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Prepare and standardize 0.1 n NaOH using succinic acid

Why acid-base titration is important in food industry

Saturday, August 27, 2022

Preparation of KCl solution

Learn how to make different concentrations of molar and normal potassium chloride solutions, which are needed for many applications such as research, practical, pharmaceutical, chemical laboratory, industries, etc.

Potassium chloride, often referred to as KCl or potassium salt, is a metal halide salt composed of potassium and chlorine anions in the ratio of 1:1. It has the appearance of a vitreous crystal that is either white or colorless and odorless.

Generally, it is mostly used in the agriculture industry for the production of crop fertilizers, as well as is also applied in the field of medicine (Pharmaceutical), food processing, and in scientific applications.

Generally, a solid form of potassium chloride (KCl) in different-sized packs is supplied in the market by vendors in the form of white crystalline solid powder.

The molecular weight of KCl is 74.555 g·mol⁻¹

The melting point of KCL is 770°C

The density of KCl is 1.984 g/cm3

The solubility of KCl: Soluble in water, highly soluble in alcohols, and insoluble in ether

Table of Contents:

Preparation of 0.02M potassium chloride
Preparation of 0.05M potassium chloride
Preparation of 0.1M potassium chloride
Preparation of 0.2M potassium chloride
Preparation of 0.25M potassium chloride
Preparation of 0.5M potassium chloride
Preparation of 1M potassium chloride
Preparation of 2M potassium chloride
Preparation of 3N potassium chloride
Preparation of 3M potassium chloride
Preparation of 2% potassium chloride
Preparation of 5% potassium chloride
Preparation of 7% potassium chloride
Preparation of 10% potassium chloride
Preparation of 20% potassium chloride

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade potassium chloride (KCl), etc.

Calculation method:

Example: To prepare 1 m KCl with a final volume of 250 ml, we can calculate using the formula below.

Molar mass KCl = 39.1+35.45 = 74.55 g/mol,

Mol KCl needed to make 250 mL of 1 M solution:

mol = 250 mL / 1000 mL/L x 1 mol /L = 0.25 mol KCl
Mass KCl required = 0.25 mol * 74.55 g/mol = 18.6375 g KCl

Therefore, to make a 01 M solution of KCl, dilute 18.63 gm of potassium chloride in 250 ml of distilled water.

Similarly, we can use the above method to determine the weight of KCl that is required to prepare any molarity/normality solution, as 0.1 N KCl is the same as 0.1 M KCl.

How to prepare a 0.02M KCl solution

Weigh accurately 01.49 gm of potassium chloride and dissolve in 250 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare a 0.05M KCl solution

Weigh accurately 3.73 gm of potassium chloride and dissolve in 250 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 0.1M KCl solution

Weigh accurately 07.45 gm of potassium chloride and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare a 0.2M KCl solution

Weigh accurately 14.90 gm of potassium chloride and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare a 0.25M potassium chloride solution

Weigh accurately 18.63 gm of KCl and dissolve it in 750 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1 liter with distilled water, and properly mix it.

How to prepare 0.5M KCl solution

Weigh accurately 09.31 gm of KCl and dissolve it in 150 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How to prepare 1M KCl solution

Weigh accurately 74.55 gm of potassium chloride and dissolve it in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 2M KCl solution

Weigh accurately 14.91 gm of KCl and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 3M KCl solution

Weigh accurately 22.36 gm of potassium chloride and dissolve it in 70 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 4m KCl solution

Weigh accurately 29.82 gm of potassium chloride and dissolve it in 70 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 2% KCl solution?

Weigh accurately 02.00 gm of potassium chloride and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare a 5% KCl solution

Weigh accurately 05.00 gm of potassium chloride and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 7% potassium chloride solution?

Weigh accurately 07.00 gm of KCl solid powder and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to make 10% KCl solution

Weigh accurately 10.00 gm of KCl and dissolve in 80 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 20% solution of potassium chloride?

