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Assume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere.

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Presentation on theme: "Assume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere."— Presentation transcript:

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4 Assume that an aqueous solution of a cation, represented as a red sphere, is allowed to mix with a solution of an anion, represented as a yellow sphere. Three possible outcomes are represented by boxes (1)–(3): 4.24 Which outcome corresponds to each of the following reactions? (a) 2 Na  (aq)  CO 3 2  (aq) (b) Ba 2  (aq)  CrO 4 2  (aq) (c) 2 Ag  (aq)  SO 3 2  (aq)

5 Assume that an aqueous solution of a cation, represented as a blue sphere, is allowed to mix with a solution of an anion, represented as a green sphere, and that the following result is obtained: 4.25 Which combinations of cation and anion, chosen from the following lists, are compatible with the observed results? Explain. Cations: Na , Ca 2 , Ag , Ni 2  Anions: Cl , Ca 3 2 , CrO 4 2 , NO 3 

6 Assume that an aqueous solution of OH , represented as a blue sphere, is allowed to mix with a solution of an acid H n A, represented as a red sphere. Three possible outcomes are depicted by boxes (1)–(3), where the green spheres represent O n , the anion of the acid: 4.26 Which outcome corresponds to each of the following reactions? (a) HF  OH  H 2 O  F  (b) H 2 SO 3  2 OH  2 H 2 O  SO 3 2  (c) H 3 PO 3  2 OH  3 H 2 O  PO 4 3 

7 The concentration of an aqueous solution of NaOCl (sodium hypochlorite; the active ingredient in household bleach) can be determined by a redox titration with iodide ion in acidic solution: Ocl  (aq)  2 I  (aq)  2 H  (aq) Cl – (aq)  I 2 (aq)  H 2 O(l) Assume that the blue spheres in the buret represent I  ions, the red spheres in the flask represent Ocl  ions, the concentration of the I  ions in the buret is M, and the volumes in the buret and the flask are identical. What is the concentration of NaOCl in the flask? What percentage of the I  solution in the buret must be added to the flask to react with all the OCl  ions? 4.27

8 Assume that the conductivity of a solution depends on the total concentration of dissolved ions and that you measure the conductivity of three different solutions while carrying out titration procedures: (a) Begin with 1.00 L of M KCl, and titrate by addition of M AgNO 3. (b) Begin with 1.00 L of M HF, and titrate by addition of M KOH. (c) Begin with 1.00 L of M BaCl 2 and titrate by addition of M Na 2 SO 4. Which of the following graphs corresponds to which titration? 4.28

9 Based on the positions in the periodic table, which of the following reactions would you expect to occur? (a) Red   Green Red  Green  (b) Blue  Green  Blue   Green (c) Red  Blue  Red   Blue 4.29


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