Preparation of oxalic acid solution

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

Oxalic acid is an organic acid having the formula HO2C−CO2H, or (CO2H) 2, and the systematic name ethanedioic acid. It is the simplest dicarboxylic acid.

It is a white, crystalline substance that dissolves in water and forms a colorless solution. Its name derives from the fact that early researchers extracted oxalic acid from flowering plants of the genus Oxalis, commonly known as wood sorrels.

Generally, a solid form of oxalic acid (C2H2O4) in different-sized packs is supplied in the market by vendors in the form of white crystalline solids that are usually about 98-100% pure.

Properties of Oxalic acid(C2H2O4):

Properties of Oxalic acid
Molecular weight	90.034 g·mol−1 (anhydrous) 126.065 g·mol−1 (dihydrate)
Appearance	White crystals
Melting point	189 to 191 °C
Density	1.90 g·cm3 (anhydrous, at 17 °C) 1.653 g·cm−3 (dihydrate)
Solubility	Soluble in water, acetone, alcohol, but poorly soluble in ether

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade oxalic acid(C2H2O4 ), etc.

Calculation method:

In this case, we must determine the mass of oxalic acid (C2H2O4) required to make 1 molar solution of C2H2O4, as well as the volume of the solution. We must use the molarity formula, which is,

Molarity= Moles of solute/Volume of solution

Step-by-step, complete answer:

We must first determine the moles of C2H2O4. The solution is 1 L in volume and has a molarity of 1 M. So, moles of C2H2O4 can be calculated as,

Moles of C2H2O4 =Molarity × Volume of solution= 1L

Moles of C2H2O4 = 1 M ×1L=1 mol

Therefore, the mole of C2H2O4 in the solution is 1 mol.

The mass of C2H2O4 is now calculated using the number of moles of C2H2O4.

Number of moles= Mass/Molar mass

The mole of C2H2O4 is 1 mol, and its molar mass is 90.03g/mol.

1=Mass/90.03g/mol

Mass of C2H2O4 =90.03 g

Therefore, to make a 1 M solution of C2H2O4, we need to dissolve 90.03 g of oxalic acid in 1 liter of distilled water.

Table of Contents: Preparation of 0.02M oxalic acid Preparation of 0.05M oxalic acid Preparation of 0.1M oxalic acid Preparation of 0.2N oxalic acid Preparation of 0.25M oxalic acid Preparation of 0.5M oxalic acid Preparation of 1N oxalic acid Preparation of 2N oxalic acid Preparation of 1% oxalic acid Preparation of 5% oxalic acid Preparation of 10% oxalic acid Preparation of 100 PPM oxalic acid Preparation of 10 PPM oxalic acid Preparation of 1 PPM oxalic acid

How to prepare 0.02M oxalic acid solution?

Weigh accurately 1.80 g of oxalic acid and dissolve it 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 0.05M oxalic acid solution?

Weigh accurately 05.50 gm of C2H2O4 and dissolve it 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 do you make a 0.1M oxalic acid solution?

Weigh accurately 09.00 gm of C2H2O4 and dissolve it 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 0.2M C2H2O4 solution?

Weigh accurately 18.00 gm of oxalic acid and dissolve it 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 oxalic acid solution?

Weigh accurately 22.05 g of C2H2O4 and dissolve it in 700 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 C2H2O4 solution?

Weigh accurately 45.00 gm of C2H2O4 and dissolve in 400 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 1M oxalic acid solution?

Weigh accurately 90.00 gm of oxalic acid and dissolve it 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 2M solution of oxalic acid?

Weigh accurately 45.00 gm of C2H2O4 and dissolve in 200 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 1% solution of oxalic acid?

Weigh accurately 01.00 gm of oxalic acid 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 5% oxalic acid solution?

Weigh accurately 05.00 gm of C2H2O4 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 10% oxalic acid solution?

Weigh accurately 10.00 gm of C2H2O4 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 100 ppm solution of oxalic acid?

