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A scientist adjusts the pH of a solution to...
I need help please To a solution containing 0.15 M Ci- ion and 0.15 M Br-...
I need help please To a solution containing 0.15 M Ci- ion and 0.15 M Br- ion, you add some solid AgNO3. Ksp for AgCl is 1.6 * 10^-10 and for AgBr is 5.0*10^-13. the addition of solid doesn't change the total volume. a) which component AgCl or AgBr precipitates first? b) what is the concentration of the first anion to precipitate when the silver halide of the second anion starts to precipitate?
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2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Kap 1.5x101) b. If NH3/NH buffer is used to control the pH, and [NHs] 0.10 M, what concentration of NH is required to prevent the precipitation of Mg(OH)2? 3. Solid AgNOs is slowly added to a solution that is 0.001OM in NaCl, NaBr...
A solution contains 0.020 mole each of I”, Br, and Cl. When the solution is mixed...
A solution contains 0.020 mole each of I”, Br, and Cl. When the solution is mixed with 200. mL of 0.28 M AgNO3, what mass of AgCl(s) precipitates out, and what is Ag+)? Assume no volume change AgI: Ksp = 1.5 x 10-16 AgBr : Ksp = 5.0 x 10-18 AgCl : Ksp = 1.6 x 10-10 00 Mass of AgCl(s) = [18+] - M
A solution is 0.10 M Cl and 0.10 M I- . Silver nitrate is slowly added...
A solution is 0.10 M Cl and 0.10 M I- . Silver nitrate is slowly added to precipitate the silver halide. Ksp(AgCl) = 1.77 x 10-10; Ksp(AgI) = 8.52 x 10-17 (A) Which solid will precipitate first? (B) What will be the [Ag+ ] when the first solid begins to precipitate? (C) What [Ag+ ] is required in order to precipitate AgCl? (D) What will be the [I- ] when the AgCl starts to precipitate? (E) What percentage of the...
27. A solution contains 0.015 mole each of I“, Br , and C1-. When the solution...
27.
A solution contains 0.015 mole each of I“, Br , and C1-. When the solution is mixed with 200. mL of 0.20 M AgNO3, what mass of AgCl(s) precipitates out, and what is Ag+ ? Assume no volume change. AgI: Ksp = 1.5 x 10-16 AgBr: Ksp = 5.0 x 10-13 AgCH: Ksp = 1.6 x 10-10 g Mass of AgCl(s) = D [Ag+1 = M
4. A solution contains 0.018 mol each of I–, Br–, and Cl–. Use the Ksp values...
4. A solution contains 0.018 mol each of I–, Br–, and Cl–. Use the Ksp values given below to determine how much AgCl(s) precipitates out when this solution is mixed with 200 mL of 0.24 M AgNO3. NOTE: This question isn’t as difficult as it looks. It’s really just stoichiometry. Ksp AgI = 1.5 x 10–16 Ksp AgBr = 5.0 x 10–13 Ksp AgCl = 1.6 x 10–10 A) 5.0 g B) 3.3 g C) 2.6 g D) 0.0 g...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except that they have the following pH values: Hint: Common ion effect. Which two ions dictate acidity and basicity? a. 3 b. 7 c. 9 d. 11 2. Potassium perchlorate has a solubility product constant of 10-2. Which is true about the following solution of KClO4: [K+] = 0.01 M, [ClO4 −] = 0.01 M a. Ksp < Q and no precipitation occurs b....
1) Write the solubility-product expression for the following mercury salts: Hg2Cl2 and HgCl2. 2) Exactly 0.133...
1) Write the solubility-product expression for the following mercury salts: Hg2Cl2 and HgCl2. 2) Exactly 0.133 mg of AgBr will dissolve in 1.00 L of water. What is the value of Ksp for AgBr? 3) By experiment, it is found that 1.2 x 10-3 mol of lead (II) iodide, PbI2, dissolves in 1.0 L of water at 25°C. What is the Ksp at this temperature? 4) What is the molar solubility of silver chloride in 1.0 L of solution that...
28) What is the molar solubility of Mg(OH)2 in a basic solution with a pH of...
28) What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 11.18? Ksp for Mg(OH)2 is 5.6x 10-12 B) 5.6x 10-10 M D) 1.1 x 10-4 M C) 2.4 x 10-6 M A) 5.6 x 10-8 M 29) What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 x 10-10 and Kf for Ag(CN) 2- is 1.0 x 1021, D) 0.050...
5. Which of the following would decrease the K for PbCl2? 2. Lower the pH of...
5. Which of the following would decrease the K for PbCl2? 2. Lower the pH of the solution b. Add a solution of Pb(NO3)2 c. Add a solution of KCI d. Both band e. None of the above the Ky of a compound is constant at constant tempera mperature, 6. In which of the following aqueous solutions would you expect AgBr to have the HIGHES solubility? a. 0.10 M LIBE b. 0.10 M AgNO3 c. 0.20 M NaBr d. 0.15...
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2. A solution is 0.10M in Mg(NO3)2. a. What concentration of OH is required to just start precipitation of Mg(OH)2? (Kap 1.5x101) b. If NH3/NH buffer is used to control the pH, and [NHs] 0.10 M, what concentration of NH is required to prevent the precipitation of Mg(OH)2? 3. Solid AgNOs is slowly added to a solution that is 0.001OM in NaCl, NaBr...
A solution contains 0.020 mole each of I”, Br, and Cl. When the solution is mixed with 200. mL of 0.28 M AgNO3, what mass of AgCl(s) precipitates out, and what is Ag+)? Assume no volume change AgI: Ksp = 1.5 x 10-16 AgBr : Ksp = 5.0 x 10-18 AgCl : Ksp = 1.6 x 10-10 00 Mass of AgCl(s) = [18+] - M
27.
A solution contains 0.015 mole each of I“, Br , and C1-. When the solution is mixed with 200. mL of 0.20 M AgNO3, what mass of AgCl(s) precipitates out, and what is Ag+ ? Assume no volume change. AgI: Ksp = 1.5 x 10-16 AgBr: Ksp = 5.0 x 10-13 AgCH: Ksp = 1.6 x 10-10 g Mass of AgCl(s) = D [Ag+1 = M
28) What is the molar solubility of Mg(OH)2 in a basic solution with a pH of 11.18? Ksp for Mg(OH)2 is 5.6x 10-12 B) 5.6x 10-10 M D) 1.1 x 10-4 M C) 2.4 x 10-6 M A) 5.6 x 10-8 M 29) What is the molar solubility of AgCl in 0.10 M NaCN if the colorless complex ion Ag(CN) 2- forms? Ksp for AgCl is 1.8 x 10-10 and Kf for Ag(CN) 2- is 1.0 x 1021, D) 0.050...
5. Which of the following would decrease the K for PbCl2? 2. Lower the pH of the solution b. Add a solution of Pb(NO3)2 c. Add a solution of KCI d. Both band e. None of the above the Ky of a compound is constant at constant tempera mperature, 6. In which of the following aqueous solutions would you expect AgBr to have the HIGHES solubility? a. 0.10 M LIBE b. 0.10 M AgNO3 c. 0.20 M NaBr d. 0.15...
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