Asked by Anonymous
How many milliliters of concentrated hydrochloric acid solution (36.0% HCl by mass, density = 1.18 g/mL) are required to produce 20.0 L of a solution that has a pH of 2.13?
Answers
Answered by
DrBob222
You need to have two pieces of information before applying the dilution formula.
1. You need to convert pH to M.
pH = -log(H^+)
2.13 = pH. I get (H^+) = approximately 0.007 but you need to do that more accurately.
2. You need to convert 36% HCl to molarity.
density = 1.18; therefore, 1000 mL has a mass of 1000 mL x 1.18 g/mL = 1180 grams
That is 36% HCl; thus, 0.36*1180 g = 425 g (approximate)
How many moles is that in the 1000 mL soln? It is 425g/molar mass HCl and that is the molarity.
Then mL x M = mL x M.
1. You need to convert pH to M.
pH = -log(H^+)
2.13 = pH. I get (H^+) = approximately 0.007 but you need to do that more accurately.
2. You need to convert 36% HCl to molarity.
density = 1.18; therefore, 1000 mL has a mass of 1000 mL x 1.18 g/mL = 1180 grams
That is 36% HCl; thus, 0.36*1180 g = 425 g (approximate)
How many moles is that in the 1000 mL soln? It is 425g/molar mass HCl and that is the molarity.
Then mL x M = mL x M.
Answered by
Tia
11.667
Answered by
Tia
molarity of 36% HCl=11.667
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.