log [H⁺]

[H⁺] = antilog(-pH) = antilog (-4.7) = 2 X 10⁻⁵ M = [MOH]

Let us calculate Ka from this,

Ka =

The relation between Ka an Kb is

KaXKb =10⁻¹⁴

i know insulin is primary but i dont know the others im sorry

explanation:

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explanation: