Question

pH= 4.75 + log (5/5)= 4.75

pH= 4.75 + log (1/5)= 4.05

pH= 4.75 + log (1/10)= 3.75

pH= 4.75 + log 10= 5.75

pH= 4.75 + log 5= 5.44

Table 3: Sodium Acetate Data

Sodium Acetate (g)	Molarity of Sodium Acetate (Step 7)
4.0 g	0.4876 M

Table 4: Buffer Solutions and pH Readings for Beakers A, B, C, D, and E

Buffer	mL of Acetic Acid	mL of Sodium Acetate	pH measured
A	5	5	4.3
B	5	1	3.6
C	10	1	3.4
D	1	10	5.3
E	1	5	5.0

Table 5: Observing the Effects of Acid on Buffer F and Buffer H

Buffer	pH with 0 mL of Cola	pH with 5 mL of Cola	pH with 10 mL of Cola	pH with 20 mL of Cola
Buffer F	4.4	4.7	4.4	4.4
Buffer H (water)	7	3.2	n/a	n/a

Table 6: Observing the Effects of Acid on Buffer G and Buffer I

Buffer	pH with 0 mL of Borax Solution	pH with 5 mL of Borax Solution	pH with 10 mL of Borax Solution	pH with 20 mL of Borax Solution
Buffer G	4.2	4.2	4.4	4.5
Buffer I (water)	7.0	8.8	n/a	n/a

Lab Questions

1. Compare the calculated buffers A, B, C, D and E (found in Pre-Lab Question #3) to the actual pH that you measured in Table 4. What do you notice? Describe what may have accounted for any variations.
2. Compare the pH of the buffer solutions A, F, and G. Is this what you would expect? Why?
3. Did either buffer F or G reach buffer capacity? How do you know? Explain your reasoning.
4. What happened when the cola and borax solutions were added to the water? Is water a good buffering system?
5. What are some systems where buffers would be important? Name two examples of buffers you might encounter in your daily life.