<h3>
Answer:</h3>
495 g K₃N
<h3>
General Formulas and Concepts:</h3>
<u>Math</u>
<u>Pre-Algebra</u>
Order of Operations: BPEMDAS
- Brackets
- Parenthesis
- Exponents
- Multiplication
- Division
- Addition
- Subtraction
<u>Chemistry</u>
<u>Atomic Structure</u>
<u>Stoichiometry</u>
- Using Dimensional Analysis
<h3>
Explanation:</h3>
<u>Step 1: Define</u>
3.77 mol K₃N
<u>Step 2: Identify Conversions</u>
Molar Mass of K - 39.10 g/mol
Molar Mass of N - 14.01 g/mol
Molar Mass of K₃N - 3(39.10) + 14.01 = 131.31 g/mol
<u>Step 3: Convert</u>
- Set up:

- Multiply/Divide:

<u>Step 4: Check</u>
<em>Follow sig fig rules and round. We are given 3 sig figs.</em>
495.039 g K₃N ≈ 495 g K₃N
Answer:
The dissociation constant of phenol from given information is
.
Explanation:
The measured pH of the solution = 5.153

Initially c
At eq'm c-x x x
The expression of dissociation constant is given as:
![K_a=\frac{[C_6H_5O^-][H^+]}{[C_6H_5OOH]}](https://tex.z-dn.net/?f=K_a%3D%5Cfrac%7B%5BC_6H_5O%5E-%5D%5BH%5E%2B%5D%7D%7B%5BC_6H_5OOH%5D%7D)
Concentration of phenoxide ions and hydrogen ions are equal to x.
![pH=-\log[x]](https://tex.z-dn.net/?f=pH%3D-%5Clog%5Bx%5D)
![5.153=-\log[x]](https://tex.z-dn.net/?f=5.153%3D-%5Clog%5Bx%5D)



The dissociation constant of phenol from given information is
.