Weigh accurately 20.00 gm of potassium chloride and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

PRECAUTIONS:

KCl crystals are hygroscopic in nature and should be stored in a tightly closed, cool, and dry place.
Stir a little amount of KCl into a large volume of water at a time, and then dilute the solution.
When making KCl solutions, it is recommended that always use distilled water.
Wear protective gloves, clothing, eye protection, and face protection.
Wash your hands/skin thoroughly after handling.
Handled the chemicals with care, follow laboratory safety measures (SOP), and please use extreme caution when preparing the solution concentrations.

References:

Wikipedia contributors. (2022, August 27). Potassium chloride. In Wikipedia, The Free Encyclopedia. Available Here:
USP Pharmacopoeia: USP29–NF24 Page 1762, Available Here:

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Friday, August 26, 2022

Preparation of sodium bicarbonate solution

Learn how to make different concentrations of molar and normal sodium bicarbonate solutions, which are needed for many applications such as research, practical, pharmaceutical, chemical laboratory, industries, etc.

Sodium bicarbonate is a chemical substance with the formula NaHCO3, also known as sodium hydrogen carbonate, monosodium salt, baking soda, or bicarbonate of soda. Sodium bicarbonate is a white, crystalline substance that often appears as a fine powder, which is a salt composed of bicarbonate anion (HCO3-) and sodium cation (Na+). Its taste is somewhat alkaline and salty, like washing soda (sodium carbonate:Na2CO3).

The molecules of sodium bicarbonate include one sodium cation and one bicarbonate anion. Here, an ionic bond is formed between the sodium ion, which has a positive charge, and the oxygen ion, which has a negative charge.

Generally, a solid form of sodium bicarbonate (NaHCO3) in different-sized packs is supplied in the market by vendors in the form of white crystals, and odorless powder.

The molecular weight of NaHCO3 is 84.0066 g mol−1

The melting point of NaHCO3 is 50°C.

The density of NaHCO3 is 2.20 g/cm3

The solubility of NaHCO3: soluble in water and insoluble in alcohol

Table of Contents:

Preparation of 0.05M sodium bicarbonate
Preparation of 0.1M sodium bicarbonate
Preparation of 0.2M sodium bicarbonate
Preparation of 0.25M sodium bicarbonate
Preparation of 0.5M sodium bicarbonate
Preparation of 1M sodium bicarbonate
Preparation of 2M sodium bicarbonate
Preparation of 3M sodium bicarbonate
Preparation of 2% sodium bicarbonate
Preparation of 5% sodium bicarbonate
Preparation of 7% sodium bicarbonate
Preparation of 10% sodium bicarbonate
Preparation of 20% sodium bicarbonate

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade sodium bicarbonate (NaHCO3), etc.

Calculation method:

Depending on the volume you want to prepare, you can prepare 01 M of NaHCO3 and use the following formula:

M = g / V x molar mass

For example, if you want to make 1M in 0.5L of NaHCO3, you need to determine the amount of sodium bicarbonate in grams.

g = M x V x m.m

g = 01 x 0.5 x 84

g =42.0 g

Therefore, to make a 01 M solution of sodium bicarbonate, dilute 42.00 gm of NaHCO3 in 500 ml of distilled water.

How to prepare a 0.05M sodium bicarbonate solution

Weigh accurately 04.20 gm of NaHCO3 and dissolve in 250 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 0.1M sodium bicarbonate solution

Weigh accurately 08.40 gm of NaHCO3 and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare a 0.2M sodium bicarbonate solution

Weigh accurately 16.80 gm of NaHCO3 and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare a 0.25M NaHCO3 solution

Weigh accurately 21.00 gm of sodium bicarbonate and dissolve it in 750 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1 liter with distilled water, and properly mix it.

How to prepare 0.5M sodium bicarbonate solution

Weigh accurately 10.50 gm of sodium bicarbonate and dissolve it in 150 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How to prepare 1M sodium bicarbonate solution

Weigh accurately 84.00 gm of NaHCO3 and dissolve it in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 2M sodium bicarbonate solution

Weigh accurately 16.80 gm of sodium bicarbonate and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 3M sodium bicarbonate solution

Weigh accurately 63.00 gm of NaHCO3 and dissolve it in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How do you make a 2% sodium bicarbonate solution?

