Molarity is moles per liter of solution.

M = moles
          liter

We use Normality when discussing solutions especially acids and bases.

HCl + Na(OH) ----> NaCl + HOH
acid       base               salt      water

If I had 100 milliliters of a 1 M HCl acid, how many moles of H⁺ would I have?

If I had 100 milliliters of a 1 M Na(OH), how many moles of (OH)^- 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)
I would have 0.10 moles of H₂(SO₄)
" " " 0.10 moles of (SO₄)⁼
" " " 0.20 moles of H⁺          Why?                 1 mole of H₂(SO₄) has 2 moles of H⁺

1 liter of a 1 M Na(OH) would have 1 mole of (OH)^-
l liter of a 1 M H₂(SO₄) would have 2 moles of H⁺

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.
1 liter of 1 M NaOH has 1 mole of Na and 1 mole of (OH)^-
1 liter of 1 M H₂(SO₄) has 1 mole of (SO₄) and 2 moles of H⁺

When using acids and bases we use Normality (N) instead of Molarity (M).

1 M HCl = 1 N HCl
1 M H₂(SO₄) = 2 N H₂(SO₄)
1 M H₃(PO₄) = __ N H₃(PO₄)

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)
for every mole of sulfuric acid, you would get 2 moles of H⁺

1 M Ca(OH)₂ = _____ N Ca(OH)₂
For every mole of calcium hydroxide, would get 2 moles of hydroxide ions.

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

Examples

                What is the normality of 3 M H₂(SO₄)?

1 M H₂(SO₄) = 2 N H₂(SO₄)
3 M H₂(SO₄) = x N H₂(SO₄)

1 = 2 criss cross multiply
3    x

x = 6

What is the molarity of 6 N H₃(PO₄) ?

1 M H₃(PO₄) = 3 N H₃(PO₄)
    x                = 6 N H₃(PO₄)

1 = 3
x    6

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
when discussing hydrogen ions or hydroxyl ions.

You can think in terms of moles of H⁺ or moles of OH^- when using the term equivalent.

Equivalents = Normality x Liters             Molarity = moles
                                                                                         L

       moles = Molarity
         L

                                                                   moles = Molarity x L

                                                                   Equivalents = Normality x L

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?

meq H+         =             meq (OH)-
N₁V₁            =             N₂V₂
(N) (mL)       =             (N) (mL)

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)?

PROBLEMS

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?
b) What is the Molarity of the solution?
c) What is the Normality of the solution?

Questions Chapter 8 8.45; 8.26; 8.47; 8.49; 8.51

PLUG-IN LOGS & pH Chapter 8

10³ = 1000
The log of 1000 is 3.

10^-2 = .01
The log of .01 is -2.
The log is the exponent of 10.

Write the log of
                10000
                      10
                        1
                        0.1
                        0.01
                        0.001
                        0.0000001

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?
    (a) log tables
    (b) calculators with log functions

From Log Tables
    log of 6 = .7782
    log of 4 = .6621

Find the log of
            3
            7
            9
            2
            1

(a) 30
(b) 300
(c) 3000
(d) 35
(e) 350
(f) 3500
(g) 82
(h) 23
(i) 54

Plug in Logs - pH and pOH
Find the log of 0.002.

Find the log of 0.0083.

Find the log of
(a) .02
(b) .002
(c) .0002
(d) .0025
(e) .0000001
(f) .0000008

pH and Hydrogen Ion Concentration

pH refers to the concentration of [H⁺].
pOH refers to the concentration of [OH]^-.
In pure water at 25^oC the concentration of [H⁺]and the concentration of hydroxyl ions [OH]^- in moles per liter equal and each is equal to 1 x 10^-7 moles/liter.

pH is the negative log of [H⁺].
    The log of the [H⁺] is -7.
    The negative log of [H⁺] is -(-7) = 7.

pOH refers to the negative log of [OH]^-.
    p[OH]^- + p[H⁺] = 14

If we know the pH we can find out the pOH.

The pH is 4. What is the pOH?

pH + pOH = 14
4 + X = 14
pOH = 10

The pOH is 3. What is the pH?

pH 7 is neutral
pH's below 7 are acid.
pH's above 7 are basic.
Scale goes from 0 to 14.

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⁺]?
(a) pH + pOH = 14                                                                   (b) pH is the neg log of H⁺
        x + 8 = 14                                                                         pH 6 = neg log of [H⁺] concentration
        x = 6                                                                                                     6 is the log

pH = 6 -6 is the neg. log.

1 x 10^-6

Drill Determine the pH of the following solutions:

(1) pOH = 4
(2) pOH = 3
(3) pOH = 11
(4) pOH = 5.6
(5) pOH = 3.5

(6) 1 x 10^-3 M H⁺
(7) 1 x 10^-6 M H⁺
(8) 1 x 10^-8 M H⁺
(9) 1 x 10^-8 M [OH]^-
(10) 1 x 10^-2 M [OH]^-
(11) 1 x 10^-4 M[OH]^-
(12) .001 M HCl
(13) .0001 M HCl
(14) .01 M Na(OH)
(15) .001 M Na(OH)
(16) 1 x 10^-2 M HCl
(17) 1 x 10^-3 M Na(OH)
(18) a solution that contains 1 x 10^-5 mole [H⁺] per liter
(19) a solution that contains .001 M [H⁺] per liter
(20) a solution that contains 1 x 10^-5 mole OH^- per liter
(21) a solution that contains .00001 M NaOH
(22) 3 x 10^-3 M HCl
(23) 5 x 10^-2 M [H⁺]
(24) 7 x 10^-5 M HCl
(25) 1.5 x 10^-5 M HCl
(26) 3.2 x 10^-2 M HCl
(27) .004 M [H⁺]
(28) .0003 M HCl
(29) .015 M [H⁺]
(30) .075 M HCl
(31) .0000025 M [H⁺]
(32) 2 x 10^-8 M Na(OH)
(33) 4 x 10^-2 M [OH]^-
(34) 7 x 10^-10 M [OH]^-
(35) 2.5 x 10^-3 M K(OH)
(36) 7.5 x 10^-6 M Na(OH)
(37) .025 M Na(OH)
(38) .0075 M Na(OH)
(39) .000015 M Na(OH)

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
2nd or inv log - 3.64

What is the H⁺ concentration in the following solutions:

pH 3             pOH 5
pH 7             pOH 7
pH 2             pOH 10
pH 5.2          pOH 2.8
pH 4.3          pOH 5.1

Questions Chapter 8: 8.28; 8.29; 8.30; 8.32

Wednesday, March 21, 2007 01:28:01 PM