I really don't get this question, could someone help
2 answers:
In this problem we need to identify the relative molar amounts of:
NH₄⁺ , ClO₄⁻ , NH₃ , HClO₄ , H₃O⁺ , H₂O, OH⁻
- The salt is completely ionized through this equation:
NH₄ClO₄ → NH₄⁺ + ClO₄⁻
0.01 M 0.01 M 0.01 M
So:
[ClO₄⁻] = 0.01 M (conjugate base of strong acid)
[HClO₄] = 0 M
Note that: NH₄⁺ is weak acid ionized as follow:
NH₄⁺ ⇄ NH₃ + H⁺
Ka =![\frac{[ H^{+}][ NH_{3}]}{ [NH_{4} ^{+}] }](https://tex.z-dn.net/?f=%20%5Cfrac%7B%5B%20H%5E%7B%2B%7D%5D%5B%20NH_%7B3%7D%5D%7D%7B%20%5BNH_%7B4%7D%20%5E%7B%2B%7D%5D%20%20%7D%20)
= 5.6 x 10⁻¹⁰
[H⁺] = [NH₃] = x and [NH₄⁺] = 0.01 - x (because Ka is very small so x will be neglected compared to 0.01)
Ka = 5.6 x 10⁻¹⁰ =
[H⁺] = [NH₃] = x = 2.37 x 10⁻⁶ M
[NH₄⁺] = 0.01 M
[OH⁻] =![\frac{1 X 10^{-14} }{[H^{+} ]}](https://tex.z-dn.net/?f=%20%5Cfrac%7B1%20X%20%2010%5E%7B-14%7D%20%7D%7B%5BH%5E%7B%2B%7D%20%5D%7D%20)
= 4.22 X 10⁻⁹ M
because water is the solvent & this is very dilute solution:
[H₂O] =
= 55.6 M H₂O
NH₄⁺ , ClO₄⁻ , NH₃ , HClO₄ , H₃O⁺ , H₂O, OH⁻
- The salt is completely ionized through this equation:
NH₄ClO₄ → NH₄⁺ + ClO₄⁻
0.01 M 0.01 M 0.01 M
So:
[ClO₄⁻] = 0.01 M (conjugate base of strong acid)
[HClO₄] = 0 M
Note that: NH₄⁺ is weak acid ionized as follow:
NH₄⁺ ⇄ NH₃ + H⁺
Ka =
[H⁺] = [NH₃] = x and [NH₄⁺] = 0.01 - x (because Ka is very small so x will be neglected compared to 0.01)
Ka = 5.6 x 10⁻¹⁰ =
[H⁺] = [NH₃] = x = 2.37 x 10⁻⁶ M
[NH₄⁺] = 0.01 M
[OH⁻] =
because water is the solvent & this is very dilute solution:
[H₂O] =
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