Respuesta :
Answer : The concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are, [tex]1.58\times 10^{-4}[/tex] and [tex]6.3\times 10^{-11}[/tex] respectively.
Explanation : Given,
pH = 10.2
pH : It is defined as the negative logarithm of the hydrogen ion concentration.
First we have to calculate the hydrogen ion concentration [tex](H^+)[/tex]
[tex]pH=-\log [H^+][/tex]
Now put the value of pH in this formula, we get the hydrogen ion concentration.
[tex]10.2=-\log [H^+][/tex]
[tex][H^+]=6.3\times 10^{-11}[/tex]
Now we have to calculate the pOH of the solution.
[tex]pH+pOH=14[/tex]
Now put the value of pH, we get the value of pOH.
[tex]10.2+pOH=14[/tex]
[tex]pOH=14-10.2[/tex]
[tex]pOH=3.8[/tex]
Now we have to calculate the hydroxide ion concentration [tex](OH^-)[/tex]
[tex]pOH=-\log [OH^-][/tex]
Now put the value of pOH in this formula, we get the hydroxide ion concentration.
[tex]3.8=-\log [OH^-][/tex]
[tex][OH^-]=1.58\times 10^{-4}[/tex]
Therefore, the concentrations of hydroxide and hydronium ions in a solution with a pH of 10.2 are, [tex]1.58\times 10^{-4}[/tex] and [tex]6.3\times 10^{-11}[/tex] respectively.
Answer: [tex][H^+]=6.3\times 10^{-11}[/tex] and [tex][OH^-]=1.58\times 10^{-4}[/tex]
Explanation:
pH or pOH is the measure of acidity or alkalinity of a solution.
pH is calculated by taking negative logarithm of hydrogen ion concentration and pOH is calculated by taking negative logarithm of hydroxide ion concentration.
[tex]pH=-\log [H^+][/tex]
[tex]pOH=-log[OH^-][/tex]
[tex]pH+pOH=14[/tex]
Given pH = 10.2
[tex]10.2=-\log [H^+][/tex]
[tex][H^+]=6.3\times 10^{-11}[/tex]
[tex]pOH=14-10.2=3.8[/tex]
[tex]3.8=-log[OH^-][/tex]
[tex][OH^-]=1.58\times 10^{-4}[/tex]
