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.
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:
|
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) |
|
Solubility |
Soluble in water, acetone, alcohol, ammonia, ether, glycerol, etc. |
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:
- Indian Pharmacopoeia : 1996
- Wikipedia contributors. (2023, Jan 31). Silver nitrate. In Wikipedia, The Free Encyclopedia. Available Here:
- What Is the Difference between Molarity and Normality? Westlab, Available Here:
- Laboratory Solution Preparation, Available Here:
People also ask:
How do you make 0.01 M of AgNO3?
How do you make a 0.05 M AgNO3 solution?
How do you make 1m AgNO3 solution?
What is the concentration of 0.1 M AgNO3?
How do you calculate 0.1 N AgNO3 solution?
1mm silver nitrate solution preparation
Standardization of silver nitrate solution with potassium chromate as indicator
How do you make 0.1 N AgNO3 solution of 100 ml?
Standardization of silver nitrate using sodium chloride
Preparation of silver nitrate solution for chloride test
How to calculate normality of silver nitrate solution
No comments:
Post a Comment