Given that PbBr2 has a Ksp of 4.0×10−5, PbCrO4 has a Ksp of 2.8×10−13, and Pb(OH)2 has a Ksp of 1.2×10−15, which of these salts would precipitate first during selective precipitation?
Given that PbBr2 has a Ksp of 4.0×10−5, PbCrO4 has a Ksp of 2.8×10−13, and Pb(OH)2...
please answer both questions
QUESTION 24 To 1.0 L of water, 3,0 x 10 mol of Pb(NO3)2, 4.0 x 10 mol of K2C+04, and 1.0 mol of NaCl are added. What will happen? Disregard the increase in volume due to added substances. Salt Esp PbC+04 1.8 * 10-14 PbCl2 16 x 10-5 A precipitate of PbCrO4 will form. b. A precipitate of KCI will form. No precipitate will form. A precipitate of PbCl2 will form QUESTION 25 What is the...
Questions 1 & 2 refer to the solubility of lead chromate, PbCrO4: PbCrO4(s) = Pb2+ (aq) + CrO42-(aq) 1. The Ks for PbCrO4 is 2.0 x 10-16 at 25 °C. What is the solubility of PbCrO4 in mol L-?? a) 1.4 x 10-8 b) 2.8 x 10-8 c) 2.0 10-16 d) 7.1 x 10 e) 5.0 x 1015 2. If 5.0 mL of 1.0 x 10-'M Pb(NO3)2 is added to 5.0 mL of a solution of 1.0 x 10-0MK2Cr04, which...
Question 3 12 pts 3. If the Ksp = 4.0 x 10-5 for PbBr2... (Select] what's the solubility in pure water? V [Select] what is the solubility in 0.100 M NaBr? Next
what is the molar solubility of Pb(OH)2 (Ksp=2.8 x10-17) in a buffer solution containing equal amounts of NH3 and NH4+? Kb=1.8X10 -5
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C. 2. Calculate the molar solubility of CaF2 (Ksp = 4.0 x 10-11) in a 0.025 M NaF solution. 3. 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 (Kop -1.7 x 10-8) precipitate under...
4. Given the Ksp values below: Ksp(BaF2) 2.4 x 10-5 Kappor KspPbF2) = 4.0 x 10-8 KsplSrF2) = 0.8 x 10-10 If I increasingly add NaF to a solution with (Ba2+1=[Pb2')= [Sr2"]=0.01 M, what is the precipitation sequence? a. SrF2 first, then PbF2, and finally BaF2 b. BaF2 first, then PbF2, and finally SrF2 c. Not enough information to tell d. SrF2 first, then BaF2, and finally PbF2
Solubility Product Constants (Ksp at 25 °C) Type Formula Кsp Bromides PbBr2 6.3 x 10-6 AgBr 3.3 * 10-13 Carbonates BaCO3 8.1 x 10-9 CaCO3 3.8 x 10-9 COCO3 8.0 × 10-13 CuCO3 2.5 10-10 FeCO3 3.5 x 10-11 PbCO3 1.5 10-13 MgCO3 4.0 x 10-5 MnCO3 1.8 10-11 NiCO3 6.6 x 10-9 Ag2CO3 8.1 x 10-12 ZnCO3 1.5 x 10-11 Chlorides PbCl2 1.7 x 10-5 AgC1 1.8 10-10 Chromates BaCrO4 2.0 x 10-10 CaCrO4 7.1 x 10-4 PbCr04 1.8...
8. Precipitation calculations with Ni2+ and Pb a. Use the solubility product for Ni(OH)2 o) to calculate the ph at which (OTH)2 begins to precipitate from a 0.18 M Ni2+ solution (3pts). (Ksp Ni(OH)2-5.5x10-16) b. Will Pb(OH) H from a0.18M Pb2 solution (3psa)? (The 2 (o) precipitate at the above p Ks for Pb(OH)2 1.2x10-15) The functional significance of the evolution of a second ventricle (as seen in alligators &their relatives, birds, & mammals) is that a second ventricle allows...
The Ksp for BaSO4 is 1.1 x 10^-10 and that for BaSeO4 is 2.8 x 10^-11. What concentration of [SO4]^-2 and [SeO4]^-2 are needed to precipitate out each salt? Which will precipitate first?
What is the least soluble salt of the following set? Cr(OH)2 with Ksp = 6.7 * 10-31 Pb(OH)2 with Ksp = 1.2 x 10-15 Ba(OH)2 with Ksp = 5.0 x 10-3 Fe(OH)2 with Ksp = 4.9 x 10-17