Weigh accurately 02.00 gm of NaHCO3 and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 5% sodium bicarbonate solution

Weigh accurately 05.00 gm of NaHCO3 and dissolve it in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 7% sodium bicarbonate solution?

Weigh accurately 07.00 gm of NaHCO3 solid powder and dissolve in 60 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to make 10% sodium bicarbonate solution

Weigh accurately 10.00 gm of sodium bicarbonate and dissolve in 80 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 20% solution of sodium bicarbonate?

Weigh accurately 20.00 gm of NaHCO3 and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

PRECAUTIONS:

Sodium bicarbonate is non-hygroscopic in nature it should be stored in a tightly closed, cool, and dry place.
Stir a little amount of sodium bicarbonate into a large volume of water at a time, and then dilute the solution.
When making sodium bicarbonate solutions, it is recommended that always use distilled water.
Wear protective gloves, clothing, eye protection, and face protection.
Wash your hands/skin thoroughly after handling.
Handled the chemicals with care, follow laboratory safety measures (SOP), and please use extreme caution when preparing the solution concentrations.

References:

Indian Pharmacopoeia 1996
Wikipedia contributors. (2022, August 23). Sodium bicarbonate. In Wikipedia, The Free Encyclopedia. Available Here:
‘Preparation of Standard Solution of Sodium bicarbonate - Chemistry Practicals Class 11’. BYJUS, Available Here:
‘How to Make a .5 Solution of Sodium Bicarbonate’. Sciencing, Available Here:

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Thursday, August 25, 2022

Preparation of sodium carbonate solution

Learn how to make different concentrations of molar and normal sodium carbonate solutions, which are needed for many applications such as research, practical, pharmaceutical, chemical laboratory, industries, etc.

Sodium carbonate is an inorganic compound with the formula Na2CO3. It is also known as washing soda, soda ash, and soda crystals. Sodium carbonate is a basic salt. All of its forms are white, odorless, water-soluble salts that make solutions in water that are moderately alkaline.

In the structure of Na2CO3, each molecule of sodium carbonate has one carbon atom, two sodium atoms, and three oxygen atoms. Each Sodium cation has a positive charge, while each Carbonate anion has a negative charge. Sodium carbonate is a molecule that has no charge because of this.

Generally, a solid form of sodium carbonate (Na2CO3) in different-sized packs is supplied in the market by vendors in the form of white solid, hygroscopic powder.

The molecular weight of Na2CO3 is 105.9888 g/mol (anhydrous).

The melting point of Na2CO3 is 851 °C

The density of Na2CO3 is 2.54 g/cm3 (25 °C, anhydrous)

The solubility of Na2CO3 is: soluble in water and slightly soluble in aqueous alcohol

Table of Contents:

Preparation of 0.05N sodium carbonate
Preparation of 0.1N sodium carbonate
Preparation of 0.2N sodium carbonate
Preparation of 0.25N sodium carbonate
Preparation of 0.5N sodium carbonate
Preparation of 1N sodium carbonate
Preparation of 2N sodium carbonate
Preparation of 3N sodium carbonate
Preparation of 2% sodium carbonate
Preparation of 5% sodium carbonate
Preparation of 7% sodium carbonate
Preparation of 10% sodium carbonate
Preparation of 20% sodium carbonate

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade sodium carbonate (Na2CO3), etc.

Calculation method:

Molecular weight sodium carbonate – (23×2) + 12 + (3×16) = 46 + 12 + 48 = 106 gm

Normality = Weight / Equivalent weight × 1000 / Volume (in ml)

0.1 = (X/106/2) × (1000 / 500)

0.1 = (X × 2 / 106 ) × (1000 / 500)

X = 0.1 × 53 × 0.5 = 2.65 gm

X = 2.65 gm

Therefore, to make a 0.1 N solution of sodium carbonate, dilute 2.65 gm of Na2CO3 in 500 ml of distilled water.

