Asked by LuigiR
1.)An ammonia/ammonium buffer solution contains 0.35 M NH3 and 0.72 M NH4+. The Kb value of ammonia is 1.8×10−5. Calculate the pH of this buffer.
2.) Nitrous acid has a Ka of 4.5×10−4. What is the pH of a buffer solution containing 0.15 M HNO2 and 0.20 M NO−2?
3.) Acetic acid has a Ka of 1.8×10−5.
What is the pH of a buffer solution containing 0.14 M HC2H3O2 (acetic acid) and 0.20 M C2H3O2−?
2.) Nitrous acid has a Ka of 4.5×10−4. What is the pH of a buffer solution containing 0.15 M HNO2 and 0.20 M NO−2?
3.) Acetic acid has a Ka of 1.8×10−5.
What is the pH of a buffer solution containing 0.14 M HC2H3O2 (acetic acid) and 0.20 M C2H3O2−?
Answers
Answered by
DrBob222
1. Use the Henderson-Hasselbalch equation. KaKb = Kw and you get Ka from that and pKa follows.
2. Ditto for 2.
3. Ditto for 3.
2. Ditto for 2.
3. Ditto for 3.
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