Answer: 2.5 × 10⁻⁵ M H₃O⁺ and 4.0 × 10⁻¹⁰ M OH⁻
Explanation:
∵ pH = - log[H₃O⁺]
∴ 4.6 = - log[H₃O⁺].
∴ log[H₃O⁺] = - 4.6.
∴ [H₃O⁺] = 2.51 x 10⁻⁵.
∵ [H₃O⁺][OH⁻] = 10⁻¹⁴.
[H₃O⁺] = 2.51 x 10⁻⁵ M.
∴ [OH⁻] = 10⁻¹⁴/[H₃O⁺] = 10⁻¹⁴/(2.51 x 10⁻⁵ M) = 3.98 × 10⁻¹⁰ M ≅ 4.0 × 10⁻¹⁰ M.
Answer : The concentration of hydroxide and hydronium ion is, [tex]3.9\times 10^{-10}M[/tex] and [tex]2.5\times 10^{-5}M[/tex]
Explanation: Given,
pH = 4.6
pH : It is defined as the negative logarithm of hydrogen ion and hydronium ion concentration.
[tex]pH=-\log [H_3O^+][/tex]
First we have to calculate the [tex]H^+[/tex] concentration.
[tex]pH=-\log [H_3O^+][/tex]
[tex]4.6=-\log [H_3O^+][/tex]
[tex][H_3O^+]=2.5\times 10^{-5}M[/tex]
Now we have to calculate the pOH.
[tex]pH+pOH=14\\\\pOH=14-pH\\\\pOH=14-4.6=9.4[/tex]
Now we have to calculate the [tex]OH^-[/tex] concentration.
[tex]pOH=-\log [OH^-][/tex]
[tex]9.4=-\log [OH^-][/tex]
[tex][OH^-]=3.9\times 10^{-10}M[/tex]
Therefore, the concentration of hydroxide and hydronium ion is, [tex]3.9\times 10^{-10}M[/tex] and [tex]2.5\times 10^{-5}M[/tex]