How to prepare a 0.05N sodium carbonate solution

Weigh accurately 02.65 gm of Na2CO3 and dissolve in 250 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 0.1N sodium carbonate solution

Weigh accurately 05.30 gm of Na2CO3 and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 0.2N sodium carbonate solution

Weigh accurately 10.60 gm of Na2CO3 and dissolve in 500 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 1000 ml with distilled water, and properly mix it.

How to prepare 0.25N Na2CO3 solution

Weigh accurately 06.63 gm of sodium carbonate and dissolve in 250 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 500 ml with distilled water, and properly mix it.

How to prepare 0.5N sodium carbonate solution

Weigh accurately 26.50 gm of sodium carbonate and dissolve in 400 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liters with distilled water, and properly mix it.

How to prepare 1N sodium carbonate solution

Weigh accurately 13.25 gm of Na2CO3 and dissolve in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How to prepare 2N sodium carbonate solution

Weigh accurately 26.50 gm of sodium carbonate and dissolve in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How to prepare 3N sodium carbonate solution

Weigh accurately 39.75 gm of Na2CO3 and dissolve in 100 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 250 ml with distilled water, and properly mix it.

How do you make a 2% sodium carbonate solution

Weigh accurately 02.00 gm of Na2CO3 and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 5% sodium carbonate solution

Weigh accurately 05.00 gm of Na2CO3 and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 7% sodium carbonate solution

Weigh accurately 07.00 gm of Na2CO3 solid powder and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How to prepare 10% sodium carbonate solution

Weigh accurately 10.00 gm of sodium carbonate and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

How do you make a 20% solution of Na2CO3?

Weigh accurately 20.00 gm of sodium carbonate and dissolve in 50 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 100 ml with distilled water, and properly mix it.

PRECAUTIONS:

Sodium carbonate is hygroscopic in nature it should be stored in a tightly closed container.
Stir a little amount of sodium carbonate into a large volume of water at a time, and then dilute the solution.
When making sodium carbonate solutions, it is recommended that always use distilled water.
Wear protective gloves, clothing, eye protection, and face protection.
Wash your hands/skin thoroughly after handling.
Solutions of sodium carbonate are highly alkaline and corrosive. Contact can cause serious skin and eye irritation. Therefore should be handled with care, follow laboratory safety measures (SOP/Procedure), and please use extreme caution when preparing the solution concentrations.

References:

Indian Pharmacopoeia : 1996
Wikipedia contributors. (2022, July 1). Sodium carbonate. In Wikipedia, The Free Encyclopedia. Available Here:
What Is the Difference between Molarity and Normality? Westlab. Available Here:
Making Percent Solutions Of Chemicals, Available Here:
Topic;- preparation properties and uses of sodium carbonate, Available Here:

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Why acid-base titration is important in food industry

Tuesday, August 23, 2022

Why acid-base titration is important in food industry

The analysis of food products by titration ensures that the foods have a balanced composition.

In the last few years, the food industry's quality standards have grown a lot and sometimes reached the level of the pharmaceutical industry. Because of this, more and more modern piston burettes and automatic titrators are being used in the food lab because they meet the requirements for accuracy, reliability, and being ability to keep records.

What is titration?

Titration is an analytical technique in chemistry used to determine the concentration of an unknown component in a sample. It is a type of quantitative chemical analysis utilized in a variety of industries, such as pharmaceutical, food processing, water, textile, dairy, petroleum, chemical manufacturing, and agriculture sector.

The principle behind titration is that we add a solution, called a titrant, to the sample (analyte) we want to analyze. A known chemical in the titrant will react with the sample. A burette is used to add the titrant. Using this tool; we can exactly know the volume of the titrant.

As soon as we do this, a chemical reaction will happen in the sample, which will change its characteristics. At the endpoint or equivalence point of the reaction, the substance reacts with the titrant and the color of the indicator changes.

