In 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)

ou are tasked with determining a way to identify the following ions in solution: Na+, Ni2+, Ag+, and Pb2+. What techniques would you use to selectively precipitate out the ions and how would you separate the precipitates from the supernatant layers? Your arsenal of compounds to use for the separation is KCl, KCH3COO, and KOH. Clearly define each step.

The Cr3+ concentration in a saturated solution of chromium(III) hydroxide is measured and found to be 1.28×10-8 M. Use this information to calculate a Ksp value for chromium(III) hydroxide.

A sample solution contains two unknown ions. A student did a series of tests on the solution, in the order listed below. If a precipitate formed at any stage, the mixture was filtered and further tests were done on the filtrate. The results are as follows. First test:Second test:Third test:Fourth test: solution is a pink colourNaIO3(aq) added and no precipitate formsflame colour is redNa2CO3(aq) is added and no precipitate forms Two possible ions that the solution contains are   a.lithium and manganese(II) b. strontium and cobalt(II) c. strontium and manganese(II) d. lithium and cobalt(II)

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20 ml of a 100 mg/l phenol solution in water is placed in a vial with 20 ml of a fluorocarbon solvent. The organic phase (fluorocarbon solvent) is immiscible with water. The vial is completely filled with the two phases, thus there is no air or contaminant volatilization. After an hour of agitation, the two phase system reaches equilibrium. The two phases are separated and the fluorocarbon is analyzed for total phenol. The resulting phenol concentration in the organic phase is 16.0 mg/l. Compute the unitless partition coefficient (KF-W) for phenol. Compare your calculation with KF-W obtained from an empirical relationship: log10KF-W 0.71 - 0.862log10 CWsat. KF-W means the partition between the fluorocarbon solvent, F, and water, W. Only typed solution.

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp Does solubility change with pH? highest solubility compound pH = 5 pH = 6 pH = 8 O yes Ba(OH), O no do O yes CuBr O no O yes AgCN O no Explanation Check Rights Reserved Terms of Use Privacy Accessibility O 10:00 O oo o0

For each of the following compounds, decide whether the compound's solubility in aqueous solution changes with pH. If the solubility does change, pick the pH at which you'd expect the highest solubility. You'll find K data in the ALEKS Data tab. sp compound Cu Br Zn S Cal₂ Does solubility change with pH? ο οίο ο yes no yes no yes no pH = 4 highest solubility pH = 5 X pH = 6

A solution contains 7.23×10-3 M ammonium chromate and 7.44×10-3 M ammonium sulfate.Solid silver nitrate is added slowly to this mixture.What is the concentration of chromate ion when sulfate ion begins to precipitate?[chromate] =  M

Select the correct mass balance equation for a saturated solution of CaCl₂ assuming that the ionic species are Ca²+, Cl-, CaCl and CaOH+. (A) (B) (C) (D) O O (A) (B) (C) (D) [CH]+[CaCl] = 2[Ca²+] + 2[CaCl*] + 2[CaOH*] [CI] + [CaCl] = 2 [Ca²+] + [CaCl*] + [CaOH*] [CI]+[CaCl] = [Ca²+] + [CaCl+] + [CaOH+] [CI] = [Ca²+] + [CaOH+]