Sure, I can guide you through the expected results after adding phenolphthalein to each of the solutions in the test tubes. Here's a step-by-step solution for what you'll observe:
1. Test Tube 1: Water
- Water is a neutral solution, meaning its pH is close to 7. Phenolphthalein remains colorless in neutral solutions.
- Color Observation: Colorless
2. Test Tube 2: Acetone
- Acetone is a neutral substance, and like water, it does not cause phenolphthalein to change color.
- Color Observation: Colorless
3. Test Tube 3: 5 M Citric Acid
- Citric acid is a strong acid solution which means it has a low pH. Phenolphthalein remains colorless in acidic solutions.
- Color Observation: Colorless
4. Test Tube 4: 5% Vinegar
- Vinegar, which contains acetic acid, is also an acidic solution thus it has a low pH. Phenolphthalein will remain colorless in such acidic environments.
- Color Observation: Colorless
5. Test Tube 5: 4 M Ammonia
- Ammonia is a basic solution with a high pH. Phenolphthalein changes to pink in basic solutions.
- Color Observation: Pink
6. Test Tube 6: Diluted Bleach
- Diluted bleach is another basic solution. Therefore, phenolphthalein will change to pink in this solution as well.
- Color Observation: Pink
So, summarizing these observations in the provided table:
```
\begin{tabular}{|c|c|c|}
\hline Test Tube Number & Solution & Color After Addition of Phenolphthalein \\
\hline 1 & water & Colorless \\
\hline 2 & acetone & Colorless \\
\hline 3 & 5 M citric acid & Colorless \\
\hline 4 & [tex]$5 \%$[/tex] vinegar & Colorless \\
\hline 5 & 4 M ammonia & Pink \\
\hline 6 & diluted bleach & Pink \\
\hline
\end{tabular}
```
These changes are due to the pH-dependent nature of phenolphthalein, which remains colorless in acidic and neutral solutions but turns pink in basic solutions.
