Multiple Choice
A 0.050 M solution of hydroxylamine, NH2OH, having Kb = 9.1 × 10^-9 has a pH of ________.
17. Acid and Base Equilibrium
pH of Weak Bases
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A solution with a hydroxide ion concentration of 4.15 × 10⁻⁵ M is considered a weak base. What is the hydrogen ion concentration of this solution?
A
1.00 × 10⁻⁷ M
B
4.15 × 10⁻⁵ M
C
2.41 × 10⁻⁵ M
D
2.41 × 10⁻¹⁰ M
Verified step by step guidance1
Start by understanding the relationship between hydroxide ion concentration \( [OH^-] \) and hydrogen ion concentration \( [H^+] \) in a solution. This relationship is given by the water dissociation constant \( K_w \), where \( K_w = [H^+][OH^-] = 1.0 \times 10^{-14} \) at 25°C.
Given the hydroxide ion concentration \( [OH^-] = 4.15 \times 10^{-5} \text{ M} \), use the formula \( [H^+] = \frac{K_w}{[OH^-]} \) to find the hydrogen ion concentration.
Substitute the known values into the formula: \( [H^+] = \frac{1.0 \times 10^{-14}}{4.15 \times 10^{-5}} \).
Perform the division to calculate \( [H^+] \). This will give you the hydrogen ion concentration in the solution.
Compare the calculated \( [H^+] \) with the given options to identify the correct answer, which should match \( 2.41 \times 10^{-10} \text{ M} \).
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