When working in a chemistry laboratory, preparing standardized solutions is a fundamental skill. One such essential solution is 1 Molar Nitric Acid (HNO₃), widely used in analytical chemistry, titration processes, and as a reagent in numerous chemical reactions. This detailed guide outlines every step involved in preparing a 1M solution of nitric acid with precision and safety.
Understanding 1 Molar Nitric Acid.
A 1 Molar (1M) solution of nitric acid contains 1 mole of HNO₃ per liter of solution. Since nitric acid is usually available as a concentrated liquid (approximately 68-70% by weight), we must dilute the concentrated acid appropriately using distilled or deionized water to achieve the required molarity.
Chemicals and Materials Required
To prepare 1M nitric acid safely and accurately, we need the following:
- Concentrated Nitric Acid (HNO₃), typically 68–70% (w/w), with a density of approximately 1.41 g/mL
- Distilled or Deionized Water
- 1-Liter Volumetric Flask
- Glass Stirring Rod
- Measuring Cylinder (preferably 100 mL)
- Pipette (Optional, for precision)
- Beaker (250 mL or larger)
- Funnel
- Lab Gloves, Goggles, and Lab Coat for Safety
Calculation to Prepare 1M HNO₃
Before we begin the practical steps, let’s calculate how much concentrated nitric acid we need.
Step 1: Molarity Equation
C₁V₁ = C₂V₂
Where:
- C₁ = Concentration of stock solution (typically ~15.8 M for 68% HNO₃)
- V₁ = Volume of stock solution required
- C₂ = Desired concentration = 1 M
- V₂ = Final volume = 1000 mL = 1 L
15.8 × V₁ = 1 × 1000 ⇒ V₁ = 1000 ÷ 15.8 = 63.2 mL
So, we need 63.2 mL of concentrated HNO₃ and will dilute it to a final volume of 1 liter.
Safety First – Important Precautions
Before you start:
- Always add acid to water, never the reverse, to prevent exothermic splashing or boiling.
- Carry out the procedure in a fume hood to avoid breathing in hazardous nitric acid fumes.
- Wear protective gloves, goggles, and a lab coat
- Keep neutralizing agents (e.g., sodium bicarbonate) nearby in case of spills.
- Work in a well-ventilated area.
Procedure: How to Prepare 1M Nitric Acid Solution
Step 1: Measure Water
- Take a 1-liter volumetric flask and add about 800 mL of distilled water into it using a funnel.
- This leaves space for the acid and reduces the risk of overshooting the mark.
Step 2: Measure Concentrated HNO₃
- Use a graduated measuring cylinder to carefully measure 63.2 mL of concentrated nitric acid.
- Handle with care, and do not inhale the vapors.
Step 3: Add Acid to Water
- Slowly pour the nitric acid into the water in the volumetric flask using a glass funnel.
- Stir gently with a clean glass rod during addition to ensure mixing.
- Allow the mixture to cool if it becomes warm.
Step 4: Make Up the Volume
- Once the mixture has cooled to room temperature, top up with distilled water to exactly 1000 mL using a dropper for accuracy.
- Seal the flask and turn it upside down several times to mix thoroughly.
Storage and Labeling
- Transfer the solution into a chemical-resistant, labeled storage bottle.
- Clearly mark:
- “1M Nitric Acid”
- Date of Preparation
- Prepared By (Name/Initials)
- Store in a cool, dark place away from organic materials and incompatible substances.
Verification of Molarity (Optional but Recommended)
For critical applications, verify the molarity using acid-base titration against a standard sodium carbonate or sodium hydroxide solution. This ensures precise concentration for analytical tasks.
Applications of 1M Nitric Acid
- Titrations in volumetric analysis.
- Etching and metal cleaning.
- Nitrate ion tests.
- Reagent in synthesis and laboratory experiments.
- Sample digestion for spectrometry.
Tips for Accurate Solution Preparation
- Always use volumetric flasks for high accuracy.
- Rinse all glassware with distilled water before use.
- Do not pipette acids by mouth; use a pipette filler.
- Check the expiry of chemicals and concentrations of commercial acids.
- Dispose of acid waste properly according to hazardous waste protocols.
Common Mistakes to Avoid
- Adding water to acid – This can cause dangerous splattering.
- Not cooling before final dilution – Heat may cause evaporation or volume distortion.
- Improper labeling Leads to confusion and safety risks.
- Ignoring ventilation – Inhalation of nitric acid fumes is hazardous.
Conversion Chart: Molarity vs Volume of Concentrated HNO₃
| Desired Molarity (M) | Volume of 68% HNO₃ per 1L Solution (mL) |
|---|---|
| 0.1 M | 6.3 mL |
| 0.5 M | 31.6 mL |
| 1 M | 63.2 mL |
| 2 M | 126.4 mL |
| 5 M | 316 mL |
Note: Always perform your calculations if your stock acid concentration varies.
