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19. In the Liebig titration of cyanide ion, a soluble complex is formed at the equivalence...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion,...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(a...
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
please solve 20 and 21!!! when the Ksp for AlPO, is 9.84 10 and the Kyfor the AMEDTA) complex ion is 1.310 19. The Kr f for the complex ion Ni(NHs) is 2.0x10. Analysis shows a solution at equilibr...
please solve 20 and 21!!!
when the Ksp for AlPO, is 9.84 10 and the Kyfor the AMEDTA) complex ion is 1.310 19. The Kr f for the complex ion Ni(NHs) is 2.0x10. Analysis shows a solution at equilibrium contains hjc"] = 0.0016 M. INHi-0.98 M, and [N产] = 9.03x10-2 M. what concentration of sulfide [Ni(N tart the precipitation of NiS(s) from the solution, if the Kse value is 3.0x1020 for NiS? 20. Decreasing the activity coefficients will increase the...
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x...
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
10. The formation of complex ions causes the solubility of a slightly soluble solid to: A...
10. The formation of complex ions causes the solubility of a slightly soluble solid to: A increase B. decrease C. stay the same D. none of the above 11. The equivalence point of a titration occurs: A. when all of the analyte has been titrated (reacted B. usually just before the endpoint. C. Both A and B D. Neither A or B 12. How does a buffer resist change in pH upon addition of a strong acid? A) The strong...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH,...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7 x 10") with 0.100 M LiOH. What is the pH of the solution before any base has been added? L 4 points b What would be the pH of the solution after the addition of 200 ml of LiOH? 4 points How many mL of the LiOH would be required to reach the halfway point of the titration? 1 4 points points d What...
i need help on question 2a,b,c and 3a,b,c on the post lab. Experiment EQ-309 Post-Lab Questions...
i
need help on question 2a,b,c and 3a,b,c on the post lab.
Experiment EQ-309 Post-Lab Questions Determination Of An Equilibrium Constant (To be answered in the "Analysis" section of your lab report) 1 a) Calculate the molarity of the silver nitrate solution provided. b) Calculate the molarity of the sodium chloride solution provided. 2 a) Use the data from each titration to calculate the value of K for the reaction, Ag(NH)2+ + Cl" - AgCl, + 2 NH, b) Calculate...
1. Calculate the pH of 1.0 M monochloroacetic acid (HCHCIO) with a K, of 1.35x10 (10...
1. Calculate the pH of 1.0 M monochloroacetic acid (HCHCIO) with a K, of 1.35x10 (10 points. HCq Ha Cload Catz (102H 0 & X y X 0 2. Calculate the erams of sodium sorbate (NaCsH-CO) required to make 1.00 liter of a 0.0860M sorbic acid solution pH 3.80. The K, for sorbic acid is 1.70 x10 (10 points). 3. A 25.0 mL sample of 0.120 M of lactic acid (HCH.0.) is titrated with 25.0 mL of sodium hydroxide to...
Vitamin C in a titration with potassium iodate References Mailings Review View AaBbcode Abccdee AaBbcc No...
Vitamin C in a titration with potassium iodate
References Mailings Review View AaBbcode Abccdee AaBbcc No Spacing Heading 1 Normal 3. A suitable method for the determination of vitamin C (C.H.O.) is a titration with potassium iodate (KIO). Potassium iodate is used as a titrant and is added to an ascorbic acid solution that contains strong acid and potassium iodide (KI). Potassium iodate reacts with excess potassium iodide, liberating molecular iodine (12): [1] KIO, + 5KI + 6H 31, +6K...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
all 5&6
5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
please solve 20 and 21!!!
when the Ksp for AlPO, is 9.84 10 and the Kyfor the AMEDTA) complex ion is 1.310 19. The Kr f for the complex ion Ni(NHs) is 2.0x10. Analysis shows a solution at equilibrium contains hjc"] = 0.0016 M. INHi-0.98 M, and [N产] = 9.03x10-2 M. what concentration of sulfide [Ni(N tart the precipitation of NiS(s) from the solution, if the Kse value is 3.0x1020 for NiS? 20. Decreasing the activity coefficients will increase the...
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
10. The formation of complex ions causes the solubility of a slightly soluble solid to: A increase B. decrease C. stay the same D. none of the above 11. The equivalence point of a titration occurs: A. when all of the analyte has been titrated (reacted B. usually just before the endpoint. C. Both A and B D. Neither A or B 12. How does a buffer resist change in pH upon addition of a strong acid? A) The strong...
1. 50.0 mL of a pH 6.00 carbonic acid buffer is titrated with 0.2857 M NaOH, requiring 17.47 mL to reach the second equivalence point. a. Calculate the molarity of carbonic acid and bicarbonate in the original buffer. (10 pts) Carbonic acid Bicarbonate: b. Calculate the pH of the solution after a total of 100.0 mL of 0.2857 M NaOH is added to the buffer and equilibrium is established. (10 pts) c. 7.833 g of solid lead(II) carbonate is added...
Consider the titration of a 40.0 ml. of 0.155 M weak acid HA (Ka = 2.7 x 10") with 0.100 M LiOH. What is the pH of the solution before any base has been added? L 4 points b What would be the pH of the solution after the addition of 200 ml of LiOH? 4 points How many mL of the LiOH would be required to reach the halfway point of the titration? 1 4 points points d What...
i
need help on question 2a,b,c and 3a,b,c on the post lab.
Experiment EQ-309 Post-Lab Questions Determination Of An Equilibrium Constant (To be answered in the "Analysis" section of your lab report) 1 a) Calculate the molarity of the silver nitrate solution provided. b) Calculate the molarity of the sodium chloride solution provided. 2 a) Use the data from each titration to calculate the value of K for the reaction, Ag(NH)2+ + Cl" - AgCl, + 2 NH, b) Calculate...
1. Calculate the pH of 1.0 M monochloroacetic acid (HCHCIO) with a K, of 1.35x10 (10 points. HCq Ha Cload Catz (102H 0 & X y X 0 2. Calculate the erams of sodium sorbate (NaCsH-CO) required to make 1.00 liter of a 0.0860M sorbic acid solution pH 3.80. The K, for sorbic acid is 1.70 x10 (10 points). 3. A 25.0 mL sample of 0.120 M of lactic acid (HCH.0.) is titrated with 25.0 mL of sodium hydroxide to...
Vitamin C in a titration with potassium iodate
References Mailings Review View AaBbcode Abccdee AaBbcc No Spacing Heading 1 Normal 3. A suitable method for the determination of vitamin C (C.H.O.) is a titration with potassium iodate (KIO). Potassium iodate is used as a titrant and is added to an ascorbic acid solution that contains strong acid and potassium iodide (KI). Potassium iodate reacts with excess potassium iodide, liberating molecular iodine (12): [1] KIO, + 5KI + 6H 31, +6K...
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