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Titration Calculator

Choose what you need to calculate, enter the values accordingly, and click on the “Calculate”.

What You Want To Calculate:

Molarity of the Acid:

M ▾

Volume of the Acid:

ml ▾

Moles of H+ Contributed:

Molarity of the Base:

M ▾

Volume of the Base:

ml ▾

Moles of OH- Contributed:

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Titration Calculator:

This titration calculator is used to determine the unknown molarity (concentration) of an acid or base solution from titration data. Also, it allows us to determine the volumes of the titrants and the moles of H+ and OH- involved in the chemical reaction. By calculating these values, it is easy to understand how strong or weak an acid or base is in a solution.

What is Titration?

"The process of chemical analysis in which a solution of known concentration (titrant) is slowly added to a solution of unknown concentration (analyte) until the reaction reaches a neutral point."

The known volume of titrant is added until a solution reaches a pH ratio of 1:1. When a base or acid is dissolved in water, its H⁺ or OH- ions will dissociate, which will change the natural self-ionization balance of water:

2H₂O ⇌ OH⁻ + H₃O⁺

It will become a stronger acid-base titration solution. At pH 7, the concentrations of H₃O⁺ and OH⁻ are 1:1 (the titration equivalence point).

Titration Formula:

This titration formula determines the unknown concentration of a solution (analyte) reacting with a solution of known concentration (titrant).

nH+ . Va . Ma = nOH- . Mb. Vb

Where:

nH+ = Number of moles of H+ ions
Va = Volume of an acid
Ma = Molarity of an acid
nOH- = Number of moles of OH- ions
Mb = Molarity of a base
Vb = Volume of a base

Method of Acid-Base Titration:

Preparation:

Dissolve the unknown acid/base in water
Make a titrant solution and fill in the burette
In a flask of analyte solution, add an indicator

Titration:

Slowly add the titrant to the analyte solution until the color changes

Endpoint:

Stop the addition of titrant when the indicator shows a change of color

How to Calculate Titration?

Record the Volume:

Note the initial volume of the titrant in the burette and the volume of the analyte from the flask.

Perform the Titration:

Add the titrant to the analyte until the indicator shows a certain change in color, and then record the final volume

Calculate the Volume of Titrant Used:

Calculate the volume of the titrant by using the formula below:

Volume of titrant used = Final volume − Initial volume

Solve the Unknown Concentration and Know the Titration Value:

Using the titration formula, the unknown concentration (molarity) is calculated. Look at the example below, which uses the same process step by step.

The method is a valuable addition when your experiment involves manual determination. To automate the process, you can use the online titration calculator.

Example (Solved):

Find the concentration of acetic acid in vinegar when the NaOH solution is 0.100 M. We used 25.00 mL of the NaOH solution to titrate the vinegar solution to the equivalence point.

CH3COOH + NaOH → CH3COONa (aq) + H2O

Solution:

Calculate the millimoles (mmol) of NaOH used:

mmol NaOH = Moles of NaOH * Volume of NaOH

= 0.100 M * 25.00 mL

= 2.50 mmol

Since the reaction between acetic acid and NaOH is 1:1, the millimoles of acetic acid used equal the millimoles of NaOH used.

mmol of CH3COOH = 2.50 mmol

Step 3: Calculate the molarity of acetic acid

Molarity = mmol of solute ÷ volume of solution

Molarity of CH₃COOH = 2.50 mmol ÷ 10.00 mL

Molarity of CH₃COOH = 0.250 M

Therefore, the concentration of acetic acid in the vinegar solution is 0.250 M.

Estimating the Equivalence Point’s pH:

The pH of the solution at the equivalence point depends on the relative concentrations of the acid and base. You can estimate the pH value of the equivalence point according to the following rule:

Strong acid reacts with a weak base to form a solution (pH < 7)
Strong acid reacts with a strong base to form a solution (pH = 7)
Weak acid reacts with a strong base to form a solution (pH > 7)

If the base is stronger than the acid, the solution will be alkaline, and if the acid is stronger than the base, the solution will be acidic. If the weak acid and weak base have equal strengths and concentrations, the resulting solution will be neutral, with a pH of 7. Therefore, it is difficult to titrate with a weak acid or base because there is no color change.

Table of Common Bases & Acids & Their Strengths:

Base:

Formula	Name	Strength
NaOH	Sodium hydroxide	Strong
KOH	Potassium hydroxide	Strong
Ca(OH)2	Calcium hydroxide	Strong
Ba(OH)2	Barium hydroxide	Strong
NH3	Ammonia	Weak
CH3NH2	Methylamine	Weak
C5H5N	Pyridine	Weak

Acid:

Formula	Name	Strength
HCl	Hydrochloric acid	Strong
HNO3	Nitric acid	Strong
H2SO4	Sulfuric acid	Strong
HBr	Hydrobromic acid	Strong
HI	Hydroiodic acid	Strong
HClO4	Perchloric acid	Strong
HClO3	Chloric acid	Strong
HCOOH	Formic acid	Weak
CH3COOH	Acetic acid	Weak
C6H5COOH	Benzoic acid	Weak
HF	Hydrofluoric acid	Weak
HNO2	Nitrous acid	Weak
H3PO4	Phosphoric acid	Weak

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