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To prepare 1 M sulfuric acid (H2SO4), you would need to dilute concentrated sulfuric acid to the desired molarity. Calculate the volume of concentrated sulfuric acid needed based on its concentration (typically around 18 M) and the final volume required. Always add acid to water slowly with stirring and proper safety equipment due to the exothermic nature of dilution and the corrosive properties of sulfuric acid. Dilute to the final volume with distilled water.
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How do you prepare 2.5 M sulphuric acid?
To prepare 2.5 M sulfuric acid solution, you would need to accurately measure out the appropriate volume of concentrated sulfuric acid and then dilute it with water to the desired final volume. Always remember to add acid to water slowly, with stirring and caution, due to its exothermic reaction. Make sure to wear appropriate personal protective equipment and work in a well-ventilated area.
How do you prepare 0.1 N sulphuric acid?
For preparation of 4N solution of sulphuric acid Dissolve 196 gm H2SO4 in 1000 ml DM water. Calculation N E V Weight = ------------ 1000 Where N= Normality E= Equivalent weight V= Volume
How do you prepare 0.4 M hydrochloric acid?
To prepare 0.4 M hydrochloric acid solution, you can dilute concentrated hydrochloric acid (typically around 12 M) with distilled water in a volumetric flask. Calculate the volume of concentrated acid needed using the formula C1V1 = C2V2, where C1 is the concentration of your concentrated acid, V1 is the volume of concentrated acid needed, C2 is the desired final concentration (0.4 M), and V2 is the final volume of the solution. Always add acid to water slowly and with stirring to avoid splattering and potential hazards.
How prepare 0.02 M H2So4?
To prepare a 0.02 M (molar) solution of H2SO4 (sulfuric acid), you would first need to calculate the amount of sulfuric acid needed based on its molar mass (98.08 g/mol). Then, measure out the calculated mass of H2SO4 using a balance and dissolve it in a known volume of water to make the desired concentration. For example, to make 1 liter of 0.02 M H2SO4, you would dissolve 19.62 grams of H2SO4 in enough water to make 1 liter of solution.
What volume of a 2.5 M stock solution of acetic acid (HCHÀO) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
To prepare a 0.50 M acetic acid solution, you would need to dilute the 2.5 M stock solution. By using the formula M1V1 = M2V2, you can calculate the volume of the stock solution needed as: (0.5 M)(100.0 mL) = (2.5 M)(V2), where V2 is the volume of the stock solution needed. So, V2 = (0.5 M x 100.0 mL) / 2.5 M = 20.0 mL. Therefore, you would need 20.0 mL of the 2.5 M stock solution to prepare the desired 100.0 mL of 0.50 M acetic acid solution.
How do you prepare 2.5 M sulphuric acid?
To prepare 2.5 M sulfuric acid solution, you would need to accurately measure out the appropriate volume of concentrated sulfuric acid and then dilute it with water to the desired final volume. Always remember to add acid to water slowly, with stirring and caution, due to its exothermic reaction. Make sure to wear appropriate personal protective equipment and work in a well-ventilated area.
How do you prepare 0.1 N sulphuric acid?
For preparation of 4N solution of sulphuric acid Dissolve 196 gm H2SO4 in 1000 ml DM water. Calculation N E V Weight = ------------ 1000 Where N= Normality E= Equivalent weight V= Volume
What has the author M Rahmani written?
M. Rahmani has written: 'Hydrodynamic modeling of corrosion of carbon steels and cast irons in sulfuric acid' -- subject(s): Carbon steel, Cast-iron, Corrosion, Corrosion and anti-corrosives, Sulphuric acid, Testing
How do you prepare 0.4 M hydrochloric acid?
To prepare 0.4 M hydrochloric acid solution, you can dilute concentrated hydrochloric acid (typically around 12 M) with distilled water in a volumetric flask. Calculate the volume of concentrated acid needed using the formula C1V1 = C2V2, where C1 is the concentration of your concentrated acid, V1 is the volume of concentrated acid needed, C2 is the desired final concentration (0.4 M), and V2 is the final volume of the solution. Always add acid to water slowly and with stirring to avoid splattering and potential hazards.
How prepare 0.02 M H2So4?
To prepare a 0.02 M (molar) solution of H2SO4 (sulfuric acid), you would first need to calculate the amount of sulfuric acid needed based on its molar mass (98.08 g/mol). Then, measure out the calculated mass of H2SO4 using a balance and dissolve it in a known volume of water to make the desired concentration. For example, to make 1 liter of 0.02 M H2SO4, you would dissolve 19.62 grams of H2SO4 in enough water to make 1 liter of solution.
What volume of a 2.5 M stock solution of acetic acid (HCHÀO) is required to prepare 100.0 milliliters of a 0.50 M acetic acid solution?
To prepare a 0.50 M acetic acid solution, you would need to dilute the 2.5 M stock solution. By using the formula M1V1 = M2V2, you can calculate the volume of the stock solution needed as: (0.5 M)(100.0 mL) = (2.5 M)(V2), where V2 is the volume of the stock solution needed. So, V2 = (0.5 M x 100.0 mL) / 2.5 M = 20.0 mL. Therefore, you would need 20.0 mL of the 2.5 M stock solution to prepare the desired 100.0 mL of 0.50 M acetic acid solution.
What volume of 2.5 m stock solution of acetic acid hc2h3o2 is required to prepare 100 mll of a .50 m acetic acid solution?
To prepare a 0.5 M acetic acid solution using a 2.5 M stock solution, you will need to dilute it. The formula for dilution is C1V1 = C2V2, where C1 is the initial concentration, V1 is the initial volume, C2 is the final concentration, and V2 is the final volume. Plugging in the values, you will need 20 ml of the 2.5 M stock solution to make 100 ml of a 0.5 M acetic acid solution.
Which part of the procedure calls for 3 M and which part of 9 M sulfuric acid?
The procedure calls for using 3 M sulfuric acid during the preparation of the standard solutions, as it is less concentrated. The 9 M sulfuric acid is typically used during the extraction or digestion steps that require a stronger acid for efficient reaction.
How do you prepare a solution of 1 M butyric acid?
To prepare a 1 M solution of butyric acid, you would need to dissolve the appropriate amount of butyric acid in a given volume of solvent, typically water. The molar mass of butyric acid (C4H8O2) is 88.11 g/mol. To make a 1 M solution, you would dissolve 88.11 g of butyric acid in enough water to make a final volume of 1 L.
How do you 0.02 m sulphuric acid standardization calculation?
To standardize 0.02 M sulfuric acid, you would titrate it against a known concentration of a base, such as sodium hydroxide. By measuring the volume of the base required to neutralize the acid, you can calculate the exact concentration of the sulfuric acid solution. The standardization calculation involves using the stoichiometry of the acid-base reaction to determine the concentration of the acid solution.
What volume of 5.75 M formic acid solution should be used to prepare 2.00 L of 1.00 M formic acid?
To prepare 2.00 L of 1.00 M formic acid solution, the initial 5.75 M solution can be diluted using the formula M1V1 = M2V2. By substituting the values, you can calculate the volume of 5.75 M formic acid solution needed, which would be about 0.35 L.
What volume of 1.75 M hydrochloric acid must be diluted with water to prepare 0.500 L of 0.250 M hydrochloric acid?
First, determine the moles of HCl required in the final solution using the dilution formula: (M1)(V1) = (M2)(V2). Then calculate the volume of the 1.75 M HCl needed by rearranging the formula to solve for V1. Finally, subtract the initial volume from the total volume to find the volume of water required to make the dilution.
