Which of the following describes what occurs as a gas becomes a liquid?
1 answer:
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Answer:
Here's what I get.
Explanation:
1. Brønsted-Lowry theory
An acid is a substance that can donate a proton to another substance.
A base is a substance that can accept a proton from another substance.
2. pH of ammonia
The chemical equation is
For simplicity, let's re-write this as
(a) Set up an ICE table.
B + H₂O ⇌ BH⁺ + OH⁻
I/mol·L⁻¹: 0.335 0 0
C/mol·L⁻¹: -x +x +x
E/mol·L⁻¹: 0.335 + x x x
Check for negligibility:
(b) Solve for [OH⁻]
(c) Calculate the pOH
(d) Calculate the pH
pH = 14.00 - pOH = 14.00 - 2.61 = 11.39
Answer:
Kₐ = 4.06 × 10⁻⁷
Explanation:
Step 1. <em>Calculate [H₃O⁺] </em>
pH = 3.94
[H₃O⁺] = 1.15 × 10⁻⁴ mol·L⁻¹
Calculate
HF + H₂O ⇌ H₃O⁺ + F⁻
I/mol·L⁻¹: 0.0326 0 0
C/mol·L⁻¹: 0.0326-1.15 × 10⁻⁴ +1.15 × 10⁻⁴ +1.15 × 10⁻⁴
E/mol·L⁻¹: 0.0325 1.15 × 10⁻⁴ 1.15 × 10⁻⁴
So, at equilibrium,
[H₃O⁺] = [F⁻] = 1.15 × 10⁻⁴ mol·L⁻¹
[HF] = 0.326 – 1.15 × 10⁻⁴ mol·L⁻¹ = 0.0325 mol·L⁻¹
Kₐ = {[H₃O⁺][F⁻]}/[HF]
Kₐ = (1.15 × 10⁻⁴ × 1.15 × 10⁻⁴)/0.0325
Kₐ = 1.32 × 10⁻⁸/0.0325
Kₐ = 4.06 × 10⁻⁷
This is <em>NOT</em> a solution of HF (Kₐ = 7.2 × 10⁻⁴). It is more likely a solution of carbonic acid (H₂CO₃; Kₐ₁ = 4.27 × 10⁻⁷).