In a volumetric flask, dissolve 10 mg of oxalic acid in 100 ml of distilled water to produce a 100 ppm stock solution.

How do you make a 10 ppm solution of oxalic acid?

Take 0.1 ml (100 microliters) from 100 ppm stock solution of oxalic acid and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

How do you make a 1 ppm solution of oxalic acid?

Take 0.1 ml from 100 ppm stock solution of oxalic acid and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• Stir a small amount of oxalic acid into a large volume of water at a time, and then dilute the solution.
• When making oxalic acid solutions, it is recommended that always use distilled/deionized water.
• Wear protective gloves, clothing, eye protection, and face protection.
• Wash your hands/skin thoroughly after handling.
• Excessive consumption of oxalic acid or prolonged skin contact can be hazardous.
• The hazards of C2H2O4 include its toxic and corrosive nature.
• Always store the oxalic acid in sealed containers or in a desiccator to protect it from moisture and light.
• Solutions are 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:

1. Indian Pharmacopoeia: 1996 Wikipedia contributors. (2023, Jan 31). Oxalic acid. In Wikipedia, The Free Encyclopedia. Available Here: 
2. What Is the Difference between Molarity and Normality? Westlab Available Here:
3. Laboratory Solution Preparation, Available Here:
4. Molarity of 0.1 N oxalic acid is: Vedantu, Available Here:

How to prepare 0.1N silver nitrate solution

To make a 0.1N silver nitrate (AgNO3) solution, perform the following steps:

1. Calculate the amount of AgNO3 needed:

• The molar mass of AgNO3 is approximately 169.87 g/mol.
• Since 0.1N means 0.1 mole per liter (1L) of the solution, the amount of AgNO3 needed can be calculated as follows:
• Amount (in grams) = Normality (N) × Volume (in liters) × Molar mass (g/mol)
• Amount = 0.1N × 1L × 169.87 g/mol = 16.987 grams

2. Weigh out 16.987 grams of silver nitrate using an analytical balance. Make sure to handle it with care as silver nitrate is a hazardous substance.

3. Transfer the weighed silver nitrate (16.987 grams) into a clean, dry, and labeled container.

4. Add distilled water to the container to make a final volume of 1 liter. You can use a measuring cylinder or a volumetric flask to measure the exact volume accurately.

5. Carefully dissolve the silver nitrate in the water by gently swirling the container. It may take some time for the solid to dissolve completely. Ensure that all the solid has dissolved before proceeding.

6. Once the silver nitrate is completely dissolved, the solution is ready. You now have a 0.1N silver nitrate solution

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• Stir a little amount of silver nitrate into a large volume of water at a time, and then dilute the solution.
• When making silver nitrate solutions, it is recommended that always use distilled/deionized water.
• Wear protective gloves, clothing, eye protection, and face protection.
• Wash your hands/skin thoroughly after handling.
• The hazards of AgNO3 include its toxic and corrosive nature.
• Always use silver nitrate that has been previously dried at 105°C for 1 hour.
• Always store the silver nitrate in sealed containers or in a desiccator to protect it from moisture and light.
• Silver nitrate produces a long-lasting stain when applied to the skin. You can remove it by applying household ammonia to the stained area of ​​the skin.

How to prepare 0.025N silver nitrate solution

Properties of Silver nitrate (AgNO3)
Molecular weight	169.872 g·mol−1
Appearance	White powder
Melting point	209.7 °C
Density	4.35 g/cm3 (24°C) 3.97 g/cm3 (210°C)
Solubility	Soluble in water, acetone, alcohol, ammonia, ether, glycerol, etc.

To prepare a 0.025N silver nitrate (AgNO3) solution, you will need to follow these steps:

1. Determine the molar mass of silver nitrate (AgNO3). The molar mass of AgNO3 is approximately 169.87 g/mol.

2. Calculate the amount of AgNO3 needed to make the desired concentration. The formula to calculate the amount in grams is:

• Amount (g) = molarity (mol/L) * volume (L) * molar mass (g/mol)
• In this case, we want to prepare 0.025N solution, which means the molarity is 0.025 mol/L. The volume will depend on how much solution you want to make.

