You need to make an aqueous solution of 0.217 m zinc fluoride for an experiment in lab, using a 250 ml volumetric flask. how much solid zinc fluoride should you add?

Explanation:

The given data is as follows.

           Volume = 250 mL,       Molarity = 0.217 M

Molar mass of is 103.406 g/mol.

As molarity is the number of moles of solute present in liter of solution.

As, it is given that molarity is 0.217 M. This means that 0.217 moles are present in 1 liter of solution.

Therefore, number of moles present in 250 mL are calculated as follows.

              = 0.05425 mol

Since, number of moles equal mass divided by molar mass. Therefore, calculate the mass of as follows.

                      Mass = no. of moles × Molar mass

                                =

                                = 5.61 g

Thus, we can conclude that mass of zinc fluoride is 5.61 g.

2fe + 3h2so4 -> fe2(so4)3 + 3h2

it is necessary to balance equations in order to get the proper amount of reactants as well as products in order not to make a miscalculation.

you cannot change the subscripts as that would change the substance itself. for instance, diatomic elements such as h2 only have the subscript two when a gas. another example would be so4, if you were to change the subscript, the element would no longer be sulfate.

we change the coefficients instead as that only changes the number of molecules rather than the substance itself.

hope this !

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