Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: Shea on August 10, 2006, 03:23:09 PM
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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?
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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) ;)
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http://www.chembuddy.com/?left=concentration&right=molarity
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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
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Volume = mole / concentration, right?
My teacher said I still had the wrong formula.
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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.
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Ok, I think I got it this time.