Final answer:
The hydroxide ion concentration [OH-] for a solution with a pH of 2.63 is calculated using the formula [OH-] = 1.0 x 10^-14 M² / [H3O+]. The [H3O+] is derived from the pH and is found to be 2.34 x 10^-3 M, leading to an [OH-] of 4.27 x 10^-12 M.
Step-by-step explanation:
The question pertains to calculating the hydroxide ion concentration ([OH-]) in an acidic solution given the lab (presumably pH) of 2.63. According to the concept of pH and pOH, these values are inversely related in a solution at 25°C, and the product of the hydrogen ion concentration ([H3O+]) and hydroxide ion concentration is always 1.0 x 10⁻¹⁴ M².
To find the [OH-], we first need to convert the pH to [H3O+] using the formula pH = -log [H3O+], then plug the [H3O+] into the formula [OH-] = 1.0 x 10⁻¹⁴ M² / [H3O+]. So let's calculate [H3O+] as follows:
[H3O+] = 10⁻¹²⁶³ = 2.34 x 10⁻³ M
Then calculate [OH-]:
[OH-] = 1.0 x 10⁻¹⁴ M² / 2.34 x 10⁻³ M = 4.27 x 10⁻¹² M