B. Using the concept of intermolecular forces of attraction, explain why butter melts at roomtemperature but solidifies when refrigerated. PERFORMANCE TASKActivity 2.2.A. Using the concept of bond polarity and solubility, explain why water (H20) and vinegar are miscible,but vinegar and oil are immiscible.

Since you have asked multiple questions, we will solve the first question for you. If you want any…

Answered: B. Using the concept of intermolecular…

B. Using the concept of intermolecular forces of attraction, explain why butter melts at room temperature but solidifies when refrigerated.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 20CR

See similar textbooks

Similar questions

4. Why do you determine a mass by difference? You use this because it's typically more accurate. 5. What are equivalence points and end points? How do they differ? equivalence point- the point @ which stoichiometric quantities are brought together, end point- the the equivalence point is theoretical, when end poi 6. Why should the standardized NaOH solution be kept in a stoppered bottle? pr 7. What is parallax? Why should you avoid it? Parallax is the upperent displacement or the di da in direction of an object as seen from two diffe points. са It should be colded because it ca errors in volume measurements. Copyright © 2018 Pearson Education, Inc.
Below is a graph of measured atmospheric CO2 levels since 1980 (from globalchange.gov). Based on these data, how has the solubility of CO2 in ocean water changed over this time period? Group of answer choices A:It is not possible to predict CO2 solubility changes based on these data. B:CO2 solubility has decreased. C:CO2 solubility has not changed. D:CO2 solubility has increased. According to this solubility graph, which solid's dissolving process is exothermic? Group of answer choices A:sugar (C12H22O11) B:KNO3 C:Ce2(SO4)3 D:KCl What effects will dissolving sugar in water have on the resulting solution? Group of answer choices A:Compared to pure water, the solution's freezing point will be lower and its boiling point will be higher B:Compared to pure water, the solution's freezing point will be higher and its boiling point will be lower C:Compared to pure water, the solution's freezing point will be lower and its boiling point will…
What is the molarity of a solution that results from dissolving 424.78 g of a compound with FW 20.76 into a total volume of 2.12 L? (Give your answer in units of M, with two places after the decimal point.)
A mixture of ethanol, benzaldehyde and KMnO4 is mixed together. Would you expect a precipitate to form based on the reactants functional groups?
1. A class organic compounds containing a six-membered ring with alternating double bonds that results in delocalization of the electrons within the ring. This class of compounds can have additional groups attached to the ring. 2. A family of organic compounds that can be represented by the general formula R-CHO. 3. A compound with the general formula R-COOH. It is a weak electrolyte that can lose an H+ ion in water solutions. 4. A hydrocarbon with a general formula of CnH(2n+2). All carbon-to-carbon bonds would be single bonds.
Place 8.5 g of sodium nitrate and 7.5 g of potassium chloride in a 100 ml beaker and add 25 ml of water. Warming and stirring to dissolve completely. Assuming a volume of 25 ml for the solution, calculate the polarity of the solution with respect to NaNO3, KCl, NaCl, KNO3.
Experiment 10-Polarity and Solubility name section date Pre-Laboratory Assignment 1. Define the terms below a. Immiscible- b. Hydrocarbon - c. Functional group - z. What is the general rule of solubility? Explain briefly what it means! 3. For a molecule of phosphorus trichloride, PCl3: a. Draw the Lewis structure of this molecule. Using the Pauling electronegativity scale, determine which bonds are polar; show them on the structure using the 8+/o- notation. b. Is this molecule polar? Explain briefly why or why not. What type of intermolecular forces should exist between two PCl3 molecules? c. d. Will PCl3 be soluble in water, H20? Explain briefly why or why not. 4. On the Worksheet, add any missing lone pairs. To avoid getting points off, have the TA or instructor check this step for completion before you turn in the pre-lab. 129
Which of the following statements regarding solubility of gases in liquids is NOT correct? A. When the Henry’s law constants are given in units of mol/L·atm, larger kH values mean higher solubility. B. The solubility of a gas depends on the identity of the solvent. C. The solubility of gases in water typically decreases as temperature increases. D. The solubility of gases in water typically increases as the mole fraction of the gas above the water’s surface increases. E. The solubility of gases in water typically decreases as the partial pressure of the gas above the water’s surface increases
150 140 130 120 110 100 90 80 70 60 50 -ха 40 FACI 30 20 KCIO 10 -Ce₂(SOs)s 0 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C) • Rectangular Snip According the solubility curve graph above, the lowest temperature in which 50 g NH4Cl can be dissolved in 100 g water is- a 10°C b 50°C с 30°C Time left for this assessment: O d 60°C 67:47 Grams of solute per 100 g H₂O B NH NaNO3 KNO₂ KHÁC
Does the commonly reported solubility of an inorganic compound in water pertain to large crystals or small crystals? Why?
Materials Needed solid I2 solid CUSO4-5H20 food dye solid (NH4)2SO4 heavy metals waste container halogenated waste container non-halogenated waste container semi-micro test tubes and rack regular test tubes and rack squash pipettes acetone cyclohexane propan-2-ol Method Part A: Solubility of ionic and molecular solids 1. Place a small amount (about the size of 1 grain of rice, see picture) of copper sulfate into each of three DRY semi-micro test tubes. Add 20 drops of water to the first test tube and gently flick the test tube with your finger to ensure mixing. 2. Repeat step 1 using acetone in place of water as the solvent in the second test tube. 3. Repeat step 2 replacing acetone with cyclohexane in the third test tube. Hold the test tubes against a white background to compare the solubility of copper sulfate in the three solvents and record your results. Discard these mixtures into the heavy metals waste container in the fume cupboard. Once these test tubes have been emptied you…
Consider the following information: Ksp(BasO4) = 1.1 x 10-10 Ksp(CasO4) = 4.9 x 10-5 Ksp(PbSO4) = 2.5 x 10-8 Ksp(Cd(OH)2) = 2.5 x 10-14 Ksp(Cr(OH)3) = 1.6 x 10-44 These compounds arranged in order of increasing aqueous solubility is a. PBSO4 < Cd(OH)2 < BaSO4 < Cr(OH)3 Ob. Cr(OH)3 < Cd(OH)2 < BasO4