To a solution of Pb (NO3)2, whose concentration is 1 x 10-6 M, an alkaline iodine...
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
question 17 & 18 Q17. A 5.0 x 10-M solution of Mn is gradually made more basic by adding NaOH. At what pH will manganese(II) hydroxide begin to precipitate? For Mn(OH)2. Kip - 2.0 x 10-13 Q18. A solution is 0.010 M in each of Pb(NO3)2. Mn(NO3). and Zn(NO3)2. Solid NaOH is added until the pH of the solution is 8.50. Which of these three metal ion(s) will precipitate as a hydroxide? Salt KR Pb(OH)2 1.4 x 10-20 Mn(OH)2 Zn(OH)2...
If 450 ml of some Pb(NO3)2 solution is mixed with 250 ml of 1.10 x 10-2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2forms? (Assume Ksp = 2.00 x 10-5 M at this temperature.) Enter the concentration in M.
If 300 mL of some Pb(NO3)2 solution is mixed with 600 mL of 2.70 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.
If 250 mL of some Pb(NO3)2 solution is mixed with 450 mL of 5.90 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.
If 400 mL of some Pb(NO3)2 solution is mixed with 400 mL of 1.10 x 10-2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10-5 M at this temperature.) Enter the concentration in M. Submit Answer Tries 0/99
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq) Pb ( NO 3 ) 2 ( aq ) , until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 10.47 g PbCl2(s) 10.47 g PbCl 2 ( s ) is obtained from 200.0 mL 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) Pb ( NO 3 ) 2 ( aq ) solution. concentration: M
8. A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 12.12 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution. concentration: M
A solution of NaCl(aq) is added slowly to a solution of lead nitrate, Pb(NO3)2(aq), until no further precipitation occurs. The precipitate is collected by filtration, dried, and weighed. A total of 15.59 g PbCl2(s) is obtained from 200.0 mL of the original solution. Calculate the molarity of the Pb(NO3)2(aq) solution. concentration: M
Calculate the concentration of 103 in a 9.27 mM Pb(NO3)2 solution saturated with Pb(IO3)2. The Ksp of Pb(IO3)2 is 2.5 x 10-13. Assume that Pb(IO3), is a negligible source of Pb2+ compared to Pb(NO3)2. [103] = M A different solution contains dissolved NalO3. What is the concentration of Naloz if adding excess Pb(IO3)2(s) produces a Pb2+ concentration of 5.20 x 10-6 M? concentration: M