[Shea]

Could I have a little assistance with these?

How many mL of 0.5M Fe(NO3)2 solution are required so that we have 0.4 moles of Fe(NO3)2.?

.5M x .4 moles = .2L

.2L = 200mL

How many mL of 2.0M AgNO3 solution are required so that we have 20 g of AgNO3?

20g of AgNO3 = .117 moles of AgNO3

2M x .117 moles of AgNO3 = .234L

Where did I go wrong with them?

[Will]

Where did I go wrong with them?

moles = concentration(M) x volume(dm³) (ie volume = moles / concentration)

(Also round up the moles of AgNO₃ from 0.1177343207 to 0.1177 or 0.118)

[Borek]

http://www.chembuddy.com/?left=concentration&right=molarity

[sdekivit]

i assume you have basic knowledge in maths. For me, the easiest way is to put the numbers in the original equation and solve the equation.

Thus for problem 1:

c = n/V --> 0,5 = 0,4 / V --> V = 0,4 / 0,5 = 0,8 L = 800 mL

[Shea]

Volume = mole / concentration, right?

My teacher said I still had the wrong formula.

[Borek]

Volume = mole / concentration, right?

My teacher said I still had the wrong formula.

The one you have listed is OK. Take the way similar to the one sdekivit proposed: start with the definition of molar concentration and solve for V.

[Shea]

Ok, I think I got it this time.