Properties of Water Lab

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1 Name Properties of Water Lab Block Directions: Please record all of your answers regarding the properties of water lab on this lab report sheet. Introduction: Water is all around you - an incredibly important molecule in biology! It s in the air that you breathe and in the majority of liquids that you drink. Water makes up between 67-70% of our body, allowing our cells to be able to effectively process a variety of chemical reactions quickly and efficiently. All life depends upon the unique features of water which result from its polar nature and stickiness. Some of the unique properties of water that allow life to exist are: It is less dense as a solid than as a liquid. It sticks to itself cohesion cohesion is also related to surface tension. It sticks to other polar or charged molecules adhesion adhesion results in phenomena such as capillary action. It is a great solvent for other polar or charged molecules. It has a very high specific heat (heat of fusion and heat of vaporization) that is, it can absorb a great deal of heat energy while displaying only small increases in temperature. Water is a polar molecule. The oxygen atom in water has a greater electronegativity, or a stronger pull on the electrons that it shares with the two hydrogens it is covalently bonded to. As a result, the molecule ends up having a partially negatively charged end, near the oxygen, and a partially positively charged end near the hydrogens much like a magnet. Much like a magnet, opposite charges will attract and likes will repel, so that the slightly negatively charged oxygen of one water molecule will be attracted to the slightly positively charged hydrogen of a neighboring water molecule. This weak attraction and sticking together of polar molecules is called hydrogen bonding. Each water molecule has the ability to attract to four different water molecules at one time, and this continues on, creating a globular shape. (Introduction has been modified from 1

2 Pre-lab questions 1. What makes water a polar molecule? 2. Label a hydrogen bond and a covalent bond in the water molecule. 3. Is water polar or nonpolar (circle correct answer)? 4. Is oil polar or nonpolar (circle correct answer)? 5. List a substance that is hydrophobic? 6. Why is water considered the universal solvent? 7. Name at least three solutes in your body. Station 1- Polar or Nonpolar Step 2 Observation: Step 4 Observation: 2

3 Step 5 Observation: Step 6: Is oil or water a better solvent? How do you know? Step 7 Observation: Step 8- Answer the questions: Think about what you observed; can you relate what you observed to anything that may occur in nature? How could this relate to an oil spill in the ocean? How could this affect an ecosystem? Station 2- Surface Tension: The Petri Dish & the Pepper 1. Why does the pepper float? 2. Record your observation. Why do you think this happened? Station 3- Paperclip Madness 1. Record the number of paper clips you were able to get to float. 2. Which property of water did this represent? 3

4 Station 4- Capillary Action 1. How did the ink change? 2. How long did it take for the water to climb to the top? Did it take 25 minutes or longer? 3. Record your data in the table below. Make a line graph to represent your data. Time (min) Distance (cm) Station 5- What s the ph? Step 1- Predict what you think the ph will be for each substance. Step 2- Record the actual ph from the ph indicator paper for each substance. Substance Predicted ph level Windex Lemon Juice Distilled Water Vinegar Orange Juice Coffee 409 disinfectant Apple Juice Pickle juice Laundry detergent Actual ph level Is it an acid / neutral / base 4

5 Use your notes to answer these questions. 1. What does ph mean? 2. What is the difference between acids and bases? 3. Draw a ph scale on the line below that represents the substances you tested above. 4. Describe the relationship between hydrogen ions and ph. 5. Compare the hydrogen ion concentrations in vinegar to Windex. Station 6- The Density of Water Analysis: Use the three sets of mass and volume measurements to calculate three density values for water (remember you are measuring the mass; the volume should be 25mL each time). Then take the average of these three density values. DENSITY = MASS VOLUME Use units!! Mass of H2O: Trial 1 (25mL)- Trial 2 (25mL)- Trial 3 (25mL)- Densities: Trial 1- Trial 2- Trial 3- What is the average of the three densities? 5

6 Station 7- Observing Capillary Action Record the date and time below that you placed the flower or celery in the colored water: Date: Time: Observation 1- Before you leave class, record what you see. Look at the cut end, what do you see? Describe and draw it. Observation 2- Come back tomorrow, record what you see. Has anything changed? Describe and draw it. Observation 3- Day 3, record what you see. Has anything changed? Describe and draw it. 1. What happened to the colored water? 2. Did the colored water travel through all parts of the flower or celery? Explain. 3. If the water traveled differently in different places, suggest a reason for the differences. 4. What properties of water are responsible for these results? 6

Procedure: 1. On your wax paper, place 5-10 drops of water in one area. 3. What do you notice the water does on the wax paper?

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