Acids and Bases

Acids and Bases

1. B.  False because the color does not tell whether it is an acid or base it is the pH scale level.
2. D. More than one is basic because two of them have a higher pH level than 7.0.
3. C. Just the one because it has more levels H30+ than the other ones.
4. B. this one is basic because the hydrogen atoms powers need to be over 7.
5. D. A and B both have higher levels of H
6. A. Adding water would increase the pH because the water lessens the acidity. More water lessens the acidity, so pH goes up.
7. B. the pH decreases when water is added resulting in a lower number. more water lessens the basicity, so pH goes down, from 10 to 9.7, but not by 2 .
8. A. A, B, C because the closer the number is to zero the more acid it is and the closest is it to 14 the more basic it is.
9. C. B, A, C because looking at the powers that the numbers have they are increasing.
10. A. Something was added that made the equilibrium shift left. 

Name:__Emily Minniecheske____

Introduction to Strong and Weak Acids and Bases PhET Lab (rvsd 5/2011)

        How does the strength of an acid or base affect conductivity?pH?

Introduction:

When you test your pool’s pH, what are you those little vials or paper strips telling you?  When you hear an acid called “strong” or “weak”, what do those terms refer to?  In aqueous solutions, compounds can exist as molecules (undissociated) or ions (dissociated).  When an acid or a base exists in solution nearly completely as dissociated ions, we refer to that acid or base as strong.  A weak acid or base will donate ions to the solution, but will remain primarily as undissociated molecules.

Notation:

Acids are abbreviated HA, with the H representing the proton (H+) the acid donates to the solution.  The A is referred to as the acidic anion (A-) that is left in solution as the proton is donated.

Strong Bases are abbreviated MOH, with the OH representing the hydroxide ion (OH-) the base donates to the solution.  The M is cation (M+) that is left in solution as the hydroxide is donated..

Autoionization:

Even without any acid or base added a very small number of water molecules will form protons (H+) and hydroxide ions (OH-).  The protons will then form hydronium ions, the acid ion.

Procedure: PhET Simulations à Play With Sims à Chemistryà Acid-Base Solutions à  

The concentration of the acids and bases used in the  at 0.010 (10^-2) Molar.

·         Begin with a strong acid and lower the pH probe into the beaker.  What is the pH of this solution? 

·         Test this strong acid with both pH paper and the conductivity probe.  What color does the pH indicator become?  Is this strong acid an electrolyte?  Does current travel through this solution?

·         Repeat the above tests with the weak acid, the strong base, and the weak base, and water.  Collect your observations in the table below:

	Strong Acid	Weak Acid	Strong Base	Weak Base	Water
pH meter read (value)	2.00 pH	4.5 pH	12.00 pH	9.50 pH	7.00 pH
pH paper (color)	2 red	5 orange	11 blue	9 green	7 yellow
Conductivity (bright/dim/none)	bright	dim	bright	dim	none
Exists as Mostly (ions/molecules)	ions	molecules	ions	molecules	ions

Procedure:

This simulation allows you to change the concentration of a strong and weak acid and base.

Complete the table below for some strong acids and bases and weak acids and bases by adjusting the concentration.

Strong Acids

Strength	Initial Acid Concentration (mol/L)	[HA] (mol/L)	[A-] (mol/L)	[H+] (mol/L)	pH
Strong	.010 M	negligible	1.00x10^-2	1.00x10^-2	2
Strong	.050 M	negligible	5.00x10^-2	5.00x10^-2	1.3
Strong	.100 M	Negligible	1.00x10^-1	1.00x10^-1	1
strong	1.00 M	negligible	1.00x10^0	1.00x10^0	0

Weak Acids

Strength (approximately)	Initial Acid Concentration (mol/L)	[HA] (mol/L)	[A-] (mol/L)	[H+] (mol/L)	pH
lower	.015 M	1.5x10^-2	3.87x10^-5	3.87x10^-5	4.41
lower	.150 M	1.5x10^-1	1.22x10^-4	1.22x10^-4	3.91
higher	.015 M	1.93x10^-4	1.48x10^-2	1.48x10^-2	1.83
higher	.150 M	1.58x10^-2	1.34x10^-1	1.34x10^-1	.87

Strong Bases

Strength	Initial Acid Concentration (mol/L)	[MOH] (mol/L)	[M+] (mol/L)	[OH-] (mol/L)	pH
strong	.010 M	negligible	1.00x10^-2	1.00x10^-2	12
strong	.050 M	Negligible	5.00x10^-2	5.00x10^-2	12.7
strong	.100 M	Negligible	1.00x10^-1	1.00x10^-1	13
strong	1.00 M	negligible	1.00x10^0	1.00x10^0	14

Weak Bases

Strength (approximately)	Initial Acid Concentration (mol/L)	[B] (mol/L)	[BH+] (mol/L)	[OH-] (mol/L)	pH
lower	.015 M	1.49x10^-2	9.74x10^-5	9.74x10^-5	9.99
lower	.150 M	1.50x10^-1	3.09x10^-4	3.09x10^-4	10.49
strong	.015 M	1.64x10^-4	1.48x10^-2	1.48x10^-2	12.17
strong	.150 M	1.38x10^-2	1.36x10^-1	1.36x10^-1	13.13

Conclusion Questions:

1.      A strong acid is very concentrated / exists primarily as ions. (circle)

2.      A weak base is a nonelectrolyte / weak electrolyte / strong electrolyte.

3.      A strong base is a nonelectrolyte / weak electrolyte / strong electrolyte.

4.      At the same concentration (Molarity) a strong acid will have a higher / lower / the same pH as a weak acid.

5.      As concentration of a weak acid increases, the pH increases / decreases / remains constant.

6.      As concentration of a weak base increases, the pH increases / decreases / remains constant.

7.      As the concentration of a weak acid increases, the number of ions increases / decreases / remains constant.

8.      As the concentration of a weak acid increases, conductivity increases / decreases / remains constant.

9.      As the strength of a weak acid increases, the proportion of ions to molecules increases / decreases.

10.  As the strength of a weak acid increases, the conductivity increases / decreases / remains constant.

11.  What are the pH values of a weak acid with a concentration of 0.10 and a strong acid with a concentration of 0.01, ten times lower?     Weak acid, 0.10 M :_6___________ Strong Acid, 0.01 M :___2_________

12.  Explain the significance of the results of your calculation above.  The stronger acid has a lower pH because there are more ions.