Let's assume you want to prepare 500 mL of the solution. The calculations would be as follows:

• Amount (g) = 0.025 mol/L * 0.5 L * 169.87 g/mol
• Amount (g) = 2.122 g
• Therefore, you would need approximately 2.122 grams of silver nitrate.

3. Weigh out the calculated amount of silver nitrate (2.122 gm) using an analytical balance. Make sure the balance is properly calibrated and that you use appropriate safety precautions when handling chemicals.

4. Dissolve the weighed silver nitrate in distilled or deionized water in a suitable container. You can start by adding a small amount of water to dissolve the solid and then gradually add more water while stirring until it is completely dissolved.

5. Once the silver nitrate is fully dissolved, transfer the solution to a volumetric flask of appropriate size (e.g., 500 mL). Rinse the container with distilled or deionized water to ensure all the solution is transferred.

6. Fill the volumetric flask up to the mark with distilled or deionized water while ensuring the bottom of the meniscus aligns with the mark on the flask. This step ensures the final volume is accurately measured.

7. Mix the solution gently by inverting the flask several times to ensure uniformity.

8. Label the container with the concentration, date of preparation, and any other relevant information.

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• Stir a little amount of silver nitrate into a large volume of water at a time, and then dilute the solution.
• When making silver nitrate solutions, it is recommended that always use distilled/deionized water.
• Wear protective gloves, clothing, eye protection, and face protection.
• Wash your hands/skin thoroughly after handling.
• The hazards of AgNO3 include its toxic and corrosive nature.
• Always use silver nitrate that has been previously dried at 105°C for 1 hour.
• Always store the silver nitrate in sealed containers or in a desiccator to protect from moisture and light.
• Silver nitrate produces a long-lasting stain when applied to the skin. You can remove it by applying household ammonia to the stained area of ​​the skin.

How to prepare 0.02N silver nitrate solution

To prepare a 0.02N (Normal) silver nitrate (AgNO3) solution, you will need to follow these steps:

1. Determine the molar mass of silver nitrate (AgNO3):

• Ag (silver) has a molar mass of 107.87 g/mol
• N (nitrogen) has a molar mass of 14.01 g/mol
• (oxygen) has a molar mass of 16.00 g/mol
• Total molar mass of AgNO3 = 107.87 + 14.01 + (3 × 16.00) = 169.87 g/mol

2. Calculate the grams of silver nitrate required to prepare the solution:

• The formula for calculating grams is: grams = normality × molar mass × volume (in liters)
• Given that the normality (N) is 0.02 and the volume will be determined later, we can calculate the grams of AgNO3.

3. Determine the volume of the solution you want to prepare:

• Let's assume you want to prepare 500 mL (0.5 L) of the silver nitrate solution.

4. Calculate the grams of silver nitrate needed:

• grams = 0.02 N × 169.87 g/mol × 0.5 L = 1.6987 grams

5. Weigh out the calculated mass of silver nitrate (1.6987 grams) using an analytical balance.

6. Dissolve the weighed silver nitrate in distilled water:

• Take a clean, dry container and add distilled water.
• Slowly add the weighed silver nitrate to the water while stirring continuously until it is completely dissolved.
• Ensure that all the solid AgNO3 is dissolved.

7. Transfer the solution to a volumetric flask:

• Once the silver nitrate is completely dissolved, transfer the solution to a 500 mL volumetric flask.
• Rinse the container used for dissolution and make sure all the solution is transferred.

8. Dilute the solution to the mark:

• Add distilled water to the volumetric flask gradually, while swirling gently, until the bottom of the meniscus aligns with the mark on the flask.
• Do not overshoot the mark. Add water cautiously to reach the desired volume.

9. Mix the solution:

• Cap the flask tightly and invert it several times to ensure proper mixing of the solution.

