Polarity Lab Discussion, chemistry homework help

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  1. based upon the experimental results for the experiment section when you mix iodine, copper(II) sulfate and sodium chloride in water and hexane. In your discussion you should make a conclusion and then explain how your experimental results and observations support your conclusion. The points below should help you identify the information you have available from this experiment to support your conclusion. Submit completed lab report by the due date. Be sure to include the following:
    1. Purpose. Based upon the introduction in your lab manual, what are you trying to find with your experiment?
    2. Claim. Based upon the purpose of your experiment, what claim can you make using your experimental evidence?
    3. Table(s) of your results for the experiment section. This should include your expected results and your experimental observations.
    4. Discussion of your results for the experiment section.
      • i.Explain how the Lewis dot structures and molecular models are the basis for your claim.
      • ii.Explain how your experiment results support your claims.
      • iii.Explain discrepancies between expected and experimental results
    5. Supporting references.
    for Experiment 4: you should write specifically about all three experiments in Part 4. However, you should use the information you learned in the previous parts of the laboratory to support your claim. You should specifically address which solvents (water and hexane) the three solutes (iodine, copper(II) sulfate and sodium chloride) are soluble in and why. Identify the types of intermolecular or attractive forces present in each mixture, relating the forces to the polarities determined above.

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Results: Polarity – Complete as a Group Names:_____________________________________________________ Molecular Models: In-Lab Exercise Compound Water Ethanol Hexane Dichloromethane Acetone Octane Iodine Sketch of Molecular Model Predicted Polarity (Explain using model) Miscibility In Lab-Exercise Predictions: When these solutions are mixed together, do you predict the two solutions to be miscible? Use your Lewis dot structures and molecular models to explain your prediction. If the solutions are not miscible, which liquid will be in the top layer and why? Water and Ethanol Miscible Water and Hexane Not miscible because its polar and non polar substances Water would be at the bottom and hexane would be at top because of density Ethanol and Hexane Not miscible because its polar and non polar substances Ethanol would be at the bottom and hexane would be at top because of density Observations: Test the miscibility of the following liquids and complete the in-lab exercise for this section. You can test the miscibility of two liquids by adding 1 mL (about 20 drops) of each liquid to a test tube, covering tightly with a piece of parafilm and then mixing for 5 seconds with a vortex mixer. Then observe the resulting solution and record observations you make in your lab notebook. If there are two layers, identify which of the substances is in the top layer and explain how you know. Note: Refer to your partner by name and page number for his/her observations for those experiments that you did not observe directly. Water and Ethanol Water and ethanol appeared to be miscible. The two substances mixed immediately and remained mixed after using the vortex mixer. This matches our prediction because both are polar. Water and Hexane Water and hexane were not miscible. After using the vortex mixer, the two solutions remained separated, showing a line between the two. Water was the bottom layer. This matches our prediction because water is polar and hexane is nonpolar. Ethanol and Hexane Ethanol and hexane were miscible. After using the vortex mixer, no separation could be seen between the two substances. This is different from our prediction. Even though ethanol is polar, it is not a strong polar molecule because it also contains nonpolar carbon-hydrogen bonds. It can mix in polar and nonpolar substances. Solubility In-Lab exercise Predictions - Water: When these solids are mixed with water do you predict that the solid will dissolve? Use your Lewis dot structures and molecular models to explain your prediction. Compound Water Sodium chloride Soluble Sucrose Soluble Octane Insoluble Iodine Soluble Copper (II) sulfate Soluble Dichloromethane Insoluble Acetone Insoluble Acetylsalicylic acid Insoluble Predictions - Hexane: When these solids are mixed with hexane do you predict that the solid will dissolve? Use your Lewis dot structures and molecular models to explain your prediction. Compound Hexane Sodium chloride Insoluble Sucrose Insoluble Octane Soluble Iodine Soluble Copper (II) sulfate Insoluble Dichloromethane Insoluble Acetone Soluble Acetylsalicylic acid Soluble Observations for Water and Hexane: Design and conduct experiments to test these predictions. Review your plan with your instructor, and divide