Use pH, pOH, [H3O+], and [OH-] relationships. (a) The hydronium ion concentration in an aqueous solution of HCI is 7.2x10-2 M. Calculate [OH-], pH, and pOH for this solution. [OH-] = M pH = (b) The pH of an aqueous solution of KOH is 11.00. Calculate [H3O+], [OH-], and pOH for this solution. [H3O+] = M [OH-] = pOH = M pOH =
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![**Use pH, pOH, [H₃O⁺], and [OH⁻] relationships.**
(a) The hydronium ion concentration in an aqueous solution of HCl is 7.2 x 10⁻² M. Calculate [OH⁻], pH, and pOH for this solution.
\[
[OH⁻] = \_\_\_\_ \, \text{M} \quad \text{pH} = \_\_\_\_ \quad \text{pOH} = \_\_\_\_
\]
(b) The pH of an aqueous solution of KOH is 11.00. Calculate [H₃O⁺], [OH⁻], and pOH for this solution.
\[
[H₃O⁺] = \_\_\_\_ \, \text{M} \quad [OH⁻] = \_\_\_\_ \, \text{M} \quad \text{pOH} = \_\_\_\_
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