Titration Calculator
Calculate unknown concentrations and volumes in acid-base titrations using molarity equations
Calculate Titration Parameters
Acid Parameters
Number of H⁺ ions per molecule (e.g., HCl = 1, H₂SO₄ = 2)
Base Parameters
Number of OH⁻ ions per molecule (e.g., NaOH = 1, Ca(OH)₂ = 2)
Titration Results
Formula used: nH⁺ × Ma × Va = nOH⁻ × Mb × Vb
Calculation: 1 × × 0 = 1 × 0 × 0
Moles: Acid: 0.000000 mol, Base: 0.000000 mol
Neutralization Analysis
Example Calculation
HCl Titration with NaOH
Problem: What is the concentration of 0.15 mL HCl if 20.7 mL of 0.5 M NaOH is required to neutralize it?
Given: NaOH: 0.5 M, 20.7 mL; HCl: ?, 0.15 mL
Reaction: HCl + NaOH → NaCl + H₂O (1:1 ratio)
Calculation
nH⁺ × Ma × Va = nOH⁻ × Mb × Vb
1 × Ma × 0.15 = 1 × 0.5 × 20.7
Ma × 0.15 = 10.35
Ma = 10.35 ÷ 0.15
Ma = 69.0 M
Titration Procedure
Fill Burette
Fill with titrant solution
Record initial volume
Prepare Analyte
Measure analyte + indicator
Place in Erlenmeyer flask
Titrate
Add titrant slowly
Watch for color change
Record Endpoint
Note final volume
Calculate titrant used
Common Indicators
Phenolphthalein
pH 8.2-10.0 (colorless → pink)
Methyl Orange
pH 3.1-4.4 (red → yellow)
Bromothymol Blue
pH 6.0-7.6 (yellow → blue)
Universal Indicator
pH 1-14 (rainbow colors)
Titration Tips
Choose appropriate indicator for pH range
Add titrant dropwise near endpoint
Swirl flask constantly during titration
Record initial and final burette readings
Understanding Titrations
What is a Titration?
Titration is an analytical technique used to determine the concentration of an unknown solution by reacting it with a solution of known concentration. The point where the reaction is complete is called the equivalence point.
Titration Equation
nH⁺ × Ma × Va = nOH⁻ × Mb × Vb
At the equivalence point
Equivalence Point
The equivalence point occurs when the moles of acid equal the moles of base, resulting in complete neutralization. This is detected by a color change in the indicator or a sharp pH change.
Types of Titrations
Strong Acid vs Strong Base
Sharp endpoint at pH 7
Example: HCl + NaOH
Strong Acid vs Weak Base
Endpoint at pH < 7
Example: HCl + NH₃
Weak Acid vs Strong Base
Endpoint at pH > 7
Example: CH₃COOH + NaOH
Note: Weak acid vs weak base titrations have irregular curves and require pH meters instead of indicators.