You have now prepared a 0.02N silver nitrate solution in a 500 mL volumetric flask. Remember to handle silver nitrate with care as it is toxic and can cause stains. Also, be cautious when using glassware and follow proper laboratory safety practices.

Properties of Silver nitrate (AgNO3)
Molecular weight	169.872 g·mol−1
Appearance	White powder
Melting point	209.7 °C
Density	4.35 g/cm3 (24°C) 3.97 g/cm3 (210°C)
Solubility	Soluble in water, acetone, alcohol, ammonia, ether, glycerol, etc.

Note:

Because the valency is 1, the molarity and normality of the AgNO3 solutions are the same.

Preparation of AgNO3 solution

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

The chemical compound denoted by the formula AgNO3 is commonly known as silver nitrate. It consists of an ionic bond between the silver cation (Ag+) and the nitrate anion (NO3–). Because of its ionic nature, this chemical dissolves easily in water and dissociates into its constituent ions.

Typically, silver nitrate is prepared by combining silver with nitric acid. Silver bullions and silver foils are typical silver materials utilized in these reactions. This reaction results in the formation of silver nitrate, water, and nitrogen oxides. Compared to halides, it is far less light sensitive.

Generally, a solid form of silver nitrate (AgNO3) in different-sized packs is supplied in the market by vendors in the form of white/colorless crystalline solid that are usually about 98-100% pure.

Table of Contents: 1. Preparation of 0.02M AgNO3 2. Preparation of 0.05M AgNO3 3. Preparation of 0.1M AgNO3 4. Preparation of 0.2N AgNO3 5. Preparation of 0.25M AgNO3 6. Preparation of 0.5M AgNO3 7. Preparation of 1N AgNO3 8. Preparation of 2N AgNO3 9. Preparation of 1% AgNO3 10. Preparation of 5% AgNO3 11. Preparation of 10% AgNO3 12. Preparation of 100 PPM AgNO3 13. Preparation of 10 PPM AgNO3 14. Preparation of 1 PPM AgNO3

Properties of Silver nitrate (AgNO3)
Molecular weight	169.872 g·mol−1
Appearance	White powder
Melting point	209.7 °C
Density	4.35 g/cm3 (24°C) 3.97 g/cm3 (210°C)
Solubility	Soluble in water, acetone, alcohol, ammonia, ether, glycerol, etc.

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade silver nitrate (AgNO3), etc.

Calculation method:

In this case, we must determine the mass of silver nitrate (AgNO3) required to make 1 molar solution of AgNO3 as well as the volume of the solution. We must use the molarity formula, which is,

Molarity= Moles of solute/Volume of solution

Step-by-step complete answer:

We must first determine the moles of AgNO3. The solution is 1 L in volume and has a molarity of 1 M.

So, moles of AgNO3 can be calculated as,

Moles of AgNO3=Molarity × Volume of solution= 1L

Moles of AgNO3= 1 M ×1L=1 mol

Therefore, the mole of AgNO3 in the solution is 1 mol.

The mass of AgNO3 now is calculated using the number of moles of AgNO3.

Number of moles= Mass/Molar mass

The mole of AgNO3 is 1 mol, and its molar mass is 169.87g /mol.

1=Mass/169.87g/mol

Mass of AgNO3=169.87 g

Therefore, to make a 1 M solution of AgNO3, we need to dissolve 169.87 g of silver nitrate in 1 liter of distilled water.

Note:

Because the valency is 1, the molarity and normality of the AgNO3 solution are the same.

How to prepare 0.02M AgNO3 solution?

Weigh accurately 3.40 g of silver nitrate and dissolve it 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 0.05M AgNO3 solution?

Weigh accurately 08.49 gm of silver nitrate and dissolve it 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 do you make a 0.1M silver nitrate solution?

Weigh accurately 16.99 gm of AgNO3 and dissolve it 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 AgNO3 solution?

Weigh accurately 33.97 gm of silver nitrate and dissolve it 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 0.25M silver nitrate solution?

