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Chemistry Chapter 13.1

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Chemistry Chapter 13.1

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    1. Chemistry Chapter 13.1 OBJECTIVES You will learn how to: Write equations for the dissolution of soluble ionic compounds in water.

    3. Compounds in Aqueous Solution As you have learned, solid compounds can be ionic or molecular. In an ionic solid, a crystal structure is made up of charged particles held together by ionic attractions. In a molecular solid, molecules are composed of covalently bonded atoms held together by intermolecular forces. When they dissolve in water, ionic compounds and molecular compounds behave differently.

    4. Dissociation Dissociation: when a compound that is made of ions dissolves on water, the ions separate from one another. Example: the dissociation of sodium chloride and calcium chloride in water can be expressed by the following equation:

    5. When NaCl dissolves in water, the ions separate as they leave the crystal.

    6. The dissociation of NaCl can be represented as follows.

    7. Write the equation for the dissolution of aluminum sulfate, Al2(SO4)3 , in water.

    9. Practice Write the equation for the dissolution of each of the following in water, and then determine the number of moles of each ion produced as well as the total number of moles of ions produced. a. 1 mol ammonium chloride [NH4Cl(s)] b. 1 mol sodium sulfide [Na2S(s)] c. 0.5 mol barium nitrate [Ba(NO3)2(s)]

    11. 1. Write the equation for the dissolution of Mg(ClO3)2(s) dissolved in water.   Write the equation for the dissolution of NH4NO3 in water.

    12. Precipitate Reactions Ionic compounds can be soluble or insoluble in water. NiCl2, KMnO4, CuSO4, and Pb(NO3)2 are soluble in water. AgCl and CdS are insoluble in water.

    13. Most sodium compounds are soluble. Sodium carbonate, Na2CO3, is soluble because it contains sodium. Its dissociation equation is as follows.

    16. The two possible products of a double-replacement reaction between (NH4)2S and Cd(NO3)2 are ammonium nitrate, NH4NO3, and cadmium sulfide, CdS.

    17. To decide whether a precipitate can form, you must know the solubilities of these two compounds. Consulting Table 14-1, you can see that NH4NO3 is soluble in water. However, CdS is insoluble. You can now predict that when solutions of ammonium sulfide and cadmium nitrate are combined, ammonium nitrate will not precipitate and cadmium sulfide will.

    18. Net Ionic Equations Net ionic equation includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution. To write a net ionic equation, you first convert the chemical equation into an overall ionic equation.

    19. Net Ionic Equations Notice that the ammonium ion, NH4 +, and the nitrate ion, NO3 -, appear on both sides of this equation. Therefore, they have NOT undergone any chemical change and are still present in their original form. Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction are spectator ions.

    20. To convert an ionic equation into a net ionic equation, the spectator ions are canceled on both sides of the equation. Eliminating the NH4 + and NO3 - ions from the overall ionic equation above gives the following net ionic equation.

    21. Identify the precipitate that forms when aqueous solutions of zinc nitrate and ammonium sulfide are combined. Write the equation for the possible double-replacement reaction. Then write the formula equation, overall ionic equation, and net ionic equation for the reaction.

    23. Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the net ionic equation for the reaction. Will a precipitate form if solutions of potassium nitrate and magnesium sulfate are combined? If so, write the net ionic equation for the reaction.

    24. 3. Will a precipitate form if solutions of barium chloride and sodium sulfate are combined? If so, identify the spectator ions and write the net ionic equation. 4. Write the net ionic equation for the precipitation of nickel(II) sulfide.

    25. Homework 13.1 Page 458 #1-13 Make NoteCards Solubility Rules Review packet pg4

    26. 1. Answer: Yes; Ba2+(aq) + SO4 2-(aq) ? BaSO4(s) 2. Answer: No 3. Answer: Yes; Na+ and Cl-; Ba2+(aq) + SO4 2-(aq) ? BaSO4(s) 4. Answer: Ni2+(aq) + S2-(aq) ? NiS(s)

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