quiz_and_test_-_student_objectives

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Quiz/Test over Acids, Bases, Salts and Buffers Quiz – Items 1-21 Test – ALL Things to Know and Do: 1. Know the Arrhenius and Bronsted-Lowry definitions of acids and bases. Identify substances as acids and bases using the two definitions. 2. Identify conjugate pairs and amphoteric species. 3. Know the structure of the hydronium and hydroxide ions. 4. Know the significance of Ka and Kb with regards to acid strength. 5. Know the following terms: oxyacid, monoprotic acid, diprotic acid, triprotic acid, organic acid, carboxyl group 6. Identify the strong acids and strong bases. 7. Be able to name acids and bases. 8. Calculate the pH, pOH, [H+], [OH-], Ka, Kb, percent dissociation, and solubility given appropriate information. 9. List the major species in a solution and calculate the concentration of all species. 10. Calculate the pH of a mixture of weak acids. 11. Calculate the pH of polyprotic acids. 12. Explain the difference between a weak acid and its conjugate base. Recognize conjugate pairs and know which is the acid and which is the base. Ex: What is the conjugate base of HCO 3 - ? Ex: What are the conjugate pairs in the following reaction? CH 3 CH 2 CH 2 NH 2 + + H 2 O  CH 3 CH 2 CH 2 NH 2 + H 3 O + 13. Know that NH 3 is ammonia and that it is a weak base. Write the reaction for ammonia in water. Know the conjugate acid of ammonia. 14. Know that amines are weak bases that contain nitrogen (as does ammonia). Solve pH problems involving amines.

15. Use principles of Le Chatelier to explain the common ion effect. Give the direction equilibrium will shift with the addition/removal of a common ion. Ex: Acetic acid is dissolved in water. Then some sodium acetate is added to the acid solution. Write the chemical equation for both processes. What will happen to the acid equilibrium when the salt is added? What will happen to the pH? 16. Given the Ka, calculate the equilibrium concentrations, the percent dissociation and the pH of a weak acid solution. Ex: Calculate the equilibrium concentrations, the percent dissociation and the pH of a .020 M HC 2 H 3 O 2 solution. The Ka of acetic acid is 1.8 x 10 -5 . (Be able to do the same for a weak base.) 17. Given the Ka, calculate the equilibrium concentration, the percent dissociation and the pH of a weak acid/salt solution. Ex: Calculate the equilibrium concentration, the percent dissociation and the pH of a solution that contains .15 M HF and .1 M NaF. The Ka of HF is 7.2 x 10 -4 . 18. Identify salts as acidic, basic or neutral. 19. Write equations for the dissociation of salts and for the hydrolysis of strong conjugate acids and bases of salts. 20. Calculate the pH of salt solutions. 21. Rank acids from strongest to weakest based on structure. 22. Explain what must be present for a buffer to exist. Explain how a buffer can be made. Explain why/how buffers work. 23. Be able to recognize buffers. Ex: Which of the following results in a buffer when equal volumes of each are mixed? A. 0.1 M KOH and 0.1 M CH 3 NH 3 Cl B. 0.1 M KOH and 0.1 M CH 3 NH 2 C. 0.1 M HCl and 0.1 M NaOH D. 0.1 M NaOH and 0.2 M HC 2 H 3 O 2 E. 0.2 M HNO 3 and 0.2 M NaNO 3 F. 0.2 M HNO 3 and 0.2 M HF

G. 0.2 M HNO 3 and 0.4 M CH 3 NH 2 H. 0.2 M CH 3 NH 2 and 0.2 M CH 3 NH 3 Cl 24. Calculate the pH of a buffer solution. Ex: What is the pH of a solution made by adding 50.0 grams of NH 4 Cl to 1.00 L of a 0.75 M solution of NH 3 . The Kb of NH 3 is 1.8 x 10 -5 . 25. Know that the pH =pKa at the half-equivalence point. 26. Calculate the concentration and pH of an acid or base, using titration data. Ex: A. 20.0 mL of HNO 3 are titrated to a phenolphthalein endpoint by 31.57 mL of M of KOH. What is the concentration and pH of the acid solution? B. 25.0 mL of 0.15 M NaOH are required to completely neutralize 10.0 mL of H 2 SO 4 . What is the concentration of the acid? 27. Know the following: buret, standard solution, endpoint, equivalence point, titrant.

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