A solution has [H3O⁺] = 6.37 x 10⁻¹⁰ . Calculate [OH-], and determine if the solution is acidic or basic.
Question
Solution
To solve this problem, we need to use the ion product of water, Kw, which is equal to [H3O+][OH-] and at 25°C is 1.0 x 10^-14.
Step 1: Write down the given [H3O+] [H3O+] = 6.37 x 10^-10
Step 2: Use the Kw expression to solve for [OH-] Kw = [H3O+][OH-] 1.0 x 10^-14 = (6.37 x 10^-10)[OH-]
Step 3: Solve for [OH-] [OH-] = (1.0 x 10^-14) / (6.37 x 10^-10) [OH-] = 1.57 x 10^-5
Step 4: Determine if the solution is acidic or basic A solution is acidic if [H3O+] > [OH-], basic if [OH-] > [H3O+], and neutral if [H3O+] = [OH-]. In this case, [H3O+] = 6.37 x 10^-10 and [OH-] = 1.57 x 10^-5. Since [OH-] > [H3O+], the solution is basic.
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