What is the pH of a 0.01 M solution of sodium hydroxide (NaOH)?
Practice Questions
Q1
What is the pH of a 0.01 M solution of sodium hydroxide (NaOH)?
12
2
10
14
Questions & Step-by-Step Solutions
What is the pH of a 0.01 M solution of sodium hydroxide (NaOH)?
Step 1: Understand that sodium hydroxide (NaOH) is a strong base that completely dissociates in water, meaning it produces hydroxide ions (OH-) equal to its concentration.
Step 2: Since the concentration of NaOH is 0.01 M, the concentration of hydroxide ions [OH-] is also 0.01 M.
Step 3: Calculate the pOH using the formula pOH = -log[OH-]. Substitute [OH-] with 0.01: pOH = -log(0.01).
Step 4: Calculate -log(0.01). The result is 2, so pOH = 2.
Step 5: Use the relationship between pH and pOH, which is pH + pOH = 14. Rearranging gives pH = 14 - pOH.
Step 6: Substitute pOH into the equation: pH = 14 - 2.
