Acid –Base Titration:
A volume of 128 mL of 0.650 M Ba(OH)2 was required to completely neutralize 50.0 mL of nitric acid solution (HNO3). What is the concentration of the acid solution?
Calculate the molar concentration of Ba2+ ions in a 500.0 mL sample of an unknown aqueous solution if 2.47 g BaSO4 is formed upon the addition of excess Na2SO4?
Stoichiometry of Acid –Base Reactions:
What volume of 0.800 M HCl is required to completely neutralize 35.0 g of Ca(OH)2?
1. Consider 125 mL of CaCl2 solution which has the molarity of 0.140M:
A. How many moles of CaCl2 are present in this solution?
B. How many grams of CaCl2 are present in this solution?
C. What is the concentration of Ca2+ ion?
D. What is the concentration of Cl- ion?
2. When 147 mL of 4.25 M NH3 solution is mixed with 353 mL of H2O, what is the concentration of the final solution?
3. What volume of 6.00 M HCl stock solution is required to prepare 725 mL of 0.120 M HCl?
4. What is the molarity of a solution made from 32.1 g KNO3 dissolved in enough water to make 500.0 mL of solution?
5. How many grams of solute are present in 275 mL of 0.150 M KOH?
In an aqueous solution 31.0 mL of 0.150 M KMnO4 was required to completely oxidize 50.0 mL of H3AsO3. What is the concentration of H3AsO3 solution using the following balanced equation?
+ 2 MnO4-
+ 6 H+ → 2 Mn2+ + 5 H3AsO4 + 3 H2O
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