The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶ M. What is [OH⁻]?
Question
The H⁺ concentration in an aqueous solution at 25 °C is 5.5 × 10⁻⁶ M. What is [OH⁻]?
Solution
To find the concentration of OH⁻ ions in the solution, we need to use the ion product of water (Kw) at 25 °C, which is 1.0 x 10⁻¹⁴.
The formula for Kw is [H⁺][OH⁻] = Kw.
We know the concentration of H⁺ ions is 5.5 x 10⁻⁶ M, so we can substitute this into the formula and solve for [OH⁻]:
[OH⁻] = Kw / [H⁺]
Substituting the known values:
[OH⁻] = (1.0 x 10⁻¹⁴) / (5.5 x 10⁻⁶)
Solving this gives:
[OH⁻] = 1.82 x 10⁻⁹ M
So, the concentration of OH⁻ ions in the solution is 1.82 x 10⁻⁹ M.
Similar Questions
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?
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?
Which of the following describes a solution with equal concentrations of OH- ions and H+ ions?Select one:a.neutralb.amphotericc.acidicd.basic
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?
A solution has [H3O⁺] = 6.37 x 10⁻¹⁰ . Calculate [OH-], and determine if the solution is acidic or basic.
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.