Name of Anion. (aq) NaCl NaNO 3 NaOH Na 2 SO 4 Na2CO3. MgSO4. AgNO 3. Ba(NO 3 ) 2. Pb(NO 3 ) 2. CuSO (1) AgNO 3 ( ) + NaCl( )

Transcription

1 Name of Compound Prelab #1 Formula Cation (Metal) Name of Cation silver nitrate Ag Ag + silver magnesium sulfate barium nitrate lead nitrate copper sulfate Cation = (+)positive ion Anion = ()negative ion Anion (nonmetal) Name of Anion nitrate Data Table (aq) NaCl Na NaOH Na 2 SO 4 Na2CO3 MgSO4 Ag Ba( ) 2 Pb 2+ NO3 Pb 2+ Pb 2+ Pb( ) 2 CuSO 4 Pb 2+ Pb 2+ If ppt: note whether solid color, cloudy, speckles, chunky, etc. Data Table (aq) NaCl Na NaOH Na 2SO 4 Na 2CO 3 MgSO 4 ppt. Ag ppt. ppt. Ba() 2 ppt. ppt. Pb() 2 ppt. ppt. When finished: Rinse off plastic transparency Dry Bring transparencies, grids, and chemicals back to front Inventory all 10 chemicals. Missing any? Report to Mr. R. Return to desk Do #3 Don't hate! Don't contaminate! CuSO 4 ppt. If ppt: solid color, cloudy, speckles, chunky, etc. Click 'n Drag: N/R ppt. N/R = No Reaction ppt. = precipitate(s) Data Table: Results 3. (1) Ag ( ) + NaCl( ) (aq) NaCl Na NaOH Na 2 SO 4 Na 2 CO 3 MgSO 4 ppt. Ag ppt. ppt. ppt. Ba( ) 2 ppt. ppt. ppt. Pb( ) 2 ppt. ppt. ppt. CuSO 4 ppt. ppt. If ppt: solid color, cloudy, speckles, chunky, etc. (2) MgSO 4 ( ) + NaOH( ) SOLUBILITY RULES (look at negative ion in the products) A. Soluble Salts (s) 1. Alkali metals (column IA Na +, K +...) and ammonium NH4 + form soluble (aq) salts 2. Nitrate form soluble salts (NO3 ) 3. Chloride(Cl ), Bromide(Br ), and Iodide(I ) generally soluble exceptions with Pb 2+, Hg2 2+, Cu +, Ag + 4. Sulfate generally soluble except insoluble BaSO4, SrSO4, PbSO4 only slightly soluble Ag2SO4, CaSO4, Hg2SO4 B. Insoluble Salts with cations other than alkali (ex. Na +, K + ) and ammonium NH4 +, 1. Sulfides usually insoluble except with Mg 2+, Ca 2+, Sr 2+, Ba Oxides usually insoluble except with Sr 2+, Ba 2+ soluble and Ca 2+ only slightly 3. Hydroxides usually insoluble except withsr 2+, Ba 2+ and Ca 2+ only slightly 4. Chromates usually insoluble except with Mg Phosphates and Carbonates usually insoluble 1

2 TOTAL NET Do steps #14 for the reaction between barium nitrate and sodium hydroxide. Use structural formulas to sketch the reactants and products. Word equation barium nitrate + sodium hydroxide barium hydroxide + sodium nitrate SOLUBILITY RULES A. Soluble Salts 1. Alkali metals (column IA Na +, K +...) and ammonium NH4 + form soluble salts 2. Nitrate form soluble salts (NO3 ) 3. Chloride(Cl ), Bromide(Br ), and Iodide(I ) generally soluble exceptions with Pb 2+, Hg2 2+, Cu +, Ag + 4. Sulfate generally soluble except insoluble BaSO4, SrSO4, PbSO4 only slightly soluble Ag2SO4, CaSO4, Hg2SO4 B. Insoluble Salts with cations other than alkali (ex. Na +, K + ) and ammonium NH4 +, 1. Sulfides usually insoluble except with Mg 2+, Ca 2+, Sr 2+, Ba Oxides usually insoluble except with Sr 2+, Ba 2+ soluble and Ca 2+ only slightly 3. Hydroxides usually insoluble except withsr 2+, Ba 2+ and Ca 2+ only slightly 4. Chromates usually insoluble except with Mg Phosphates and Carbonates usually insoluble total ionic equation: net ionic equation: total ionic equation: net ionic equation: TOTAL / ONIC 2

