7. A 25.0 mL solution of 0.0015M BaCl2 is added to 20.0 mLs of 0.0010 M Na2SO4. Determine if the resulting solution wil...
4. If 20.0 mL of 2.40 x 10-4 M Na2SO4 is mixed with 25.0 mL of 8.20 x 10-6 M CaCl2. Will a precipitate of CaSO4 (Ksp = 9.1 x 10-) form? Explain your choice in PDF submission. O No precipitate forms Insufficient information to answer the problem. O Precipitate forms
A 40.0-mL solution contains 0.033 M barium chloride (BaCl2). What is the minimum concentration of sodium sulfate (Na2SO4) required in the solution to produce a barium sulfate (BaSO4) precipitate? The solubility product for barium sulfate is Ksp = 1.1 ✕ 10−10.
Determine the minimum number of moles of Na2SO4 that must be added to 5.00 mL of a 2.00 x 10' M BaSO4 solution to precipitate BaSO4. Ksp (BaSO4)= 1.08 10-10 a. 1.98 x 105 mol b. 4.00 x 10'mol C. 2.70 x 10 mol d. 6.53 x 106 mol
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?
453 mg of a mixture of BaCl2 and RaCl2 was dissolved in 500 mL of water and 100.0 mL of 1 M Na2SO4 was added. The resulting precipitate was filtered through a tared weighing crucible, washed and dried at 110 C. the weight of the precipitate was 505 mg. Calculate the mole% Radium in the mixture. MW: BaCl2 208.23, RaCl2: 296.09, BaSO4: 233.38, RaSO4: 322 Why would this experiment never be conducted in a teaching laboratory?
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)
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 40.0-ml solution contains 0.021 M barium chloride (BaCl2). What is the minimum concentration of sodium sulfate (Na2SO4) required in the solution to produce a barium sulfate (BaSO4) precipitate? The solubility product for barium sulfate is Ksp = 1.1x10-10 Supporting Materials Periodic Table Supplemental Data Constants and Factors
6. The Ksp of AgBr is 4.8 x 10-13. If 50.0 mLs of 0.010 M AgNO3 are added to 100.0 mLs of 0.0020 M KBr, determine if the resulting solution will be saturated, supersaturated or unsaturated? Will a ppt form? Explain.
if 25.0 mL of 2.00 M K2SO4 is added to 20.0 mL of a 2.00 M Pb(NO3)2 solution what is the mass (in grams) of the precipitate?