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- Calculate the % relative error in solubility by using concentrations instead of activitiesfor Fe(OH)2 in 0.0500 M KNO3 (give the source for thermodynamic solubility).Referring to Fig. 5.8, deduce the molar solubility of (i) NH4Cl, (ii) (NH4)2SO4 in water at 25 °C.Give techniques on how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry.
- Calculate the solubility of the BaSO4 solid in 0.0167 M Ba (NO3) 2 solution, taking into account the activity. (The activity coefficients for BaSO4 Kçç, 1.1 10-10 Ba ++ and SO42- ions are 0.46 and 0.44, respectively)Write the expression for the solubility-product constant for CaF2, and look up the corresponding Ksp value.If 0.454g of thyroxine is dissolved in 10g of benzene, the freezing point of the solution could be measured as 5.144 C. Pure benzene freezes at 5.444C and has a value for the molal freezing point depression constant of Kf of 5.12C/m. What is the approximate molar mass of thyroxine?
- The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?I have a question. If the solubility product of CaF2 is 1.46 x 10 ^-10 mol3 dm^-9, what mass of calcium fluoride will dissolve in 500 cm3 of 0.10mol dm-3 sodium fluoride solution? The molar mass of CaF2 would be 78.1g mol^-1what is the purpose of preparing of a standard sodium hydroxide solution in determination of purity of impure KHP?
- 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)Explain how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry.1. The Ksp of Ca3(PO4)2 is 1.3 × 10−26. Estimate the solubility of this salt in units of g. L−12. If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence.