i cant figure out how to solve this problem
Hydrochloric acid is usually purchased in concentrated form with a 37.0% HCl concentration by mass and a density of 1.20 g/mL. How much of the concentrated solution in milliliters should you use to make 1.5 L of 0.535 M HCl?
_______ mL
2007-04-02 09:31:07 · 2 answers · asked by Krazyk78 1 in Science & Mathematics ➔ Chemistry
First calculate the moles of pure acid you need. Multiply 1.5 L by 0.535 M and you get moles of pure HCl needed. Multiply that by the molecular mass (36.5) and you get grams of pure HCl. Divide that by 0.370 and you have grams of the concenttrated acid. Finally, divide by the density and you get ml of conc. acid required
2007-04-02 09:46:00 · answer #1 · answered by reb1240 7 · 0⤊ 0⤋
0.535 M:1000 ml=mol:1500 => x=0.5366 mol*MW=13g of HCl. if 37g:100 slz=13g:x so x(grams of slz at 37%m)=35.13
so u get 35.13g of slz (=27.28 ml) and u put water till 1.5 lit
2007-04-02 16:59:06 · answer #2 · answered by ue amici 2 · 0⤊ 0⤋