OCE 2001L: OCEANOGRAPHY LAB Water Masses and Density Stratification
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1 OCE 2001L: OCEANOGRAPHY LAB Water Masses and Density Stratification Objective: To examine the stratification of seawater into water masses of different densities. Materials Needed: brine no color very cold brine (blue) pure water (yellow) seawater (red) 400 ml beakers (4) 100 ml graduated cylinder centigrade thermometer Introduction: Seawater is a mixture of water and minerals (salts) that covers 71% of the earth. The oceans of the world have an impact on many almost every aspect of our lives, and part of this is due to some of the very special properties of seawater. As you will learn in lecture, the density of pure water is at 4 ºC is g/cm 3. When salt is added to water, the density is increased. Consequently, seawater is denser (or heavier) that pure water. The density of water also changes with temperature. Salinity and temperature are the two main factors that determine the density of seawater. (The density of seawater also depends on pressure, but the effect is negligible except in the deepest parts of the ocean.) In last week s lab, you measured the density of water at different temperatures and salinities. This week you are going to explore how temperature and salinity characteristics create separate water masses that coexist in the ocean in density layers (strata). Oceanographers often characterize the ocean as having two layers. Warmed by energy from the sun, a thin layer of low density water is formed at the surface. Underlying this is a very deep layer of cold, high density water. The boundary between the two layers is the pycnocline, where the density changes rapidly over a short change in depth. When lighter water overlies a denser layer, the ocean is said to be stably stratified, since gravity will keep the heavier water mass on the bottom. Mixing between the layers occurs by molecular diffusion, the random movement of molecules across the density interface, or by eddy diffusion, where friction between the two produces waves and turbulence that exchanges larger volumes of water. Despite the mixing at the pycnocline, constant warming from the sun maintains the stable two layer ocean. However, there are several areas where conditions are favorable for the formation of high density water at the ocean surface. When this form of stratification occurs, it is unstable. Gravity immediately forces the high density surface water to sink to a depth where the water density matches. Water motion that arises from density differences is referred to as thermohaline circulation, since the density differences
2 are a consequence of temperature and salinity variations. Although very slow-moving, deep-water thermohaline currents carry an enormous volume of water and can be traced through every ocean basin. These currents may also play an important role in moderating and stabilizing the Earth s climate. For today s lab exercise, you will be provided with four jugs of water. There will be a jug of yellow water that was made up by adding a small amount of yellow food coloring to distilled water. A second jug will have red dye added to local seawater that has a salinity of about 30 parts per thousand ( ). This red jug will also be left in a cooler overnight, so it should be at a temperature of about 10º C. A third jug will have a mixture of salt so concentrated that there will be some undissolved salt on the bottom of the jug. This then is a very salty or brine solution and it will be a room temperature. It has no coloring added, so it will be mostly clear. The forth jug will have some blue food coloring added to a very salty brine solution that has been left in the freezer and crushed ice added to drop its temperature down to almost 0º C, or even slightly lower. There will be a large 2,000ml beaker at your lab station that you will be using for this experiment. You will also have several 300 ml beakers to collect the water samples. You will notice that these beakers are marked off in 50 ml increments, however those marks are not very accurate, so when you are asked to measure out 200 ml of one of the samples provided you must use the graduated cylinder provided at your lab station. Directions: 1. Since density is always the weight of a given volume we first need to determine the weight of the beaker we plan to use to hold this 200 ml sample of red seawater. Using the triple beam balance at your lab station, measure the weight in grams of a 300 ml beaker. Record this weight in Table I below. Next measure out 200 ml of the red solution and place it in the beaker. Now measure the weight of the red solution and the beaker and record it in Table I. When you subtract the weight of the beaker from the weight of beaker and solution, you have the weight of the 200 ml of red solution. Record this number in Table I. Since temperature also plays an important role in density, you will need to use the Centigrade thermometer provided and record the temperature of the red water sample in Table I. 2. Now after first measuring the weight of a second beaker, measure out 200 ml of the clear brine solution in a graduate cylinder and again record the temperature and weight of the clear solution on Table I. Now take a clear plastic bag and place the large 2,000 ml beaker on top of the plastic bag
3 and draw the outline with a marker, but leave a one inch wide tab as shown below. This tab will give you something to hold onto later when you must gently remove the clear plastic circle. 3. Next pour the clear solution from the small beaker, into the large 2,000ml beaker. Then gently place the clear plastic circle on the top of this clear sample and 1 have the one inch tab up the side of the large beaker. Using the funnel provided, carefully pour the red solution onto the center of the floating plastic circle in the large beaker. The clear plastic circle should prevent most of the red sample from spilling over into the clear water sample. (A small amount of seepage around the edges of the plastic is no problem.) Now carefully use the tab to pull the clear plastic circle out of the large beaker. What happened? If the red sample was more dense than the clear one, would the two solutions have remained in their original positions? So which of the two solutions used so far has the greater density? 4. Now place an ice cube carefully on top of the red solution, and watch what happens as it melts. (The ice cube is made from tap water). Did the water from the melted ice cube sink or remain on the surface? What does that tell us about the density of the tap water as compared to the water in the large beaker? 5. Now replace the circle of plastic on the surface of the large beaker and using the funnel, pour out a 200 ml sample from the blue jug. First however you must determine the weight and temperature of the green water just like you did for the clear and red samples, and record the data on the blue water in Table I. 6. Once you have the blue sample poured into the large beaker, pull the tab again. What happened? From this, what can we conclude about the density of the blue water?
4 7. Next measure out 200 ml of the yellow water sample and again measure and record its temperature and weight on Table I. Again using the plastic circle, pour the yellow water sample onto the top of the large beaker using the funnel. What happened to the yellow sample once you pulled the tab out? What can we conclude about the density of the yellow sample from this? Density is always the weight of a given volume, so now calculate the density of all four layers by dividing the weight of each sample by 200 (the volume of each sample) and add that to Table I. Now we can see that the most dense water was on the bottom, the least dense on the top. Table I. Temperature, Weight, and Density of Water Samples Clear Sample Red Sample Blue Sample Yellow Sample Temperature ( C) Weight (g) Density (g/cm 3 )
5 8. On Table II, sketch out a drawing of the large beaker and label each layer. Now rank your four layers with numbers from 1 to 4 with number 1 being the greater density, number 4 the least dense. Table II. Density Layers in the Beaker
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