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- 1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 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 1.1? Explain you answer in a short sentence.The following evidence was obtained from an experiment to determine the solubility of calcium chloride at room temperature. A sample of saturated calcium chloride solution was evaporated to dryness, and the mass of solid residue was measured.EvidenceVolume of solution (mL) = 15.0Mass of empty beaker (g) = 90.54Mass of beaker and residue (g) = 101.36The solubility of calcium chloride is g/100 mLLactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte.found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs:CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac)and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.
- Lactic acid (CH3 - CH(OH) - COOH) is a weak acid and therefore a weak electrolyte. found in "cut milk". The freezing point of an aqueous solution 0.01 m of lactic acid is 0.0206 ºC. Knowing that in aqueous solution the following equilibrium occurs: CH3 -CH(OH) -COOH(ac) = CH3 -CH(OH) -COO(-)(ac) + H(+)(ac) and that, therefore, there are three species (solutes) in solution, calculate their percentage of ionization.What wt of magnetite should be taken for analysis in order that after converting to a precipitate of Fe2O3.xH2O, the percentage of Fe3O4 in the sample can be found by multiplying the wt in grams of the ignited precipitate (Fe2O3) by 100.The bisulfate (or hydrogen sulfate) anion, HSO4 , is a weak acid. The equilibrium constant for the aqueous acid reaction HSO4 (ag) = H* (ag) + SO,2- (ag) is 1.2 x 10-2 (a) Calculate AG° for this equilibrium. Assume a tempera- ture of 25.0°C. (b) At low concentrations, activity coefficients are approxi- mately 1 and the activity of a dissolved solute equals its molality. Determine the equilibrium molalities of a 0.010-molal solution of sodium hydrogen sulfate.
- A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar anda NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) formixture 1 at 298 K. A second reaction mixture (mixture 2) is prepared at 298 K with a N2O4(g) partialpressure of 0.05 bar and a NO2(g) partial pressure of 0.10 bar. (i) Calculate the reaction Gibbs energy (∆??) for mixture 2 at 298 K. (ii) Comment on the spontaneity of the forward reaction for mixture 1 and mixture 2.Support your answer with the values of ∆?? calculated for the two mixtures. please give solution and answerCalculate 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).Calculate the solubility at 25°C of CuBr in pure water and in a 0.0100M CoBr2 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0100 M CoBr2solution: gL
- A 50.00 mL volume of 0.0600M K2CrO4 is mixed with 50.00 mL 0.0800 M AgNO3. Calculate the concentration of Ag+, CrO42-, K+, and NO3- at equilibrium. The solubility product of Ag2CrO4(s) is 1.20 x 10-12. Please show workCalculate the solubility at 25°C of PbCO3 in pure water and in a 0.0110M PbNO32 solution. You'll find Ksp data in the ALEKS Data tab. Round both of your answers to 2 significant digits. solubility in pure water: gL solubility in 0.0110 M Pb(NO3)2solution: gL1. 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.