Weigh accurately 42.47 gm of AgNO3 and dissolve in 700 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 0.5M AgNO3 solution?

Weigh accurately 84.94 gm of AgNO3 and dissolve in 400 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 1N silver nitrate solution?

Weigh accurately 169.87 gm of silver nitrate and dissolve it 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 2N solution of silver nitrate?

Weigh accurately 84.93 gm of AgNO3 and dissolve in 200 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 1% solution of AgNO3?

Weigh accurately 01.00 gm of silver nitrate 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 5% silver nitrate solution?

Weigh accurately 05.00 gm of AgNO3 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 10% silver nitrate solution?

Weigh accurately 10.00 gm of AgNO3 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 100 ppm solution of AgNO3?

In a volumetric flask, dissolve 10 mg of silver nitrate in 100 ml of distilled water to produce a 100 ppm stock solution.

How do you make a 10 ppm solution of silver nitrate?

Take 0.1 ml (100 microliters) from 100 ppm stock solution of silver nitrate and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

How do you make a 1 ppm solution of silver nitrate?

Take 0.1 ml from 100 ppm stock solution of silver nitrate and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• Stir a little amount of silver nitrate into a large volume of water at a time, and then dilute the solution.
• When making silver nitrate solutions, it is recommended that always use distilled/deionized water.
• Wear protective gloves, clothing, eye protection, and face protection.
• Wash your hands/skin thoroughly after handling.
• The hazards of AgNO3 include its toxic and corrosive nature.
• Always use silver nitrate that has been previously dried at 105°C for 1 hour.
• Always store the silver nitrate in sealed containers or in a desiccator to protect from moisture and light.
• Silver nitrate produces a long-lasting stain when applied to the skin. You can remove it by applying household ammonia to the stained area of the skin.
• Solutions 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:

1. Indian Pharmacopoeia : 1996
2. Wikipedia contributors. (2023, Jan 31). Silver nitrate. In Wikipedia, The Free Encyclopedia. Available Here: 
3. What Is the Difference between Molarity and Normality? Westlab, Available Here:
4. Laboratory Solution Preparation, Available Here:

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Preparation of NaCl solution

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

Sodium chloride, also known as salt, is an ionic substance having the chemical formula NaCl with a sodium and chloride ions ratio of 1:1. It is a crystalline solid with an fcc structure, and it contains four ions of each Na+ and Cl-.

The reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) produces NaCl. In this reaction, both the acid and the base are strong. It can be found in the oceans and seawater, as well as in rock salt.

It is used in medicine (saline solution), fire extinguishers, the textile industry, and the paper industry as well as to produce sodium carbonate, and also used in water softening, etc.

Generally, a solid form of sodium chloride (NaCl) in different-sized packs is supplied in the market by vendors in the form of white/colorless crystalline or cubic crystals that are usually about 98-100% pure.

Table of Contents: Preparation of 0.02M NaCl Preparation of 0.05M NaCl Preparation of 0.1M NaCl Preparation of 0.2M NaCl Preparation of 0.25 M NaCl Preparation of 0.5M NaCl Preparation of 1M NaCl Preparation of 2M NaCl Preparation of 1% NaCl Preparation of 5% NaCl Preparation of 10% NaCl Preparation of 100 ppm NaCl Preparation of 1 ppm NaCl Preparation of 10 ppm NaCl

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 chloride (NaCl), etc.

Calculation method:

In this case, we must determine the mass of sodium chloride (NaCl) required to make 1 molar solution of NaCl as well as the volume of the solution. We must use the molarity formula, which is,

Molarity= Moles of solute/Volume of solution

Step-by-step complete answer:

We must first determine the moles of NaCl. The solution is 1 L in volume and has a molarity of 1 M.

So, moles of NaCl can be calculated as,

Moles of NaCl=Molarity × Volume of solution= 1L

Moles of NaCl= 1 M ×1L=1 mol

Therefore, the mole of NaCl in the solution is 1 mol.

