Acids & Bases Worksheet
1.    Explain the meaning of the terms "strong" and "weak" when applied to acids and bases.
2. Give illustrations of a strong acid, a strong base, a weak acid and a weak base.
3. Phosphoric acid is the acitve ingredient in many commerical rust-removing solutions.  Calculate the volume of concentrated phosphoric aicd (14.6 M) that must be diluted to prepare 500 mL of a 1.25 M solution?
4. How did Arrhenius define and acid and a base?
5. Pure HClO4 is molecular.  Write an equation for its disoolution in water.
6. What is the difference between a strong electrolyte and a weak electrolyte.
7. If asubstance is a weak electrolyte, what does this mean in terms of the tendency of the ions to react to form the molecular compound?  How does this compare with strong electrolytes?
8.  Nitrous acid, HNO2, is a weak acid.  Write an equation showing its reaction with water.
9. Hydrazine is a toxic substance that can be formed when household ammonia is mixed with a bleach such as CloroxTM.  Its formula is N2H4  and it is a weak base.  Write a chemical equation showing its reaction with water.
10. HClO3 is a strong acid.  Write an equation for its reaction with water.
11.   Formic acid, HCHO2, is the substance that is responsible for the painful bites of fire ants.  It is a weak electrolyte and reacts with water in the same manner as acetic acid.  Write a chemical equation that shows its ionization in water.
12. Write the formula for the conjugate bases for each of these acids:

a) HCl;   b) CH4;    c) HSO3-1;     d)   H2SO4;     e) NH3;    f) HClO4
13. Show how each of these acids react with water and forms a conjugate acid-base pair:

a)  HCl;    b)  HNO3;    c) H2SO4;   d) HClO4;   e) H2S;    f)   H3PO4
14. Calculate the molarity of a solution that contains 10 grams of HCl in 100 mL of solution.
15. A solution contains 0.1 mole of HC2H3O2 dissolved in 0.5 L of solution. Calculate the molarity of the solution.
16. 500 mL of a solution contain 0.1 mole of HC2H3O2. The solution is diluted with water to the 1 L mark. Calculate the molarity of the resulting solution.
17. A 250 mL solution of H2SO4 has a strength of 0.2 M. The solution is diluted with water to the 1 L mark. What is the molarity of the solution so formed?
18. If 0.3 mole of acetic acid is present in 150 mL of solution, calculate the molarity of the acid solution.
19. How many moles of acetic acid are required to make 125 ml of a 0.5 M solution.
20. To what volume must 125 mL of a 2 M solution of HCl  be diluted to make the solution 0.05M?
21. What is the concentration of a solution formed by diluting 300 mL of a solution containing 0.1 mole of HCl to 6 L?
22. Give directions for preparing 2.0 L of 0.250 mol/L HCl using 11.7 M HCl.
23. Give directions for preparing 5.00 L of 0.15 mol/L H2SO4 using 18.0 M H2SO4.
24. What volume of 2.00 mol/L HNO3 is needed to yield 10.00 grams of HNO3?
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