A 0.25 M aqueous solution of hypobromous acid, HOBr, has a pH of 4.50 at 25oC. What is the concentration of hydronioum ions, [H3O+] in this solution? 5.01x10−7 M 1.04x10−5 M 2.53x10−6 M 5.01x10−6 M 3.16x10−5 M
Question
A 0.25 M aqueous solution of hypobromous acid, HOBr, has a pH of 4.50 at 25oC. What is the concentration of hydronioum ions, [H3O+] in this solution? 5.01x10−7 M 1.04x10−5 M 2.53x10−6 M 5.01x10−6 M 3.16x10−5 M
Solution
The pH of a solution is defined as the negative logarithm (base 10) of the hydronium ion concentration. This means that if you know the pH of a solution, you can calculate the hydronium ion concentration using the following formula:
[H3O+] = 10^(-pH)
Given that the pH of the solution is 4.50, you can substitute this value into the formula to find the hydronium ion concentration:
[H3O+] = 10^(-4.50)
This calculation gives a hydronium ion concentration of 3.16x10^-5 M. Therefore, the correct answer is 3.16x10^-5 M.
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