The mass of NaCl now is calculated using the number of moles of NaCl.

Number of moles= Mass/Molar mass

The mole of NaCl is 1 mol, and its molar mass is 58.44 g/mol.

1=Mass/58.44g/mol

Mass of NaCl=58.44 g

Therefore, to make a 1 M solution of NaCl, we need to dissolve 58.44 g of sodium chloride in 1 liter of distilled water.

Note:

Because the valency of NaCl is 1, the molarity and normality of the solution are the same.

How to prepare 0.02M NaCl solution?

Weigh accurately 01.17 g of sodium chloride and dissolve it 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 0.05M NaCl solution?

Weigh accurately 02.92 gm of sodium chloride and dissolve it 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 do you make a 0.1M sodium chloride solution?

Weigh accurately 05.84 gm of sodium chloride and dissolve it 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 NaCl solution?

Weigh accurately 11.69 gm of sodium chloride and dissolve it 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 0.25M sodium chloride solution?

Weigh accurately 14.61 gm of NaCl and dissolve in 700 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 0.5N NaCl solution?

Weigh accurately 29.22 gm of NaCl and dissolve in 400 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 1N NaCl solution?

Weigh accurately 58.44 gm of sodium chloride and dissolve it 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 2N solution of pentahydrate sodium chloride?

Weigh accurately 29.22 gm of NaCl and dissolve in 200 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 1% solution of NaCl?

Weigh accurately 01.00 gm of sodium 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 5% sodium chloride solution?

Weigh accurately 05.00 gm of NaCl 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 10% sodium chloride solution?

Weigh accurately 10.00 gm of NaCl 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 100 ppm solution of NaCl?

In a volumetric flask, dissolve 10 mg of sodium chloride in 100 ml of distilled water to produce a 100 ppm stock solution.

How do you make a 1 ppm solution of sodium chloride?

Take 0.1 ml (100 microliters) from 100 ppm stock solution of sodium chloride and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

How do you make a 10 ppm solution of sodium chloride?

Take 01 ml from 100 ppm stock solution of sodium chloride and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• NaCl is hygroscopic in nature it should be stored in a tightly closed container.
• Stir a little amount of sodium chloride into a large volume of water at a time, and then dilute the solution.
• When making sodium chloride 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 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:

1. Indian Pharmacopoeia : 1996
2. Wikipedia contributors. (2023, March 11). Sodium chloride. In Wikipedia, The Free Encyclopedia. Available Here: 
3. sWhat Is the Difference between Molarity and Normality? Westlab, Available Here:
4. Laboratory Solution Preparation, Available Here:

Preparation of copper sulphate solution

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

Copper (II) sulphate, more commonly referred to as copper sulphate, is an inorganic compound that has the formula CuSO4. It forms hydrates CuSO4•nH2O, where n can range from 1 to 7. Copper sulphate is manufactured by treating copper metal with sulfuric acid or copper oxides with sulfuric acid (H2SO4).

Copper sulfate is used as a drying agent and in several industrial applications. It is also employed in different chemical tests such as Fehling's, Benedict's, and Biuret reagents to test for proteins, and reducing sugars.

Generally, a solid form of copper sulphate (CuSO4•5H2O pentahydrate) in different-sized packs is supplied in the market by vendors in the form of blue (pentahydrate) crystals that are usually about 98% pure.

• The molecular weight of CuSO4•5H2O is 249.685 g/mol (pentahydrate)
• The melting point of CuSO4•5H2O is 560 °C
• The density of CuSO4•5H2O is 2.286 g/cm3
• The solubility of CuSO4•5H2O is: highly soluble in water and methanol but insoluble in ethanol and acetone.

