Normality and Molarity p 218
Molarity is moles per liter of solution.
M = moles
We use Normality when discussing solutions especially acids and bases.
HCl + Na(OH) ----> NaCl + HOH
If I had 100 milliliters of a 1 M HCl acid, how many moles of H+ would I have?
Let's look at H2(SO4)
H2(S04) -------> 2 H+ + 1 (SO4)=
Each molecule of H2(SO4) would give 2 H+ and 1 (SO4)=
If I had 100 mL of a 1 M H2(SO4)
1 liter of a 1 M Na(OH) would have 1 mole of (OH)-
If I mixed 1 L of 1 M Na(OH) with 1 L of 1 M H2(SO4) I would have an acid solution. Why?
I have 2 times as much H+'s as I have (OH)-'s.
When using acids and bases we use Normality (N) instead of Molarity (M).
1 M HCl = 1 N HCl
H2(SO4) + 2 Na(OH) ------> Na2(SO4) + 2 HOH
If I had 100 milliliters of a 1 M H2(SO4), how many moles of H+ would I have?
a 1 M H2(SO4) solution is a 2 N H2(SO4)
1 M Ca(OH)2 = _____ N Ca(OH)2
HCl has only 1 hydrogen
H2SO4 has 2 hydrogens
a 1 M HCl is a 1 N HCl
a 1 M H2SO4 is 2 N H2SO4
What is the normality of 3 M H2(SO4)?
1 = 2 criss cross multiply
x = 6
What is the molarity of 6 N H3(PO4) ?
1 M H3(PO4) = 3 N H3(PO4)
1 = 3
x = 2
Determine the normality of
1.5 M HNO3
0.55 M H2SO4
0.0023 M Ca(OH)2
Determine the molarity of
0.9 N NaOH
1.3 N HCl
0.06 N H2SO4
0.3 N H3PO4
12 N Ca(OH)2
Neutralization p 203
If I had 50 H+'s how many (OH)- s would I need to neutralize it?
If I had 50 H+, how many (OH)- would I need to neutralize it?
We frequently use the term EQUIVALENTS or MILLIQUIVALENTS
You can think in terms of moles of H+ or moles of OH- when using the term equivalent.
Equivalents = Normality x Liters
Molarity = moles
moles = Molarity x L
Equivalents = Normality x L
Milliequivalents = Normality x Milliliters
If I had 50 mL of a 2 N H(SO)4 how many milliequivalents of H+ do I have?
How many milliequivalents of hydroxyl would I need to neutralize it?
1. How many milliliters of a 0.02 N NaOH would be needed to neuralize 35milliliters of a 0.15 N HCl?
2. What is the normality of a solution of HCl, if 50 mL of the HCl were neutralized by 30 mL of a 0.15 N NaOH?
Suppose I had 12 N HCl and wanted to make up 200 mL of 0.1 N solution. How many milliliters of the concentrated solution would I need to make up 200 mL of the dilute solution?
How many milliequivalents of H+ would I need in 200 mL of
0.1 N HCl
Meq = (N) (mL)
So how many milliequivalents would I need to take out of the concentrated HCl solution?
How many milliliters would have that number of milliequivalents?
Formula for dilutions
meq = meq
(N) (ml) = (N) (mL)
How many milliliters of a 6 N NaOH would I need to make up 100 mL of a 1 N NaOH?
1. How many milliliters of 2N HCl would be needed to make 100 mL of 0.1 N HCl?
2. What is the Normality of a NaOH solution if it took 25 mL of a 0.1 N HCl to neutralize 10 mL of the NaOH?
3. How many milliequivalents of H+ are there in 200 mL of 0.25 N solution?
4. What is the normality of a HCl solution if 10 mL of 12 N HCl were brought up to a 1 L volume?
5. How many milliequivalents of NaOH are needed to neutralize 50 mL of a 0.2 N HCl solution?
6. How many grams of NaOH are needed to make 100 mL of 0.5 N NaOH? (hint: N = M for NaOH M = grams/ MW)
7. How many grams of H2(SO4) are present in 50 mL of a 0.1 N H2(SO4)?
1. Calculate the mass percent of solute in 25.0 g of KNO3 in 850 grams of H2O.
2. Calculate the mass, in grams, of solute needed to prepare 24.0 grams of a 13.5% by mass sucrose (C12H22O11) (MW 342) solution.