up the tasks. Keep in mind Green Chemistry Principle # 1 – Prevention (https://www.acs.org/content/acs/en/greenchemistry/what-is-green-chemistry/principles/12principles-of-green-chemistry.html ), and that all waste MUST be disposed of properly. Use only a very small amount of the solid substances to determine whether they dissolve or not. Review your answers to the waste section in the in-lab assignment prior to disposing of your mixtures. Each student should record only the work he/she does in the individual notebook. Complete the in-lab exercise as a group for this section. Did your predictions agree with your observations? Explain. Solvent System Compound Water Hexane Sodium chloride Soluble Insoluble Sucrose Soluble Insoluble Octane Insoluble Soluble Iodine Partially soluble and the Soluble (dark purple) water color turned to light brown Copper (II) sulfate Partially soluble and the Insoluble water color turned to blue Dichloromethane Insoluble Soluble Acetone Soluble Soluble Acetylsalicylic acid Partially soluble and formed some clouds Insoluble Explanations: Iodine only partially mixed with water, probably because water is polar and iodine is nonpolar. Copper (II) Sulfate only partially mixed with water because it is ionic. Acetone was soluble with water and hexane because it has polar and nonpolar bonds. The C-O bond is polar. Acetylsalicylic acid was partially soluble with water because it has some polar bonds (C-O and OH). Observations: Experimental Observations for Mixtures Iodine, Water and Hexane The iodine mixed with the hexane and not the water. The hexane turned to a dark purple color while the water turned to a light brown color. To test the idea of iodine preferring hexane then water was we took new hexane and added into another test with the water and iodine mix. The results showed that the iodine moved from the water to the hexane. Copper (II) sulfate, Water and Hexane The cooper sulfate mixed with water but did not mixed with the hexane. The color change only happened with the water showing that it’s soluble with water and insoluble with hexane. The blue was at the bottom with the water while the top stayed clear with hexane. Sodium chloride, Water and Hexane The sodium chloride mixed with the water but not the hexane. The sodium chloride dissolved in the water and didn’t dissolve with the hexane. We took the aqueous solution of the water and sodium chloride and heated on the hot plate. What were left were sodium chloride and the water boiled off. That shows the presents of sodium chloride in the water. Experiment 1: Polarity Question: How does the polarity of a molecule affect its solubility? Goals 1. Students understand polarity. Objectives 1. Students can draw Lewis dot structures. 2. Students can make molecular models. 3. Students can use Lewis dot structures and molecular models to predict the polarity of a compound. 4. Students can predict the solubility and miscibility of different substances. Introduction Background: The polarity of a molecule plays an important role in its physical properties and its chemical behavior. In this experiment you will predict the polarity of a series of different compounds and then develop tests to obtain experimental evidence that you can use to support or refute your prediction. Equipment 1. Molecular model kit 2. Vortex mixer 3. Parafilm 4. Disposable pipettes 5. Hot Plate Reagents 1. Sodium chloride 2. Sucrose 3. Water 4. Ethanol 5. Hexane 6. Octane 7. Iodine 8. Copper (II) sulfate 9. Dichloromethane 10. Acetone 11. Acetylsalicylic acid Procedure 1. Molecular Models - In-Lab Exercise a. Use the molecular model kits to make models of the following compounds. i. Water ii. Ethanol iii. Hexane iiii. Dichloromethane V. Acetone vi. Octane vii. Iodine b. Sketch your model in your notebook and in the space provided in the data template. c. Based upon your molecular model, predict the polarity for each compound and record in your data template. d. Review your answers with your instructor. 2. Miscibility - In-Lab Exercise a. Prediction: When these solutions are mixed together, do you predict the two solutions to be miscible? Use your Lewis dot structures and molecular models to explain your prediction. If the solutions are not miscible, which liquid will be in the top layer and why? Record your answers in the data sheet. i. Water and ethanol ii. Water and hexane iii. Ethanol and hexane b. Observations: Test the miscibility of the following liquids and complete the in-lab exercise for this section. You can test the miscibility of two liquids by adding 1 mL - about 20 drops - of each liquid to a test tube, covering tightly with a piece of parafilm and then mixing for 5 seconds with a vortex mixer. Then observe the resulting solution and record your observations for at least one mixture in your laboratory notebook. For other mixtures, you may refer to your lab partners’ notebook by page number. Record all observations on the data sheet. If there are two layers, identify which of the substances is in the top layer. Consider what you could do to prove which