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what mass of concentrated sulfuric acid (96% solution of H2SO4) and water is needed to prepare 500g of 10% solution of H2SO4?

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Related questions

Concentrated sulfuric acid (18.4-molar H2SO4) has a density of 1.84 grams per milliliter. After dilution with water to 5.20-molar, the solution has a density of 1.38 grams per milliliter and can be used as an electrolyte in lead storage batteries for automobiles. (a) Calculate the volume of concentrated acid required to prepare 1.00 liter of 5.20-molar H2SO4. (b) Determine the mass percent of H2SO4 in the original concentrated solution. (c) Calculate the volume of 5.20-molar H2SO4 that can be completely neutralized with 10.5 grams of sodium bicarbonate, NaHCO3. (d) What is the molality of the 5.20-molar H2SO4?

Concentrated sulfuric acid is 18.0M and 96.0% H2SO4 by mass. What is the density of concentrated sulfuric acid?

Add 5 mL of 75% H2SO4 (make from concentrated sulfuric acid which is 96%) how would I do this? help! what would be the mL needed to use? please show all steps

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