Table of Contents: Preparation of 0.02M CuSO4 Preparation of 0.05M CuSO4 Preparation of 0.1M CuSO4 Preparation of 0.2M CuSO4 Preparation of 0.25 M CuSO4 Preparation of 0.5M CuSO4 Preparation of 1M CuSO4 Preparation of 2M CuSO4 Preparation of 1% CuSO4 Preparation of 2% CuSO4 Preparation of 5% CuSO4 Preparation of 10% CuSO4 Preparation of 20% CuSO4 Preparation of 100 ppm CuSO4 Preparation of 1 ppm CuSO4 Preparation of 10 ppm CuSO4

Requirements of glassware, chemicals, and apparatus:

Digital balance, beaker, pipette, pipette bulb, volumetric flask, measuring cylinder, glass rod, funnel, distilled water, AR/LR grade copper sulfate (CuSO4), etc.

Calculation method:

For example, we calculate how much weight of solid copper sulfate is needed to prepare a 0.1M solution in a 500 ml flask.

The following equation can be used to determine the molarity of a given solution:

Molarity=W/m×1000/V

Rearranging this equation to account for the weight necessary gives us,

W =Molarity × m × V/ 1000

Putting the given values in this equation,

W=0.5×249.685 ×500/1000 =62.42 gm

Therefore, to make a 0.1 N solution of copper sulphate, dilute 62.42 gm of CuSO4 in 500 ml of distilled water.

Note:

We have calculated the concentration based on CuSO4.5H2O (Pentahydrate) for preparing the solutions listed below.

How to prepare 0.02M CuSO4 solution?

Weigh accurately 04.99 g of copper sulphate and dissolve it 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 0.05M CuSO4 solution?

Weigh accurately 06.24 gm of copper sulphate and dissolve it 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 do you make a 0.1 M copper sulfate solution?

Weigh accurately 24.97 gm of copper sulphate and dissolve it 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 0.2M CuSO4 solution?

Weigh accurately 49.94 gm of copper sulphate and dissolve it 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 0.25M Copper sulphate solution?

Weigh accurately 62.42 gm of CuSO4 and dissolve in 700 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 0.5M CuSO4 solution?

Weigh accurately 124.84 gm of CuSO4 and dissolve in 400 ml of distilled water in a volumetric flask. Once it has completely dissolved, make up the volume to 01 liter with distilled water, and properly mix it.

How to prepare 1M CuSO4 solution?

Weigh accurately 24.97 gm of copper sulphate 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 2M solution of pentahydrate copper sulphate?

Weigh accurately 124.84 gm of CuSO4 and dissolve in 200 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 1% solution of CuSO4?

Weigh accurately 01.00 gm of copper sulphate 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 2% CuSO4 solution?

Weigh accurately 02.00 gm of copper sulphate 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 5% copper sulphate solution?

Weigh accurately 05.00 gm of CuSO4 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% copper sulphate solution?

Weigh accurately 10.00 gm of CuSO4 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 copper sulphate?

Weigh accurately 20.00 gm of CuSO4 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 a 100 ppm solution of CuSO4?

In a volumetric flask, dissolve 10 mg of copper sulphate in 100 ml of distilled water to produce a 100 ppm stock solution.

How do you make a 1 ppm solution of copper sulphate?

Take 0.1 ml (100 microlitres) from 100 ppm stock solution of copper sulphate and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

How do you make a 10 ppm solution of copper sulphate?

Take 01 ml from 100 ppm stock solution of copper sulphate and dilute it to 10 ml, the resulting solution has a concentration of 1 ppm.

PRECAUTIONS:

• When working with chemicals, avoid contact with skin, eyes, clothing, ingestion, and inhalation.
• CuSO4 is hygroscopic in nature it should be stored in a tightly closed container.
• Stir a little amount of copper sulphate into a large volume of water at a time, and then dilute the solution.
• When making copper sulphate 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 CuSO4 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:

1. Indian Pharmacopoeia : 1996
2. Wikipedia contributors. (2023, March 7). Copper(II) sulfate. In Wikipedia, The Free Encyclopedia. Available Here:
3. What Is the Difference between Molarity and Normality? Westlab. Available Here:
4. Making Percent Solutions Of Chemicals, Available Here: