If 15.0 mL of
8.80×10-4 M
Pb(NO3)2 are added to
22.0 mL of 3.10×10-5 M
KI, will solid PbI2
(Ksp = 8.7×10-9)
precipitate?
If a precipitate will not form, what iodide ion
concentration will cause a precipitate of lead
iodide to form? If a precipitate will form, what is the
minimum [I-] that could have been
present without initiating precipitation? Assume the total volume
used in the above example.
M
If 15.0 mL of 8.80×10-4 M Pb(NO3)2 are added to 22.0 mL of 3.10×10-5 M KI,...
If 15.0 mL of 7.25×10-4 M MgI2 are added to 22.0 mL of 1.80×10-5 M KF, will solid MgF2 (Ksp = 6.4×10-9) precipitate? _____yes/no If a precipitate will not form, what fluoride ion concentration will cause a precipitate of magnesium fluoride to form? If a precipitate will form, what is the minimum [F-] that could have been present without initiating precipitation? Assume the total volume used in the above example. ______M
If 15.0 mL of 5.92×10-4 M MgI2 are added to 12.0 mL of 5.60×10-5 M NaF, will solid MgF2 (Ksp = 6.4×10-9) precipitate? _____yesno If a precipitate will not form, what fluoride ion concentration will cause a precipitate of magnesium fluoride to form? If a precipitate will form, what is the minimum [F-] that could have been present without initiating precipitation? Assume the total volume used in the above example.
If 15.0 mL of 7.28×10-4 M Cu(CH3COO)2 are added to 18.0 mL of 8.90×10-5 M K2CO3, will solid CuCO3 (Ksp = 2.5×10-10) precipitate? _____ yes or no If a precipitate will not form, what carbonate ion concentration will cause a precipitate of copper(II) carbonate to form? If a precipitate will form, what is the minimum [CO32-] that could have been present without initiating precipitation? Assume the total volume used in the above example. M
A26. What will be observed when 15.0 mL of 0.040 M lead(II) nitrate, Pb(NO3)2, is mixed with 15.0 mL of 0.040 M sodium chloride? (lead chloride Ksp = 1.7 × 10–5). (A) A clear solution with no precipitate will result. (B) Solid PbCl2 will precipitate and excess Pb2+ ions will remain in solution. (C) Solid PbCl2 will precipitate and excess Cl– ions will remain in solution. (D) Solid PbCl2 will precipitate and there will be no excess ions in solution....
Use the reaction quotient to predict whether a precipitate will form. If 18.0 mL of 7.46x104 M CaCl2 are added to 15.0 mL of 1.30x10M (NH4)2S, will solid CaS (Ksp = 8.0x10 precipitate? no If a precipitate will not form, what sulfide ion concentration will cause a precipitate of calcium sulfide to form? If a precipitate will form, what is the minimum [S2] that could have been present without initiating precipitation? Assume the total volume used in the above example.
Potassium iodide reacts with lead (ii) nitrate in the following precipitation reaction: 2KI (aq) + Pb(NO3)2 (aq)---> 2KNO3 (aq) + PbI2 (s) What minimum volume of 0.200 M potassium iodide solution is required to completely precipitate all the lead in 155.0 mL of a 0.122 M lead (ii) nitrate solution?
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
1. When 25.0 mL of a 2.11×10-4 M magnesium bromide solution is combined with 15.0 mL of a 9.37×10-4 M ammonium fluoride solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to . 2. Solid potassium hydroxide is slowly added to 175 mL of a 0.0511 M calcium acetatesolution. The concentration of hydroxide ion required to just initiate precipitation is M. 3. Solid aluminum nitrate is slowly added to 50.0 mL of a 0.0350...
Consider the balanced equation of KI reacting with Pb(NO3)2 to form a precipitate. 2KI(aq)+Pb(NO3)2(aq)⟶PbI2(s)+2KNO3(aq) What mass of PbI2 can be formed by adding 0.413 L of a 0.140 M solution of KI to a solution of excess Pb(NO3)2?
QUESTION 21 A solution is 0.012 Min Pb(NO3)2 and 0.20 Min Sr(NO3)2. Solid Na2SO4 is added until a precipitate just begins to form. The precipitate is and the concentration of sulfate ion at this point is Ksp for PbSO4 is 1.8 x 10-8 and for SrS04 is 2.8 x 10-7 PbSO4: 1.5 10 M SrS04; 1.4 x 10-6M PbSO4; 6.3 * 10 M "SrS04; 8.3 x 10-?M S-S04:2.6 x 10-7M