Ow many coulombs of charge are needed to produce 35.2 mol of solid zinc?
2 answers:
Answer:
6.79 × 10⁶ c
Explanation:
Zn can be produced from the electrolysis of an aqueous solution of a Zn salt. The reduction reaction is:
Zn²⁺(aq) + 2 e⁻ → Zn(s)
We can establish the following relations.
- 1 mol of Zn is produced when 2 moles of e⁻ are gained.
- 1 mole of e⁻ has a charge of 96468 c (Faraday's constant).
The charge needed to produce 35.2 mol of Zn is:
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Answer:
Explanation:
To calculate pH you need to use Henderson-Hasselbalch formula:
pH = pka + log₁₀
Where HA is the acid concentration and A⁻ is the conjugate base concentration.
The equilibrium of acetic acid is:
CH₃COOH ⇄ CH₃COO⁻ + H⁺ pka: 4,75
Where <em>CH₃COOH </em>is the acid and <em>CH₃COO⁻ </em>is the conjugate base.
Thus, Henderson-Hasselbalch formula for acetic acid equilibrium is:
pH = 4,75 + log₁₀
a) The pH is:
pH = 4,75 + log₁₀
<em>pH = 4,75</em>
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b) The pH is:
pH = 4,75 + log₁₀
<em>pH = 5,05</em>
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I hope it helps!