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Problem 109a
Determine the pH of each solution. a. 0.10 M NH4Cl
Problem 111
Calculate the concentration of all species in a 0.15 M KF solution.
Problem 112
Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
Problem 113
Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.
Problem 114
Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.
Problem 115a
Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.350 M H3PO4
Problem 115b
Calculate the [H3O+] and pH of each polyprotic acid solution. b. 0.350 M H2C2O4
Problem 116a
Calculate the [H3O+] and pH of each polyprotic acid solution.
a. 0.125 M H2CO3
Problem 116b
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 117
Problem 118
Calculate the concentration of all species in a 0.155 M solution of H2CO3.
Problem 119
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 120a
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 121
Problem 122
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 123
Problem 124
Based on molecular structure, arrange the oxyacids in order of increasing acid strength. Explain your choice. HClO3, HIO3, HBrO3
Problem 125
Which is a stronger base, S2– or Se2–? Explain.
- Which is a stronger base, PO4^3- or AsO4^3-? Explain.
Problem 126
Problem 127
Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F-
Problem 128a
Classify each species as either a Lewis acid or a Lewis base. a. BeCl2
Problem 128b
Classify each species as either a Lewis acid or a Lewis base. b. OH–
Problem 128c
Classify each species as either a Lewis acid or a Lewis base. c. B(OH)3
Problem 128d
Classify each species as either a Lewis acid or a Lewis base. d. CN–
Problem 129
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 130a
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 130b,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 131c
Based on these molecular views, determine whether each pictured acid is weak or strong.
Problem 132
Based on these molecular views, determine whether each pictured acid is weak or strong.
Problem 133
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)?