yesterday’s homework. the concentration of either the h + ion or the oh - ion is given for three...

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Yesterday’s Homework

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Page 1: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

Page 2: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

The concentration of either the H+ ion or the OH- ion is given for three aqueous solutions at 298oK. For each solution, calculate [H+] or [OH-]. State whether the solution is acidic, basic, or neutral.

Page 3: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

If this wasn’t easy, you’re doing it wrong.

Page 4: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[H+] = 1.0 x 10-13M

Page 5: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[H+] = 1.0 x 10-13M[OH-] = 1.0 x 10-1M

Page 6: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[H+] = 1.0 x 10-13M[OH-] = 1.0 x 10-1M

basic

Page 7: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-7M

Page 8: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-7M[H+] = 1.0 x 10-7M

Page 9: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-7M[H+] = 1.0 x 10-7M

neutral

Page 10: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-3M

Page 11: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-3M[H+] = 1.0 x 10-11M

Page 12: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

[OH-] = 1.0 x 10-3M[H+] = 1.0 x 10-11M

basic

Page 13: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Yesterday’s Homework

Any questions?

Page 14: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

Page 15: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

1. What is true of [H+] and [OH-]?

a. [H+] = [OH-]

b. [H+] x [OH-] = 1 x 10-7

c. [H+] ÷ [OH-] = 1 x 10-7

d. [H+] x [OH-] = 1 x 10-14

e. [H+] ÷ [OH-] = 1 x 10-14

Page 16: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

2. In a neutral solution, pH =

a. 0

b. 0.5

c. 1

d. 7

e. 14

Page 17: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

3. 1 x 10-5 = ?

a. 5

b. 100,000

c. 0.000,01

d. 0.000,001

Page 18: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

4. Which number is bigger?

a. 1 x 10-2

b. 1 x 10-6

.

Page 19: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

1. What is true of [H+] and [OH-]?

a. [H+] = [OH-]

b. [H+] x [OH-] = 1 x 10-7

c. [H+] ÷ [OH-] = 1 x 10-7

d. [H+] x [OH-] = 1 x 10-14

e. [H+] ÷ [OH-] = 1 x 10-14

Page 20: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

1. What is true of [H+] and [OH-]?

a. [H+] = [OH-]

b. [H+] x [OH-] = 1 x 10-7

c. [H+] ÷ [OH-] = 1 x 10-7

d. [H+] x [OH-] = 1 x 10-14

e. [H+] ÷ [OH-] = 1 x 10-14

Page 21: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

2. In a neutral solution, pH =

a. 0

b. 0.5

c. 1

d. 7

e. 14

Page 22: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

2. In a neutral solution, pH =

a. 0

b. 0.5

c. 1

d. 7

e. 14

Page 23: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

3. 1 x 10-5 = ?

a. 5

b. 100,000

c. 0.000,01

d. 0.000,001

Page 24: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

3. 1 x 10-5 = ?

a. 5

b. 100,000

c. 0.000,01

d. 0.000,001

Page 25: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

4. Which number is bigger?

a. 1 x 10-2

b. 1 x 10-6

Page 26: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Daily Quiz Questions

4. Which number is bigger?

a. 1 x 10-2

b. 1 x 10-6

Page 27: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

Page 28: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

The logarithm of a number is the number of times

10 must be multiplied by itself to equal that number.

Page 29: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

1000 = 10 x 10 x 10

log 1000 = 3

Page 30: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

To find the logarithm of a number, count the zeroes or, if the number is in scientific notation, look at the exponent.

Page 31: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

1 = 1 x 100

10 = 1 x 101

100 = 1 x 102

0.1 = 1 x 10-1

0.01 = 1 x 10-2

log 1 = 0

log 10 = 1

log 100 = 2

log 0.1 = -1

log 0.01 = -2

Page 32: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

Page 33: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

Page 34: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

100 x 1000 = 100,000

Page 35: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

100 x 1000 = 100,000

2 + 3 = 5

Page 36: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

1 x 108 = 100,000,000

Page 37: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

1 x 108 = 100,000,000

0 + 8 = 8

Page 38: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can multiply two numbers by adding their logarithms.

2 x 108 = 200,000,000

? + 8 = ?

Page 39: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

So what’s the logarithm of 2? You have to look it up.

2 x 108 = 200,000,000

? + 8 = ?

Page 40: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

So what’s the logarithm of 2? You have to look it up.

2 x 108 = 200,000,000

0.301 + 8 = 8.301

Page 41: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

What if the number is small instead of big?

Page 42: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

What if the number is small instead of big?

0.0003 = 3 x 10-4

Page 43: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

What if the number is small instead of big?

0.0003 = 3 x 10-4

log 0.0003 = log 3 + log 10-4

Page 44: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

What if the number is small instead of big?

0.0003 = 3 x 10-4

log 0.0003 = log 3 + log 10-4

= 0.477 – 4

Page 45: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

What if the number is small instead of big?

0.0003 = 3 x 10-4

log 0.0003 = log 3 + log 10-4

= 0.477 – 4

= -3.523

Page 46: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can find the logarithm of any number by pressing the “log” key on a calculator…

Page 47: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can find the logarithm of any number by pressing the “log” key on a calculator…

but

Page 48: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

You can find the logarithm of any number by pressing the “log” key on a calculator…

but

…if you don’t understand what the calculator is doing, the

information is useless to you.

Page 49: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

Try a few!

Page 50: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 103 =

Page 51: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 103 = 3

Page 52: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 108 =

Page 53: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 108 = 8

Page 54: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 10-10 =

Page 55: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 10-10 = -10

Page 56: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 2 =

Page 57: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 2 = 0.301

Page 58: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 5.8 =

Page 59: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 5.8 = 0.763

Page 60: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 9.2 =

Page 61: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 9.2 = 0.963

Page 62: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4 x 1012 =

Page 63: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4 x 1012 = 0.602 + 12

Page 64: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4 x 1012 = 12.602

Page 65: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 8.3 x 105 =

Page 66: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 8.3 x 105 = 0.919 + 5

Page 67: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 8.3 x 105 = 5.919

Page 68: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 7.1 x 10-3 =

Page 69: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 7.1 x 10-3 = 0.851 - 3

Page 70: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 7.1 x 10-3 = -2.149

Page 71: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4.8 x 10-11 =

Page 72: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4.8 x 10-11 = 0.681 - 11

Page 73: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Logarithms

log 4.8 x 10-11 = -10.319

Page 74: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

pH

pH = -log [H+]pOH = -log [OH-]

pH + pOH = 14

Page 75: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

What is the pH?

What is the pOH?

Is it acidic or basic?

Page 76: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

Page 77: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

0.0035 = 3.5 x 10-3

Page 78: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

0.0035 = 3.5 x 10-3

log 0.0035 = log 3.5 + log 10-3

Page 79: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

0.0035 = 3.5 x 10-3

log 0.0035 = log 3.5 + log 10-3

= 0.544 – 3

Page 80: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

0.0035 = 3.5 x 10-3

log 0.0035 = log 3.5 + log 10-3

= 0.544 – 3

= –2.456

Page 81: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

0.0035 = 3.5 x 10-3

log 0.0035 = log 3.5 + log 10-3

= 0.544 – 3

= –2.456

pH = 2.456

Page 82: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

[H+] = 0.0035

pH = 2.456

pOH = 14 – 2.456

= 11.544The solution is acidic.

Page 83: Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate

Homework

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