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문제 96c
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–
문제 97
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⁻.
문제 98
문제 99a
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+
문제 99b
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+
문제 99c
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+
문제 99d
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+
문제 100a,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+
문제 100d
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+
문제 101a,b,c,d
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. FeCl3 b. NaF c. CaBr2 d. NH4Br
문제 101e
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. e. C6H5NH3NO2
문제 102a
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. Al(NO3)3
문제 102b,c,d,e
Determine if each salt will form a solution that is acidic, basic, or pH-neutral. b. C2H5NH3NO3 c. K2CO3 d. RbI e. NH4ClO
문제 103
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.
문제 104
문제 105a
Determine the pH of each solution. a. 0.10 M NH4Cl
문제 106
Determine the pH of each solution. a. 0.20 M KCHO2 b. 0.20 M CH3NH3I c. 0.20 M KI
문제 107
Calculate the concentration of all species in a 0.15 M KF solution.
문제 108
Calculate the concentration of all species in a 0.225 M C6H5NH3Cl solution.
문제 109
Write chemical equations and corresponding equilibrium expressions for each of the three ionization steps of phosphoric acid.
문제 110
Write chemical equations and corresponding equilibrium expressions for each of the two ionization steps of carbonic acid.
문제 111a
Calculate the [H3O+] and pH of each polyprotic acid solution. a. 0.350 M H3PO4
문제 111b
Calculate the [H3O+] and pH of each polyprotic acid solution. b. 0.350 M H2C2O4
문제 112a
Calculate the [H3O+] and pH of each polyprotic acid solution.
a. 0.125 M H2CO3
문제 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.
문제 113
문제 114
Calculate the concentration of all species in a 0.155 M solution of H2CO3.
문제 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
문제 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?
- Consider a 0.10 M solution of a weak polyprotic acid (H2A) with the possible values of Ka1 and Ka2 given here: b. Ka1 = 1.0 * 10^-4; Ka2 = 1.0 * 10^-5. Calculate the contributions to [H3O+] from each ionization step. At what point can the contribution of the second step be neglected? c. Ka1 = 1.0 * 10^-4; Ka2 = 1.0 * 10^-6.
문제 116b