Select all that applyWhat are [H+] and [OH–] in a solution that has a pH of 9.80?Multiple select question.[H+] = 1.6M[H+] = 1.6 × 10–10M[OH–] = 6.3 × 10–5M[OH–] = 6.3M[H+] = 6.3 × 10–5M[OH–] = 1.6 × 10–10M
Question
Select all that applyWhat are [H+] and [OH–] in a solution that has a pH of 9.80?Multiple select question.[H+] = 1.6M[H+] = 1.6 × 10–10M[OH–] = 6.3 × 10–5M[OH–] = 6.3M[H+] = 6.3 × 10–5M[OH–] = 1.6 × 10–10M
Solution
The pH of a solution is calculated using the formula pH = -log[H+]. So, to find the concentration of [H+], we rearrange the formula to [H+] = 10^-pH.
Substituting the given pH of 9.80 into the formula gives [H+] = 10^-9.80 = 1.58 x 10^-10 M. This is approximately equal to 1.6 x 10^-10 M.
The pOH of a solution is calculated using the formula pOH = -log[OH-]. Since pH + pOH = 14 at 25 degrees Celsius, we can find the pOH by subtracting the given pH from 14.
So, pOH = 14 - 9.80 = 4.20.
Substituting this into the formula gives [OH-] = 10^-4.20 = 6.31 x 10^-5 M. This is approximately equal to 6.3 x 10^-5 M.
Therefore, the correct answers are [H+] = 1.6 x 10^-10 M and [OH–] = 6.3 x 10^-5 M.
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