Please check my work-

what is the molarity of a solution that has 34.85 g of Potassium sulfate dissolved in one liter of solution?

so K2(SO4) molar mass is 174.26,
34.85 grams x 1mol/174.26 than divided by 1 Liter equals
.19998 Molarity with sig figs would it be .1999 or .2000?

molarity=mass/(molmass*volumeinliters)

One liter: is that absolutely precise? It is not 1.00000000 liter.

Ok, ignoring the volume precision, the mass is five sig digits, mass is four, so I would take it to four sig digits, but honestly, one liter...in the real world one would be much more careful with the volume precision. My guess in the best lab, it is no more than three sig digits precise.
your question on rounding the five digits to two, yes it would be .2000 by the rules, but the rules also include volume precision.

thats tricky than and your right 1 liter isn't technically exact but I believe since its a conversion factor we never acknowledge it for sig fig sake (intro chemistry) so .2000 ? that just doesn't sit right though, something about that answer... what if i made it 1.999x10^-1?

To find the molarity of a solution, you correctly used the formula:

Molarity (M) = moles of solute / volume of solution (in liters)

First, determine the moles of Potassium sulfate (K2(SO4)) using its molar mass:

molar mass of K2(SO4) = 2(atomic mass of K) + atomic mass of S + 4(atomic mass of O)
= 2(39.10 g/mol) + 32.07 g/mol + 4(16.00 g/mol)
= 174.26 g/mol

Now, divide the given mass by the molar mass to find the number of moles:

moles of K2(SO4) = 34.85 g / 174.26 g/mol
≈ 0.1999 mol (rounded to four significant figures)

Finally, divide the moles by the volume in liters (which is given as 1 liter):

Molarity = 0.1999 mol / 1 L
= 0.1999 M

Considering significant figures, the molarity should also be reported with three significant figures, as the given mass has four significant figures. Therefore, the molarity of the solution would be 0.200 M.