Open Question
What is the ph of an aqueous solution with the hydronium ion concentration
17. Acid and Base Equilibrium
The pH Scale
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
In a solution whose [H⁺] = 1.9 x 10⁻⁵ M at 25°C, what is the [OH⁻]? Is this solution acidic, basic, or neutral?
A
[OH⁻] = 5.3 x 10⁻¹⁰ M; the solution is acidic.
B
[OH⁻] = 1.0 x 10⁻⁷ M; the solution is neutral.
C
[OH⁻] = 5.3 x 10⁻¹⁰ M; the solution is basic.
D
[OH⁻] = 1.9 x 10⁻⁵ M; the solution is neutral.
Verified step by step guidance1
Start by recalling the relationship between hydrogen ion concentration [H⁺] and hydroxide ion concentration [OH⁻] in water at 25°C, which is given by the ion product of water: \( K_w = [H^+] \times [OH^-] = 1.0 \times 10^{-14} \).
Given the [H⁺] concentration is \( 1.9 \times 10^{-5} \) M, use the formula \( [OH^-] = \frac{K_w}{[H^+]} \) to find the [OH⁻] concentration.
Substitute the known values into the equation: \( [OH^-] = \frac{1.0 \times 10^{-14}}{1.9 \times 10^{-5}} \).
Calculate the [OH⁻] concentration using the division of the ion product of water by the given [H⁺] concentration.
Determine the nature of the solution: if \( [H^+] > [OH^-] \), the solution is acidic; if \( [H^+] < [OH^-] \), the solution is basic; if \( [H^+] = [OH^-] \), the solution is neutral.
Related Videos
Related Practice
