student mixes 39.0 mL of 3.32M Pb(NO_3)_2(aq) with 20.0 mL of 0.00223 M Na_2SO_4(aq). How many...
A student mixes 39.0 mL of 2.88 M Pb(NO3)2(aq) with 20.0 mL of 0.00197 M Na2C2O4(aq). How many moles of PbC2O4(s) precipitate from the resulting solution? What are the values of [Pb2 ], [C2O42–], [NO3–], and [Na ] after the solution has reached equilibrium at 25 °C?
A student mixes 41.0 mL of 2.84 M Pb(NO3)2(aq) with 20.0 mL of 0.00235 M Nal(aq). How many moles of Pbla(s) precipitate from the resulting solution? Number K,,[Pb12()] – 9810 mol What are the values of [Pb2+), [1]. [NO3-), and [Na*) after the solution has reached equilibrium at 25 °C? Number Number [Pb?*] = Number Number [no; ]- 0 M [nat)-
student mixes 35.0 mL of 3.18 M Pb(NO3)2(aq) with 20.0 mL of 0.00151 M Nal(aq). How many moles of Pbl2(s) precipitate from the resulting solution? Number 3.02x 10-5mol What are the values of [P NO3, and [Na'] after the solution has reached equilibrium at 25 °C? Number Number Pb2.02 111-114.84 ×10-9 IM Number Number NO4.05
I need full explanation, please! A solution of Pb(NO_3)_2 is added to a second solution in which [Cl^-] = [F^-] = [I^-] = [SO_4^2-] = 0.001 M. What is the first precipitate that forms? A) PbI_2 (K_sp = 8.5 times 10^-9) B) PbSO_4 (K_sp= 1.8 times 10^-8) C) PbCl_2 (K_sp = 1.5 times10^-5) D) PbF_2 (K_sp = 3.7 times 10^-8)
Please help!!!!! A 80.0 mL aliquot of a 0.250 M Ca(NO_3)_2 solution was mixed with 60.0 mL of a 0.500 M NaF solution. K_sp(CaF_2) = 3.90 times 10^-11. Calculate the mass of CaF_2 that was formed. Determine the equilibrium concentrations of Ca^2+ and F^- ions remaining in the resultant solution.
Will a precipitate of BaSO_3 form if solution of 10 mL 0.050 M Ba(NO_3)_2 is added to 15 mL of a 0.020 M Na_2SO_3? (K_sp = 5.0 times 10^-10) A. Yes, because Q < K B. Yes, because Q > K C. No, because Q < K D. No, because Q > K
A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00 times 10^-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2^+ is 1.40 times 10^-4 M. a) What is the initial concentration in solution of the Fe^3+ and SCN^-? b) What is the equilibrium constant for the reaction?
How many grams of KI should be dissolved in 10.5L of 0.00200 M Pb(NO_3)_s solution so that precipitation of Pbl_2(s) will just begin? K_sp = 7.1 times 10^-9
How many grams of each of the following substances will dissolve in 100 mL of cold water? Consult a handbook or the Internet and cite your source. Ce(IO_3)_4 RaSO_4 Pb(NO_3)_2 (NH_4)_2SeO_4 Which of these substances is least soluble on a gram-per-100 mL basis? Suppose you have a solution that might contain any or all of the following cations. Cu^2+, Ag^+, Ba^2+, and Mn^2+. The addition of HBr causes a precipitate to form. After the precipitate is filtered off, H_2SO_4 is...
A student begins with 10.2 mL of a 0.28 M Cu(NO_3)_2 solution and performs copper cycle lab She recovers 0.079 grams of copper metal. What is the theoretical ytetd of copper in grams? What is the actual yield of copper in grams? What is tho percent yield of copper?