Chemistry 12th Edition solutions

Chemistry 12
If 2.50 g of CuSO4 are dissolved in 9.0 3 102 mL of 0.30 M NH3, what are the concentrations of Cu21, Cu(NH3)4 21, and NH3 at equilibrium?

Chemistry 12
What is the number of significant figures in each of the following measurements? (a) 4867 mi (b) 56 mL (c) 60,104 tons (d) 2900 g (e) 40.2 g/cm3 (f) 0.0000003 cm (g) 0.7 min (h) 4.6 3 1019 atoms

Chemistry 12
Predict the geometries of the following ions: (a) NH4 1, (b) NH2 2, (c) CO3 22, (d) ICl2 2, (e) ICl4 2, (f) AlH4 2, (g) SnCl5 2, (h) H3O1, (i) BeF4 22.

Chemistry 12
Calculate the percent ionization of hydrofluoric acid at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends.

Chemistry 12
Calculate the molar mass of a particular polyethylene sample, ( CH2CH2)n, where n 5 4600.

Chemistry 12
Name these compounds: (a) Na2CrO4, (b) K2HPO4, (c) HBr (gas), (d) HBr (in water), (e) Li2CO3, (f) K2Cr2O7, (g) NH4NO2, (h) PF3, (i) PF5, (j) P4O6, (k) CdI2, (l) SrSO4, (m) Al(OH)3, (n) Na2CO3 ? 10H2O.

Chemistry 12
The following compounds, listed with their boiling points, are liquid at 210C: butane, 20.5C; ethanol, 78.3C; toluene, 110.6C. At 210C, which of these liquids would you expect to have the highest vapor pressure? Which the lowest? Explain.

Chemistry 12
Sketch the bond moments and resultant dipole moments for the following molecules: H2O, PCl3, XeF4, PCl5, SF6.

Chemistry 12
Use BaSO4 to distinguish between solubility, molar solubility, and solubility product

Chemistry 12
(1) Which of the following diagrams represents a solution of a weak diprotic acid? (2) Which diagrams represent chemically implausible situations? (The hydrated proton is shown as a hydronium ion. Water molecules are omitted for clarity.) (a) (b) (c) (d)

Chemistry 12
Which of the following species are capable of hydrogen-bonding among themselves? (a) C2H6, (b) HI, (c) KF, (d) BeH2, (e) CH3COOH

Chemistry 12
Classify the following redox reactions: (a) 2H2O2 2H2O 1 O2 (b) Mg 1 2AgNO3 Mg(NO3)2 1 2Ag (c) NH4NO2 N2 1 2H2O (d) H2 1 Br2 2HBr

Chemistry 12
Write the numbers represented by the following prefixes: (a) mega-, (b) kilo-, (c) deci-, (d) centi-, (e) milli-, (f) micro-, (g) nano-, (h) pico-.

Chemistry 12
Sucrose (C12H22O11), commonly called table sugar, undergoes hydrolysis (reaction with water) to produce fructose (C6H12O6) and glucose (C6H12O6): C12H22O11 1 H2O C6H12O6 1 C6H12O6 fructose glucose This reaction is of considerable importance in the candy industry. First, fructose is sweeter than sucr

Chemistry 12
What is the mass of one mole of ants? (Useful information: A mole is the unit used for atomic and subatomic particles. It is approximately 6 3 1023. A 1-cm-long ant weighs about 3 mg.)

Chemistry 12
How many grams of urea [(NH2)2CO] must be added to 450 g of water to give a solution with a vapor pressure 2.50 mmHg less than that of pure water at 30C? (The vapor pressure of water at 30C is 31.8 mmHg.)

Chemistry 12
Name five metals and five nonmetals that are very likely to form ionic compounds. Write formulas for compounds that might result from the combination of these metals and nonmetals. Name these compounds.

Chemistry 12
The diagrams here show three weak acids HA (A 5 X, Y, or Z) in solution. (a) Arrange the acids in order of increasing Ka. (b) Arrange the conjugate bases in increasing order of Kb. (c) Calculate the percent ionization of each acid. (d) Which of the 0.1 M sodium salt solutions (NaX, NaY, or NaZ)

Chemistry 12
An aqueous solution contains the amino acid glycine (NH2CH2COOH). Assuming that the acid does not ionize in water, calculate the molality of the solution if it freezes at 21.1C

Chemistry 12
What is the osmotic pressure (in atm) of a 1.36 M aqueous solution of urea [(NH2)2CO] at 22.0C?