2- a. Find the conditional formation constant for Mg(EDTA)² at pH 9.00. b. Find the concentration of free Mg²+ in 0.050 M Na2 [Mg(EDTA)] at pH 9.00.
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- The Ksp of Al(OH)3 (MM: 78) is 1.90 xx 10^(-33). a) What is the molar solubility of Al(OH)3?What effect would it have on calculated value of Ksp if insufficient time was allowed for the Ca(IO3)2 solution to reach equilibrium?The Ksp of Pb(OH)2 at 25 °C is 1.4 x 10-15. What concentration of NaOH will commence precipitation of Pb(OH)2(s) from a solution that contains 0.025 mol L-1 Pb2+(aq) ion?
- On titrating 50 ml of 0.01 M KI with 0.01 M AgNO3 . The value of pAg after addition of 30 ml AgNO3 is ...................................................................... ( Ksp= 5.2 xl0 -13 )Following the monograph procedure, determine the weight in grams of sodium carbonate (MW-106 g/mol) used to standardize a 0.987 N sulfuric acid solution. 1. What specific type of titration is involved? A. Direct Acidemetry B. Direct Alkalimetry C. Residual Acidemetry D. Residual Alkalimetry 2. What is the analyte- titrant chemical reaction involved? A. Strong Base+Weak Acid B. Weak Acid+Strong Base C. Strong Acid+Weak Base D. Weak Base+Strong Acid 3. What is the preferred indicator for the chosen type of reaction above? A. Methyl Orange B. Penolphtalein C. Methyl Red 4. Consider that the burette was completely filled to the 0mp mark before titrating. What is the volume of titrant consumed based from the image below? A. 22.9 mL B. 22.2 mL C. 21.3 mL D. 22.7 mL 5. What is the unknown weight (grams) the problem? Your Answer:Calculate the solubility of lead(II) sulfate (Ksp = 2.53x10-8) in a 0.0034 M solution of sodium sulfate. Give your answer to three sig. figs. and in exponential form (e. g. 1.23E-3).
- For a solution in which m is 5.0 x 10-2, calculate Ksp for a. AgSCNb. La(IO3)3c. PbI2d. MgNH4PO4Construct a titration curve (pCl^- vs. Vtitrant) for the titration of 25.0 mL of 0.100 M Cl^– solution with 0.100 M AgNO3. MS Excel® can be used. Titrant volumes: 0.00 mL, 10.00 mL, 15.00 mL, 20.00 mL, 25.00 mL, and 30.00 mL.AgCl: Ksp = 1.82 x 10^-10Use the data below to determine the % by mass of Fe to TWO decimal places, if a 0.02 M KMnO4 solution was used for the titration. gH * + MnO 4 + 5Fe 2+ -> SFe 3+ + Mn 2+ + 4H 20 (MM Fe = 56 a/moll mass of iron compound (g) 0.604 initial buret reading (mL) 0.94 Tinal buret reading (mL 16.21