Titration Calculator

You might know the fact that whenever an acid or base dissolves in water their H⁺ and OH⁻ dissociate and shift the natural self-ionisation equilibrium of water thus making the solution more acidic or basic. Usually, we have solutions with known volume and unknown molarity for which a color indicator is added. The indicator will alter its color whenever it reaches 1:1 ratio. On adding acid or base with known molarity we can find out how much is needed for this change. Molarity of unknown can be found using the formula nH*Ma*Va=nOH*Mb*Vb

• nH = number of H+ ions contributed per molecule of acid
• Ma = molarity of the acid
• Va = volume of the acid
• nOH = number of OH- ions contributed per molecule of base
• Mb = molarity of base
• Vb = volume of the base.

---

Acid Base Titration Method

Go through the simple guidelines listed below to follow in the Acid Base Titration Method. They are as such

• Firstly, fill the burette with titrant solution. Remember not to pour the solution above your head and take out the funnel once you pour. Then, keep the burrette on a burette stand and note down the starting point of solution within burette. Remove some solution to determine where the measurements began.
• In the next step, measure the amount of analyte and add it to the Erlenmeyer flask. Add indicator to flask and keep a white tile under the burette for better identification of the color.
• Add the titrant slowly by swirling the Erlenmeyer flask constantly. Once the color change becomes slow add the titrant drop by drop. If you observe the color change is permanent then don't add solution anymore.
• Make a note of the endpoint of burette. The difference between both the points will tell you the volume and through which you can find out the molarity of analyte.
• Throw away all the chemicals safely.

---

Titration Curves

Titration Curve is nothing but a plot between concentration of analyte at a given point in experiment to volume of titrant added. In case of Acid base titration using this curve we can decide whether it is a weak or strong acid/base. If you are dealing with a strong acid and strong base the curve around equivalence point is relatively steep and smooth. The curve indicates that a small increase in amount of titrant will have a greater change in pH value.

While dealing with a strong acid and weak base the titration curve is more irregular. Weak acids and bases will not dissociate completely in a solution. Since these molecules doesn't dissociate completely pH shifts less when it is near to the equivalence point.

---

Common Acids Bases and their Strengths

Acids:

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

Bases:

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

---

FAQs on Titration Calculator

1. What is meant by Titration?

Titration Process is a quantitative and volumetric technique used for determining the unknown concentration of a solution by using the known concentration of solution using an indicator.

---

2. What is the aim of Titration?

The Purpose of Titration is to determine an unknown concentration in a sample using analytical method.

---

3. What are the 4 types of Titration?

The 4 types of Titrations are Acid Base Titrations, Redox Titrations, Precipitation Titrations, Complexometric Titrations.