This is part 1!: What volume of a 0.630 M NaF solution is required to react completely with 235 mL of a 0.340 M SrCl2 solution?
Should I use this? How? Please help me!
Strontium chloride and sodium fluoride react to form strontium fluoride and sodium chloride, according to the reaction shown.
SrCl2(aq)+2NaF(aq)⟶SrF2(s)+2NaCl(aq)
How many moles of SrF2 are formed from this reaction?
IN DESPERATE NEED OF HELP, ONLY HAVE 3 ATTEMPTS LEFT, PLEASE HELP ME, i tried a lot on my own but even socratic and chegg could not solve it :(
0.1598 is wrong, idk what is right, please help me
3 answers
0.0799 was the answer! I multiplied Molarity with Volume to find the moles! n=MV, so 235 mL x0.340 = 79.9 then converted these millimoles to moles to get 0.0799!
If you have stated the problem correctly 0.0799 L is NOT the answer. mL x M = millimoles so 235 mL x 0.340 M = 79.9 mmols SrCl2 initially. That will require 2*79.9 mmoles NaF to react completely. Then
M = mmoles/mL or mL = mmoles/M = 2*79.9/0.630 = 253.6 mL NaF solution required.
If these numbers are what you omitted from the problem that Chegg and Socratic couldn't do (because you didn't give them enough information) then 79.9 millimoles (0.0799 moles) SrF2 will be formed.
M = mmoles/mL or mL = mmoles/M = 2*79.9/0.630 = 253.6 mL NaF solution required.
If these numbers are what you omitted from the problem that Chegg and Socratic couldn't do (because you didn't give them enough information) then 79.9 millimoles (0.0799 moles) SrF2 will be formed.
2 answers