Example: Calculate the equilibrium concentrations of metal in aqueous and organic phases if 50 cm3 of 0.5 M MCI solution, buffered at pH 2, is mixed with 100 cm3 of pure organic phase (extractant + diluent) that has 1 mol of reaction sites per liter. Assume activity coefficients are 1 and K = 6. %3D conc
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- 0.1 g of the mixture of na2so4 and k2so4 is taken and 100 ml of solution is prepared. 10 ml of this prepared solution is placed in a beaker and some distilled water is added. A mass of 15.5 mg is obtained by precipitation with Bacl2 at PH=5, then filtering and bringing to a constant weight at 800 °C. Calculate the percentages of Na2so4 and K2so4 in the mixture accordingly.Calculate the solubility of BaSO4 with the Ksp = 1.08 x 10-10 ,in an aqueous solution with I = 0.0010 mol kg-1What is the solubility of AgCN (Ksp= 6.0 x 10^-17) in 0.20 M Na2S2O3 solution? Note that silver and the anion S2O3^- 2 can form a complex Ag(S2O3)2^3- which has Kf= 1.3 x 10^21.
- Q: The concentration of the sulphate ion in a mineral water can be determinedby the turbidity which results from the addition of excess BaCl2, to a quantityof measured sample. A turbidometer used for this analysis has been standardisedwith a series of standard solutions of NaSO4. The following resultswere obtained:Standard solution Conc. (SO4)2− (mg/L) Reading of turbidometerS0 0.00 0.06S1 5.00 1.48S2 10.00 2.28S3 15.00 3.98S4 20.00 4.61i. In supposing that a linear relationship exists between the readings takenfrom the apparatus and the sulphur ion concentration, derive an equationrelating readings of the turbidometer and sulphate concentration(method of least squares).ii. Calculate the concentration of sulphate in a sample of mineral waterfor which the turbidometer gives a reading of 3.67.Use systematic treatment of equilibrium to calculate the molar solubility of AgIO3 in an aqueous solution with a pH of 2.00. Ignore activity coefficients. Ksp for AgIO3 is 3.17*10-8 and Ka for HIO3 is 0.17.Hexanoic acid was added to an immiscible biphasic solvent sysem, water and CCl4 at 20.0OC and the equilibrium concentrations of hexanoic acid were determined to be 3.66 g/L in H2O and 67.0 g/L in CCl4. Caluclate the distrubution coeffiecent (D1) of hexanoic acid in CCl4 with respect to water.
- Dissolved 0.273 grams of pure sodium oxalate (NaCO) in distilled water and added sulfuric acid and titration the solution at 70 ° C by using 42.68 ml of KMNO. solution and has exceeded end point limits by using 1.46 ml of standard oxalic acid (HCO) with 0.1024 N Calculate the normlity of KMNO Note that the molecular weight of sodium oxalate (NaCO) = 134 and its equivalent weight = 67One gram of sodium hydroxide (NaOH) is used to adjust the pH of an aqueous solution (200 gallons) thatcontains 10 lbs of finely ground rhodochrosite (MnCO3) ore. Does the NaOH raise or lower the solutionpH? What is the amount of NaOH added in lbs/ton? What is the molarity (mol/l) of the system? Assumingthe NaOH is completely soluble and the system is at room temperature, what is the solid-to-liquid ratio(wt%) of the system?The molar solubility of MgCO3 (Ksp = 3.50 x 10-8) in distilled water at room temperature is ______ M. Titration of a 50.00-mL aliquot of the saturated solution will require ______mL of 0.005000 M HCl to reach the phenolphthalein endpoint.
- The Ksp of CaC2O4 at 298 K is 2.30×10-9. Determine the molar solubility of this salt.Calculate the solubility of the BaSO4 solid in 0.0167 M Ba (NO3) 2 solution, taking into account the activity. (Ksp for BaSO4, activity coefficients for 1.1x10^-10 Ba^2+ and SO4^2- ions are 0.46 and 0.44, respectively)Considering only the equilibrium HgBr21s2 Δ Hg21 1 2Br2, and includingactivity coefficients, calculate the solubility of HgBr2 in 0.050 M NaBr. The ionic strength is due almost entirely to 0.050 M NaBr.