3 TOTAL NET Copper (II) sulfate reacting with sodium hydroxide. Directions: 1. Write the predicted products in words. 2. Write the formulas. 3. Identify the insoluble precipitate. 4. Balance the equations. 5. Write the total ionic equation 6. Write the net ionic equation Copper (II) sulfate reacting with sodium hydroxide. 1 2 Copper sulfate + sodium hydroxide > ( ) + ( ) > ( ) + ( ) 7 Total ionic equation ( )+ ( )+ ( )+ ( ) > ( )+ ( )+ ( ) 15 Net ionic equation ( ) + ( ) > ( ) 19 Directions: 1. Write the predicted products in words. 2. Write the formulas. 3. Identify the insoluble precipitate. 4. Balance the equations. 5. Write the total ionic equation 6. Write the net ionic equation 5. How does the Ksp of the soluble compounds compare to the Ksp of the insoluble precipitates? Explain to show your understanding of dissolving, Ksp, and equilibrium. Explain why ionic compounds differ in their solubilities in water. Use Ksp to explain the formation of the precipitate. 6. Select one of the reactions that formed a precipitate. a. Draw a visual representation of each of the reactants and the products in the mix. Show the ions in each. b. Use a collision model to explain the reaction. Include relative attractions between the ions and the water molecules. c. What ions were unchanged in the reaction? Explain. These ions are the spectator ions. d. Write an equation to show the ions that have combined to form a precipitate. This is a net ionic equation. The net ionic equation omits the spectator ion. e. Compare the Ksp of the precipitate to the Ksp of the ionic compounds that are soluble. 3

4 Chem Lab 4.notebook May 09, 2014 calcium hydroxide + hydrogen phosphate > calcium phosphate + hydrogen hydroxide 6. Select one of the reactions that formed a precipitate. a. Draw a visual representation of each of the reactants and the products in the mix. Show the ions in each. b. Use a collision model to explain the reaction. Include relative attractions between the ions and the water molecules. c. What ions were unchanged in the reaction? Explain. These ions are the spectator ions. d. Write an equation to show the ions that have combined to form a precipitate. This is a net ionic equation. The net ionic equation omits the spectator ion. e. Compare the Ksp of the precipitate to the Ksp of the ionic compounds that are soluble. 1/16/13 (in words) potassium carbonate + barium chloride > On the worksheet: Balance 5 equations Pick one: total, net ionic equation 1/17/13 (in words) Complete and balance the equation: Al2(SO4)3(aq) + KOH(aq) > potassium carbonate + barium chloride > On the worksheet: Write the Total Ionic Equation show the ionic compounds in solution as separated ions: Balance 5 equations > Pick one: total, net ionic equation 1/17/13 Write the Net Ionic Equation eliminate the spectator ions summarize reaction to show what changed > Description (in words) Drawing The Reactants Two solutions, aluminum sulfate an dissolved in water, the ionic bond b postive ions are attracted to the neg (hydrogenend) of water molecules. because the ions are so small and ra One of the Products Insoluble precipitate The Other Product soluble compound 4

5 Two solutions, aluminum sulfate and potassium hydroxide, form a cloudy precipitate when mixed. When these ionic compounds are dissolved in water, the ionic bond breaks and the ions dissocate (split up). The ions are then attracted to polar water molecules. The postive ions are attracted to the negativeend (the oxygenend) of water molecules and the negative ions are attracted to positiveend (hydrogenend) of water molecules. The iondipole atractions allow the ions to remain in solution. The solutions appear clear because the ions are so small and randomly distributed in the solution. Yesterday's worksheet (side 2): pick 3 reactions write total & net ionic equations Describe and draw one of the three reactions (just like today's worksheet) Lab 4 Practice Name period Finish the word equation. Write the formula equation below the words. You will need to write the correct formula using the charges on the ions. THEN balance the equation to show conservation of ions. Fill in (s) or (aq) for each. Write the total ionic equation by showing the ions split up (if they are in solution) and leave the ions together (if they are a solid). Write the net ionic equation. Cross out the spectator ions (ions that were attracted to water before and after) in the total ionic equation to show only the ions that change. nickel (II) bromide + sodium carbonate nickel (II) carbonate solid + sodium bromide Write the total ionic equation. Write the net ionic equation. SOLUBILITY RULES A. Soluble Salts 1. Alkali metals (column IA Na +, K +...) and ammonium NH4 + form soluble salts 2. Nitrate form soluble salts (NO3 ) 3. Chloride(Cl ), Bromide(Br ), and Iodide(I ) generally soluble exceptions with Pb 2+, Hg2 2+, Cu +, Ag + 4. Sulfate generally soluble except insoluble BaSO4, SrSO4, PbSO4 only slightly soluble Ag2SO4, CaSO4, Hg2SO4 B. Insoluble Salts with cations other than alkali (ex. Na +, K + ) and ammonium NH4 +, 1. Sulfides usually insoluble except with Mg 2+, Ca 2+, Sr 2+, Ba Oxides usually insoluble except with Sr 2+, Ba 2+ soluble and Ca 2+ only slightly 3. Hydroxides usually insoluble except withsr 2+, Ba 2+ and Ca 2+ only slightly 4. Chromates usually insoluble except with Mg Phosphates and Carbonates usually insoluble Lab #4 worksheet Name period Predicting the Products of Double Replacement Reactions Directions: 1. Write the predicted products in words. 2. Write the formulas. 3. Identify the insoluble precipitate. 4. Balance the equations. P to Ag (aq) + NaCl(aq) Ag Cl ( ) + Na ( ) 1. aluminum sulfate + calcium phosphate > 4. Identify solid precipitate (ppt.) and aqueous sol'n (use "Solubility Rules") 5

