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# Titration

In order to utilize any matter just knowing a substance is not enough. One has to know about its properties and its characteristics. There are various methods to determine the properties of a
chemical substance.

One of the most common and most reliable methods is the method of titration. Titration can be broadly described as finding out the strength of an unknown solution with a standard solution whose strength is known.

## What is Titration?

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Titration is a method of finding out the strength of a solution either in the terms of molarity or normality or molality or acidity or alkalinity or precipitatability.Titration can also be used to find out the presence of elements either in their elemental state or in their compound state. Some substances get adsorbed on the surface of other substances and this can also be estimated by the process of titration.
Formation of complexes is the characteristic of certain metals. Different varieties co complexes are formed by the group of same elements and these will have different properties. This is possible because of the change in the oxidation number of the metal which we call as variable valency.

By the method of titration the changes in the oxidation states can be established and in turn the strength of the solution. Estimation of amino acids are also done by the method of titration.

## Titration Equation

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Titrations are done in liquid medium generally between clear solutions. The solutions are measured in volumes and the amount of the substance dissolved in the solvent gives the concentration of the solution. The concentration of solution is in terms of molarity or normality.

Molarity (M) is defined as the number of moles present in one litre of solution. Mole is a number which is also called Avogadro number of molecules.

Number of moles of a substance is the ratio of the mass of the substance and the molecular mass.

M = $\frac{mass}{mol\ mass}$

Normality(N) is defined as the ratio between the mass of the substance and its equivalent mass.

N = $\frac{mass}{Eq\ mass}$

Equivalent mass is defined as the ratio between the molecular mass ans the valency of the substance

Eq.mass(E) = $\frac{Mol\ mass}{Valency}$

In titrations the concentration of one of the solutions is known which is called standard solution or titrant. The solution of which the concentration is to be found is called aliquot or titrate.

According to the Stoichiometric equation, a reaction takes place in equivalent proportions. Thus the product of Volume(V) and molarity(M) or the normality(N) of one of the solutions is equal to that of the other solution at the equivalence point or end point of the titration.

Indicator is used to get a sharp end point in a titration.

Thus the Titration equation is V1M1 = V2M2 Where V1is the volume and M1 is the molarity of standard solution. V2 is the volume of the unknown concentration solution of which the molarity is to be found.

Therefore
M2 = $\frac{V_1M_1}{V_2}$

Concentration of the unknown solution is M X mol.mass. This is the titration equation.

## Titration Formula

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Since titrations are mostly meant to find the concentrations we can use a direct equation for titration formula. If Ck is the concentration of known solution the volume of which is found to be Vk. To find the concentration Cuk of Vuk volume of given unknown solution, the concentration.

Cuk = $\frac{C_k X V_k}{V_uk}$

This is titration formula.

## End Point of Titration

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End point of titration is also known as equivalence point. At this point both the titrant and titrate are in stoichiometric proportions. If it is an acid base titration the endpoint of titration is thee point at which the acid and base are stoichiometrically balanced in reaction and the pH of the mixture is neutral.

The endpoint of titration is indicated sharply by a suitable indicator either added directly to the solution or used externally.

## Titration Procedure

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The titration procedure is very simple.
1. The apparatus used are a conical flask of 25mL or 50 mL or 100 mL capacity depending on the type of titration, a pipette of suitable capacity marking, a volumetric flask suitable to make the standard solution, sensitive balance and a burner if heating is required.
2. A solution of known concentration is made in a volumetric flask. This gives us the known volume and known normality or molarity.
3. This is filled in a burette and the readings are noted.
4. Care should be taken to avoid the presence of air gaps in the burette.
5. With the help of a pipette a fixed volume of the unknown concentration solution is taken in a conical flask and this is called aliquot.
6. A few drops of suitable indicator is added to this solution in the flask.
7. Keeping the flask under the nozzle of the burette which is fixed vertically on a stand slowly the standard solution is run in to the flask with consistent stirring.
8. At the end point the indicator changes its color. The same procedure is repeated several times until concurrent values are obtained.

## Titration Examples

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The common classroom examples of titrations are the determination of the strength of NaOH solution by titrating with Hydrochloric acid. It is not possible to make a standard solution of NaOH by molecular mass method since it is highly hygroscopic crystals.

