CHM 113L RS W5 Chemical Reactions In Aqueous Solutions PDF

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Lab, Professor John Stark ...

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CHM-113L Lab 5 Chemical Reactions in Aqueous Solutions Assignment Name: ____________________________________

Section: __________________

Directions: Please complete this worksheet and staple the duplicate copy pages containing the data and calculations from your notebook. Include all work and calculations as indicated. Students with unclear handwriting may be required to type their non-calculation based answers as directed by the instructor. All data and analysis should be completed in the notebook. All worksheets should be completed in this packet and do not need to go in the notebook. This packet contains:    

Data and Analysis Worksheet 1: Chemical Reactions Worksheet Worksheet 2: Precipitation Reactions Worksheet Worksheet 3: Redox Reactions Worksheet

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Part A 1. Using the Table of Reactions and GCU’s simple rules for solubility, write the molecular equation for all 36 reactions. Be sure to correctly predict the products, indicate the states of each substance, and balance your equation. You will want to leave at least 3 lines of space after any reaction in which a solid is predicted. 2. For all reactions in (1) that produced a precipitate, write the complete ionic equation, and net ionic equation. For any reactions that did not precipitate, write No reaction. 3. Indicate any spectator ions. Be sure to correctly write the charges. 4. List all the cations and anions from the 12 reactions you tested. You should have one line for each one listed. 5. For each cation, review your results and indicate if it was always soluble, or always soluble except when, or always insoluble. Do not use the simple rules, use your results only. For cations containing exceptions, list those exceptions. Be sure to use correct charges on all ions. 6. For each anion, review your results and indicate if it was always soluble, or always soluble except when, or always insoluble. Do not use the simple rules, use your results only. For anions containing exceptions, list those exceptions. Be sure to use correct charges on all ions. Part C Create the following table and label it as Part C Analysis Table. You will fill in the table using values from the analysis questions below. Part C Analysis Table Final mass of solid in test tube Theoretical yield Percent error 1. Write the balanced decomposition reaction for NaHCO3. 2. Calculate the final mass of solid in the test tube. Be sure to label and show this calculation. 3. Calculate the theoretical yield of the final product using your balanced equation in (1). NaHCO3. Be sure to label and show this calculation. 4. Determine the percent yield of the final product using your final mass in (2) as the actual yield and the value calculated in (3) as your theoretical yield. Be sure to label and show this calculation.

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Part D 1. For each base, write the balanced acid-base neutralization reaction. Be sure to correctly predict the products, indicate the states of each substance, and balance your equation. Table of Reactions

GCU’s Simple Rules for Solubility 1. Most nitrates (NO3-), acetates (C2H3O2-), bicarbonates (HCO3-), chlorates (ClO3-) are soluble. 2. Most ionic compounds containing Group 1A Alkali metal ions and ammonium ion (NH4+) are soluble. 3. Most ionic compounds containing chlorides (Cl-), bromides (Br-), iodides (l-) are soluble. Notable exceptions include ionic compounds containing Ag+, Pb2+, Hg22+, Hg2+. 4. Most ionic compounds containing sulfates (SO42-) are soluble. Notable exceptions include ionic compounds containing Ba2+, Ag+, Pb2+, Hg22+, Ca2+, Sr2+. 5. Most ionic compounds containing hydroxides (OH-), sulfides (S2-), carbonates (CO32-), chromates (CrO42-), phosphates (PO43-), oxides (O2-) are, or insoluble. Notable exceptions include ionic compounds containing Group 1A Alkali metal ions and ammonium ion (NH4+).

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Worksheet 1: Chemical Reactions For each of the following, balance the chemical reaction and identify the type of reaction as combustion, decomposition, synthesis, single-replacement, precipitation, acid-base neutralization. Type of Reaction 1. ____ NaBr + ____ Ca(OH)2  ___ CaBr2 + ____ NaOH 2. ____ NH3+ ____ H2SO4  ____ (NH4)2SO4 3. ____ C5H9O + ____ O2  ____ CO2 + ____ H2O 4. ____ CuCl₂ + Na₂S  ____ CuS + ____ NaCl 5. ____ Pb + ____ H3PO4  ____ H2 + ____ Pb3(PO4)2 6. ____ Li3N + ____ NH4NO3  ___ LiNO3 + ___ (NH4)3N 7. ____ HBr + ___ Al(OH)3  ___ H2O + ___ AlBr3 8. ____ HBr + ___ Al(OH)3  ___ H2O + ___ AlBr3 9. ___ Zn(CO₃)  ___ ZnO + ___ CO₂ 10. ___ C₆H₁₀O₃ + ___ O₂  ___ CO₂ + ___ H₂O 11. ___ CaCl₂ + ___ K₂CO₃  ___ CaCO₃ + ___ KCl

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Worksheet 2: Precipitation Reactions For each of the following, write the molecular equation and net ionic equation. List the spectator ions. Be sure to correctly predict the products, indicate the states of each substance, and balance your equation. Be sure to correctly indicate the charges on spectator ions. 1.

KI is mixed with Pb(NO₃)₂

Spectator Ions:

2.

MgI2 is mixed with Na2CO3

Spectator Ions:

3.

Al2(SO4)3 is mixed with Ca(OH)2

Spectator Ions:

4.

Aluminum chloride and sodium hydroxide are mixed.

Spectator Ions:

5.

Lithium sulfate and calcium nitrate are mixed.

Spectator Ions:

6.

Iron (II) sulfate and barium hydroxide are mixed.

Spectator Ions:

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Worksheet 3: Reduction and Oxidation Reactions For each oxidation-reduction reaction below, use the changes in oxidation number for each atom and identify the reactants as the oxidizing agent (OA), reducing agent (RA), oxidized species (Ox), and reduced species (Red). 1.

Mg(s) + 2HCl(g)  MgCl2(s) + H2(g)

Ox: Red: RA: OA:

2.

2Fe(s) + 3V2O3(s)  Fe2O3(s) + 6VO(g)

Ox: Red: RA: OA:

3.

2Sr(s) + O2(g) 2SrO(s)

Ox: Red: RA: OA:

4.

2Li(s) + S(g)  Li2S(s)

Ox: Red: RA: OA:

5.

Cu(s) + 4HNO3(aq)  Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) Ox: Red: RA: OA:

6.

4 Ag(s) + 2 H2S(g) + O2(g)

2 Ag2S(s) + 2 H2O(g)

Ox: Red: RA: OA:

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