Discus Water as an Acid Assignment 12.3.1 Calculate [OH−] in a solution in which [H3O ] = 0.0012 M at 25°C. a) 1.2 × 10−3 M d) 8.3 × 10−12 M b) 8.3 × 10−17 M e) 1.2 × 1011 M c) 1.0 × 10−14 M 12.3.2 Calculate [H3O ] in a solution in which [OH−] = 0.25 M at 25°C. a) 4.0 × 10−14 […]

Order Weak Acids and Bases Assignment 12.6.1 Place the solutions in order of decreasing pH: 0.067 M HCl, 0.067 M CH3NH2, 0.067 M HF. a) HCl > HF > CH3NH2 c) CH3NH2 > HCl > HF e) CH3NH2 > HF > HCl b) HCl > CH3NH2 > HF d) HF > CH3NH2 > HCl 12.6.2 Place the solutions in order of increasing pH: 0.155 M […]

Order Acid-Base Titrations Assignment 12.7.1 If 15.0 mL of an HNO3 solution requires 22.6 mL of 0.117 M LiOH to neutralize, what is the concentration of the HNO3 solution? a) 0.264 M d) 0.176 M b) 0.0777 M e) 0.568 M c) 0.117 M 12.7.2 If 37.5 mL of an HC2H3O2 solution requires 48.6 mL of 0.0578 M KOH to neutralize, what is the concentration […]

Order Identifying Acids and Bases Assignment Which of the following compounds are strong acids? (Select all that apply.) a) NaOH c) H2SO4 e) HF b) CH3COOH d) Ba(OH)2 12.2 Which of the following compounds are strong bases? (Select all that apply.) a) NH3 c) HNO2 e) LiOH b) KOH d) HNO3 12.3 Which of the following compounds are weak acids? (Select all that apply.) a) […]

Order Factors That Affect Equilibrium Assignment 13.4.1 Which of the following equilibria will shift to the right when H2 is added? (Select all that apply.) a) 2H2 O2 ⟶⟵ 2H2O b) 2HI ⟶⟵ H2 I2 c) H2 CO2 ⟶⟵ H2O CO d) 2NaHCO3 ⟶⟵ Na2CO3 H2O CO2 e) 2CO2 O2 ⟶⟵ 2CO2 13.4.2 Which of the following equilibria will shift to the left when the […]

Order Organic Chemistry Assignment 14.5 Identify the compounds that are hydrocarbons. (a) Ca(C2H3O2)2 (c) CH3CH2CH3 (b) CH4O (d) CH3COOH 14.6 Identify the compounds that are hydrocarbons. (a) LiHCO3 (c) NH4CN (b) CH3CH2OH (d) CH3CHCH2 14.7 Identify each hydrocarbon as an alkane, alkene, or alkyne. (a) CH3CHCH2 (c) CH3CCH (b) CH3CH2CH2CH3 (d) CH2CHCH2CH2CH3 14.8 Identify each hydrocarbon as an alkane, alkene, or alkyne. (a) C4H8 (b) […]

Order Radioactive Decay Assignment 16.1 How do nuclear reactions differ from ordinary chemical reactions? 16.2 What are the steps in balancing nuclear equations? 16.3 What is the difference between −1 0 e and −1 0 β? 16.4 What is the difference between an electron and a positron? 16.5 Complete the following nuclear equations, and identify X in each case: (a) 26 12Mg 1 1p⟶ 4 […]

Order Dating Using Radioactive Decay 16.24 Define the term half-life. 16.25 What percentage of a radioactive isotope remains after 20.0 days if its half-life is 10.0 days? 16.26 The radioactive decay of Tl-206 to Pb-206 has a half-life of 4.20 min. Starting with 5.00 × 1022 atoms of T1-206, calculate the number of such atoms left after 42.0 min. 16.27 A radioactive isotope of copper […]

Order Balancing Oxidation-Reduction Reactions Assignment 17.1 Arrange the following species in order of increasing oxidation number of the sulfur atom: (a) H2S, (b) S8, (c) H2SO4, (d) S2−, (e) HS−, (f) SO2, (g) SO3. 17.2 Phosphorus forms many oxoacids. Indicate the oxidation number of phosphorus in each of the following acids: (a) HPO3, (b) H3PO2, (c) H3PO3, (d) H3PO4, (e) H4P2O7, (f) H5P3O10. 17.3 Give […]

Order Basic Optical Principles Assignment 1.1 Orbitals have regions in which they have negative and positive signs. Explain the physical background of the signs and how this relates to the probability of finding electrons at a certain place. 1.2 Spectroscopists often describe energies that are necessary to excite certain electronic states by the wave number of the corresponding photons in units of cm1 . Why […]