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Lab 1

by: Caitlin McConnell
Caitlin McConnell
Virginia Tech

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General Chemistry
Class Notes
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This 3 page Class Notes was uploaded by Caitlin McConnell on Tuesday September 20, 2016. The Class Notes belongs to Chem 2535 at Virginia Polytechnic Institute and State University taught by in Fall 2016. Since its upload, it has received 4 views. For similar materials see General Chemistry in Chemistry at Virginia Polytechnic Institute and State University.


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Date Created: 09/20/16
Caitlin McConnell Post-lab1 Questions: 7/11/16 Partner: Erinn Brooks 1. Table 1:Observations of Precipitation Reactions Ba(NO ) 3 2 Pb(NO )3 2 Co(NO ) 3 2 Ni(NO ) 3 2 NH N4 3 AgNO 3 NaCl No  No  No  No precipitate No  Precipitate precipitate precipitate precipitate precipitate white,  cloudy Na 2O 4 Precipitate Precipitate No  No precipitate No  No  white,  white,  precipitate precipitate precipitate cloudy cloudy Na 3O 4 Precipitate Precipitate Precipitate Precipitate  No  Precipitate white,  white,  purple greenish/whit precipitate yellow,  clumpy cloudy e cloudy NaOH No  Precipitate Precipitate Precipitate  No  Precipitate precipitate white dark blue light blue precipitate brown KI No  Precipitate No  No precipitate No  Precipitate precipitate yellow  precipitate precipitate white,  cloudy Na 2O 3 Precipitate Precipitate Precipitate Precipitate  No  Precipitate white,  white purple greenish/whit precipitate brown cloudy e 2.   1. a.)NaCl (aq) + AgNO (aq)3AgCl(s) + NaNO (aq) 3 ­ + b.) NO  3nd Na c.) Ag (aq)+Cl(aq)AgCl(s) 2. Na 2O (4q)+ Ba(NO ) (a3 2BaSO (s)+ Na4O (aq) 3 ­ + b.) NO  3nd Na c.) Ba (aq)+SO (aq)BaSO (s) 4 4 3. a.) Na2SO (4q)+ Pb(NO ) (a3 2PbSO (s)+ Na4O (aq) 3 b.) NO  3nd Na + 2+ 2­ c.)Pb (aq)+SO (aq4 PbSO (s) 4 4. a.) NaOH(aq)+ Pb(NO ) (aq3 2b(OH) (s)+ NaN2 (aq) 3 ­ + b.) NO  3nd Na c.)Pb (aq)+OH(aq) Pb(OH) (s) 2 5. a.) NaOH(aq)+ AgNO (aq)AgOH(s)+ NaNO (aq) ­ + 3 3 b.) NO  3nd Na c.)Ag (aq)+OH(aq)AgOH(s) 6. a.) NaOH(aq)+ Ni(NO ) (aq3 2i(OH) (s) + Na2O (aq) 3 b.) NO  3nd Na + Caitlin McConnell Post-lab1 Questions: 7/11/16 Partner: Erinn Brooks c.)Ni (aq)+OH(aq) Ni(OH) (s) 2 7. a.) KI(aq)+ Pb(NO ) (a3 2PbI (s)+KNO2(aq) 3 b.) NO  and K + 3 c.) Pb (aq)+I(aq) PbI (s) 2 8. a.) NaOH(aq)+ Co(NO ) (aq)3 2OH) (s) + NaNO (2q) 3 b.) NO  3nd Na + 2+ ­ c.)Co (aq)+NO  Co(3H) (s) 2 9. a.) Na CO (aq)+AgNO (aq)Ag CO (s)+ NaNO (aq) 2 3 3 2 3 3 b.) NO  3nd Na + + 2­ c.)Ag (aq)+CO (aq)3 Ag CO (s) 2 3 10. a.) Na C2 (aq3+ Pb(NO ) (aq)3 2O (s)+ NaNO (3q) 3 ­ + b.) NO  3nd Na 2+ 2­ c.)Pb +CO (aq)3 PbCO (s) 3 3. None of the salts were insoluble in water; therefore, unless the salt reaches its solubility limit  and becomes saturated in NaCl, it will continue to dissolve in water. 4. a.) Most chloride salts are soluble in water, except silver, mercury, and lead,  because the “like dissolves like” concept and they dissociate complete when contacted with water. b.) Many phosphate salts are not soluble in water, except phosphates of GroupA(1) and  ammonium, in standard conditions because they only form ionic compounds when a positive  charged ion comes in contact with a negatively charged oxygen on phosphate. c.) All ammonium salts are soluble in water because the N­H hydrogen bond within ammonium  will dissolve in water because hydrogen bonds are present within water. 5.  Table 2:Observations of Separation of a Precipitation Reaction Procedure Results Conclusions + 2+ Step 1 Add 3 M NaCl White ppt. forms Ag  and/or Pb Step 2 Heat ppt in hot water bath The ppt began to separate and Ag  and/or Pb 2+ remained white 2+  Step 3 Add 0.1 M KI The ppt turned bright yellow Pb is present Step 4  Add NH  an3 HNO 3 The ppt dissolved when NH   3 Ag  is present was added and the solution  turned the litmus paper red to  show acidity when HNO  was 3 added Caitlin McConnell Post-lab1 Questions: 7/11/16 Partner: Erinn Brooks 6. Step 1: Ag (aq)+Pb (aq)+2NaCl(aq)AgCl(s)+PbCl (s)+2Na (aq) 2 + + ­ Step 2: AgCl+ PbCl (s)+h2t waterAgCl(s)+ Pb (aq)+2Cl(aq) 2+ + Step 3: Pb (aq)+KI(aq)PbI (s)+K (a2) + ­ Step 4: AgCl(s)+2NH (aq)+2H3O (aq)AgCl(s)32NH (aq)+2NO (aq) 4 3


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