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?
You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) + 2KNO3 (aq) You mix a 25.0 mL sample of a 20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) ® PbCl2 (s) +...
You mix a 25.0 mL sample of a 1.20 M potassium chloride solution with 20.0 mL of a 0.900 M lead(II) nitrate solution, and this precipitation reaction occurs: (5 pts) 2KCl (aq) + Pb(NO3)2 (aq) → PbCl2 (s) + 2KNO3 (aq) You collect and dry the solid PbCl2 and find that it has a mass of 3.45 g. Determine the limiting reactant, and the percent yield? How many grams of excess reactant will remain when the reaction is complete?
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
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?
14. 30.0 mL of 0.150 M KASO, is mixed with 20.0 mL of 2.00 M AgNO, and a precipitate forms. What are the equilibrium (Ag+] and [AsOd") in the resulting solution?
How many grams of PbBr2 will precipitate when excess CaBr2 solution is added to 61.0 mL of 0.615 M Pb(NO3)2 solution? g
How many grams of PbBr2 will precipitate when excess CrBr3 solution is added to 61.0 mL of 0.743 M Pb(NO3)2 solution? 3Pb(NO3)2(aq) + 2CrBr3(aq) 3PbBr2(s) + 2Cr(NO3)3(aq)
How many grams of PbBr2 will precipitate when excess AlBr3 solution is added to 45.0 mL of 0.745 M Pb(NO3)2 solution? 3Pb(NO3)2(aq) + 2AlBr3(aq) 3PbBr2(s) + 2Al(NO3)3(aq) ______g
How many grams of PbBr2 will precipitate when excess FeBr3 solution is added to 49.0 mL of 0.793 M Pb(NO3)2 solution? 3Pb(NO3)2(aq) + 2FeBr3(aq) ->3PbBr2(s) + 2Fe(NO3)3(aq) g
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)-