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- Based on their molecular structure, choose the stronger acid from each pair of binary acids, and explain your choice: a. HF and HCl b. H2O and HF c. H2Se and H2S.
Problem 117
Problem 118
Based on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your choice. H2Te, HI, H2S, NaH
- Based on their molecular structure, pick the stronger acid from each pair of oxyacids. Explain your choice for the following pairs: a. H2SO4 or H2SO3 b. HClO2 or HClO c. HClO or HBrO d. CCl3COOH or CH3COOH.
Problem 119
Problem 120
Based on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice. HClO3, HIO3, HBrO3
Problem 121
Which is a stronger base, S2– or Se2–? Explain.
- Which is a stronger base, PO4^3- or AsO4^3-? Explain.
Problem 122
Problem 123
Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F-
Problem 124a
Classify each species as either a Lewis acid or a Lewis base. a. BeCl2
Problem 124b
Classify each species as either a Lewis acid or a Lewis base. b. OH–
Problem 124c
Classify each species as either a Lewis acid or a Lewis base. c. B(OH)3
Problem 124d
Classify each species as either a Lewis acid or a Lewis base. d. CN–
Problem 125
Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Fe3+(aq) + 6 H2O(l) ⇌ Fe(H2O)63+(aq) b. Zn2+(aq) + 4 NH3(aq) ⇌ Zn(NH3)42+(aq) c. (CH3)3N(g) + BF3(g) ⇌ (CH3)3NBF3(s)
Problem 126a
Identify the Lewis acid and Lewis base from among the reactants in each equation. a. Ag+(aq) + 2 NH3(aq) ⇌ Ag(NH3)2+(aq)
Problem 126b,c
Identify the Lewis acid and Lewis base from among the reactants in each equation. b. AlBr3 + NH3 ⇌ H3NAlBr3 c. F–(aq) + BF3(aq) ⇌ BF4–(aq)
Problem 127c
Based on these molecular views, determine whether each pictured acid is weak or strong.
Problem 128
Based on these molecular views, determine whether each pictured acid is weak or strong.
Problem 129
The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction: HbH+(aq) + O2(aq) ⇌ HbO2(aq) + H+(aq) In this equation, Hb is hemoglobin. The pH of normal human blood is highly controlled within a range of 7.35 to 7.45. Given the above equilibrium, why is this important? What would happen to the oxygen-carrying capacity of hemoglobin if blood became too acidic (a dangerous condition known as acidosis)?
Problem 130
Carbon dioxide dissolves in water according to the equations:
CO2(g) + H2O(l) ⇌ H2CO3(aq)
H2CO3(aq) + H2O(l) ⇌ HCO3–(aq) + H3O+(aq)
Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earth's oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO2 be having on the pH of the world's oceans? What effect might this change be having on the limestone structures (primarily CaCO3) of coral reefs and marine shells?
Problem 131
People often take milk of magnesia to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon, which contains 4.00×102 mg of Mg(OH)2. What volume of an HCl solution with a pH of 1.3 can be neutralized by one dose of milk of magnesia? If the stomach contains 2.00×102 mL of pH 1.3 solution, is all the acid neutralized? If not, what fraction is neutralized?
Problem 132
Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?
- Acid rain over the Great Lakes has a pH of about 4.5. Calculate the [H3O+] concentration of this rain and compare that value to the [H3O+] concentration of rain over the West Coast, which has a pH of 5.4. How many times more concentrated is the acid in the rain over the Great Lakes compared to the rain over the West Coast?
Problem 133
- White wines tend to be more acidic than red wines. Find the [H3O+] concentration in a Sauvignon Blanc with a pH of 3.23 and a Cabernet Sauvignon with a pH of 3.64. How many times more acidic is the Sauvignon Blanc than the Cabernet Sauvignon?
Problem 134
- Common aspirin is acetylsalicylic acid, which has the structure shown here and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin (6.5 * 10^2 mg) is dissolved in 8.0 ounces of water.
Problem 135
Problem 136
The AIDS drug zalcitabine (also known as ddC) is a weak base with a pKb of 9.8. What percentage of the base is protonated in an aqueous zalcitabine solution containing 565 mg/L?
Problem 137
Determine the pH of each solution. a. 0.0100 M HClO4 b. 0.115 M HClO2 c. 0.045 M Sr(OH)2 d. 0.0852 M KCN e. 0.155 M NH4Cl
Problem 138
Determine the pH of each solution. a. 0.0650 M HNO3 b. 0.150 M HNO2 c. 0.0195 M KOH d. 0.245 M CH3NH3I e. 0.318 M KC6H5O
Problem 139
Determine the pH of each two-component solution. a. 0.0550 M in HI and 0.00850 M in HF b. 0.112 M in NaCl and 0.0953 M in KF c. 0.132 M in NH4Cl and 0.150 M HNO3 d. 0.0887 M in sodium benzoate and 0.225 M in potassium bromide e. 0.0450 M in HCl and 0.0225 M in HNO3
Problem 140a,b,c,e
Determine the pH of each two-component solution. a. 0.050 M KOH and 0.015 M Ba(OH)2 b. 0.265 M NH4NO3 and 0.102 M HCN c. 0.075 M RbOH and 0.100 M NaHCO3 e. 0.115 M NaClO and 0.0500 M KI
Problem 140d
Determine the pH of each two-component solution. d. 0.088 M HClO4 and 0.022 M KOH
Problem 141
Write net ionic equations for the reactions that take place when aqueous solutions of the following substances are mixed: a. sodium cyanide and nitric acid b. ammonium chloride and sodium hydroxide c. sodium cyanide and ammonium bromide d. potassium hydrogen sulfate and lithium acetate e. sodium hypochlorite and ammonia