Chemistry for Today: General, Organic, and Biochemistry
9th Edition
ISBN: 9781305960060
Author: Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher: Cengage Learning
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Question
Chapter 7, Problem 7.104E
Interpretation Introduction
Interpretation:
The reason corresponding to the fact that oil and water are immiscible (do not mix) is to be stated.
Concept introduction:
The property of a solid, liquid or gas to dissolve in another substance is referred to as the solubility. The rule “Like dissolves like” means that polar solutes are soluble in polar solvents and nonpolar solutes are soluble in nonpolar solvents.
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Students have asked these similar questions
1. Such as in the interior of giant planets, it is argued that water exists as ionic water in which the molecules break down into hydrogen and oxygen ions. What conditions are required for water to exist in its ionic form?a. High temperature, low pressureb. Low temperature, low pressurec. High temperature, high pressured. Low temperature, high pressure
2. Water is a polar molecule with an electrical dipole moment. The polarity of water is due toa. Higher electronegativity of oxygen atomsb. Hydrogen atoms are slightly positivec. Oxygen carries a slight negative charged. All of the above
3. A good clean potable water will give dissolved oxygen value close to the theoretical value for the saturated solution of oxygen in water.a. Trueb. Falsec. Sometimesd. Insufficient data
POLAR molecules does not easily evaporate due to
strong intermolecular force acting on it. *
Determine if the CAPITALIZED WORD(S) make the
statement correct. Choose TRUE if it does, choose
FALSE if otherwise.
A. TRUE
B. FALSE
Read and explain the foowing based on your own understanding.
1. How will you know if a certain molecule is a polar or non-polar?
2. Explain the four types of intermolecular forces
Chapter 7 Solutions
Chemistry for Today: General, Organic, and Biochemistry
Ch. 7 - Many solutions are found in the home. Some are...Ch. 7 - Prob. 7.2ECh. 7 - Classify the following as being a solution or not...Ch. 7 - Classify the following as being a solution or not...Ch. 7 - Use the term soluble, insoluble, or immiscible to...Ch. 7 - Use the term soluble, insoluble, or immiscible to...Ch. 7 - Define the term miscible. It is not defined in the...Ch. 7 - Classify the following solutions as unsaturated,...Ch. 7 - Prob. 7.9ECh. 7 - Prob. 7.10E
Ch. 7 - Prob. 7.11ECh. 7 - Classify each of the following solutes into the...Ch. 7 - Prob. 7.13ECh. 7 - Prob. 7.14ECh. 7 - Prob. 7.15ECh. 7 - Prob. 7.16ECh. 7 - Prob. 7.17ECh. 7 - Prob. 7.18ECh. 7 - Prob. 7.19ECh. 7 - Prob. 7.20ECh. 7 - Prob. 7.21ECh. 7 - Prob. 7.22ECh. 7 - Calculate the molarity of the following solutions:...Ch. 7 - Prob. 7.24ECh. 7 - Prob. 7.25ECh. 7 - Calculate: a. How many grams of solid would be...Ch. 7 - Prob. 7.27ECh. 7 - Prob. 7.28ECh. 7 - Calculate the concentration in (w/w) of the...Ch. 7 - Calculate the concentration in (w/w) of the...Ch. 7 - Prob. 7.31ECh. 7 - Calculate the concentration in (w/w) of the...Ch. 7 - Prob. 7.33ECh. 7 - Calculate the concentration in (v/v) of the...Ch. 7 - Calculate the concentration in (v/v) of the...Ch. 7 - Consider the blood volume of an adult to be 5.0L....Ch. 7 - Prob. 7.37ECh. 7 - Calculate the concentration in (w/v) of the...Ch. 7 - Calculate the concentration in (w/v) of the...Ch. 7 - Prob. 7.40ECh. 7 - Prob. 7.41ECh. 7 - Prob. 7.42ECh. 7 - Explain how you would prepare the following...Ch. 7 - Prob. 7.44ECh. 7 - Prob. 7.45ECh. 7 - Calculate the following: a. The number of grams of...Ch. 7 - Prob. 7.47ECh. 7 - Explain how you would prepare the following dilute...Ch. 7 - Prob. 7.49ECh. 7 - Prob. 7.50ECh. 7 - Prob. 7.51ECh. 7 - How many grams of solid Na2CO3 will react with...Ch. 7 - Prob. 7.53ECh. 7 - Prob. 7.54ECh. 7 - Prob. 7.55ECh. 7 - Prob. 7.56ECh. 7 - How many milliliters of 0.124MNaOH solution will...Ch. 7 - How many milliliters of 0.124MNaOH solution will...Ch. 7 - How many milliliters of 0.115MNaOH solution will...Ch. 7 - Stomach acid is essentially 0.10MHCl. An active...Ch. 7 - Prob. 7.61ECh. 7 - Prob. 7.62ECh. 7 - Prob. 7.63ECh. 7 - Calculate the boiling and freezing points of water...Ch. 7 - Calculate the boiling and freezing points of water...Ch. 7 - Prob. 7.66ECh. 7 - Prob. 7.67ECh. 7 - Prob. 7.68ECh. 7 - Calculate the osmolarity for the following...Ch. 7 - Prob. 7.70ECh. 7 - Calculate the osmotic pressure of a 0.125M...Ch. 7 - Prob. 7.72ECh. 7 - Prob. 7.73ECh. 7 - Calculate the osmotic pressure of a solution that...Ch. 7 - Prob. 7.75ECh. 7 - Prob. 7.77ECh. 7 - Prob. 7.78ECh. 7 - Prob. 7.79ECh. 7 - Suppose an osmotic membrane separates a 5.00 sugar...Ch. 7 - Prob. 7.81ECh. 7 - Prob. 7.82ECh. 7 - Suppose you have a bag made of a membrane like...Ch. 7 - Prob. 7.84ECh. 7 - Prob. 7.85ECh. 7 - Prob. 7.86ECh. 7 - Prob. 7.87ECh. 7 - Prob. 7.88ECh. 7 - Prob. 7.89ECh. 7 - When a patient has blood cleansed by hemodialysis,...Ch. 7 - Prob. 7.91ECh. 7 - Prob. 7.92ECh. 7 - Prob. 7.93ECh. 7 - Prob. 7.94ECh. 7 - Prob. 7.95ECh. 7 - Strips of fresh meat can be preserved by drying....Ch. 7 - If a salt is added to water, which of the...Ch. 7 - Prob. 7.98ECh. 7 - Prob. 7.99ECh. 7 - Prob. 7.100ECh. 7 - Which one of the following compounds is a...Ch. 7 - Prob. 7.102ECh. 7 - Prob. 7.103ECh. 7 - Prob. 7.104ECh. 7 - Prob. 7.105ECh. 7 - Prob. 7.106ECh. 7 - Prob. 7.107ECh. 7 - Prob. 7.108ECh. 7 - Prob. 7.109ECh. 7 - Prob. 7.110ECh. 7 - In a dilute solution of sodium chloride in water,...Ch. 7 - A salt solution has a molarity of 1.5M. How many...Ch. 7 - Prob. 7.113ECh. 7 - Prob. 7.114ECh. 7 - Prob. 7.115ECh. 7 - Prob. 7.116ECh. 7 - Prob. 7.117ECh. 7 - Prob. 7.118ECh. 7 - Prob. 7.119ECh. 7 - Prob. 7.120ECh. 7 - Prob. 7.121ECh. 7 - Prob. 7.122E
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Similar questions
- Why do polar molecules have a greater tendency to remain a liquid or a solid at room temperature?arrow_forwardIn order to have a large partial positive charge to be involved in a hydrogen bond, the molecule must be polar and have a In order to have a large partial negative charge to be involved in a hydrogen bond, the molecule must be polar and have an a. F-H, O-H, or N-H bond b. F, O, or Narrow_forwardWhich reasoning best supports the fact that H2, has a higher melting point than he? A. The phase changes of melting breaks the covalent bond in H2, and HE done any have a covalent bond b. H2 has a greater surface area than he we used more polarizadle c. He has more electrons than H2 and forms stronger attractionsarrow_forward
- 1) is this molecule polar or non-polar? 2) what is the strongest intermolecular force you would expect to see in this molecule?arrow_forwardHydrogen bonding in water is best explained by the : a. shape of water b. polar nature of water c. composition of water d. molecular weight of waterarrow_forward1) is this molecule polar or non-polar? 2) what is the strongest intermolecular force you would expect to see in this molecule?arrow_forward
- See the attraction between atoms between weak and strong. A. How would you describe the spacing between the atoms? Are the atoms free to move around? Explain. B. What is the likely phase (solid, liquid, or gas) of the substance that is comprised of the atoms you have just describe? Explain.arrow_forward2 questionsarrow_forwardTrue or false 1. Hydrogen bonds are present in the gaseous state of water molecules only 2. The attraction between gas molecules counteracts the tendency of kinetic energy that will move the molecules further apart 3. Gaseous chlorine, liquid bromine and solid iodine are all nonpolar. 4. Highly electronegative ions tend to attract negative charges to themselves when bonded to other atoms 5. At specified temperatures, only gas molecules have great London forces of attraction.arrow_forward
- London forces are forces of attraction between what molecules. a. polar b. nonpolar c. slightly polararrow_forwardBased on the formula and geometries of the substances(water, ethyl alcohol, vinegar and acetone), are the molecules that can hold more drops on the coin polar or non polar? What about those that took longer to evaporate? Explain.arrow_forward22. The dipole-dipole interactions experienced when H is bonded to N, O, or F are unusually strong. We call these interactions Covalent bonds Polar bonds d. Weak bond a. C. b. Hydrogen bonds. 23. What is the correct chemical formula of water? a. НО b. HO с. Н20 d. 2HO 24. How many molecules of water make up a one raindrop? a. Tens C. Thousands b. Hundreds d. Millionsarrow_forward
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