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How many moles of sulfuric acid are in 500 mL of 0.324 M sulfuric acid solution?
To find the number of moles of sulfuric acid in the solution, multiply the volume of the solution (in liters) by the molarity. First, convert 500 mL to liters by dividing by 1000 (500 mL = 0.5 L). Then, multiply 0.5 L by 0.324 mol/L to get 0.162 moles of sulfuric acid in 500 mL of the 0.324 M solution.
How to prepare 0.5M sulfuric acid?
To prepare 0.5M sulfuric acid, you would mix concentrated sulfuric acid with water in the correct ratio. For example, to make 500 mL of 0.5M sulfuric acid, you could mix 25 mL of concentrated sulfuric acid with 475 mL of water. Always remember to add acid to water slowly to avoid splashing and heat generation.
How is a 0.1n solution of perchloric acid prepared?
pipette out 8.5 ml perchloric acid in to 500 ml acetic acid and add 21 ml of acetic anhydride make up to volume to 1000 ml with acetic acid*. * Let this solution stand for one day and check the water content
How do you prepare 2N H2SO4 and 2M H2SO4?
MW of H2SO4 is 98.08. 2M = 2 x 98.08 in 1 L of water (1 gram=1 ml). Take 500 ml water in a 1 L measuring cylinder. Add 196.16 ml slowly along the side into water in the measuring cylinder. Use 50 ml pipette with automated pipettor. If needed you may want to keep the cylinder in ice to take care of the heat generated. Then make up to volume to 1 L with water. Eq. wt for H2SO4 = 98.08/2 = 49.039. SO for 2N solution, 2 eq.wt in 1 L. 98.08 ml in 1 L water adopting the method cited above.
How much does sulfuric acid cost?
The cost of sulfuric acid can vary widely depending on factors such as purity, quantity, and supplier. It is commonly priced per gallon or per ton, with industrial-grade sulfuric acid typically costing around $200-$500 per ton. Specialty grades may be more expensive.
How many moles of sulfuric acid are in 500 mL of 0.324 M sulfuric acid solution?
To find the number of moles of sulfuric acid in the solution, multiply the volume of the solution (in liters) by the molarity. First, convert 500 mL to liters by dividing by 1000 (500 mL = 0.5 L). Then, multiply 0.5 L by 0.324 mol/L to get 0.162 moles of sulfuric acid in 500 mL of the 0.324 M solution.
How to prepare 0.5M sulfuric acid?
To prepare 0.5M sulfuric acid, you would mix concentrated sulfuric acid with water in the correct ratio. For example, to make 500 mL of 0.5M sulfuric acid, you could mix 25 mL of concentrated sulfuric acid with 475 mL of water. Always remember to add acid to water slowly to avoid splashing and heat generation.
How is a 0.1 N solution of perchloric acid prepared?
pipette out 8.5 ml perchloric acid in to 500 ml acetic acid and add 21 ml of acetic anhydride make up to volume to 1000 ml with acetic acid.Stand iday this solution and and check the water content not exceedsto 0.025 to 0.5% then standardize the solution by PHP
How is a 0.1n solution of perchloric acid prepared?
pipette out 8.5 ml perchloric acid in to 500 ml acetic acid and add 21 ml of acetic anhydride make up to volume to 1000 ml with acetic acid*. * Let this solution stand for one day and check the water content
Why acid solution turn blue litmus red?
500
How do you prepare 2N H2SO4 and 2M H2SO4?
MW of H2SO4 is 98.08. 2M = 2 x 98.08 in 1 L of water (1 gram=1 ml). Take 500 ml water in a 1 L measuring cylinder. Add 196.16 ml slowly along the side into water in the measuring cylinder. Use 50 ml pipette with automated pipettor. If needed you may want to keep the cylinder in ice to take care of the heat generated. Then make up to volume to 1 L with water. Eq. wt for H2SO4 = 98.08/2 = 49.039. SO for 2N solution, 2 eq.wt in 1 L. 98.08 ml in 1 L water adopting the method cited above.
How much does sulfuric acid cost?
The cost of sulfuric acid can vary widely depending on factors such as purity, quantity, and supplier. It is commonly priced per gallon or per ton, with industrial-grade sulfuric acid typically costing around $200-$500 per ton. Specialty grades may be more expensive.
How do you prepare 1M sulfuric acid from concentrated sulfuric acid?
To prepare 1M sulphuric acid from concentrated sulphuric acid:First consider the molecular weight of H2SO4 = 98 g/mol, so you have to add 98g of conc. acid and make up to 1 liter of water (as pointed out at the 4thpoint).Considering that acid is a liquid, you should also consider density: where density = mass/volume, which is said on the bottle to be (about) 1.84 g/mL,so then you have: volume = 98g / 1.84(g/mL) = 53.2 mLNow you have to consider the acid purity, usually 98% then you have to do this: 53.2 mL if the acid were 100% pure convert in mL given with the purity of 98%, so 100% x 53.2 mL / 98% = 54.3 mL of (98%) concentrated acid.Finally CAREFULLY add this 54.3 mL (or 98 g, cf. first point) to about 0.9 L dist. water while continuously stirring (evolving heat!), and after that fill it up to 1.00 L with also dist. water. Never reverse this: DO NOT add water to concentrated fluids!
How would you prepare 500 mL of a 1M solution of acetic acid -HC2H3O2- from a stock solution of 6M of acetic acid?
You would need to dilute the 6M acetic acid solution by adding the appropriate volume of water. To prepare 500 mL of 1M solution, you would need to take (1/6)th of the volume of the 6M solution, which is (1/6) x 500 mL = 83.33 mL of the 6M solution. Dilute this with water to reach a final volume of 500 mL.
How do you prepare liebermann burchard reagent?
To prepare the Liebermann-Burchard reagent you add 200 ml of cold acetic anhydride and 200 ml of glacial acetic acid at room temperature to a 500 ml amber glass bottle that has a polyseal cap. Turn the bottle upside down to mix the solution then add 30 ml of cold concentrated sulfuric acid.
What volume of a 2.5 M stock solution of acetic acid (HC2H3O2) is required to prepare?
To prepare 500 mL of a 0.5 M solution of acetic acid, you would need to take 100 mL of the 2.5 M stock solution and dilute it to 500 mL. This is because the molarity equation (M1V1 = M2V2) can be used to calculate the volume of stock solution needed for dilution.
300.0g of ammonia react with 36.0 moles of sulfuric acid to produce ammonium sulfate how many moles of excess sulfuric acid are left over after the reaction is complete?
The equation for the reaction is: H{2}SO{4} + 2NH{3} → (NH{4}){2}SO{4} [Numbers in braces are supposed to be subscripts, but I can't do them here.] This says that 1 mole of sulphuric acid reacts with 2 moles of nitrogen to create 1 mole of ammonium sulphate. 1 mole of a substance weighs the same as its atomic weight in grams. 1 mole of NH{3} weighs 14 + 3 × 1 = 17 g Thus 2 × 17 g = 34 g of ammonia react with 1 mole of sulphuric acid. To react with 500 g of ammonia requires 500 g ÷ 34 g/mol ≈ 14.7 moles of sulphuric acid Therefore there will be 51.0 - 14.7 = 36.3 moles of sulphuric acid left.
