Question: What is the pH of a 0.05 M solution of sulfuric acid (H2SO4)?
Options:
1
1.3
1.7
2
Correct Answer: 1.3
Solution:
H2SO4 is a strong acid and dissociates completely; [H+] = 0.05 M, so pH = -log(0.05) ≈ 1.3
What is the pH of a 0.05 M solution of sulfuric acid (H2SO4)?
Practice Questions
Q1
What is the pH of a 0.05 M solution of sulfuric acid (H2SO4)?
1
1.3
1.7
2
Questions & Step-by-Step Solutions
What is the pH of a 0.05 M solution of sulfuric acid (H2SO4)?
Step 1: Identify the concentration of the sulfuric acid solution, which is 0.05 M.
Step 2: Recognize that sulfuric acid (H2SO4) is a strong acid, meaning it dissociates completely in water.
Step 3: Since H2SO4 dissociates completely, the concentration of hydrogen ions [H+] in the solution is equal to the concentration of the acid, which is 0.05 M.
Step 4: Use the formula for pH, which is pH = -log[H+].
Step 5: Substitute the value of [H+] into the formula: pH = -log(0.05).
Step 6: Calculate the logarithm: pH ≈ 1.3.
No concepts available.
Soulshift Feedback×
On a scale of 0–10, how likely are you to recommend
The Soulshift Academy?