3. Calculate the volume percent of solute in 75.0 g ethylene glycol in enough water to give 200 mL of solution.
4. What is the percent by volume of isopropyl alcohol in an aqueous solution made by diluting 20 mL of pure isopropyl alcohol to a volume of 125 mL.
5. Calculate the mass/volume percent of magnesium chloride of 1.0 g MgCl2 in enough water to give 45 mL of solution.
6. How many grams of NaCl are present in 15 mL of a 2.0% solution?
7. How many grams of solute are present in 375 mL of 7.5 M CaCl2 solution?
8. Given a 2.0 M solution of NaCl. How many milliliters of the solution would be needed to get 1.0 gram of NaCl?
9. 5.85 grams of NaCl were dissolved in water. The final volume was 100 mL. A) What is the molarity? B) What is % w/v?
10. Concentrated HCl is 12 N. How many milliliters of the concentrated acid wuld be needed for 100mL of a 0.15 N solution?
11. How many grams of sulfuric acid H2(SO4) are in 1 liter of a 1.50 N solution?
12. How many meq of H+ are ther ein 29 mL of a 2 N solution of HCl?
13. What is the normality of a HCl solution which contains 50grams of HCl per liter?
14. What is the normality of a 4 M H2SO4?
15. How many mL of a 0.3 N NaOH solution would be required toneutralize 50 mL of a 0.4 N solution of H2SO4?
16. How many milliequivalents are present in 15 mL of a 2 N solution?
17. How many milliquivalents of acid are requird to neutralize 20 milliequivalents of base?
18. How many mL of a 0.15 N HCl would be required to neutralize 40 mL of a 0.20 N NaOH?
19. It took 35 mL of an acid of unknown normality to neutralize 25 mL of 0.12 N NaOH. What is the normality?
20. How many milliliters of a a 0.20 M H2SO4 would be required to neutralize 80 mL of a 0.10 N NaOH?
21. How many mL of a 12 N HCl solution would be needed to make 100 mL of a 0.15 N solution?
22. 15 mL of a 10 N NaOH solution was diluted to a volume of 1 liter. What is the normality of the new solution.?
23. Given 3.92 grams of H2SO4, (MW 98) in 250 mL of solution.
a) What is the Percent solution?
Questions Chapter 8 8.45; 8.26; 8.47; 8.49; 8.51
PLUG-IN LOGS & pH Chapter 8
103 = 1000
10-2 = .01
Write the log of
We can do logs of numbers other than powers of 10.
100 = 1 log of 1 = 0
101 = 10
log of 10 = 1
so the logs of numbers between 1 and 10 are decimals.
Where do we get them?
From Log Tables
Find the log of
Plug in Logs - pH and pOH
Find the log of 0.0083.
Find the log of
pH and Hydrogen Ion Concentration
pH refers to the concentration of [H+].
pH is the negative log of [H+].
pOH refers to the negative log of [OH]-.
If we know the pH we can find out the pOH.
The pH is 4. What is the pOH?
pH + pOH = 14
The pOH is 3. What is the pH?
pH 7 is neutral
The molarity of a solution of HCl is .015 M. What is its pH? (Find the log of 0.015).
What is the pH corresponding to a hydrogen ion concentration of 5 x 10-4?
The pOH is 8. (a) What is the pH?
(b) What is the [H+]?
pH = 6 -6 is the neg. log.
1 x 10-6
Drill Determine the pH of the following solutions:
(1) pOH = 4
(6) 1 x 10-3 M H+
To go from the pH to the concentration, we must reverse the steps.
To find the pH from the concentration of 2.3 x 10-4 M HCl, the steps are
2.30 exp 4 +/- log +/- Ans 3.64
To go from the pH 3.64 to concentration, the steps are
3.64 +/- inv or 2nd log Ans 2.30 x 10-4
On some calculators the steps are
What is the H+ concentration in the following solutions:
Questions Chapter 8: 8.28; 8.29; 8.30; 8.32
Wednesday, March 21, 2007 01:28:01 PM