Conclusion
Preparing 1 molar nitric acid is a straightforward but precise laboratory task. By following the proper calculations, safety protocols, and dilution steps, we can produce a reliable and standardized acid solution for a wide range of chemical processes. Whether for titration or synthesis, 1M HNO₃ remains a cornerstone in the chemistry lab.
How to prepare 1 molar nitric acid?
When working in a chemistry laboratory, preparing standardized solutions is a fundamental skill. One such essential solution is 1 Molar Nitric Acid (HNO₃), widely used in analytical chemistry, titration processes, and as a reagent in numerous chemical reactions. This detailed guide outlines every step involved in preparing a 1M solution of nitric acid with precision and safety.
Understanding 1 Molar Nitric Acid.
A 1 Molar (1M) solution of nitric acid contains 1 mole of HNO₃ per liter of solution. Since nitric acid is usually available as a concentrated liquid (approximately 68-70% by weight), we must dilute the concentrated acid appropriately using distilled or deionized water to achieve the required molarity.
Chemicals and Materials Required for 1 Molar Nitric Acid
To prepare 1M nitric acid safely and accurately, we need the following:
Concentrated Nitric Acid (HNO₃), typically 68–70% (w/w), with a density of approximately 1.41 g/mL
Distilled or Deionized Water
1-Liter Volumetric Flask
Glass Stirring Rod
Measuring Cylinder (preferably 100 mL)
Pipette (Optional, for precision)
Beaker (250 mL or larger)
Funnel
Lab Gloves, Goggles, and Lab Coat for Safety
Calculation to Prepare 1 Molar Nitric Acid
Before we begin the practical steps, let’s calculate how much concentrated nitric acid we need.
Step 1: Molarity Equation
C₁V₁ = C₂V₂
Where:
C₁ = Concentration of stock solution (typically ~15.8 M for 68% HNO₃)
V₁ = Volume of stock solution required
C₂ = Desired concentration = 1 M
V₂ = Final volume = 1000 mL = 1 L
15.8 × V₁ = 1 × 1000 ⇒ V₁ = 1000 ÷ 15.8 = 63.2 mL
So, we need 63.2 mL of concentrated HNO₃ and will dilute it to a final volume of 1 liter.
Safety First – Important Precautions
Before you start:
Always add acid to water, never the reverse, to prevent exothermic splashing or boiling.
Carry out the procedure in a fume hood to avoid breathing in hazardous nitric acid fumes.
Wear protective gloves, goggles, and a lab coat
Keep neutralizing agents (e.g., sodium bicarbonate) nearby in case of spills.
Work in a well-ventilated area.
Procedure: How to Prepare 1 Molar Nitric acid Solution
Step 1: Measure Water
Take a 1-liter volumetric flask and add about 800 mL of distilled water into it using a funnel.
This leaves space for the acid and reduces the risk of overshooting the mark.
Step 2: Measure Concentrated HNO₃
Use a graduated measuring cylinder to carefully measure 63.2 mL of concentrated nitric acid.
Handle with care, and do not inhale the vapors.
Step 3: Add Acid to Water
Slowly pour the nitric acid into the water in the volumetric flask using a glass funnel.
Stir gently with a clean glass rod during addition to ensure mixing.
Allow the mixture to cool if it becomes warm.
Step 4: Make Up the Volume
Once the mixture has cooled to room temperature, top up with distilled water to exactly 1000 mL using a dropper for accuracy.
Seal the flask and turn it upside down several times to mix thoroughly.
Storage and Labeling
Transfer the solution into a chemical-resistant, labeled storage bottle.
Clearly mark: “1 Molar Nitric acid”
Date of Preparation
Prepared By (Name/Initials)
Store in a cool, dark place away from organic materials and incompatible substances.
Verification of Molarity (Optional but Recommended)
For critical applications, verify the molarity using acid-base titration against a standard sodium carbonate or sodium hydroxide solution. This ensures precise concentration for analytical tasks.
Applications of 1M Nitric Acid
Titrations in volumetric analysis.
Etching and metal cleaning.
Nitrate ion tests.
Reagent in synthesis and laboratory experiments.
Sample digestion for spectrometry.
Tips for Accurate Solution Preparation
Always use volumetric flasks for high accuracy.
Rinse all glassware with distilled water before use.
Do not pipette acids by mouth; use a pipette filler.
Check the expiry of chemicals and concentrations of commercial acids.
Dispose of acid waste properly according to hazardous waste protocols.
Common Mistakes to Avoid
Adding water to acid – This can cause dangerous splattering.
Not cooling before final dilution – Heat may cause evaporation or volume distortion.
