A 0.0251-L sample of a solution of \(\mathrm{Cu}^{+}\) requires 0.0322 L of 0.129M \(\mathrm{KMnO}_{4}\) solution to reach the equivalence point. The products of the reaction are \(\mathrm{Cu}^{2+}\) and \(\mathrm{Mn}^{2+}\). What is the concentration of the \(\mathrm{Cu}^{2+}\) solution?
Text Transcription:
Cu^+
Cu^2+
KMnO_4
Mn^2+
CHM 031 Chemical Equilibria in Aqueous Systems Chapter 11 Notes Chapter 11 Solutions: Properties and Behavior 11.2 Energy Changes during Formation and Dissolution of Ionic Compounds ❏ Enthalpy of solution (ΔH solution the overall energy change when a solute is dissolved in a solvent ❏ Enthalpy of hydration (ΔH hydration the energy change when gas-phase ions dissolve in a solvent ❏ Lattice energy (U) - the enthalpy change that occurs when 1 mole of an ionic compound forms from its free ions in the gas phase ❏ Born-Haber cycle - a series of steps with corresponding enthalpy changes that describes the formation of an ionic solid from its constituent elements 11.3 Vapor Pressure of Solutions ❏ Raoult’s law - the principle that the vapor pressure of the solvent in a solution is equal to the vapor pressure of the pure solvent multiplied by the mole fraction of the solvent in the solution ❏ Ideal solution - a solution that obeys Raoult’s law 11.4 Mixtures of Volatile Solutes ❏ Fractional distillation - a method of separating a mixture of compounds on the basis of their different boiling points 11.5 C olligative Properties of Solutions ❏ Colligative properties - characteristics of solutions that depend on the concentration and not the identity of particles dissolved in the solvent ❏ Molality (m) - concentration expressed as the number of moles of solute per kilogram of solvent ❏ Van ‘t Hoff
