Table 3: Add 6 M HCl Table 4: Add 6 M NaOH Table 5: Add 0.1 M HCl Table 6: Add 0
ID: 832797 • Letter: T
Question
Table 3:
Add 6 M HCl
Table 4:
Add 6 M NaOH
Table 5:
Add 0.1 M HCl
Table 6:
Add 0.1 M NaOH
Drops
pH
Paper Color
Drops
pH
Paper Color
Drops
pH
Paper Color
Drops
pH
Paper Color
0
12
Violet
0
2.7
Red
0
0
1
1
1
1
2
2
2
2
3
3
3
3
4
4
4
4
5
5
5
5
In my laboratory exercise I was testing buffers.
First I added 4 drops of concentrated NaOH into 2mL of vinegar to make buffer.
Then I added 2 drops of DILUTED HCL. The pH didnt change as expected. The same I did with adding diluted NaOH into above buffer. Again, no change of pH.
For the second part I added CONCENTRATED HCl into the buffer (vinegat + diluted NaOH) and the changes in pH were from 6- 4. Then I added CONCENTRATED NaOH into the buffer and the changes in pH were from 6-8.
Table 3:
Add 6 M HCl
Table 4:
Add 6 M NaOH
Table 5:
Add 0.1 M HCl
Table 6:
Add 0.1 M NaOH
Drops
pH
Paper Color
Drops
pH
Paper Color
Drops
pH
Paper Color
Drops
pH
Paper Color
0
12
Violet
0
2.7
Red
0
0
1
1
1
1
2
2
2
2
3
3
3
3
4
4
4
4
5
5
5
5
Explanation / Answer
ionic
Intermolecular means between molecules. There are many types of intermolecular bonds: The ones you should be most familiar with would probably be the Van Der Waals and the hydrogen bond. The Van Der Waals would be the majority of all intermolecular bonding. However, what we need to know is the most powerful intermolecular force: namely, the hydrogen bond. In some special cases, if hydrogen is bound to a special atom with high electronegativity, creating an extra-strong dipole. That would be the hydrogen bond.
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