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To prepare 0.125 N sulfuric acid, you would first need to calculate the amount of sulfuric acid needed by using the formula: (desired normality) x (equivalent weight) x (volume in liters) = mass of the substance. Then, weigh out the required amount of sulfuric acid and dissolve it in water to make the desired volume of solution.
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Ho to prepare 0.02 N sulfuric acid?
To prepare 0.02 N sulfuric acid, dilute concentrated sulfuric acid with water in a specific ratio. For example, to prepare 100 ml of 0.02 N sulfuric acid, you would mix 0.4 ml of concentrated sulfuric acid (98% purity) with 99.6 ml of water. It's crucial to handle concentrated sulfuric acid with caution due to its corrosive nature.
How do you prepare 7 N sulfuric acid?
To prepare a 7 N (Normal) solution of sulfuric acid, you would first need to calculate the molarity of the solution. Sulfuric acid is a diprotic acid, so its equivalent weight is half its molecular weight. To prepare a 7 N solution, you would dissolve 7 moles of sulfuric acid in enough water to make 1 liter of solution. It is crucial to wear appropriate personal protective equipment and handle sulfuric acid with extreme caution due to its corrosive nature.
How do you prepare 0.5 N sulphuric acid?
To prepare 0.5 N sulfuric acid, you can mix 49 g of sulfuric acid (H2SO4) into enough water to make 1 liter of solution. This will give you a solution that has a concentration of 0.5 N, meaning it contains 0.5 moles of H2SO4 per liter of solution. Remember to always add acid to water slowly while stirring to avoid splashing and to ensure a safe preparation process.
What does the N in 18 N mean when discussing sulfuric acid?
The (N) stands for Normal. 1 Normal is 28 ml of concentrated sulfuric acid added to deionized water for a final volume of 1 Liter (L). 18 N is roughly a 50 percent concentration sulfuric acid.
How would you prepare 4N dilute sulfuric acid from concentrated sulfuric acid for use in an experiment?
To prepare 4N dilute sulfuric acid, you would first calculate the volume of concentrated sulfuric acid needed based on its concentration. Then, slowly add the calculated volume of concentrated sulfuric acid to an appropriate volume of water while stirring continuously. Finally, dilute the solution to the desired volume with water and ensure proper mixing to obtain 4N dilute sulfuric acid for use in the experiment.
Ho to prepare 0.02 N sulfuric acid?
To prepare 0.02 N sulfuric acid, dilute concentrated sulfuric acid with water in a specific ratio. For example, to prepare 100 ml of 0.02 N sulfuric acid, you would mix 0.4 ml of concentrated sulfuric acid (98% purity) with 99.6 ml of water. It's crucial to handle concentrated sulfuric acid with caution due to its corrosive nature.
How do you prepare 7 N sulfuric acid?
To prepare a 7 N (Normal) solution of sulfuric acid, you would first need to calculate the molarity of the solution. Sulfuric acid is a diprotic acid, so its equivalent weight is half its molecular weight. To prepare a 7 N solution, you would dissolve 7 moles of sulfuric acid in enough water to make 1 liter of solution. It is crucial to wear appropriate personal protective equipment and handle sulfuric acid with extreme caution due to its corrosive nature.
How do you prepare 0.5 N sulphuric acid?
To prepare 0.5 N sulfuric acid, you can mix 49 g of sulfuric acid (H2SO4) into enough water to make 1 liter of solution. This will give you a solution that has a concentration of 0.5 N, meaning it contains 0.5 moles of H2SO4 per liter of solution. Remember to always add acid to water slowly while stirring to avoid splashing and to ensure a safe preparation process.
What does the N in 18 N mean when discussing sulfuric acid?
The (N) stands for Normal. 1 Normal is 28 ml of concentrated sulfuric acid added to deionized water for a final volume of 1 Liter (L). 18 N is roughly a 50 percent concentration sulfuric acid.
How would you prepare 4N dilute sulfuric acid from concentrated sulfuric acid for use in an experiment?
To prepare 4N dilute sulfuric acid, you would first calculate the volume of concentrated sulfuric acid needed based on its concentration. Then, slowly add the calculated volume of concentrated sulfuric acid to an appropriate volume of water while stirring continuously. Finally, dilute the solution to the desired volume with water and ensure proper mixing to obtain 4N dilute sulfuric acid for use in the experiment.
When someone says 0.2 N sulfuric acid what is meant by 0.2 N?
This means that one liter of the solution of sulfuric acid contains 0.2 gram-equivalent mass of sulfuric acid. For this acid, the equivalent mass is one half the molar mass, since each molecule of H2SO4 supplies two hydrogen atoms to neutralize alkaline materials.
What is formed when aminobenzoic acid reacts with sulfuric acid?
When aminobenzoic acid reacts with sulfuric acid, it can form an amide derivative known as N-acetylanthranilic acid. This reaction involves the sulfonation of the amine group in aminobenzoic acid by sulfuric acid.
What is Normality for concentrated sulfuric acid?
Normality for concentrated sulfuric acid (H2SO4) is typically 18 N, as sulfuric acid is a diprotic acid, meaning each molecule can donate two hydrogen ions. This value is calculated based on the molarity of the acid and the number of protons it can donate.
What is the molarity of concentrated sulfuric acid?
Concentrated sulfuric acid is typically around 18 M in strength.
How do make a 5.25N sulfuric acid solution from concentrated sulfuric acid solution?
con.H2SO4 is 98%(v/v)ie 980ml/litre.or 980X1.84(specific gravity of H2So4)ie wt/litre is 1803.2Normality= wt per litre/ Eq.wtie 1803.2/49=36.8 NHence con H2So4 is 36.8 NTo prepare 5 N , It has be diluted 7.36 times with water68
What is the normality of 98 g of sulfuric acid in 500 mL of solution?
To determine normality, you first need to calculate the number of equivalents in the solution. Sulfuric acid (H2SO4) is a diprotic acid, so it can donate two equivalents of acid per molecule. The molar mass of sulfuric acid is 98 g/mol. Hence, there are 98 grams of sulfuric acid in 500 mL or 0.5 L of solution, which is equivalent to 1 mol/L. Therefore, the normality of the solution is 2 N (since sulfuric acid is diprotic).
How do I make a 1 N sulfuric acid solution from 5.25 N sulfuric acid what is the dilution?
To make a 1 N sulfuric acid solution from 5.25 N sulfuric acid, you need to dilute the concentrated solution with water. The dilution ratio can be calculated using the formula M1V1 = M2V2, where M1 is the initial concentration (5.25 N), V1 is the volume of the concentrated solution you'll use, M2 is the final concentration (1 N), and V2 is the total volume of the diluted solution you want to make. Calculate V1 and dilute the concentrated acid with the appropriate amount of water to achieve the desired 1 N concentration.
