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Problem 99
Determine if each anion acts as a weak base in solution. For those anions that are basic, write an equation that shows how the anion acts as a base. a. Br– b. ClO– c. CN– d. Cl–
Problem 100c
Determine whether each anion is basic or neutral. For those anions that are basic, write an equation that shows how the anion acts as a base. c. NO3–
Problem 101
Determine the [OH–] and pH of a solution that is 0.140 M in F–.
- Determine the [OH-] and pH of a solution that is 0.250 M in HCO3⁻.
Problem 102
Problem 103a
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. a. NH4+
Problem 103b
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. b. Na+
Problem 103c
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. c. Co3+
Problem 103d
Determine whether each cation is acidic or pH-neutral. For those cations that are acidic, write an equation that shows how the cation acts as an acid. d. CH2NH3+
Problem 104a,b,c
Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. a. Sr2+ b. Mn3+ c. C5H5NH+
Problem 104d
Determine whether each cation is acidic or pH-neutral. For each cation that is acidic, write an equation that shows how the cation acts as an acid. d. Li+
Problem 105e
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO2
Problem 106a
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3
Problem 107
Arrange the solutions in order of increasing acidity. NaCl, NH4Cl, NaHCO3, NH4ClO2, NaOH
- Arrange the solutions in order of increasing basicity: CH3NH3Br, KOH, KBr, KCN, C5H5NHNO2.
Problem 108
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