The lattice enthalpy of KCI is positive, indicating that it takes energy to break the ions apart in KCI. However, the dissolution of KCI in water is an exothermic process. Identify all particle-particle interactions that contribute significantly to the exothermic dissolution process being exothermic. For each interaction, include the particles that interact and the specific type of intermolecular force between those particles.
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- A friend of yours who is taking a biochemistry class saysthat salting out works because the waters of hydration thatsurround the protein prefer to surround the electrolyte asthe electrolyte is added; therefore, the protein’s hydrationshell is stripped away, leading to protein precipitation. Anotherfriend of yours in the same biochemistry class saysthat salting out works because the incoming ions adsorbtightly to the protein, making ion pairs on the protein surface,which end up giving the protein a zero net charge inwater and therefore leading to precipitation. Discuss thesetwo hypotheses. What kind of measurements would youneed to make to distinguish between these two hypotheses?Which of the following statement/s is/are TRUE? The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. The ions interact with the solvent molecules through dipole-dipole interaction. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified. I, II, IV I, III II, III, IV I, II I, II, IIIWhich of the following statement/s is/are TRUE? The Arrhenius Theory cannot be applied to account for the behavior of the molar conductivity of strong electrolytes, since these solutes are completely dissociated, at least in dilute solutions. Debye=Huckel Theory of interionic attraction satisfactorily explains the variation of the molecular conductivity of strong electrolytes with concentration. The ions interact with the solvent molecules through dipole-dipole interaction. When an electric potential is applied across the solution, the ions migrate and the ionic atmosphere around these ions is modified.
- The vapor pressures of 1,2-dibromoethane (M = 187.9 g mol-1and 1,2-dibromopropane (M =201.9 g mol-1), both measured at 343 K, are 12.90 and 9.17 kPa, respectively. Assuming thatthese two liquids form an ideal mixture, calculate the pressure of the vapor phase which is inequilibrium at 343 K with a liquid containing 50 % by mass of each of these componentsMatch the following: Freezing point depressionThe effect of supercoolingFreezing point of pure solventRegion where liquid is coolingRegion where liquid is freezing I have attached a picture for this question. I guessed the answers to be B,D,E,F,A but i am not sure if it is correctA dissolution is prepared dissolving 396 g of sacarose (C12H22O11) in 624 g of water. What is the vapor presurre at 30ºC? The vapor presurre of water at 30ºC is 31.8 torr and sacarose is a non-volatile solute.
- The freezing-point of depression of a 0.010 b acetic acid solution is 0.00193 K. Calculate thedegree of dissociation for acetic acid at this concentration. Cryoscopic constant for the aceticacid is 1.86 K mol kg mol-1.a) For a compound with a molecular weight of 130 g / mol, at a melting temperature of 425.15 K under 1 bar pressure, the solid and liquid phases have a density of 1100 and 1024 kg / m3, respectively. When the pressure is increased to 125 bar, the melting temperature rises to 427.45 K. Calculate the ΔSo and ΔHo values for this compound during the transition from solid to liquid phase.b) Explain why molality is preferred over molarity in applications of numerical (colligative) properties.The density of the solution prepared by dissolving 53.85 g of calcium chloride in 100 g of water at 18 C was measured as 1.3420 g/cm3. Calculate the mass fraction, mole fraction, molasses, molarity and normality of the dissolution.
- A vapour solution with a mole percentage of 10% benzene is cooled gradually. At what temperature does liquid first appear?List 7 real-life applications in Chemical Equilibrium in a Liquid Phase and list 7 real-life applications in Distribution of a Solute between Immiscible Solvents.Water and 1-butanol are only partially miscible, so that when the two liquids are mixed, separate phases are formed. A mixture is prepared, in which the volumes of the aqueous and organic phases are equal. Ethanoic acid is then added to the mixture. The concentration in the aqueous phase is 0.094 mol dm-3 and in the organic phase 0.014 mol dm-3 . Additional solvent is then added such that the volume of the aqueous phase becomes double that of the organic phase. What are the new concentrations?