6 5. How does the Ksp of the soluble compounds compare to the Ksp of the insoluble precipitates? Explain to show your understanding of dissolving, Ksp, and equilibrium. Explain why ionic compounds differ in their solubilities in water. Use Ksp to explain the formation of the precipitate. 6. Select one of the reactions that formed a precipitate. a. Draw a visual representation of each of the reactants and the products in the mix. Show the ions in each. b. Use a collision model to explain the reaction. Include relative attractions between the ions and the water molecules. c. What ions were unchanged in the reaction? Explain. These ions are the spectator ions. d. Write an equation to show the ions that have combined to form a precipitate. This is a net ionic equation. The net ionic equation omits the spectator ion. e. Compare the Ksp of the precipitate to the Ksp of the ionic compounds that are soluble. For #6, Do reaction #2: MgSO 4 (aq) + NaOH (aq) Example: Ag (aq) + NaCl(aq) AgCl (s) + Na (aq) For #6, Do reaction #2: MgSO 4 (aq) + NaOH (aq) Na + Ag+ Cl Na + Ag Cl Complete the word equation, write the balanced equation, and determine solubilities A. Ca(OH) 2+ H 3PO 4 B. K 2CO 3 + BaCl 2 C. Cadmium (II) phosphate + ammonium sulfide Cd 3 (PO 4 ) 2 + (NH 4 ) 2 S 4. Identify solid precipitate (ppt.) and aqueous sol'n (use "Solubility Rules") Worksheet- Solutions 1. aluminum iodide + mercury(ii) chloride aluminum chloride + mercury(ii) iodide 2AlI3 + 3HgCl2 2AlCl3 + 3HgI2(s) 2. silver nitrate + potassium phosphate silver phosphate + potassium nitrate 3AgNO3 + K3PO4 Ag3PO4(s) + 3KNO3 3. copper(ii) bromide + aluminum chloride copper(ii) chloride + aluminum bromide 3CuBr2 + 2AlCl3 3CuCl2(s) + 2AlBr3 4. calcium acetate + sodium carbonate calcium carbonate + sodium acetate Ca(C2H3O2)2 + Na2CO3 CaCO3(s) + 2NaC2H3O2 5. ammonium chloride + mercury(i) acetate ammonium acetate + mercury(i) chloride 2NH4Cl + Hg2(C2H3O2)2 2NH4 C2H3O2 + Hg2Cl2(s) 6. calcium nitrate + hydrochloric acid calcium chloride + nitric acid Ca(NO3)2 + 2HCl CaCl2 + 2HNO3 N/R 7. iron(ii) sulfide + hydrochloric acid iron(ii) chloride + hydrogen sulfide (g) FeS + 2HCl FeCl2 + H2S 8. copper(ii) hydroxide + acetic acid copper(ii) acetate + water Cu(OH)2 + 2HC2H3O2 Cu(C2H3O2)2 + 2H2O 9. calcium hydroxide + phosphoric acid calcium phosphate + water 3Ca(OH)2 + 2H3PO4 Ca3(PO4)2 + 6H2O 10. calcium bromide + potassium hydroxide calcium hydroxide + potassium bromide CaBr2 + 2KOH Ca(OH)2 + 2KBr 6