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Catalyst

Catalyst. Write the Molecular, Total Ionic, and Net Ionic Reactions for the chemical reactions below: AgSO 4 + K 3 PO 4  Reacting Magnesium Sulfate and Lithium Fluoride. GRADE!. Catalyst. Pick up Papers from the front

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Catalyst

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  1. Catalyst • Write the Molecular, Total Ionic, and Net Ionic Reactions for the chemical reactions below: • AgSO4 + K3PO4 • Reacting Magnesium Sulfate and Lithium Fluoride

  2. GRADE!

  3. Catalyst • Pick up Papers from the front • Calculate the actual yieldof Potassium Sulfate if you started with 15 g of Silver (II) Sulfate and excess Potassium Phosphate, which produced Potassium Sulfate at a 75% yield. • Use the following equation: • AgSO4 + K3PO4 Ag3(PO4)2 + K2SO4

  4. BIG GOAL

  5. Explosion! (3 MINUTES) ? ? ? ? ? ? ? ? ? ? ?

  6. Explosion Questions • What is the formula for density? • Give an example of a chemical property. • Give an example of a physical property. • What is the law of conservation of mass? • What is the law of definite proportions? • What is the law of multiple proportions? • Who discovered the electron? • What are the three types of radiation? • Which particle is the biggest? • Which is the smallest? • Who is Ernest Rutherford? • How do you find the number of neutrons? • What is an isotope? • What is the formula for Nitrite? • What is the formula for Perchlorate? • What is the formula for Hyposulfite? • What is the empirical formula? • What is the molecular formula? • What is the limiting reagent? • What is the excess reagent? • What is the % yield? • What is % composition? • What does it mean to be aqueous? • Name 3 strong acids • Name 3 Strong bases

  7. How to Remember Solubility RULES! Always Soluble: CASH – N – GIA C: Chlorates A: Ammonium S: Sulfates – CBS/PBS H: Halogens – F: CBS-PM Cl/Br/I: HAPpy N: Nitrates GIA: Group 1A

  8. How to Remember Solubility RULES! Always Soluble: kNights can take on anything Acetate : the Ace I ClBr except Silver Lead and Mercury C: Chlorates A: Ammonium S: Sulfates – CBS/PBs H: Halogens – F: CBS-PM Cl/Br/I: HAPpy N: Nitrates GI: Group 1 A: Acetates

  9. Acid/Base Reactions

  10. Acid/Base Reactions: form a SALT and WATER as the only products HA + BOH  BA + H2O Bronsted Lowry Acid Definition: Proton donor Base Definition: Proton Acceptor

  11. MUST REMEMBER: STRONG electrolytes (acids and bases) dissociate completely, weak electrolytes Do NOT! ALWAYS WRITE THESE EQUATIONS IN NET IONIC REACTION FORM!

  12. Example Equations: Hydrochloric Acid reacts with Sodium Hydroxide Remember: Write the NET IONIC Equation!

  13. Identify the Type of Reaction below: 1)  Does your reaction have oxygen as one of it's reactants and carbon dioxide and water as products? If yes, then it's a combustion reaction 2)  Does your reaction have two (or more) chemicals combining to form one chemical? If yes, then it's a synthesis reaction 3)  Does your reaction have one large molecule falling apart to make several small ones? If yes, then it's a decomposition reaction 4)  Does your reaction have any molecules that contain only one element? If yes, then it's a single displacement reaction 5)  Does your reaction have water as one of the products? If yes, then it's an acid-base reaction 6)  If you haven't answered "yes" to any of the questions above, then you've got a double displacement reaction

  14. Identify the Type of Reaction below: List what type the following reactions are: 1)  NaOH + KNO3 --> NaNO3 + KOH 2)  CH4 + 2 O2 --> CO2 + 2 H2O 3)  2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na 4)  CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4 5)  NH4OH + HBr --> H2O + NH4Br 6)  Pb + O2 --> PbO2 7)  Na2CO3 --> Na2O + CO2

  15. Identify the Type of Reaction below: List what type the following reactions are: 1)  double displacement 
2)  combustion 
3)  single displacement 
4)  double displacement 
5)  acid-base 
6)  synthesis 
7)  decomposition

  16. Acid/Base Reaction Calculations

  17. Steps to perform Acid-Base Reaction Calculations or any precipitation reaction • List the compounds present before the reaction occurs • Write the balanced net ionic equation • Calculate the moles of reactants (may use volume and molarity) • Determine the limiting reactant • Calculate the moles of the required reactant or product • Convert to grams or volume as required

  18. Example 1: When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed. Calculate the mass of Lead (II) Sulfate formed when 1.25 L of 0.0500 M Lead (II) Nitrate and 2.00 L of 0.250 M Sodium Sulfate are mixed. Is this a precipitation or Acid/Base reaction?

  19. Example 2: What volume of a 0.100 M HCl solution is needed to neutralize 25.0 mL of 0.350 M NaOH? Is this a precipitation or Acid/Base reaction?

  20. Example 3: In a certain experiment, 28.0 mL of 0.250 M HNO3 and 53.0 mL of 0.320 M KOH are mixed. Calculate the amount of water formed in the resulting reation. What is the concentration of H+ or OH- ions in excess after the reaction goes to completion?

  21. Acid/Base Reaction Titrations

  22. We use this technique for Volumetric Analysis! Buret Endpoint: when the solution changes colorin a titration Titrant Analyte

  23. Endpoint: when the solution changes color Buret Equivalence Point: point where enough titrant has been added to react exactly with the amount of analyte (no limiting reagent) Titrant Analyte

  24. Practice Problems

  25. Redox Reactions (aka Oxidation Reduction Reactions)

  26. Oxidation-Reduction Reactions/Redox Reactions – when one or more electrons are transferred • Oxidation States/Oxidation numbers - Table 4.2 Rules of Assigning oxidation states… • **the sum of the oxidation states must add to the original ion charge

  27. Oxidation State Assignments:

  28. Practice Assigning Oxidation States:

  29. If an element is oxidized…it LOST electrons Oxidation involves an increase in oxidation state If an element is reduced…it GAINED electrons Reduction involves a decrease in oxidation state

  30. In other words… Oxidizing agent means the Reduction means to GAIN electrons LEO the lion goes…GER OR OIL RIG (Oxidation is loss/Reduction is gain)

  31. Oxidizing Agent – A compound that accepts electrons Reducing Agent – A compound that donates electrons whereas… An ELEMENT (within that compound) can be oxidized or reduced!

  32. Balancing Redox Reactions!

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