To be honest the first sentence makes no sense whatsoever (what's a, what's /H2O, what's the salt mixture) so I'll assume that CaCl2.2H2O in a basic solution will ppt Ca(OH)2. Assuming that do this.
1. Convert 0.375 g Ca(OH2 to CaCl2.2H2O.
2. Solve for % CaCl2.2H2O in the sample.
Answers:
1. 0.375 g Ca(OH)2 x [molar mass CaCl2.2H2O/molar mass Ca(OH)2] = ?
2. %CaCl2.2H2O = (mass CaCl2.2H2O from #1/0.972)*100 = ?
Post your work if you get stuck. I may have not made the correct assumptions.
A 0.972-g; CaCl 2 2H 2 C 4. sample of a / H2O solid salt mixture is dissolved in 150 of deionized water , previously adjusted to a pH that is basic . The precipitate , after having been filtered and air - dried , has a mass of 0.375 g . The limiting reactant in the salt mixture was later determined to be CaCl 2 2H 2 O a . What is the percent by mass of CaCl 2 2H 2 O in the salt mixture ?
2 answers
no tutor should have to assume what a student is asking.
and, students who can't put the correct word in the School Subject box probably aren't learning much English or science. how sad.
and, students who can't put the correct word in the School Subject box probably aren't learning much English or science. how sad.
4 answers