Consider the 0.01M of the following solutions:
a. 0.01 M NaCl
b. 0.0033 M MgCl2
c. 0.0025 M MgSO4
Calculate the activity coefficient of the ions in each solution
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Consider the 0.01M of the following solutions: a. 0.01 M NaCl b. 0.0033 M MgCl2 c. 0.0025 M MgSO4...
Determine the ionic strength of each of the following solutions: a) 0.05M MgCl2 = b) 0.05M NaCl = c) 0.05M NaOH plus 0.05M MgCl2 (all in the same solution) = d) 0.05M K2SO4 = e) Water that is pH 2 from addition of HCl =
A solution is 0.126 M in KCl, 0.197 M in NaCl, and 0.148 M in MgCl2. What are the molarities of K + (aq), Na+ (aq), Mg2+ (aq), and Cl- (aq) in the solution? Hint: these are all ionic solutes and the salts fully dissociate into ions. Add up the concentrations of each ion that stem from each individual salt and then add them up as appropriate.
Consider the following reaction. MgCl2(aq)+2NaOH(aq)⟶Mg(OH)2(s)+2NaCl(aq) A 166.0 mL solution of 0.381 M MgCl2 reacts with a 47.33 mL solution of 0.568 M NaOH to produce Mg(OH)2 and NaCl. Identify the limiting reactant. NaOH Mg(OH)2 MgCl2 NaCl Caclulate the mass of Mg(OH)2 that can be produced. The actual mass of Mg(OH)2 isolated was 0.559 g. Calculate the percent yield of Mg(OH)2.
Question #2 determine the ionic strength of each of the following solutions (a) 0.05 M MgCl2 ANS= (b) 0.05 M NaCI ANS= (c) 0.05 M NaOH plus 0.05 M MgCl2 (all in the same solution) ANS= (d) 0.05 M K2SO4 ANS= (e) water that is pH 2 from addition of HCI ANS=-
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