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

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!

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!

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.

To find the number of moles of SrF2 formed in the reaction, we need to use the balanced equation and the given information.

From the balanced equation:

1 mole of SrCl2 reacts with 2 moles of NaF to form 1 mole of SrF2.

So, the molar ratio between SrCl2 and SrF2 is 1:1.

If we know the number of moles of SrCl2, then we can directly say that the same number of moles of SrF2 is formed.

Since the question does not provide the number of moles of SrCl2, we need to use the given information differently.

You mentioned that the answer 0.1598 is wrong. It means you attempted to find the moles of SrF2 using that value. It seems you made a calculation mistake along the way.

Here's how you can correctly find the moles of SrF2:

Let's assume you have given the mass of SrCl2. Convert that mass into moles using its molar mass.

For example, if the mass of SrCl2 = 10 grams:
1. Find the molar mass of SrCl2. It consists of Sr (strontium) with an atomic mass of 87.62 g/mol and Cl (chlorine) with an atomic mass of 35.45 g/mol.
Molar mass of SrCl2 = (87.62 g/mol) + 2 * (35.45 g/mol) = 158.52 g/mol

2. Use the given mass and the molar mass to calculate the number of moles:
Moles of SrCl2 = Mass / Molar mass = 10 g / 158.52 g/mol = 0.063 mol (approx.)

Since the molar ratio between SrCl2 and SrF2 is 1:1, the number of moles of SrF2 will also be 0.063 mol in this case.

Please note that you need to substitute the actual given mass of SrCl2 into the calculations, as I used 10 grams just for illustration.

I hope this helps! Let me know if you have any further questions.