Improper labeling Leads to confusion and safety risks.
Ignoring ventilation – Inhalation of nitric acid fumes is hazardous.
Conversion Chart: Molarity vs Volume of Concentrated HNO₃
| Desired Molarity (M) | Volume of 68% HNO₃ per 1L Solution (mL) |
|---|---|
| 0.1 M | 6.3 mL |
| 0.5 M | 31.6 mL |
| 1 M | 63.2 mL |
| 2 M | 126.4 mL |
| 5 M | 316 mL |
Conclusion
Preparing 1 molar nitric acid is a straightforward but precise laboratory task. By following the proper calculations, safety protocols, and dilution steps, we can produce a reliable and standardized acid solution for a wide range of chemical processes. Whether for titration or synthesis, 1M HNO₃ remains a cornerstone in the chemistry lab.
What is the procedure to prepare a 1 molar Nitric acid solution?
Procedure to Prepare 1 Molar Nitric Acid Solution
Step 1: Measure Water
Take a 1-liter volumetric flask and add about 800 mL of distilled water into it using a funnel.
This leaves space for the acid and reduces the risk of overshooting the mark.
Step 2: Measure Concentrated HNO₃
Use a graduated measuring cylinder to carefully measure 63.2 mL of concentrated nitric acid.
Handle with care, and do not inhale the vapors.
Step 3: Add Acid to Water
Slowly pour the nitric acid into the water in the volumetric flask using a glass funnel.
Stir gently with a clean glass rod during addition to ensure mixing.
Allow the mixture to cool if it becomes warm.
Step 4: Make Up the Volume
Once the mixture has cooled to room temperature, top up with distilled water to exactly 1000 mL using a dropper for accuracy.
Seal the flask and turn it upside down several times to mix thoroughly.
Storage and Labeling
Transfer the solution into a chemical-resistant, labeled storage bottle.
Clearly mark: “1M Nitric Acid”
Date of Preparation
Prepared By (Name/Initials)
Store in a cool, dark place away from organic materials and incompatible substances.
Step 1: Measure Water
Take a 1-liter volumetric flask and add about 800 mL of distilled water into it using a funnel.
This leaves space for the acid and reduces the risk of overshooting the mark.
Step 2: Measure Concentrated HNO₃
Use a graduated measuring cylinder to carefully measure 63.2 mL of concentrated nitric acid.
Handle with care, and do not inhale the vapors.
Step 3: Add Acid to Water
Slowly pour the nitric acid into the water in the volumetric flask using a glass funnel.
Stir gently with a clean glass rod during addition to ensure mixing.
Allow the mixture to cool if it becomes warm.
Step 4: Make Up the Volume
Once the mixture has cooled to room temperature, top up with distilled water to exactly 1000 mL using a dropper for accuracy.
Seal the flask and turn it upside down several times to mix thoroughly.
Storage and Labeling
Transfer the solution into a chemical-resistant, labeled storage bottle.
Clearly mark: “1M Nitric Acid”
Date of Preparation
Prepared By (Name/Initials)
Store in a cool, dark place away from organic materials and incompatible substances.
How to calculate the molarity of 1 molar nitric acid?
Calculation to Prepare 1 Molar Nitric Acid (HNO₃)
Before we begin the practical steps, let’s calculate how much concentrated nitric acid we need.
Step 1: Molarity Equation
C₁V₁ = C₂V₂
Where:
C₁ = Concentration of stock solution (typically ~15.8 M for 68% HNO₃)
V₁ = Volume of stock solution required
C₂ = Desired concentration = 1 M
V₂ = Final volume = 1000 mL = 1 L
15.8 × V₁ = 1 × 1000 ⇒ V₁ = 1000 ÷ 15.8 = 63.2 mL
So, we need 63.2 mL of concentrated HNO₃ and will dilute it to a final volume.
Before we begin the practical steps, let’s calculate how much concentrated nitric acid we need.
Step 1: Molarity Equation
C₁V₁ = C₂V₂
Where:
C₁ = Concentration of stock solution (typically ~15.8 M for 68% HNO₃)
V₁ = Volume of stock solution required
C₂ = Desired concentration = 1 M
V₂ = Final volume = 1000 mL = 1 L
15.8 × V₁ = 1 × 1000 ⇒ V₁ = 1000 ÷ 15.8 = 63.2 mL
So, we need 63.2 mL of concentrated HNO₃ and will dilute it to a final volume.
How do you make a 1 Molar Nitric acid solution?
When working in a chemistry laboratory, preparing standardized solutions is a fundamental skill. One such essential solution is 1 Molar Nitric Acid (HNO₃), widely used in analytical chemistry, titration processes, and as a reagent in numerous chemical reactions. This detailed guide outlines every step involved in preparing a 1M solution of nitric acid with precision and safety.