Similarly hydrochloric acid is a liquid and difficult to get the exact strength. While to conduct the experiment first a standard sodium carbonate solution is made by weighing pure anhydrous sodium carbonate and dissolving it in known quantity of water. This standard solution is used to establish the strength of HCl, which in turn is used to determine the strength of NaOH.

## Titration Calculations

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For a typical acid base titration in which the strength of the base is to be found out, the calculations can be as follows.

Base: Volume of the base taken (Pipette reading) Vb mL
Normality of the base (To be foundout) Nb mL
Acid: Volume of the acid (Burette reading) Va mL
Normality of the acid (Known) Na mL

Normality of Base

Nb = $\frac{V_a X N_a}{V_b}$

Concentration of the base in given solution in percentage is

Nb X E.W. X 100/1000 = x%

## Back Titration

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1. Back titration is a slightly complicated titration procedure than the simple or direct titration. In this one reagent with known concentration is added in excess.
2. The volatile component of the original compound whose concentration is to be established is allowed to react with the excess solution.
3. The remaining quantity of the known reagent is titrated which will give the value that is consumed by the volatile component.
4. For example, to know the strength of Ammonium sulphate, the compound is mixed with excess sodium hydroxide in a specially designed glass flask (kjeldahl flask).
5. Sodium hydroxide reacts with the salt and releases ammonia gas. The released gas is absorbed in known excess volume of sulfuric acid.
6. All the gas is driven out by heating the flask. The excess sulfuric acid is back titrated which will give the acid consumed by the ammonia gas which in turn gives the content of ammonia in the salt.

## Redox Titration

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Redox titration is also known as Oxidation reduction titration. In this type of titration the change in oxidation states give the amount of metal present in the given unknown quality substance.

Generally these titration use oxidizing agents like Potassium permanganate and Potassium di chromate in acid medium.

## Titration Graph

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• Titration is a technique of finding the concentration of a particular variety in a solution whose concentration is unknown.
• The process of titration involves two components titrant and titrate.
• Titrant is generally the liquid of unknown concentration and titrant is the solution the concentration of which is known and by adding which in small quantities the process of titration is performed. The point at which the change one is looking for arrives is called end point.
• There are varieties of titrations such as acid base titration, oxidation reduction (redox) titrations, precipitation titrations, adsorption titrations and complex titrations etc.,
• A titration graph or titration curve is obtained in a graph one the graph is plotted with the readings of a titration.
• Since it is a titration of volumes and one of the volumes is generally fixed, the other quality of the fixed volume is taken one axis.
• The other axis is for the volume that is added to achieve the end point. A line joining the volumes to the changing quality on the other axis is called the titration curve.
• The advantage of the titration curve is that it gives an accurate measure and value of the titration.
• There are different varieties of titration graphs. Acid-base graph, pH graph, pKa titration graph etc.

## Titrations Problems

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Below you could see problems

### Solved Examples

Question 1: 25 mL of sulfuric acid is found to be a deci-normal solution. When it is titrated against NaOH of unknown strength, it took 28.8 mL to reach the neutralization point. Calculate the normality of NaOH and How many grams of NaOH is required to dissolve in 2 L to get this strength solution?
Solution:

• Volume of acid = Va = 25 mL
• Normality of acid = Na = 1/10 = 0.1N
• Volume of alkali = Vb = 28.8 mL
• Normality of base = Nb = 25 X 0.1 / 28.8 = 0.0868 N
• Grams of NaOH per 1L = Normality X Mol.
• mass/ valency = 25X0.1X40/ 28.8X1 = 3.47222 g
• Grams of NaOH in 2 L = 3.472 X 2 = 6.974 g. Ans.

Question 2: What will be medium of the resultant solution when 200 mL of deci-normal solution of sulfuric acid is mixed with 2.12 g of anhydrous sodium carbonate. Will it be neutral, acidic or basic?
Solution:

Molarity M = N/2 . 0.1 N = 0.05 M. That is 0.05 moles in 1L. In 200 mL it will be 0.05 X200/1000 = 0.01 moles.
106 g of Na2CO3 is 1 mole. Then 2.12 g will be 2.12/106 = 0.02 moles.
The solution is basic in nature since the molar ratio is is 1:2; 2 being the base.

 More topics in Titration Amperometry Equivalence Point Acid Base Titration Indicators Complexometric Titration Karl Fischer Titration Iodometric Titration Redox Titration pH Indicators Titration Curve
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