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Writing Reactions

Writing Reactions. --for unbalanced students. A few things to recall--. Synthesis Decomposition Single replacement Double replacement Other redox. A+B  AB. AB  A+B. A+BC  AC+B Or D+BC  C+BD. AB+CD  AD+BC. AB+CD  a whole bunch of other things. A few things to recall--.

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Writing Reactions

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  1. Writing Reactions --for unbalanced students

  2. A few things to recall-- • Synthesis • Decomposition • Single replacement • Double replacement • Other redox

  3. A+BAB

  4. AB  A+B

  5. A+BC  AC+B Or D+BC  C+BD

  6. AB+CD  AD+BC

  7. AB+CD  a whole bunch of other things.

  8. A few things to recall-- • Metallic oxides and water make hydroxides • M2O+H2O2MOH • MO+H2OM(OH)2 • 2M2O3+3H2O 2M(OH)3

  9. A few things to recall-- • Nonmetallic oxides and water make acids • YO + H2O H2YO2 • YO2 + H2OH2YO3 • YO3 + H2OH2YO4 • 2Y2O5 + H2O2HYO3

  10. A few things to recall-- • In a single replacement reaction—the more reactive element replaces the less reactive • X +MYY +MX means X is a more reactive nonmetal than Y • A + BCB + AC means A is a more reactive metal than B

  11. A few things to recall-- • In a double replacement reaction, you need a molecule or a precipitate formed • AB +CD AD + BC if AD and BC are both soluble salts

  12. A few things to recall-- • Carbonates decompose with heat or acid

  13. A few things to recall-- • In a redox reaction, hydrogen ions and water can be reactants or products.

  14. A few things to recall-- • In a redox reaction, you have to balance the charge as well

  15. A few things to recall-- • Net ionic equations show dissociated ions, spectators are omitted • AB +CD AD + BC, if AD is soluble, • Write: B- +C+ BC

  16. Predict the products • AKA: Descriptive chemistry • You are given to reactants. What products are formed? Go!

  17. Predict the products • Old Rules— • 8 sets, you choose 5 • Don’t balance • Use a net ionic equation • New rules– • Three sets, do all of them • Balance • Use a net ionic equation • Answer a question

  18. Predict the products • We will practice old rules first.

  19. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride.

  20. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. It will burn

  21. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Can only be oxidized

  22. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Look for a precipitate

  23. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Look for a precipitate

  24. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Can be reduced

  25. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Weak base

  26. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. Can be reduced

  27. What do you see? • 1. A piece of solid bismuth is heated strongly in oxygen. • 2. A strip or copper metal is added to a concentrated solution of sulfuric acid. • 3. Solutions of zinc sulfate and sodium phosphate are mixed. • 4. Solutions of silver nitrate and lithium bromide are mixed. • 5. A stream of chlorine gas is passed through a solution of cold dilute sodium hydroxide. • 6. Excess hydrochloric acid solution is added to a solution of potassium sulfite. • 7. Asolution of tin (II) chloride is added to an acidified solution of potassium permanganate • 8. A solution of ammonium thiocyanate is added to a solution of iron (III) chloride. It’s complex

  28. Arrhenius acids and bases • Substances that ionize in water to form H+ ions are acids. • Substances that ionize in water to form OH-ions are bases.

  29. BrØnsted-Lowry Definition • Substances that donate a proton (H+ ion) in a reaction are acids. • Substances that accept a proton (H+ ion) are bases.

  30. Lewis Definition • Substances that accept an electron pair in a reaction are acids. • Substances that donate an electron pair are bases.

  31. Conjugates • After an acid has donated a proton, the rest of the species is the conjugate base. HAA- + H+ • After a base has accepted a proton, the resulting species is the conjugate acid. B- + H+ HB

  32. Please recall: • Strongacids and bases dissociate completely in a water environment. Weak acids and bases do not. • Strong acids= nitric, hydrochloric, sulfuric, hydrobromic, hydroiodic, perchloric • Strong bases-Group 1 & 2 hydroxides—(group 2’s might not dissolve well)

  33. Solubility Rules

  34. We did not use:(but you still have to know) These ions:Precipitate like: • MnO4-, O2-2,CN- ,ClO4-like NO3- • F- like Cl- • Mn+2,Fe+2 like Fe+3 • C2O4-2 like CO3-2 • S-2 like OH- • Hg2+2  like Ag+ • (oxides do not exist in a water solution!)

  35. H+ + OH-H2O • Just remember– One H+ neutralizes one OH- • It’s true for strong and weak acids and bases.

  36. H+ + OH-H2O • Just remember– One H+ neutralizes one OH- • It’s true for strong and weak acids and bases. M1V1=M2V2 Moles of H+ Moles of OH-

  37. A titration • If 23.56 ml of a .115M NaOH solution neutralizes 10.00 ml of HCl solution, what is the concentration of the original acid?

  38. Another titration • If 14.78 ml of a .115M H2SO4 solution neutralizes 25.00 ml of NaOH solution, what is the concentration of the base?

  39. Another titration • If 14.78 ml of a .115M H2SO4 solution neutralizes 25.00 ml of NaOH solution, what is the concentration of the base? Did you catch that?

  40. Dilution • Add more solvent to a solution, the concentration decreases. M1V1=M2V2 Moles of solute Moles of solute

  41. A dilution • If 150 ml of a .30 M NaOH solution is diluted to 250 ml, what is the new concentration of the base?

  42. Another dilution • What volume of solvent must be added to 100. ml of 1.5 M NaCl to make a solution that is .30 M [Cl-]?

  43. Another dilution • What volume of solvent must be added to 100. ml of 1.5 M NaCl to make a solution that is .30 M [Cl-]? Did you catch that? Not “to what new volume must it be diluted?”

  44. “Life is pain, Your Highness.” Wesley, from the Princess Bride by William Goldman

  45. What is [Cl-]? • 150 ml of .2 M NaCl, • 250 ml of .4 M AlCl3 • 200 ml of .35 M MgCl2 and • 100 ml H20 --are mixed (assume volumes are additive, that is, Vfinal=700 ml)

  46. What will happen… ...if you add, to 1.0 L H2O at room temperature, the following substances, in order: 5 g Na(s) 5 g Mg(s) 5 g NaCl(s) 5 g Zn(C2H3O2)2(s) 5 g HCl(g) 5 g H3PO4(l)

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