(Example One) 500 mL of 0 250 M HC 2 H 3 O 2 and 300 mL of 0 100 M Ba(OH) 2 Net Ionic Equation HC 2 H 3 O 2 O H C 2 H 3 O 2 H 2 O HC 2 H 3 O 2 Ba 2 OH C 2 H 3 O 2 H 2 O Initial mmol 125 30 0 60 0 0 N A Change mmol 60 0 0 0 60 0 60 0 60 0 Final mmol 65 30 0 0 0 60 0 N A Final Molarity 0 081 0 0375 0 0 0 0750 N A (no molarity is calculated for H 2 O because it is the solvent) (Example 2) 50 0 mL of 0 100 M Ba(OH) 2 and 75 0 mL of 0 200 M H 2 SO 4 Net Ionic Equation Two reactions occur First H OH H 2 O Second Ba 2 SO 4 2 BaSO 4(s) Ba 2 OH H SO 4 2 BaSO 4 H 2 O Initial mmol 5 00 10 0 30 0 15 0 0 N A Change mmol 5 00 10 0 10 0 5 00 5 00 10 0 Final mmol 0 00 0 0 20 0 10 0 5 00 N A Final Molarity 0 00 0 0 0 160 0 0800 N A N A (no molarity is calculated for BaSO 4 because it is a solid and therefore not in solution) Using net ionic equations and solution stoichiometry, calculate the molarity of the principal substances (ions and or molecules) in solution, or the number of millimoles of insoluble species (solids or gases) present after the following are mixed YOU MUST USE A TABLE FORMAT AS SHOWN ON THE EXAMPLE PROBLEMS 1 ) 1 00 L of 0 200 M Na 2 SO 4 and 2 00 L of 0 100 M K 2 CO 3

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(Example One): 500. mL of 0.250 M HC 2 H 3 O 2 and 300. mL of 0.100 M Ba(OH) 2 : Net Ionic Equation:

(Example One): 500. mL of 0.250 M HC₂H₃O₂ and 300. mL of 0.100 M Ba(OH)₂:

Net Ionic Equation: HC₂H₃O₂ + O H^- -------> C₂H₃O₂^- + H₂O

	HC₂H₃O₂	Ba²⁺	OH^-	C₂H₃O₂^-	H₂O
Initial mmol	125	30.0	60.0	0	N/A
Change mmol	-60.0	0.0	-60.0	+60.0	+60.0
Final mmol	65	30.0	0.0	60.0	N/A
Final Molarity	0.081	0.0375	0.0	0.0750	N/A

(no molarity is calculated for H₂O because it is the solvent)

(Example 2): 50.0 mL of 0.100 M Ba(OH)₂ and 75.0 mL of 0.200 M H₂SO₄:

Net Ionic Equation: Two reactions occur

First: H⁺ + OH^- -------> H₂O

Second: Ba²⁺ + SO₄^2- ------> BaSO_4(s)

	Ba²⁺	OH^-	H⁺	SO₄^2-	BaSO₄	H₂O
Initial mmol	5.00	10.0	30.0	15.0	0	N/A
Change mmol	-5.00	-10.0	-10.0	-5.00	+5.00	+10.0
Final mmol	0.00	0.0	20.0	10.0	5.00	N/A
Final Molarity	0.00	0.0	0.160	0.0800	N/A	N/A

(no molarity is calculated for BaSO₄ because it is a solid and therefore not in solution)

Using net ionic equations and solution stoichiometry, calculate the molarity of the principal substances (ions and/or molecules) in solution, or the number of millimoles of insoluble species (solids or gases) present after the following are mixed: YOU MUST USE A TABLE FORMAT AS SHOWN ON THE EXAMPLE PROBLEMS

1.) 1.00 L of 0.200 M Na₂SO₄ and 2.00 L of 0.100 M K₂CO₃