the question you tried to answer. Answer: How salt effects the temperature of the water hot and cold? (3 points) 2. Which observations or experiences helped you form your hypothesis? Answer: When I did beaker A which was cold with salt. And When I did beakers B-D that were hot with salt. (3 points) 3. State your hypothesis. Answer: If the water is cold with salt what way does the temperature go up or down. Verses if the water is hot with salt. (15 points) 4. Use the data from Part 1 of
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electrode in another beaker. 4. Attach the electrodes to the voltmeter. 5. Roll a lengthy piece of paper towel and wet it with sodium chloride (salt bridge ) 6. Place each end of the salt bridge in the beakers. Make sure it’s dipped in the electrolyte solution. 7. Apparatus should be set as in the diagram below. 8. Keep spraying the salt bridge with sodium chloride to keep moist. 9. Record the voltmeter reading and observe clearly for any changes. 10. Repeat step 2 to 9 for
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solid 15x150mm test tube clamp watch acetone Ice cyclohexane sodium chloride Lab Safety: Wear protective googles‚ apron‚ and gloves. Procedures: Prepare ice/salt/water bath Place 50g of solid NaCl in a 400mL beaker and add just enough water to dissolve the salt. Fill an 800mL beaker 2/3 full of ice‚ and then pour salt water mixture into the beaker‚ stir. In the hood‚ into two nested test tubes‚ add 10 mL of cyclohexane from a buret. Record initial and final buret readings. Then measure
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Introduction : Copper(II) sulphate‚ is a type of salt which it is formed by combining both copper ion and sulphate ion through the experiment of double displacement between dilute sulphuric acid ‚ and copper(II) carbonate ‚ . Through this process‚ the copper ion will displace the hydrogen ion as it is more electropositive and sulphate ion will displace carbonate ion as it is more electronegative. The resulting copper (II) sulphate solution when cooled can easily crystalize
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square of paper‚ carefully remove the plastic and allow all the iron to fall onto the paper. Weigh and determine the net mass of the iron powder/filings. 2. Separating out the Sand a. Put the remaining mixture‚ containing sand‚ benzoic acid‚ and table salt into your beaker and add 50 mL of distilled water. b. Set up the beaker stand and burner fuel and heat the beaker of solids and water to near boiling. Stir the mixture to make sure all soluble material dissolves. At this point‚ the benzoic acid and
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occurs when water becomes tightly attracted to a metal salt base on it’s polarity. The water molecules maintain integrity as molecules‚ however they are considered to be part of the formula of the hydrate. When the hydrate metal salt crystal is heated‚ the attractions to the water are broken by the heat energy and the water escape from the crystal. After heating the salt crystal is called as anhydrous‚ which means without water. Many of the salt contain transition metals such as cobalt that is colorful
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swirled around to have everything mixed. Cup #2 then had half a teaspoon of table sugar added and cup #3 had half a teaspoon of table salt added to them. After that‚ a straw was dipped into each solution separately‚ and blown through in order to make bubbles. Data was recorded while blowing bubbles. Data Table 1: Bubbles Using Different Solutions Control Sugar Salt Appearance of Solution -Colorless -More translucent than cup one -Cloudy Bubble Size -Generally small -Occasionally medium
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mass an object has. Adding salt to the water adjusted the water. Squeeze the bottle hard enough‚ putting pressure to the packet. This causes the bubbles to get smaller and the entire packet to become more dense. Objective: The objective of this experiment is to find the density and buoyancy which is an upward force exerted by a fluid. Hypothesis: Think that all the packages are going to float and when squeezed‚ the package elevates more. It will sink as you add more salt Materials: A 1 liter
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all different shapes‚ abt .25 inch‚ cloudy color.After crushing: breaks into different sized shards‚ some smaller crystals‚ Wet: Salt mostly dissolves although layer of tiny granules is visible at bottom of water bubble. | c) Appearance of sand | Dry: multicolored‚ different shapes and sizes‚ generallty smaller than the salt crystals‚ very hard‚ not as sharp as salt crystals. Feels course. Some grains look more uniform to each other than others do.Wet: did not dissolve. Seemingly unchanged. |
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seeds tolerant to higher concentrations of saline? “All soil contains salts‚ many of which are essential nutrients for plants. Salinity occurs when soluble salts (usually NaCl) are elevated in soil and water. Every continent is affected by salinized soil and water; approximately 7% of the world’s land area.” (Nerissa Hannink‚ 2005). “But why should we care about how a plant copes with excess salt? Once inside the cell‚ salt can cause ionic stresses‚ largely as Na+ (and Cl-) inhibit metabolic
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