Based on the fgiven K_{a} values of the acids, the equilibrim concentrations of[tex]HC_{2}H_{2}O_{2}[/tex] and [tex]NH_{4}^{+}[/tex] is dtermined using ICE tables.
What are acid dissociatio constants [tex]K_{a}[/tex]?
An acid dissociation constant, [tex]K_{a}[/tex] of an acid is a measure of the strength of the acid in solution. The larger the [tex]K_{a}[/tex] value of an acid, the stronger the acid, therefore, acid dissociation constants are usually apply to only weak acids because strong acids have exceedingly large [tex]K_{a}[/tex] values.
It is written as a qoutient of the equilibrium concentrations of the aqueous species in the acid solution.
- [tex]K_{a} = \frac{[H^{+}] [A^-{}]}{HA}[/tex]
For the weak acids such as [tex]HC_{2}H_{2}O_{2}[/tex] and [tex]NH_{4}^{+}[/tex], their equilibrim concentrations are determined using their [tex]K_{a}[/tex] values and an ICE table.
The pH of solutions are estimated using indicators such as methyl orange, methyl red and phenolphthalein. The colors of indicators change according to the pH of the solution
Acidic solutions have pH less than 7 while alkaline solutions have pH greater than 7.
Therefore, acids have low pH and weak acids have low [tex]K_{a}[/tex] values.
Learn more about acid dissociation constant at: https://brainly.com/question/3006391
