Question

In an experiment, 8.67 ml of a .87M acetic acid solution was titrated with .250 sodium hydroxide. Predict by calculating the volume of base that should be used?

Answer 1

We need 30.2 mL of NaOH

Step-by-step explanation:

Step 1: Data given

Volume of acetic acid solution = 8.67 mL = 0.00867 L

Concentration of acetic acid solution = 0.87 M

Concentration of sodium hydroxide = 0.250 M

Step 2: The balanced equation

CH3COOH + NaOH → CH3COONa+ + H2O

Step 3: Calculate the volume of sodium hydroxide

b*Ca*Va = a*Cb*Vb

⇒with b = the coefficient of NaOH = 1

⇒with Ca = the concentration of CH3COOH = 0.87 M

⇒with Va = the volume of CH3COOH = 0.00867 L

⇒with a = the coefficient of CH3COOH = 1

⇒with Cb = the concentration of NaOH = 0.250 M

⇒with Vb = the volume of NaOH = TO BE DETERMINED

1 * 0.87 M * 0.00867 L = 1 *0.250 M * Vb

Vb = (0.87 M * 0.00867 L) / 0.250 M

Vb = 0.0302 L = 30.2 mL

We need 30.2 mL of NaOH