Question
What is the Kb value for a 0.20M solution with a 3.0% ionization? NH3 + H2O <—> NH4^+ + OH^-
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Answer to a math question What is the Kb value for a 0.20M solution with a 3.0% ionization? NH3 + H2O <—> NH4^+ + OH^-
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To find the K_b OH^- NH_3
Given:
- Initial concentration[NH_3]
- Ionization percentage = 3.0%
Concentration ofOH^-
\text{Concentration of } OH^- = 0.20 \, \text{M} \times \frac{3.0}{100} = 0.006 \, \text{M}
Since each molecule ofNH_3 NH_4^+ OH^-
K_b = \frac{[NH_4^+][OH^-]}{[NH_3]} = \frac{0.006 \times 0.006}{0.20} = 1.8 \times 10^{-4}
Therefore, theK_b NH_3 1.8 \times 10^{-4}
\boxed{K_b \approx 1.8 \times 10^{-4}}
Given:
- Initial concentration
- Ionization percentage = 3.0%
Concentration of
Since each molecule of
Therefore, the
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