Posted by Robert on Monday, February 22, 2010 at 1:30pm.
1- How many milliliters of 0.140 M HCl are needed to completely neutralize 42.0mL of 0.106 M Ba(OH)2 solution?
Step 1. Write a balanced equation.
2HCl + Ba(OH)2 ==> BaCl2 + 2H2O
Step 2. How many moles of the base do we have. moles = M x L = 0.106 M x 0.042 L = 0.00445.
Step 3. How many moles of HCl are needed? Use the coefficients in the balanced equation to do this. We have 0.00445 moles Ba(OH)2. It takes twice as much HCl as it does Ba(OH)2; therefore, we must have used 2 x 0.00445 moles HCl = 0.00890 mols HCl.
Step 4. Remember the definition of molarity. M = moles/L. For the HCl we have 0.00890 moles and the molarity is 0.140 M, so solve for L.
L = mols/M = 0.00890/0.140 = 0.0636 L or 63.6 mL.
All of the solution problems are worked the same way. If the problem throws in a solid instead of a solution, just remember that moles = grams/molar mass. After converting into moles, everything is worked the same way. Try it, you'll like it.
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