Solubility
Solutions
Concentrations
Polarity
Misc.
100
Define: (1) Solubility (2) Saturation (3) Unsaturated (4) Supersaturated
Solubility - the amount of a substance that will dissolve in a solvent Saturation - holding as much solute as is allowed at a stated temperature Unsaturated - there are fewer particles of solute than there are of solvent. More solute can be dissolved into the solvent Supersaturated - solution that contains more of the dissolved material than could be dissolved by the solvent under normal circumstances
100
What is a mixture a)a combination of elements to make a new substance b)a chemically combined substance c)a combination of substances where new substances are formed through a reaction d)a combination of substances in which the atoms of the substance do not chemically combine
d)a combination of substances in which the atoms of the substance do not chemically combine
100
Write the formulas for Molarity, Molality, Mass Percent, Mole fraction and parts per million and billion
Molarity = mol solute/ volume of solution Molality = mol solute/ kg of solvent Mass Percent = (mass of A in solution / mass of solution) x 100 Parts per million (10^6) Parts per billion (10^9) Mole Fraction (Xa) = moles of A / total moles in solution
100
Which of the following pairs of elements will likely form a polar covalent bond? And which will likely form a nonpolar covalent bond? a)H + Cl b)Na + Na c)Na + Cl d)H + H
(1) polar covalent: H + Cl (2) nonpolar covalent: H + H
100
How is surface tension related to the strength of intermolecular forces?
Surface tension decreases as intermolecular forces decrease and vice versa
200
Which of the following substances would be least soluble in water? a) C5H12 b) HNO3 c) MgCl2 d) H2CO3
a) C5H12
200
This type of mixture contains two or more substances that are visibly distinguishable.
Heterogeneous mixture
200
A solution is prepared by dissolving 15.0 g of NH3 in 250 g of water. The density of the resulting solution is 0.974 g/mL. The mole fraction of NH3 and the mass percent in the solution are __________. A) 0.940; 0.0597% B) 0.640; 5.66% C) 16.8; 0.922% D) 0.0597; 5.66% E) 0.922; 0.922%
D) 0.0597; 5.66%
200
If the H-F bond in the following molecule is polar, which of the following statements is true? a)The molecule is a dipole b)The molecule is not a dipole c)The molecule is nonpolar d)The molecule has no dipole moment
a)The molecule is a dipole
200
What is capillary action? And how does capillary action depend on the relative strengths of adhesive and cohesive forces?
(1) The ability of a liquid to flow against gravity up a narrow tube. (2) Cohesive forces cause the liquid to stay together, adhesive forces cause the liquid to spread out over the surface of the tube. If the adhesive forces are greater than the cohesive forces, the liquid goes up the tube.
300
What happens to the solubility of a gas in a liquid if the partial pressure of the gas above the liquid decreases
Solubility decreases
300
True or False: A heterogeneous mixture is also considered a solution
False. A homogeneous mixture is a solution because it is the same throughout
300
Calculate the molarity of each of the following solutions: a. 12.4 g KCl in 289.2 mL solution b. 16.4 g CaCl2 in 0.614 L solution
a)0.576 M KCl b) 0.241 M CaCl2
300
Which of the following has the greatest dipole moment? a) HCN b) SO2 c) H2O d) PCl4
a) HCN HCN has the largest difference in electronegativity, and the atoms in a linear configuration. There is a strong dipole moment in the direction of the nitrogen, without anything cancelling it out. Water has a dipole moment from each H, and the molecule is bent so the dipoles partially cancel each other out. SO2 also has a bet configuration, so its dipoles partially cancel each other out as well. PCl4 is tetrahedral and all the dipoles cancel out, leaving no net.
300
Which of the following compounds will likely have the highest melting point? a)NaCl (ionic) b)CH4 (nonpolar) c)CH3OH (slightly polar) d)HCl (polar)
a) NaCl
400
The solubility of nitrogen gas in water at 25C and a nitrogen pressure of 1 atm is 2.6x10^-3M. The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm
Sgas = 2.1x10^-3 Extra Practice: http://alpha.chem.umb.edu/chemistry/ch115/Mridula/CHEM%20116/documents/Chapter13.PracticeQuestions.tst-TestGen.pdf
400
Name the different components of a solution with their definition. Give an example of a solution and name the different components.
Solute - dissolved substance, dispersed uniformly throughout the solvent Solvent - dissolves substances. Example: Kool-Aid Solute - powder Solvent - water Example: Vinegar Solute - acetic acid Solvent - water
400
Calculate the molalities of the following aqueous solutions: a. 0.840 M sugar (C12H22O11) solution (density= 1.12 g/mL) b. 4.91 M NaOH solution (density = 1.04 g/mL) c. 0.79 M NaHCO3 solution (density = 1.19 g/mL)
a. 1.01 molal C12H22O11 b. 5.82 molal NaOH c. 0.703 molal NaHCO3
400
A type of bond that results from the equal sharing of electrons is A) ionic bond B) a nonpolar covalent bond C) polar covalent bond D) None of the other choices
B) a nonpolar covalent bond
400
Which of the following compounds will have the most ionic bond character? a)LiF b) NO3- c) CO d)BaO e) (PO4)3-
a) LiF from a large difference in electronegativity and usually arises from metals and non-metals
500
Which of the following combinations would increase the solubility of a gas in a liquid? A. Decrease the pressure and decrease the temperature B. Decrease the pressure and increase the temperature C. Increase the pressure and decrease the temperature D. Increase the pressure and increase the temperature
C. Increase the pressure and decrease the temperature
500
The solute that is found in the greatest amount in ocean water is______. A. H20 B. KCl C. NaCl D. CuSO4
C. NaCl
500
Calculate the mole fraction, molarity and molality of NH3 if it is in a solution composed of 30.6 g NH3 in 81.3 g of H2O. The density of the solution is 0.982 g/mL and the density of water is 1.00 g/mL
Molarity: 15.8 M NH3, molality: 22.1 molal NH3, mole fraction(NH3): 0.285
500
Which of the following attractive forces occurs in a nonpolar molecule? A) Dispersion forces B) Dipole-dipole forces C) Hydrogen Bonding
A) Dispersion forces
500
Which of the following bonds is most likely going to form an ionic bond? • N-N • P-S • K-Cl • F-I
• K-Cl
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