Answer:
3.98 x 10⁻⁴ M.
Explanation:
∵ pH = - log[H₃O⁺]
∴ 3.4 = - log[H₃O⁺].
∴ log[H₃O⁺] = - 3.4.
∴ [H₃O⁺] = 3.98 x 10⁻⁴ M.
Answer: The hydronium ion concentration for the solution is [tex]3.98\times 10^{-4}M[/tex]
Explanation:
pH is defined as the negative logarithm of hydrogen ion concentration or hydronium ion concentration present in a solution.
To calculate the pH of the reaction, we use the equation:
[tex]pH=-\log[H_3O^+][/tex]
We are given:
pH of the solution = 3.40
Putting values in above equation, we get:
[tex]3.40=-\log[H_3O^+][/tex]
[tex][H_3O^+]=3.98\times 10^{-4}M[/tex]
Hence, the hydronium ion concentration for the solution is [tex]3.98\times 10^{-4}M[/tex]
