By Jack Brubaker
Updated Aug 30, 2022

Step 1: Write the Balanced Equation

Before starting, identify the titrant and analyte, then write the balanced reaction they undergo. For example, titrating acetic acid (CH₃COOH) with sodium hydroxide (NaOH) yields:

CH₃COOH + NaOH → CH₃COONa + H₂O

The coefficients on the left side give the molar ratio—in this case 1:1.

Step 2: Convert Titrant Volume to Liters

Record the burette reading at the end point (when the analyte is fully consumed). Convert milliliters to liters by dividing by 1,000. For instance, 39.75 mL of NaOH becomes:

39.75 mL ÷ 1,000 mL L^-1 = 0.03975 L NaOH

Step 3: Calculate Moles of Titrant

Multiply the volume of titrant by its known concentration. If the NaOH solution is 0.1044 mol L^-1:

0.03975 L × 0.1044 mol L^-1 = 0.004150 mol NaOH

Step 4: Determine Moles of Analyte

Use the molar ratio from Step 1 to convert titrant moles to analyte moles:

0.004150 mol NaOH × (1 mol CH₃COOH ÷ 1 mol NaOH) = 0.004150 mol CH₃COOH

Step 5: Compute Analyte Concentration

Divide the moles of analyte by the volume of the sample (in liters). If 5.00 mL of vinegar was used:

5.00 mL = 0.00500 L
(0.004150 mol CH₃COOH) ÷ 0.00500 L = 0.830 mol L^-1

Thus, the vinegar contains 0.830 mol L^-1 of acetic acid.

Things Needed

• Accurate calculator
• Recorded titration data (volumes, concentrations)