Answer:
[H₃O⁺] ≈ 0.00282 M
General Formulas and Concepts:
Acid/Base Equilibria
Bronsted Acid/Bronsted Base
pH Formula: pH = -log[H₃O⁺]
[H₃O⁺] Formula: [tex]\displaystyle [H_3O^+] = 10^{-pH}[/tex]
Explanation:
Step 1: Define
pH = 2.55 (Acidic)
Step 2: Solve
- Substitute in pH [Molar Concentration Formula]: [tex]\displaystyle [H_3O^+] = 10^{-2.55}[/tex]
- Evaluate exponent: [tex]\displaystyle [H_3O^+] = 0.002818[/tex]
Step 3: Check
Follow sig fig rules and round. We are given 3 sig figs.
0.002818 M ≈ 0.00282 M
