CHEMISTRY 12 – APPLICATIONS OF ACIDS AND BASES Review KEY F1) Demonstrate an ability to design and analyse a titration experiment 1. Calculate the pH resulting from mixing 35.0 mL of 0.200 M HCl with 75.0 mL of 0.150 M NaOH. (3 marks) 2. What mass of Ca(OH)2(s) must be added to 750 mL of 0.250 M HCl to create a solution with a pH = 3.150? (3 marks) 3. Write the net ionic reaction that occurs when NaOH is titrated with HNO3.
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CHEMISTRY 12 – APPLICATIONS OF ACIDS AND BASES Review KEY
F1) Demonstrate an ability to design and analyse a titration experiment
1. Calculate the pH resulting from mixing 35.0 mL of 0.200 M HCl with 75.0 mL of 0.150 M NaOH. (3 marks)
2. What mass of Ca(OH)2(s) must be added to 750 mL of 0.250 M HCl to
create a solution with a pH = 3.150? (3 marks)
3. Write the net ionic reaction that occurs when NaOH is titrated with HNO3.
4.
5. What does the term end point mean?
6. What is a standardized solution?
7. When titrating HCl with NH3, what indicator should be used and why?
8. In the reaction:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
an equivalence point occurs when 22.74 mL of 0.1893 M NaOH is added
to a 25.00 mL portion of H2SO4.
a. What is the [H2SO4]?
b. What indicator would you choose for the reaction and why?
9. A 25.00 mL of an H3PO4 is titrated using 0.1472 M NaOH. The results
obtained are:
Trial 1 Trial 2 Trial 3
Final Volume 37.89 46.82 39.50
Initial Volume 1.25 10.58 3.24
Calculate the [acid].
10. What is the approximate pH value at the equivalence point for the
following titrations. Draw the titration curves you would see.
A. HCN and KOH
B. HClO4 and LiOH
C. NH3 and HCl
11. Explain why the pH for the titration of CH3COOH and NaOH will not be at
pH 7 at the equivalence point
F2) Describe an indicator as an equilibrium system
12. What is the transition point of an indicator?
13. Consider the following equilibrium for an indicator that changes at a pH of
6-8:
HInd + H2O <—> Ind- + H3O+
yellow blue
a. What colour will be in an acid? Why?
b. What colour will it be in a base? Why?
F3) Perform and interpret calculations involving the pH and Ka for an indicator
14. What is the Ka for the indicator phenolpthalein?
15. Which of the following is/are true at the transition point of an indicator?
A. Ka = [HInd]
B. [HInd] = [Ind-]
C. pH = [HInd]
D. Ka = [H3O+]
E. Ka = Kb
F. pH = pKa
F4) Describe the hydrolysis of ions in salt solutions
16. What hydrolysis reaction will occur when the salt NH4Cl is dissolved in water?
F5) Analyse the extent of hydrolysis in salt solutions and predict whether a salt
solution would be acidic, basic, or neutral (compare Ka and Kb values, if
necessary)
17. Consider the salt NaH2PO4.
a. Write the dissociation reaction
b. Write the hydrolysis reaction
c. Determine if the salt forms an acidic, basic, or neutral solution.
F6) Describe buffers as equilibrium systems
18.
19. Explain the answer to the above question
F7) Describe the preparation of buffer systems
20. Describe how you would make a buffer.
F8) Predict what will happen when oxides dissolve in rain water
21.
22. Which of the following combinations will form a buffer solution.
A. HI and NaI
B. HF and KF
C. NH4Cl and NH3
D. HCN and NaCl
E. KHCO3 and H2CO3
23. What is the approximate pH of normal rainwater? Why?
24. List 2 gases responsible for acid rain and their sources.
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