Naphthalene is separated in the mixture (methylene blue, sodium chloride and and is converted back to the naphthalene) through the process solid state through filtration, distillation distillation, filtration sublimation, deposition filtration, adsorption
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- Consider a solution that is made from mixing 122.3ml of 0.333M ZnCl2 and 83.57ml of 0.654M Na2CO3 a. What is the concentration of cations and anions at equilibrium(in molarity)? Use x-is-small approximation. b. What is the ‘net’ amount of precipitate produced(in moles)? ksp (ZNCO3) = 1 x 10^-10In an experiment the equilibrium between ethanol, acetic acid, ethyl acetate, and water is studied, and the reaction is catalyzed by the addition of hydrochloric acid. Following mixtures were prepared and titrated with 0.953M NaOH solution to calculate equilibrium constant of the reaction. Mixture 1. 2.5ml 3M HCl+ 2.5ml Water Mixture 2. 2.5mL 3M HCl + 2ml Ethyl Acetate + 0.5ml Acetic Acid End points were reached at 6.68 ml and 24.36 ml, respectively. Calculate the equilibrium constant using mole fractions for the reaction (MWHCl: 36.46g/mol, MWCH3COOH: 60.05g/mol, MWH2O: 18.02g/mol, MWCH3COOC2H5: 88.11g/mol, ρwater = ρHCl =0.998g/ml, ρCH3COOH = 1.05g/ml, ρCH3COC2H5 =0.902g/ml)The Ksp for silver chromate (Ag2CrO4) is 1.1x10-12. Using the same initial set up of 10mL of 1M silver nitrate is combined with 25mL of 0.1M sodium chromate, what is the mass of the silver chromate precipitate in grams?
- The concentration of a pure solid is left out of a equilibrium constant expression but a pure liquid is includedCalcium carbonate (e.g. from limestone) is relatively insoluble in water, and the solubilitydecreases with rising temperature. This is why CaCO3 precipitates out as ‘scale’ in hot watermore readily than cold water. At a temperature of 20oC , calcium carbonate pKs = 8 . 8; at35oC , pKs = 9 . 25. If you had water that was at equilibrium with excess calcium carbonate at20oC and then raised the temperature to 35oC , what is the mass of CaCO3 that will precipitateout per litre of water? Hint: the difference in solubility will drive the reaction back to solid. CaCO3 <-> Ca2+ + CO32-A solution is prepared by combining 20.00ml of 0.150 molar Ba2+ and 25.00ml of 0.125 molar Cl- Using concentrations and volumes above, determine if a precipitate will form when these solutions are mixed at 25C. Provide a calculation to support your answer, keep in mind the system is not at standard state. Ba2+ (aq) -560.77 kJ/mol Delta Gfo Cl- (aq) -131.228 kJ/mol Delta Gfo BaCl2 -1296.32 kJ/mol Delta Gfo
- 25 mL of a saturated solution of K2Cr2O7 was cooled from 90oC to 50oC, how many moles solid will precipitate from solution?Nitrosyl chloride, NOCl, dissociates on heating as shown below. When a 1.50 gram sample of pure NOCl is heated at 350 oC in a volume of 1.00 liter, the percent dissociation is found to be 57.2%. What is the quilibbrium constant?5. For the solubility of a molecule A2B explain how the concentrations of the species A+ and B2- dictate if a precipitate will form or not. Formulate your answer using the idea of the reaction quotient (Q) and Le Chatlier’s principle. (hint: What must be true about the concentrations of these two species with regard to the Ksp for a precipitate to form or not form.)
- After mixing an execess PbCl2 with a fixed amount of water, it is found that the equilibrium concentration of Pb2+ is 1.6 x 10-2 M . What is is Ksp for PbCl2?Solid potassium hydroxide is slowly added to 175 mL of a 0.318 M nickel(II) acetate solution until the concentration of hydroxide ion is 0.0568 M. The percent of nickel ion remaining in solution is __ % Solubility Product Constants (Ksp at 25 oC) Type Formula Ksp Bromides PbBr2 6.3 × 10-6 AgBr 3.3 × 10-13 Carbonates BaCO3 8.1 × 10-9 CaCO3 3.8 × 10-9 CoCO3 8.0 × 10-13 CuCO3 2.5 × 10-10 FeCO3 3.5 × 10-11 PbCO3 1.5 × 10-13 MgCO3 4.0 × 10-5 MnCO3 1.8 × 10-11 NiCO3 6.6 × 10-9 Ag2CO3 8.1 × 10-12 ZnCO3 1.5 × 10-11 Chlorides PbCl2 1.7 × 10-5 AgCl 1.8 × 10-10 Chromates BaCrO4 2.0 × 10-10 CaCrO4 7.1 × 10-4 PbCrO4 1.8 × 10-14 Ag2CrO4 9.0 × 10-12 Cyanides Ni(CN)2 3.0 × 10-23 AgCN 1.2 × 10-16 Zn(CN)2 8.0 × 10-12 Fluorides BaF2 1.7 × 10-6 CaF2 3.9 × 10-11 PbF2 3.7 × 10-8 MgF2 6.4 × 10-9 Hydroxides AgOH 2.0 × 10-8 Al(OH)3 1.9 × 10-33 Ca(OH)2 7.9 × 10-6 Cr(OH)3 6.7 × 10-31 Co(OH)2 2.5 ×…A 500 mL sample of a solution saturated at 25°C with calcium oxalate is evaporated to dryness, giving a 0.00305 gram residue of calcium oxalate. Calculate the solubility product constant for this salt at 25°C.