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The readings in volumetric ANALYSIS which differ by less than 0.05 ML EIRE KNOWN as concordant readings

The readings in volumetric analysis which differ by less than 0.05 mL Eire known as concordant readings

A solution CONTAINING 1 mole of SOLUTE per LITRE of solution is 1.0M solution

A solution containing 1 mole of solute per litre of solution is 1.0M solution

It is the NUMBER of replaceable hydrogen ATOMS in MOLECULE of the ACID.

It is the number of replaceable hydrogen atoms in molecule of the acid.

METHYL ORANGE. The COLOUR change is yellow to pinkish RED

Methyl orange. The colour change is yellow to pinkish red

EQUIVALENT weight of a base is defined as the NUMBER of parts by mass of a base that is required to NEUTRALISE COMPLETELY one equivalent weight of an acid.

Equivalent weight of a base = molecular weight / acidity

EX: Equivalent weight of NaOH =40/1=40

Equivalent weight of a base is defined as the number of parts by mass of a base that is required to neutralise completely one equivalent weight of an acid.

Equivalent weight of a base = molecular weight / acidity

EX: Equivalent weight of NaOH =40/1=40

Equivalent WEIGHT of an acid is defined as the NUMBER of parts by MASS of an acid that is neutralised completely by ONE equivalent weight of base.

Equivalent weight of an acid = molecular weight / BASICITY

Equivalent weight of an acid is defined as the number of parts by mass of an acid that is neutralised completely by one equivalent weight of base.

Equivalent weight of an acid = molecular weight / basicity

The point at which the reaction b/w titrant & titrate is just complete is called equivalence point or THEORETICAL point.

The point at which a clear visual change is observed after the reaction b/w titranta and titrate is practically complete is end point.

THUS there exists a very SMALL DIFFERENCE b/w the end point & equivalence point.

The point at which the reaction b/w titrant & titrate is just complete is called equivalence point or theoretical point.

The point at which a clear visual change is observed after the reaction b/w titranta and titrate is practically complete is end point.

Thus there exists a very small difference b/w the end point & equivalence point.

UPPER MENISCUS in CASE COLORED SOLUTION.

Upper Meniscus in case colored solution.

The solution of ACCURATELY known strength is called the standard solution and it CONTAINS known WEIGHT of the SOLUTE in a definite volume of the solution.

The solution of accurately known strength is called the standard solution and it contains known weight of the solute in a definite volume of the solution.

1. SELF INDICATOR
2. INTERNAL indicator
3. EXTERNAL indicator

END point is the point which indicates the completion of REACTION by changing its COLOR. It is indicated by the indicator. While equivalence point is the theoretical point at which the equivalent amount of titrand and titrant are ADDED together. It is a theoretical point.

End point is the point which indicates the completion of reaction by changing its color. It is indicated by the indicator. While equivalence point is the theoretical point at which the equivalent amount of titrand and titrant are added together. It is a theoretical point.

The STANDARD SOLUTION whose concentration is measured with the help of PRIMARY standard solution is called secondary standard solution.

Example: NaOH, HCL, H2­SO4 etc.

The standard solution whose concentration is measured with the help of primary standard solution is called secondary standard solution.

Example: NaOH, HCL, H2­SO4 etc.

The stage during titration at which the REACTION is just complete is KNOWN as the END POINT of titration

The stage during titration at which the reaction is just complete is known as the end point of titration

INDICATOR is a CHEMICAL SUBSTANCE which changes colour at the END point.

Indicator is a chemical substance which changes colour at the end point.

The process of ADDING ONE solution from the burette to another in the TITRATION flask in ORDER to complete the chemical reaction involved, is KNOWN as titration

The process of adding one solution from the burette to another in the titration flask in order to complete the chemical reaction involved, is known as titration

100 GRAMS

100 Grams

The equation which is USED to determine the strength of UNKNOWN solution is CALLED normality equation.

It’s mathematical equation is:

Volume of ACID × Normality of acid = Volume of Base × Normality of base

The equation which is used to determine the strength of unknown solution is called normality equation.

It’s mathematical equation is:

Volume of acid × Normality of acid = Volume of Base × Normality of base

The NUMBER of GRAM EQUIVALENT of solute present in in 1 litre of the solution is called normality. It is represented by N.

Normality=Number of gram equivalent of solute/volume of solution in litre

It is RELATED to molarity as:

Normality (N) = Molarity × Basicity of acid

also, Normality (N) = Molarity × Acidity of base

The number of gram equivalent of solute present in in 1 litre of the solution is called normality. It is represented by N.

Normality=Number of gram equivalent of solute/volume of solution in litre

It is related to molarity as:

Normality (N) = Molarity × Basicity of acid

also, Normality (N) = Molarity × Acidity of base

The CRITERIA for a solution to be primary standard solution are as follows:

1. It should be available in pure and dry STATE.
2. Its composition should not be CHANGED on storage. i.e., It should not be toxic, volatile, hygroscopic and deliquescent.
3. It should be highly soluble in WATER without any change in its composition.
4. It should have higher molecular and equivalent weight.

Some of the examples of primary standard solution are:

Sodium carbonate (Na2CO3), Potassium DICHROMATE (K2Cr2O7), oxalic acid (COOH)2.2H2­O, Mohr’s salt etc.

The criteria for a solution to be primary standard solution are as follows:

Some of the examples of primary standard solution are:

Sodium carbonate (Na2CO3), Potassium dichromate (K2Cr2O7), oxalic acid (COOH)2.2H2­O, Mohr’s salt etc.

The solution that contains 1/10th GRAM equivalent of SOLUTE in one liter of its solution is called decinormal solution.

The solution that contains 1/10th gram equivalent of solute in one liter of its solution is called decinormal solution.