If the hydronium ion (H3O+) concentration of an aqueous solution at 25°C is 5 × 10−6 M, what is the hydroxide ion (OH–) concentration?
Question
If the hydronium ion (H3O+) concentration of an aqueous solution at 25°C is 5 × 10−6 M, what is the hydroxide ion (OH–) concentration?
Solution
To find the hydroxide ion (OH-) concentration, we need to use the ion product of water (Kw) at 25°C, which is 1.0 x 10^-14.
The ion product of water (Kw) is given by the equation:
Kw = [H3O+] [OH-]
We know the hydronium ion (H3O+) concentration, which is 5 x 10^-6 M. We can substitute this into the equation and solve for the hydroxide ion (OH-) concentration:
1.0 x 10^-14 = (5 x 10^-6) [OH-]
To solve for [OH-], we divide both sides of the equation by 5 x 10^-6:
[OH-] = (1.0 x 10^-14) / (5 x 10^-6)
[OH-] = 2 x 10^-9 M
So, the hydroxide ion (OH-) concentration is 2 x 10^-9 M.
Similar Questions
The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶ M. What is [OH⁻]?
If a water sample has a hydrogen ion concentration of 4.0 x 10-5, what is the concentration of OH-? Is the solution acidic or basic?
A solution has [H3O⁺] = 6.37 x 10⁻¹⁰ . Calculate [OH-], and determine if the solution is acidic or basic.
What is the pH of a solution that contains hydroxide ions at a concentration of 6.3 x 10-4 M ?Question 13Select one:a.3.23.2b.6.36.3c.1.61.6d.10.8
What is the [OH−] in the final solution prepared by mixing 20.0 mL of 0.050 M HCl with 30.0 mL of 0.10 MBa(OH)2?
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.