Question

# Consider an electrolyte solution formed by the dissociation of the MgCl₂ in pure water at standard temperature 298 K and standard pressure 1.00 bar. You must make 100.0 mL ofa 10.0 mM aqueous solution of MgCl₂. In the lab, only solid magnesium chloridehexahydrate, MgCl₂(H₂O)6, which has a molar mass of 203.3 g/mol, is available for your use. The reported solubility limit of MgCl₂(H₂O)6 is 235 g per 100. mL of water. 5. (a) Regarding MgCl₂, what are the values of the cationic and anionic dissociation stoichiometric coefficients, v4 and v-, respectively? What are the values of the cationic and anionic charge numbers, z+ and z-, respectively? 5. (b) Calculate the mass of MgCl₂(H₂O)6 must be added to 1.00 L of water to obtain the desired 10.0 mM electrolyte solution of magnesium chloride. You may neglect volume changes caused by the addition of MgCl₂(H₂O)6. (c) Determine the value of the ionic strength I in molar units (i.e. express your answerin M) of the electrolyte solution that has been made. d) Calculate the value of the Debye length (i.e. Debye screening length), lambda D = K¹¹, oft his electrolyte solution. 5. (e) Calculate the mean activity coefficient of this electrolyte solution. Briefly justify any equation used in your calculation (one or two sentences). n the given information, estimate the dimensionless solubility product Ksp ofsalt MgCl₂ at standard conditions. Would you expect this value to be highly rate? Briefly comment in one or two sentences.  Fig: 1  Fig: 2  Fig: 3  Fig: 4  Fig: 5  Fig: 6  Fig: 7