Catalyst

Write the Molecular, Total Ionic, and Net Ionic Reactions for the chemical reactions below: a) AgSO4 + K3PO4

b) Reacting Magnesium Sulfate and Lithium Fluoride

GRADE!

Catalyst

Pick up Papers from the frontCalculate the actual yield of 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

BIG GOAL

Explosion!(3 MINUTES)

?

?

???

?

?

??

? ?

Explosion Questions1. What is the formula for

density?2. Give an example of a chemical

property.3. Give an example of a physical

property.4. What is the law of

conservation of mass?5. What is the law of definite

proportions?6. What is the law of multiple

proportions?7. Who discovered the electron?8. What are the three types of

radiation?9. Which particle is the biggest?10. Which is the smallest?11. Who is Ernest Rutherford?12. How do you find the number of

neutrons?13. What is an isotope?

14. What is the formula for Nitrite?15. What is the formula for

Perchlorate?16. What is the formula for

Hyposulfite?17. What is the empirical formula?18. What is the molecular

formula?19. What is the limiting reagent?20. What is the excess reagent?21. What is the % yield?22. What is % composition?23. What does it mean to be

aqueous?24. Name 3 strong acids25. Name 3 Strong bases

How to Remember Solubility RULES!Always Soluble:CASH – N – GIA

C: ChloratesA: AmmoniumS: Sulfates – CBS/PBSH: Halogens – F: CBS-PM

Cl/Br/I: HAPpyN: NitratesGIA: Group 1A

How to Remember Solubility RULES!Always Soluble:

kNights can take on anythingAcetate : the Ace

I ClBr except Silver Lead and Mercury

C: ChloratesA: AmmoniumS: Sulfates – CBS/PBsH: Halogens – F: CBS-PM

Cl/Br/I: HAPpyN: NitratesGI: Group 1A: Acetates

Acid/Base Reactions

Acid/Base Reactions: form a SALT and WATER as the only products

HA + BOH BA + H2O

Bronsted Lowry Acid Definition: Proton

donorBase Definition:Proton Acceptor

MUST REMEMBER: STRONG electrolytes (acids and bases) dissociate completely, weak electrolytes Do NOT!

ALWAYS WRITE THESE EQUATIONS IN NET IONIC REACTION FORM!

Example Equations:

Hydrochloric Acid reacts with Sodium Hydroxide

Remember: Write the NET IONIC Equation!

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 reaction2) Does your reaction have two (or more) chemicals combining to form one chemical?

If yes, then it's a synthesis reaction3) Does your reaction have one large molecule falling apart to make several small ones?

If yes, then it's a decomposition reaction4) Does your reaction have any molecules that contain only one element?

If yes, then it's a single displacement reaction5) Does your reaction have water as one of the products?

If yes, then it's an acid-base reaction6) If you haven't answered "yes" to any of the questions above, then you've got a double displacement reaction

Identify the Type of Reaction below:List what type the following reactions are:1) NaOH + KNO3 --> NaNO3 + KOH2) CH4 + 2 O2 --> CO2 + 2 H2O3) 2 Fe + 6 NaBr --> 2 FeBr3 + 6 Na4) CaSO4 + Mg(OH)2 --> Ca(OH)2 + MgSO4

5) NH4OH + HBr --> H2O + NH4Br6) Pb + O2 --> PbO2

7) Na2CO3 --> Na2O + CO2

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

Acid/Base Reaction Calculations

Steps to perform Acid-Base Reaction Calculations or any precipitation reaction

1. List the compounds present before the reaction occurs

2. Write the balanced net ionic equation3. Calculate the moles of reactants (may use

volume and molarity)4. Determine the limiting reactant5. Calculate the moles of the required

reactant or product6. Convert to grams or volume as required

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?

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?

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?

Acid/Base Reaction Titrations

We use this technique for

Volumetric Analysis!Buret

Titrant

Analyte

Endpoint: when the solution

changes color in a titration

Buret

Titrant

Analyte

Endpoint: when the solution changes color

Equivalence Point: point where enough

titrant has been added to react exactly

with the amount of analyte (no limiting

reagent)

Practice Problems

Redox Reactions (aka Oxidation Reduction

Reactions)

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

Oxidation State Assignments:

Practice Assigning Oxidation States:

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

In other words…

Oxidizing agent means theReduction means to GAIN electrons

LEO the lion goes…GEROR

OIL RIG (Oxidation is loss/Reduction is gain)

Oxidizing Agent – A compound that accepts electronsReducing Agent – A compound that donates electrons

whereas…An ELEMENT (within that compound) can be oxidized or reduced!

Balancing Redox Reactions!