Understanding 1 Molar Nitric Acid.
A 1 Molar (1M) solution of nitric acid contains 1 mole of HNO₃ per liter of solution. Since nitric acid is usually available as a concentrated liquid (approximately 68-70% by weight), we must dilute the concentrated acid appropriately using distilled or deionized water to achieve the required molarity.
Chemicals and Materials Required
To prepare 1M nitric acid safely and accurately, we need the following:
Concentrated Nitric Acid (HNO₃), typically 68–70% (w/w), with a density of approximately 1.41 g/mL
Distilled or Deionized Water
1-Liter Volumetric Flask
Glass Stirring Rod
Measuring Cylinder (preferably 100 mL)
Pipette (Optional, for precision)
Beaker (250 mL or larger)
Funnel
Lab Gloves, Goggles, and Lab Coat for Safety
Calculation to Prepare 1M HNO₃
Before we begin the practical steps, let’s calculate how much concentrated nitric acid we need.
Step 1: Molarity Equation
C₁V₁ = C₂V₂
Where:
C₁ = Concentration of stock solution (typically ~15.8 M for 68% HNO₃)
V₁ = Volume of stock solution required
C₂ = Desired concentration = 1 M
V₂ = Final volume = 1000 mL = 1 L
15.8 × V₁ = 1 × 1000 ⇒ V₁ = 1000 ÷ 15.8 = 63.2 mL
So, we need 63.2 mL of concentrated HNO₃ and will dilute it to a final volume of 1 liter.
Safety First – Important Precautions
Before you start:
Always add acid to water, never the reverse, to prevent exothermic splashing or boiling.
Carry out the procedure in a fume hood to avoid breathing in hazardous nitric acid fumes.
Wear protective gloves, goggles, and a lab coat
Keep neutralizing agents (e.g., sodium bicarbonate) nearby in case of spills.
Work in a well-ventilated area.
Procedure: How to Prepare 1M Nitric Acid Solution
Step 1: Measure Water
Take a 1-liter volumetric flask and add about 800 mL of distilled water into it using a funnel.
This leaves space for the acid and reduces the risk of overshooting the mark.
Step 2: Measure Concentrated HNO₃
Use a graduated measuring cylinder to carefully measure 63.2 mL of concentrated nitric acid.
Handle with care, and do not inhale the vapors.
Step 3: Add Acid to Water
Slowly pour the nitric acid into the water in the volumetric flask using a glass funnel.
Stir gently with a clean glass rod during addition to ensure mixing.
Allow the mixture to cool if it becomes warm.
Step 4: Make Up the Volume
Once the mixture has cooled to room temperature, top up with distilled water to exactly 1000 mL using a dropper for accuracy.
Seal the flask and turn it upside down several times to mix thoroughly.
Storage and Labeling
Transfer the solution into a chemical-resistant, labeled storage bottle.
Mark: “1M Nitric Acid”
Date of Preparation
Prepared By (Name/Initials)
Store in a cool, dark place away from organic materials and incompatible substances.
Verification of Molarity (Optional but Recommended)
For critical applications, verify the molarity using acid-base titration against a standard sodium carbonate or sodium hydroxide solution. This ensures precise concentration for analytical tasks.
Applications of 1M Nitric Acid
Titrations in volumetric analysis.
Etching and metal cleaning.
Nitrate ion tests.
Reagent in synthesis and laboratory experiments.
Sample digestion for spectrometry.
Tips for Accurate Solution Preparation
Always use volumetric flasks for high accuracy.
Rinse all glassware with distilled water before use.
Do not pipette acids by mouth; use a pipette filler.
Check the expiry of chemicals and concentrations of commercial acids.
Dispose of acid waste properly according to hazardous waste protocols.
Common Mistakes to Avoid
Adding water to acid – This can cause dangerous splattering.
Not cooling before final dilution – Heat may cause evaporation or volume distortion.
Improper labeling Leads to confusion and safety risks.
Ignoring ventilation – Inhalation of nitric acid fumes is hazardous.
Conversion Chart: Molarity vs Volume of Concentrated HNO₃
| Desired Molarity (M) | Volume of 68% HNO₃ per 1L Solution (mL) |
|---|---|
| 0.1 M | 6.3 mL |
| 0.5 M | 31.6 mL |
| 1 M | 63.2 mL |
| 2 M | 126.4 mL |
| 5 M | 316 mL |
Conclusion
Preparing 1 molar nitric acid is a straightforward but precise laboratory task. By following the proper calculations, safety protocols, and dilution steps, we can produce a reliable and standardized acid solution for a wide range of chemical processes. Whether for titration or synthesis, 1M HNO₃ remains a cornerstone in the chemistry lab.