A solution contains 2.0 x10-4 M Ag+(aq) and1.5 x 10-3 M Pb2 + (aq). If NaI is added , wi l l AgI(Ksp = 8.3 x10-17)or PbI2 (Ksp = 7.9x 10-9) precipitatefirst? Specify the concentration of I-(aq) needed to beginprecipitation.
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A solution contains 2.0 x10-4 M Ag+(aq) and
1.5 x 10-3 M Pb2 + (aq). If NaI is added , wi l l AgI
(Ksp = 8.3 x10-17)or PbI2 (Ksp = 7.9x 10-9) precipitate
first? Specify the concentration of I-(aq) needed to begin
precipitation.
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- The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mLA solution contains 1.0 x 10-2 M Ag+(aq) and 2.0 x 10-2 M Pb2 +(aq). When Cl-(aq) is added, both AgCl(Ksp = 1.8 x 10-10) and PbCl2 (Ksp = 1.7 x 10-5) can precipitate. What concentration of Cl-(aq) is necessary to begin theprecipitation of each salt? Which salt precipitates first?
- After addition of HNO, to the mixture (1st addition), why did the precipitate dissolve? Consider the following equilibria: 2 Ag* (aq) + CO, (ag) = Ag2CO3(s) CO" (aq) +2H*(aq) = H2O(1) + CO2(9)A solution contains three anions with the followingconcentra t i o n s : 0.20 M CrO42 - , 0.10 M CO32 - , and0.010 M Cl-. If a dilute AgNO3 solution is slowly added tothe solution, what is the first compound to precipitate:Ag2CrO4 (Ksp = 1.2 x 10-122, Ag2CO3 (Ksp = 8.1 x 10-12 ),or AgCl (Ksp = 1.8 x 10-10 )?The solubility product constant of barium fluoride in water at 25o C is Ksp = 1.3 x 10-6. Calculate the solubility of this compound in 1.00 M Ba(NO3)2 (aq) at 25o If 15 mL of 0.024 M lead (II) nitrate is mixed with 30 mL of 0.030 M potassium chromate, will a precipitate form? (Ksp = 2.0 x 10-16 for PbCrO4) Calculate the ionic strength of the following solutions: 25 M Cr(NO3)3 05 M Al(ClO4) Using simple Debye-Huckel equation, estimate the following activity coefficients: SO42- at µ = 0.025 Fe(CN)63- at µ = 0.005 The solubility product constant of cuprous chloride in water at 25o C is Ksp = 1.0 x 10-6. Calculate the solubility of this compound in 0.020 M KCl(aq) at 25o
- The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. a) Sketch the pH vs volume of added base titration curve for this reaction. pH vertically, volume of base horizontally. Label your axes with correct pH and volumes. (Attach more space, if needed) b) what is the pH at the beginning of the titration, Vbase = 0.00 mL ? c) what is the volume of the base needed to reach the equivalence point ? (label the equiv. point) d) what is the pH at the equivalence point?e) what is the pH of the titration when 5.00 mL of base have been added ? f) what is the pH when the volume of base added equals half the volume of the equivalence point? g) what is the pH of the titration when 20.00 mL of base have been added? h) what is the pH of the titration…The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. 1. what is the pH when the volume of base added equals half the volume of the equivalence point? 2. what is the pH of the titration when 20.00 mL of base have been added? 3. what is the pH of the titration when 30.00 mL of base have been added?A solution contains 1.0 * 10-2 M Ag+(aq) and 2.0 * 10-2 M Pb2+(aq). When Cl-(aq) is added, both AgCl (Ksp = 1.8 * 10-10) and PbCl2 (Ksp = 1.7 * 10-5) can precipitate. What concentration of Cl-(aq) is necessary to begin the precipitation of each salt? Which salt precipitates first?
- The weak monoprotic acid, acetic acid, is titrated with the strong base, potassium hydroxide as follows: HC2H3O2(aq) + K+ OH- (aq) → K+ C2H3O2-(aq) + H2O(l) Ka for acetic acid is 1.81 x 10-5 (at 25 oC). A 25.00 mL sample of a solution of acetic acid with concentration 0.0833 M is titrated with 0.1000 M KOH. A. What is the pH at the beginning of the titration, Vbase = 0.00 mL? B. What is the pH at the equivalence point? C. What is the pH of the titration when 5.00 mL of base have been added? D. What is the pH when the volume of base added equals half the volume of the equivalence point? E. What is the pH of the titration when 20.00 mL of base have been added? F. What is the pH of the titration when 30.00 mL of base have been added?(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/LSodium sulfate is slowly added to a solution containing 0.0500 M Ca² +(aq) and 0.0210 M Ag+ (aq). What will be the concentration of Ca² +(aq) when Ag₂SO4(s) begins to precipitate? Solubility-product constants, K₁p, can be found in the chempendix. [Ca²+] = What percentage of the Ca² +(aq) can be precipitated from the Ag+ (aq) by selective precipitation? percentage: M %
