Textbook Question
By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution: (d) Pb(NO3)2.
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Ch.13 - Properties of Solutions
Chapter 13, Problem 27
Consider water and glycerol, CH2(OH)CH(OH)CH2OH. (b) List the intermolecular attractions that occur between a water molecule and a glycerol molecule.
Verified step by step guidance1
Identify the types of intermolecular forces present in water. Water molecules exhibit hydrogen bonding due to the presence of highly electronegative oxygen atoms bonded to hydrogen atoms.
Identify the types of intermolecular forces present in glycerol. Glycerol, with its three hydroxyl (OH) groups, also exhibits hydrogen bonding due to the presence of oxygen atoms bonded to hydrogen atoms.
Consider the interaction between a water molecule and a glycerol molecule. Both molecules can form hydrogen bonds with each other due to the presence of hydroxyl groups.
Recognize that in addition to hydrogen bonding, there are also dipole-dipole interactions between the polar regions of the water and glycerol molecules.
Acknowledge that while hydrogen bonding is the dominant force, London dispersion forces (induced dipole-induced dipole interactions) are also present, although they are weaker compared to hydrogen bonds.
Related Practice
Textbook Question
By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (b) Pb(NO3)2,
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Textbook Question
By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (c) Ce2(SO4)3.
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Textbook Question
Oil and water are immiscible. Which is the most likely reason? (a) Oil molecules are denser than water. (b) Oil molecules are composed mostly of carbon and hydrogen. (c) Oil molecules have higher molar masses than water. (d) Oil molecules have higher vapor pressures than water. (e) Oil molecules have higher boiling points than water.
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Open Question
Common laboratory solvents include acetone (CH3COCH3), methanol (CH3OH), toluene (C6H5CH3), and water. Which of these is the best solvent for nonpolar solutes?
Textbook Question
Which of the following in each pair is likely to be more soluble in hexane, C6H14: b. benzene (C6H6) or glycerol, CH2(OH)CH(OH)CH2OH,
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