A solution is 1×10-4 M in NaF, Na,S, and Na3PO4 What would be the order of precipitation as a source of Pb2* is added gradually to the solution? - The relevant Ken values are: sp Kgp(PbF,) Ksp(PbS) Ksp[Pb3(PO,)2] = 1 x 10-54 = 4 x 10-8 = 7 x 10-29 %3D
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- The Ksp for PbI2(s) is 1.4 × 10-8. Calculate the solubility of PbI2(s) in 0.061 M NaI.How many grams of PbF2 (molar mass = 245.2) will dissolve in 700 mL of 0.60 M NaF solution? The Ksp for PbF2 is 2.69e-08.A. Calgon conditioning can be done by____________________________.B. The colour of metal-EBT complex is ___________________________ .C. If P is less than half M (or T) then alkalinity is due to _____________________.D. Hydroxide alkalinity is determined by ____________________ indicator.E. If sample water contains Mg(HCO3)2 = 14.6 mg/lit, Ca(HCO3)2 = 16.2 mg/lit, MgCO3 = 8.4mg/lit. The temporary hardness present per litre of the sample is__________________.
- Janine's research focuses on the ability of quercetin, a flavonoid and natural dye, to detect the presence of Co2+ in wastewater samples. She prepared a set of calibration standard solutions by adding an excess of quercetin to solutions of varying Co2+ concentration and maintaining it at pH 6.4 using a Tris-HCl buffer. The reaction yields a colored complex solution that has a maximum absorbance at 440 nm:Co2+ + 2 Quercetin --> Co(Quercetin)22+ The absorbance measurements for the calibration solutions prepared are shown in the tables; a cuvette with a 2.50 cm path length was used. [Co2+], in M Absorbance Color Wavelength range (nm) 0.05 0.100 Red 625-740 0.10 0.166 Orange 590-625 0.20 0.285 Yellow 565-590 0.30 0.367 Green 490-565 0.40 0.454 Blue 440-490 0.50 0.571 Violet 380-440 Part of her research is to determine the extent of Co2+ pollution in a stream near a pharmaceutical company. She obtained a 50.0-mL sample of the stream water and buffered it to pH 6.4. She…Calculate the solubility of Au2CrO4 in a 0.13 M solution of Na2CrO4. Ksp for Au2CrO4 is 7.3x10^-40Silver carbonate has a Ksp = 9.05×10-10 and a solubility of 0.0006093 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×10-10 M? [AgNO3] = ____ M
- The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14. When Na2CO3 is added dropwise to a solution containing 0.010 M Co2+ and 0.010 M Pb2+, which ion will precipitate first? What must the [CO32–] be so that the first ion to precipitate comes out of solution, but the second ion does not?Calculate the molar solubility of Ag2S (pKsp = 48.70) in a solution maintained at pH 9.00 and where the concentration of ammonia is 0.200 M.H2S: Ka1 = 1.0 x 10-7, Ka2 = 1.2 x 10-15[Ag(NH3)2]+ : Kf1 = 2.04 x 103, Kf2 = 8.13 x 103The value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?
- (a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/LDetermine the solubility of KIO4 in water. Volume of saturated KIO4 in conical flask is 25.0 ml,KI is 2g,H2SO4 (3.0M) is 20.0 ml added to KI solution , volume of 0.200 M sodium thiosulphate used for titration is 8.00 ml.and if mean ionic activity co efficient,y+- of KIO4 in the saturated solution is 0.85 ,what is Ksp. .CuBr is dissolved in water and the following concentrations were found: [Cu+]=1.06*10^-6 M and [Br-]=1.06*10^-6 M. What is the ion product Ksp of the solution?