According to the nature of the chemical reaction occurring between the titrant and sample, there are four types of titrations, including acid-base, redox, complexometric, and precipitation titration. They make it possible for food manufacturers to determine the amount of a reactant present in a sample.

For example, it can be used to determine the amount of salt or sugar present in a product, as well as the concentration of vitamin C or vitamin E, both of which affect the color of the product.

Importance of acid-base titration:

The purpose of a titration is to determine the concentration of the sample solution by titrating the acid solution with a basic solution whose concentration is already known, or vice versa, until the solution is neutralized.

In food processing, the acidity of fruit juice is determined using acid-base titration. Redox titration can be used to determine the concentration of vitamin C in orange juice. The salt content of various foods can be determined using the precipitation titration method.

For salt testing, several food manufacturers employ manual titration techniques. To measure the concentration of salt the Mohr's method one of the oldest titration methods, this uses a silver nitrate solution. The potentiometric titration method is one option that can be performed automatically. This sample measures the change in the membrane potential of the substance.

Three industries in the industrial sector that depends on titration techniques are food processing, pharmaceutical production, and chemical manufacturing. They are used in many significant fields including product research and development, quality control, and large-scale production. In these fields, raw materials need to be calibrated at a high level, and titration can help with this.

Titration is essential to ensure the consistency of products sold, even when advanced processes such as gas chromatography (GC) or liquid chromatography (HPLC) are unavailable to most wineries for practical reasons.

Here are some of the reasons why titration is still used so often today.

It is one of the most accurate quantitative analysis techniques.
It is simple to perform and is economical, requiring little in the way of equipment.
Methods can use for concentrations of the ppm up to 100%.
It does not require a high level of skill.
The results are readily available right away.

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Determination of acetic acid in vinegar

Learn about the assay of acetic acid in a given sample of vinegar using 0.1 n sodium hydroxide through a laboratory experiment or practical.

To determine the percentage purity of acetic acid in a given sample of vinegar using 0.1 n NaOH

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, wash bottle, etc.

Chemicals: LR grade sodium hydroxide (NaOH), acetic acid (CH3COOH), phenolphthalein indicator, etc.

Apparatus: Digital/analytical balance

The determination of acetic acid in vinegar by direct titration:

The major components in vinegar are acetic acid and water. It is a carbon-based compound with a –COOH functional moiety with a single ionizable proton. Vinegar derives its acidity from acetic acid (CH3COOH or HC2H2O2). Acetic acid, (Ethanoic acid), is a weak acid that is a type of organic acid (carboxylic acid).

CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l)

Phenolphthalein or thymol blue are ideal indicators for this titration since the pH at the equivalence point will be larger than 07 when weak acids like acetic acid are titrated with strong bases like NaOH solution.

By titrating an appropriate sample of commercial vinegar with the standardized NaOH solution, it is simple to determine the amount of acetic acid (CH3COOH) present in the vinegar. This experiment requires two steps; first, we must standardize the sodium hydroxide standard solution, followed by the acetic acid test.

Click here to get the procedure for standardization of the sodium hydroxide solution:

Titration procedure:

All glassware should be cleaned and dried according to standard laboratory procedures.
Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
Remove air bubbles from the burette and adjust the reading to zero.
Take 10.00 ml of commercial vinegar sample and pour it into a 250 ml conical flask.
Add 5 ml of distilled water using a pipette.
Add 2-4 drops of phenolphthalein indicator and thoroughly mix the mixture.
Titrate this solution with NaOH solution until the endpoint is reached.
The actual endpoint is indicated by the appearance of a pale pink color.
To get accurate results, repeat the titration three times.
Properly record the readings of the burette.
Take their mean and calculate the % acetic acid in vinegar.

