Indietro
Problema 110a
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (a) HCl
Problema 110b
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (b) KF
Problema 110c
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (c) NaNO3
Problema 110d
Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (d) Ba1NO322
- Calculate the molar solubility of PbCrO4 in: (a) Pure Water (d) 1.0 x 10^-3 M K2CrO4
Problema 111
- Calculate the molar solubility of SrF2 in: (a) 0.010 M Sr(NO3)2 (b) 0.010 M NaF.
Problema 112
- Which of the following compounds are more soluble in an acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction: (b) CaCO3, (c) Ni(OH)2, (d) Ca3(PO4)2.
Problema 113
- Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (a) MnS (b) AgCl (c) BaCO3
Problema 114
Problema 114b
Which of the following compounds are more soluble in acidic solution than in pure water? Write a balanced net ionic equation for each dissolution reaction. (b) Fe(OH)3
- Consider saturated solutions of the slightly soluble salt AgBr. Is the solubility of AgBr increased, decreased, or unaffected by the addition of each of the following substances? (a) HBr, (b) HNO3, (c) AgNO3, (d) NH3.
Problema 115
- Consider saturated solutions of the slightly soluble salt BaCO3. Is the solubility of BaCO3 increased, decreased, or unaffected by the addition of each of the following substances? (a) HNO3 (b) Ba(NO3)2 (c) Na2CO3 (d) CH3CO2H
Problema 116
Problema 117a
Is the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (a) HCl
Problema 117b
Is the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (b) KOH
Problema 117c
Is the solubility of Zn(OH)2 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (c) NaCN
- Is the solubility of Fe(OH)3 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (b) NaOH(aq)
Problema 118
- Silver ion reacts with excess CN- to form a colorless complex ion, [Ag(CN)2]-, which has a formation constant Kf = 3.0 x 10^20. Calculate the concentration of Ag+ in a solution prepared by mixing equal volumes of 2.0 x 10^-3 M AgNO3 and 0.20 M NaCN.
Problema 119
- Dissolution of 5.0 x 10^-3 mol of Cr(OH)3 in 1.0 L of 1.0 M NaOH gives a solution of the complex ion [Cr(OH)4]- (Kf = 8 x10^29). What fraction of the chromium in such a solution is present as uncomplexed Cr3+?
Problema 120
- Write a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each. (a) AgI in aqueous NaCN to form [Ag(CN)2]-
Problema 121
- Write a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each. (b) Cu(OH)2 in aqueous NH3 to form [Cu(NH3)4]2+
Problema 122
- Calculate the molar solubility of AgI in: (a) Pure Water (b) 0.10 M NaCN: Kf for [Ag(CN)2]- is 3.0 x 10^20
Problema 123
- Calculate the molar solubility of Cr(OH)3 in 0.50 M NaOH; Kf for Cr(OH)4- is 8 x 10^29.
Problema 124
- Zinc hydroxide, Zn(OH)2 (Ksp = 4.1 x 10^-17), is nearly insoluble in water but is more soluble in strong base because Zn2+ forms the soluble complex ion [Zn(OH)4]2- (Kf = 3 x 10^15). (a) What is the molar solubility of Zn(OH)2 in pure water? (You may ignore the OH- from the self-dissociation of water.) (b) What is the pH of the solution in part (a)? (c) What is the molar solubility of Zn(OH)2 in 0.10 M NaOH?
Problema 125
- Citric acid (H3Cit) can be used as a household cleaning agent to dissolve rust stains. The rust, represented as Fe(OH)3, dissolves because the citrate ion forms a soluble complex with Fe3+ (a) Using the equilibrium constants in Appendix C and Kf = 6.3 x 10^11 for Fe(Cit), calculate the equilibrium constant K for the reaction. (b) Calculate the molar solubility of Fe(OH)3 in 0.500 M solution of H3Cit.
Problema 126
- Hard water contains alkaline earth cations such as Ca2+, which react with CO32- to form insoluble deposits of CaCO3. Will a precipitate of CaCO3 form if a 250 mL sample of hard water having [Ca2+] = 8.0 x 10^-4 M is treated with the following? (a) 0.10 mL of 2.0 x 10^-3 M Na2CO3 (b) 10 mg of solid Na2CO3
Problema 128
- The pH of a sample of hard water having [Mg2+] = 2.5 x 10^-4 M is adjusted to pH 10.80. Will Mg(OH)2 precipitate?
Problema 129
- In quantitative analysis, Al3+ and Mg2+ are separated in an NH4+ - NH3 buffer having pH approximately equal to 8. Assuming cation concentrations of 0.010 M, show why Al(OH)3 precipitates but Mg(OH)2 does not.
Problema 131
- Can Fe2+ be separated from Sn2+ by bubbling H2S through a 0.3 M HCl solution that contains 0.01 M Fe2+ and 0.01 M Sn2+? A saturated solution of H2S has [H2S] ≈ 0.10 M. Values of Kspa are 6 x 10^2 for FeS andd 1 x 10^-5 for SnS.
Problema 132
- Can Co2+ be separated from Zn2+ by bubbling H2S through a 0.3 M HCl solution that contains 0.01 M Co2+ and 0.011 M Zn2+? A saturated solution of H2S has [H2S] approximately equal to 0.10 M. Values of Ksp are 3 for CoS and 3 x 10^-2 for ZnS.
Problema 133
- Will FeS precipitate in a solution that is 0.10 M in Fe(NO3)2, 0.4 M in HCl, and 0.10 M in H2S? Will FeS precipitate if the pH of the solution is adjusted to pH 8 with an NH4+ - NH3 buffer? Kspa = 6 x 10^2 for FeS.
Problema 134
- Will CoS precipitate in a solution that is 0.10 M in Co(NO3)2, 0.5 M in HCl, and 0.10 M in H2S? Will CoS precipitate if the pH of the solution is adjusted to pH 8 with an NH4+ - NH3 buffer? Ksp for CoS is 3.
Problema 135