Determine the minimum number of moles of Na2SO4 that must be added to 5.00 mL of...
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 will have a precipitate form or if it will remain unsaturated. Ksp (BaSO4) = 1.1.x 10-10
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 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.
Which of the following is the minimum amount of moles of NaOH that must be added to a 1 L solution that contains 4.3 x 10–6 M Cd2+ for the sparingly soluble salt Cd(OH)2 (Ksp = 2.5 x 10–14) to crystallize?
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?
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
A solution contains 0.040 M of Na2SO4 and 0.050 M of NaIO3. Another solution of Ba2+ is added to the first solution.( You must accept that the original solution does not include HSO-4). a) Which of the Baryum salts precipitate firstly? b) Calculate the Ba2+ concentration while the first precipitate is occuring. c) While the more dissolved precipitate is precipitating, what is the concentration of anion which forms the less dissolved Baryum salt ? Ba(IO3) Ksp= 1.57x10-9 BaSO4 Ksp= 1.1x10-10
If 100 mL of a .100 mol/L CaCl2(aq) and 100 mL of 0.0400 mol/L Na2SO4(aq) are mixed at 20°C, determine whether a precipitate will form. For CaSO4(aq) at 20°C, Ksp is 3.6 x 10-5.
23. Will a precipitate form when 100. mL of 8.0x 103 M Pb(NO3)2 is added to 400. mL of 5.0 x 10-3 M Na2SO4? The Ksp of PbSO4 is 6.3 x 10-7 A. No precipitate forms because Qsp Ksp B. Yes, a precipitate forms because Qsp>Ksp C. No precipitate forms because Qsp> Ksp es, a precipitate forms because Qsp Ksp