Observation table:

Sr. No.	Content in conical flask	Burette reading		Volume of titrant used (ml)
Sr. No.	Content in conical flask	Initial	Final	Volume of titrant used (ml)
1
2
3
				Mean:

Calculations:

Calculate the solution's molarity using the following formula.
Moles of acetic acid = (M_NaOH)(V_NaOH)

Grams of acetic acid = (moles of acetic acid)(MW)

Grams of vinegar =(volume of vinegar)(density of vinegar)

% acetic acid = (grams of acetic acid / grams of vinegar) x 100

Result:

The concentration of acetic acid in the vinegar solution: _________ %.

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Monday, August 22, 2022

Prepare and standardize 0.1 n NaOH using succinic acid

Learn about the preparation and standardization of 0.1 n NaOH solution using succinic acid through a laboratory experiment or practical.

To prepare and standardize 0.1 n NaOH using succinic acid as a primary standard

Requirements:

Glasswares: Burette, burette stand, conical flask, volumetric pipette, beaker, volumetric flask, funnel, glass rod, wash bottle, etc.

Chemicals: LR grade sodium hydroxide (NaOH), succinic acid (C4H6O4), phenolphthalein indicator, etc.

Apparatus: Digital/analytical balance

Theory:

Solid NaOH can't be used as a primary standard as it can't be available in a pure form. This is because it absorbs moisture and carbon dioxide from the air when it is stored and also when it is weighed.

This reaction consumes hydroxide ions, changing the concentration of a standard sodium hydroxide solution. Thus, sodium hydroxide solutions must be standardized before any analytical use.

For standardizing NaOH, we can use various primary standards such as potassium hydrogen phthalate (PHP), succinic acid, benzoic acid, sulfamic acid, etc.

In this experiment, a standard solution of succinic acid is used as a primary standard to determine the exact concentration of sodium hydroxide. Succinic acid, which dissolves in water to form H+ and succinate ions, is a pure and stable substance that contains two titrable acidic hydrogens.

In this reaction, we use phenolphthalein as an indicator that changes color from colorless to faint pink at the endpoint/equivalence point.

Preparation of 0.1 M NaOH solution:

To make 0.1 M NaOH solution, weigh accurately 02.00 gm of NaOH and dissolve in 200 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 500 ml.

Preparation of 0.1 M standard succinic acid solution:

To make 0.1 M standard succinic acid solution, weigh accurately 0.59 gm of succinic acid and dissolve in 70 ml of distilled water in a volumetric flask, and properly mix it. Once it has completely dissolved, make up the volume to 100 ml.

Titration procedure:

All glassware should be cleaned and dried according to standard laboratory procedures.
Before filling the burette for the titration, rinse it with distilled water and then pre-rinse it with a portion of the titrant solution. Pre-rinsing is required to make sure that all solution in the burette is the desired solution, not a contaminated or diluted solution.
Take the unknown stock solution of titrant in a clean and dry beaker then fill the burette using the funnel.
Remove air bubbles from the burette and adjust the reading to zero.
Take 10.00 ml of succinic acid solution and pour it into a 250 ml conical flask.
Add 2-4 drops of phenolphthalein indicator and mixed thoroughly the mixture.
Titrate this solution with NaOH solution until the endpoint is reached.
The actual endpoint is indicated by the appearance of a faint pink color.
To get accurate results, repeat the titration three times.
Properly record the readings of the burette.
Take their mean and calculate the molarity of sodium hydroxide solution.

Observation table:

Sr. No.	Content in conical flask	Burette reading		Volume of titrant used (ml)
Sr. No.	Content in conical flask	Initial	Final	Volume of titrant used (ml)
1
2
3
				Mean:

Calculations:

Calculate the solution's molarity using given formula.

NNaOH x VNaOH = N(succ. acid.) x V(succ.acid.)

Volume of succinic acid solution in each titration = 10 m

Normality of succinic acid = 0.1 M

Result:

The strength of the prepared sodium hydroxide (NaOH), solution was found to be_____M.

People also ask:

How do you prepare and standardize 0.1 N NaOH solution?

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What is the reaction between succinic acid and NaOH?

What is the type of titration between succinic acid and sodium hydroxide?

What is the standardization of NaOH?

Standardization of NaOH solution lab report

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