What is the [h3o+] in a solution that consists of 1.0 m nh3 and 2.5 m nh4cl? [kb (nh3) = 1.8 ×10-5]a) 1.1 × 10-5 mb) 4.5 × 10-5 mc) 3.3 × 10-9 md) 1.4 × 10-9 m) 5.6 × x10-10 m?

[H₃O⁺] = 1.4 × 10⁻⁹ M.

Explanation:

NH₄Cl is a salt that dissolves well in water. The 2.5 M NH₄Cl will give an initial NH₄⁺ concentration of 2.5 M.

NH₃ is a weak base. It combines with water to produce NH₄⁺ and OH⁻. The opposite process can also take place. NH₄⁺ combines with OH⁻ to produce NH₃ and H₂O. The final H₃O⁺ concentration can be found from the OH⁻ concentration. What will be the final OH⁻ concentration?

Let the increase in OH⁻ concentration be x. The initial OH⁻ concentration at room temperature is 10⁻⁷ M.

Construct a RICE table for the equilibrium between NH₃ and NH₄⁺:

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The value for ammonia is small. The value of x will be so small that at equilibrium, and .

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Again, at room temperature.

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