Answer:
Acetic acid Ka = 1.74 × 10⁻⁵
Trichloroacetic acid Ka = 2 × 10⁻¹
Explanation:
Let's consider the acid dissociation of acetic acid.
CH₃COOH(aq) ⇄ CH₃COO⁻(aq) + H⁺(aq)
The pKa of acetic acid is 4.76. The acid dissociation constant (Ka) is:
pKa = -log Ka
- pKa = log Ka
Ka = anti log (-pKa)
Ka = anti log (-4.76)
Ka = 1.74 × 10⁻⁵
Let's consider the acid dissociation of trichloroacetic acid.
CCl₃COOH(aq) ⇄ CCl₃COO⁻(aq) + H⁺(aq)
The pKa of trichloroacetic acid is 0.7. The acid dissociation constant (Ka) is:
pKa = -log Ka
- pKa = log Ka
Ka = anti log (-pKa)
Ka = anti log (-0.7)
Ka = 2 × 10⁻¹
Answer:
1.86% NH₃
Explanation:
The reaction that takes place is:
- HCl(aq) + NH₃(aq) → NH₄Cl(aq)
We <u>calculate the moles of HCl that reacted</u>, using the volume used and the concentration:
- 32.27 mL ⇒ 32.27/1000 = 0.03227 L
- 0.1080 M * 0.03227 L = 3.4852x10⁻³ mol HCl
The moles of HCl are equal to the moles of NH₃, so now we <u>calculate the mass of NH₃ that was titrated</u>, using its molecular weight:
- 3.4852x10⁻³ mol NH₃ * 17 g/mol = 0.0592 g NH₃
The weight percent NH₃ in the aliquot (and thus in the diluted sample) is:
- 0.0592 / 12.949 * 100% = 0.4575%
Now we <u>calculate the total mass of NH₃ in the diluted sample</u>:
Diluted sample total mass = Aqueous waste Mass + Water mass = 23.495 + 72.311 = 95.806 g
- 0.4575% * 95.806 g = 0.4383 g NH₃
Finally we calculate the weight percent NH₃ in the original sample of aqueous waste:
- 0.4383 g NH₃ / 23.495 g * 100% = 1.86% NH₃
2.75 x 10^24
Hope this helped :)
"K" is Potassium. If that is the answer you are needing.
Answer:
<h2><em><u>MASS</u></em></h2>
Explanation:
Inertia increases as an object's <u>Mass</u> increases.