substance is the top layer. i. Water and ethanol ii. Water and hexane iii. Ethanol and hexane 3. Solubility – In-Lab Exercise a. Prediction: Water - When these solids are mixed with water do you predict that the solid will dissolve? Use your Lewis dot structures and molecular models to explain your prediction. Record your answers in the data sheet. i. Sodium chloride with water ii. Sucrose with water iii. Octane with water iiii. Iodine with water v. Copper (II) sulfate with water vi. Dichloromethane with water vii. Acetone with water viii. Acetylsalicylic acid with water b. Prediction: Hexane - When these solids are mixed with hexane do you predict that the solid will dissolve? Use your Lewis dot structures and molecular models to explain your prediction. Record your answers in the data sheet i. Sodium chloride with hexane ii. Sucrose with hexane iii. Octane with hexane iiii. Iodine with hexane v. Copper (II) sulfate with hexane vi. Dichloromethane with hexane vii. Acetone with hexane viii. Acetylsalicylic acid with hexane c. Observations: Design and conduct experiments test these predictions. Review your plan with your instructor, and divide up the tasks. Keep in mind Green Chemistry Principle # 1 - Prevention (https://www.acs.org/content/acs/en/greenchemistry/what -is-green-chemistry/principles/12-principles-of-green- chemistry.html ), and that all waste MUST be disposed of properly. Use only a very small amount of the solid substances to determine whether they dissolve or not. Review your answers to the waste section in the In-Lab assignment prior to disposing of your mixtures. Each student should record only the work he/she does in the individual notebook. Complete the In-Lab exercise as a group for both water and hexane. Record all information on the data sheet. Each group member should have recorded observations for at least one mixture in his/her laboratory notebook. For other mixtures, you may refer to your lab partners' notebook by page number. 4. Experiment – for your individual discussion a. Prediction: For your discussion, based on the experimental results above, together with the polarity that you predicted from the molecular models, predict what will happen when you mix the following. Write your predictions in your notebook. i. Add iodine to a mixture of water and hexane. ii. Add copper(II) sulfate to a mixture of water and hexane. iii. Add sodium chloride to a mixture of water and kane – then separate the layers and evaporate off the water. b. Experiment and observations: Conduct an experiment to test your predictions. Review this with your instructor before proceeding. Record observations for at least one mixture in your laboratory notebook. For other mixtures, you may refer to your lab partners’ notebook by page number. You will discuss these results in your individual discussion. i. Add iodine to a mixture of water and hexane. 1. Mix together 2. Observe 3. Remove the aqueous layer 4. Add hexane to the aqueous layer 5. Observe. ii. Add copper(II) sulfate to a mixture of water and hexane. 1. Mix together 2. Observe iii. Add sodium chloride to a mixture of water and hexane – then separate the layers and evaporate off the water. 1. Mix together 2. Observe 3. Remove aqueous layer 4. Evaporate aqueous layer to dryness c. For your discussion, you should write specifically about all three experiments in 4. However, you should use the information you learned in the previous parts of the laboratory to support your claim. You should specifically address which solvents (water and hexane) the three solutes (iodine, copper(II) sulfate and sodium chloride) are soluble in and why. Identify the types of intermolecular or attractive forces present in each mixture, relating the forces to the polarities determined above.
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Explanation & Answer

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Polarity is a physical property of mixes which relates other physical properties, for example,
liquefying and breaking points, solvency, and intermolecular communications between particles.
And the purpose of the following experiments is to test it effects on solubility of compounds in
various solvents.
Generally, there is an immediate relationship between's the polarity of a particle and number and
sorts of polar or non-polar covalent bonds which are available. In a couple of cases, a particle
may have polar bonds, however in a symmetrical plan which at that point offers ascend to a nonpolar atom, for example, carbon dioxide.
Predictions:
Water and Ethanol

Miscible

Water and Hexane

Not miscible because its polar and non polar substances
Water would be at the bottom and hexane would be at top because of density

Ethanol and Hexane

Not miscible because its polar and non polar substances
Ethanol would be at the bottom and hexane would be at top because of density

Observations:
Water and Ethanol

Water and ethanol appeared to be miscible. The two substances mixed immediately and
remained mixed after using th...


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