What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?
Practice Questions
1 question
Q1
What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?
4.76
7.00
9.24
10.00
Sodium acetate is a salt of a weak acid (acetic acid) and a strong base (sodium hydroxide). The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]), where pKa of acetic acid is 4.76.
Questions & Step-by-step Solutions
1 item
Q
Q: What is the pH of a 0.01 M solution of sodium acetate (CH3COONa)?
Solution: Sodium acetate is a salt of a weak acid (acetic acid) and a strong base (sodium hydroxide). The pH can be calculated using the formula pH = 7 + 0.5(pKa - log[C]), where pKa of acetic acid is 4.76.
Steps: 8
Step 1: Identify the components of sodium acetate (CH3COONa). It is made from acetic acid (a weak acid) and sodium hydroxide (a strong base).
Step 2: Understand that when sodium acetate dissolves in water, it will create a basic solution because it comes from a weak acid and a strong base.
Step 3: Find the pKa value of acetic acid, which is 4.76.
Step 4: Use the formula to calculate the pH: pH = 7 + 0.5(pKa - log[C]). Here, C is the concentration of the sodium acetate solution, which is 0.01 M.
Step 5: Calculate log[C]: log[0.01] = -2.
Step 6: Substitute the values into the formula: pH = 7 + 0.5(4.76 - (-2)).
