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Problem 106
Determine the pH of each solution. a. 0.20 M KCHO2 b. 0.20 M CH3NH3I c. 0.20 M KI
Problem 107
Calculate the concentration of all species in a 0.15 M KF solution.
Problem 108
Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
Problem 109
Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.
Problem 110
Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.
Problem 111a
Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.350 M H3PO4
Problem 111b
Calculate the [H3O+] and pH of each polyprotic acid solution. b. 0.350 M H2C2O4
Problem 112a
Calculate the [H3O+] and pH of each polyprotic acid solution.
a. 0.125 M H2CO3
Problem 112b
Calculate the [H3O+] and pH of each polyprotic acid solution.
b. 0.125 M H3C6H5O7
- Is this question correctly formulated? If so, could you provide it as is; if not, modify it as needed and return it in JSON format: Calculate the concentration of all species in a 0.500 M solution of H2SO3.
Problem 113
Problem 114
Calculate the concentration of all species in a 0.155 M solution of H2CO3.
Problem 115
Calculate the [H3O+] and pH of each H2SO4 solution. At approximately what concentration does the x is small approximation break down?
a. 0.50 M b. 0.10 M c. 0.050 M
Problem 116a
Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here.
a. Ka1 = 1.0 × 10–4; Ka2 = 5.0 × 10–5
Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected?
- 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)?