2. A solution is 0.01 M in Ba2+ and 0.01 M in Cal. Sodium sulfate is added to selectively precipitate one of the ca...
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
Solubility Rules TABLE 1: SOLUBILITY RULES FOR CATIONS Precipitating agent lons that will form a precipitate Cl", Br", Agt, Pb2+, and Hg22 Ca2+, Sr2+, Ba2+, Agt, and Pb2+ All metal ions (with widely varying Ksp values) except Li, Na+, K+, and NHA All metal ions except Lit, Na, K, NH4+, Ca?, Srl, and Ba? CO32- All metal ions except Lit, Na, K, and NHA PO43- All metal ions except Lit, Na, K, and NH4 50,2- OH S2- Pre-Lab Questions 1....
A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. The solubility-product constants are as follows: BaSO4:SrSO4:KspKsp==1.1×10−103.2×10−7 You may want to reference(Pages 751 - 753) Section 17.6 while completing this problem. Which cation will precipitate first? Ba2+ precipitates first. Sr2+ precipitates first. What concentration of SO42− is necessary to begin precipitation? (Neglect volume changes.) Express the molarity to two significant digits. 1.0×10−8 M ***Need help with this answer. 1.)...
A solution of Na2SO4 is added dropwise to a solution that is 1.1×10−2 M in Ba2+ and 1.1×10−2 M in Sr2+. 1. What concentration of SO2−4 is necessary to begin precipitation? (Neglect volume changes. BaSO4:Ksp=1.1×10−10; SrSO4:Ksp=3.2×10−7.) 2. What is the concentration of SO2−4 when the second cation begins to precipitate?
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is dissolved in 1.00 grams of Nal can be dissolved in this solution without a precipitate 4.) (Modified from Chemistry: A Molecular Approach, 1" Ed. by Tro) Consider a solution that is 0.024 M in Cu and 0.017 M in Fe (a) If sodium hydroxide is used to selectively...
2002 - Review Constants Periodic Consider a solution that is 1.3x10-2 Min Ba? and 20x10-2 Min Cat - Part A sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? Ba? О саа Submit Request Answer Part B What minimum concentration of N, 80, is required to cause the precipitation of the cation that precipitate Express your answer using two significant figures. ? AERO? Na,80 Submit Request...
Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in both Ba2+ and Pb2+ until [SO42-] reaches 1.0 x 10^-4 M. Would either BaSO4 (Ksp = 1.1 x 10^-10) or PbSO4 (Ksp = 1.7 x 10^-8) precipitate under these conditions?
A solution of Na2SO4 is added dropwise to a solution with 0.020 M Ba2+ and 0.020 M Sr2+. (for BaSO4, Ksp = 1.1x10–10 and for SrSO4, Ksp = 3.2x10–7) (a) What precipitate will form first? Why? (b) What concentration of SO4 2– in the solution is necessary to begin precipitation? (neglect any volume change)
A solution contains 1.07×10-2 M sodium sulfate and 9.52×10-3 M potassium iodide. Solid lead acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of lead ion when this precipitation first begins? [Pb2+] = M
A solution contains 1.07×10-2 M sodium sulfate and 9.52×10-3 M potassium iodide. Solid lead acetate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of lead ion when this precipitation first begins? [Pb2+] = M