Commercially available concentrated hydrochloric acid is 37.0% w/w HCl. Its
density is 1.18 g/mL. Using this information, calculate: i. the molarity of
concentrated HCl, and ii. the mass (g) and volume (ml) of solution containing
0.315 mol HCl.
2006-09-28 09:57:55 · 4 answers · asked by hye212 1 in Science & Mathematics ➔ Chemistry
Assume 100 grams of the solution, which means there are 37.0 g HCl in 100 grams solution. Since molarity is in moles/L, you convert the mass of HCl to moles and the mass of the solution to volume to determine molarity.
moles HCl = 37.0g/36.5 g/mol = 1.014 moles
volume solution = 100g/1.18g/mL = 84.75 mL, or 0.08475 L
molarity HCl = 1.014 moles/0.08475 L = 11.96 M
The volume of a solution containing 0.315 mol HCl would be:
0.315 moles / 11.96 moles/L = 0.0263 L or 26.3 mL. That solution would weigh 26.3 mL * 1.18 g/mL or 31.0 g.
2006-09-28 10:08:48 · answer #1 · answered by TheOnlyBeldin 7 · 1⤊ 0⤋
Concentrated Hydrochloric Acid
2016-09-30 06:08:03 · answer #2 · answered by youngman 4 · 0⤊ 0⤋
i think thats very simple,, you must work your mind to get your answer..lol
2006-09-28 10:05:49 · answer #3 · answered by source_of_love_69 3 · 0⤊ 0⤋
man i wish they had this when i was in school
2006-09-28 09:59:18 · answer #4 · answered by justin s 2 · 0⤊ 0⤋