Normality Dr. Steve Badger
Dec 14, 2015
Concentrations of Solutions
A brief review of molarity & molality
Molarity =
Number of moles of soluteLiter of solution
Molality =
Number of moles of soluteKg of solvent
Would you use a volumetric flask to prepare a solution of known molality?
How would you prepare a solution of known molality?
Another way to express solution concentration
• Now that you understand molarity…
Normality =
Number of equivalents of soluteLiter of solution
…let’s consider normality!
Molarity =
Number of moles of soluteLiter of solution
What’s an equivalent ?
• An equivalent of a substance is the mass (grams) of that substance that will combine with one mole of another reactant.
• In an acid-base reaction, an equivalent is that amount of a substance that reacts with or liberates 1.0 mole of H+.
What’s an equivalent ?
• An equivalent of a substance is the mass (grams) of that substance that will combine with one mole of another reactant.
• In a redox reaction, an equivalent is that amount of a substance that gains or loses 1.0 mole of e–s.
Making a 1.00N Solution
• Calculate the mass of one equivalent of the substance, then measure that number of grams of the substance.
• Put that substance in…. ??• Add how much solvent?
AbNormality?
• Why don’t many modern chemistry textbooks cover normality?
• If we take a dimensional analysis approach to problems solving, normality is a superfluous concept.
• Consider the following problem:
H2SO4 + KOH H2O + K2SO4
What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution?
MaVa = MbVb
Could we just use this equation?
Here’s what we’d get if we used
MaVa = MbVb
0.20 M H2SO4 X 10.0 mL = 0.500 M KOH X ? mL
Solving this, we get 4.0 mL of 0.500 M KOH.But is this correct? No, it’s wrong! Why?
So let’s see how we solve this correctly.
volume acid moles acid moles base volume base
H2SO4 + KOH H2O + K2SO4
M
acid
rx
coef.
M
base
What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution?
BALANCE THE CHEMICAL EQUATION!
What volume of a 0.500 M KOH solution is required to titrate 10.0 mL of a 0.20 M H2SO4 solution?
volume acid moles acid moles base volume base
___ mol H2SO4
____ mL solnx
__ mol KOH
__ mol H2SO4
x____ ml soln
____ mol KOHx10.0 mL = ___ mL
M
acid
rx
coef.
M
base
H2SO4 + 2KOH 2H2O + K2SO4
What volume of a 0.500 M KOH solution is required to titrate 10.00 mL of a 0.20 M H2SO4 solution?
volume acid moles acid moles base volume base
H2SO4 + 2KOH 2H2O + K2SO4
0.20 mol H2SO4
1000 mL solnx
2 mol KOH
1 mol H2SO4
x1000 ml soln
0.500 mol KOHx10.0 mL = 8.0 mL
M
acid
rx
coef.
M
base
volume acid moles acid moles base volume base
0.20 mol H2SO4
1000 mL solnx
2 mol KOH
1 mol H2SO4
x1000 ml soln
0.500 mol KOHx10.0 mL = 8.0 mL
M
acid
rx
coef.
M
base
Notice this!
Notice this!
This is what makes normality superfluous!
Is the following statement true or false?
• Any volume of a base will completely react with (neutralize) that same volume of acid if the two solutions have the same normality (vice versa too).
• In other words, is this true:
NaVa = NbVb
Is the following statement true or false?
• Any volume of a reducing agent will completely react with that same volume of an oxidizing agent if the two solutions have the same normality.
• In other words, is this true:
NoxVox = NredVred
Let’s solve a few problems using
normality
• Look at the handout that has sample problems and work the first one.
And another thing…
• We also use equivalents and milliequivalents as an amount of a substance
• The same way that we use moles (mol) and millimoles (mmol) as an amount of a substance
If you need more help:
Come by my office and I can give you a few pages of worked examples from a Schaum’s Solved Problems Series.
You can download this PowerPoint file at my EU web site:
www.evangel.edu/Personal/badgers/Web/