1a) Molecular equation: Ba(NO3)2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaNO3 (aq)
Ionic equation: Ba2+ + SO42- → BaSO4 (s)
Molecular equation: Ba(NO3)2(aq) + 2NaOH(aq) → Ba(OH)2(s) + 2NaNO3(aq)
Ionic equation: Ba2+(aq) + 2OH-(aq) → Ba(OH)2(s)
Molecular equation: Ba(NO3)2(aq) + Na2CO3(aq) --> BaCO3(s) + 2NaNO3(aq)
Ionic equation: Ba2+(aq) + CO32-(aq) → BaCO3(s)
Molecular equation: 2 AgNO3(aq) + Na2SO4(aq) → Ag2SO4(s) + 2 NaNO3(aq)
Ionic equation: 2Ag+(aq) + SO42-(aq) → AgSO4(s)
Molecular equation: AgNO3(aq) + NaOH(aq)→ AgOH(s) + NaNO3(aq)
Ag+(aq) + OH-(aq) → AgOH(s)
Molecular equation: 2AgNO3(aq) + Na2CO3(aq) → Ag2CO3(s) + 2NaNO3(aq)
2Ag+ + CO32- → Ag2CO3(s)
Molecular equation: Na2SO4 (aq) + Pb(NO3)2(aq) → 2NaNO3 (aq) + PbSO4 (s)
Pb2+ (aq) + SO42-(aq) → PbSO4(s)
Molecular equation: 2NaOH (aq) + Pb(NO3)2(aq) → 2NaNO3 (aq) + Pb(OH)2(s)
Pb2+ (aq) + 2OH-(aq) → Pb(OH)2(s)
Molecular equation: Na2CO3 (aq) + Pb(NO3)2(aq) → 2NaNO3 (aq) + PbCO3(s)
Pb2+ (aq) + CO32-(aq) → PbCO3(s)
Molecular equation: Ni(NO3)2(aq) + Na2SO4(aq) → NiSO4(aq) + 2NaNO3(aq)
Ni+2(aq) + SO4-2(aq) → NiSO4 (s)
Molecular equation: Ni(NO3)2(aq) + 2 NaOH(aq) → Ni(OH)2(s) + 2 NaNO3(aq)
Ni+2(aq) + 2HO-(aq) → Ni(OH)2 (s)
Molecular equation: Ni(NO3)2 (aq) + Na2CO3 (aq) → NiCO3 (s) + 2NaNO3 (aq)
Ni+2(aq) + CO3-2(aq) → NiCO3 (s)
1b) Compounds with group 1A ions, nitrates and sulphates are soluble. Hydroxide ions are soluble with group 1A ions, ammonium ion, Ca2+, Sr2+, Ba2+. Carbonates and phosphates are also soluble with group 1A ions and ammonium ion.
2a) Red litmus paper turns blue when comes in contact with base while it remains red with acid or neutral solution. When base solution comes in contact with red litmus paper, hydrogen ion reacts with base to form conjugate base which has blue color, due to presence of weak diprotic acid in red litmus paper.
2b) Blue litmus paper turns red when comes in contact with acid whereas it remains blue with base and neutral solution. The pigment in blue litmus paper reacts with hydrogen ions wich tunes the bond to give color with longer wavelength i.e. red color.
2c) For acid blue litmus paper is used because change in color of pH below 4.5 turns red.
2d) For base red litmus paper is used because change in color of pH above 8.3 turns blue.
3a) CaCO₃(s) + 2HCl(aq) → CaCl₂(aq) + CO₂(g) + H₂O(l)
Ionic equation: CaCO₃(s) + 2H+(aq) → Ca2+(aq) + CO₂(g) + H₂O(l)
3b) In Both reaction heat is not evolved HCl + NH3 and NaOH + HC2H3O2
I need answers for the questions. Questions 1. Write balanced molecular and ionic equations for each...
Write balanced molecular, ionic and net-ionic equations for 10 reactions (8 precipitate (P) and 2 neautralization) Use the next few pages to write balanced MOLECULAR, IONIC, and NET-IONIC equations for 10 reactions that occurred during this laboratory experiment. There are more than 10 possible reactions. Choose precipitation reactions and 2 neutralization reactions. Make sure to include the physical states of all the products. Class (circle one): Precipitation or Neutralization Reaction 1. Molecular: Complete lonic: Net lonic: no I reaction/ no...
just the equations i want to check if i am correct please QUESTIONS: Write balanced molecular, total ionic and net ionic equations for all the reactions performed in this experiment. RESULTS: Na,Co, + HCO NHOH + precipitate from AgNO, + HCI NaNO, Ni(NO), Cu(NO) Test Ba(NO, NH.NO, Fe(NO), AgNO, HCI H SO. Napoy H,PO Whitesolid propitates Clear stays dead Yellow Preapitated Brun Precipitation Milky white Preupatation Lcclar NaOH K.CO, ALT doudy idear NaC,H,02 Instructor's signature
for this problem I dont know how to write the equations. we need six equations with Ni(NO3)2. the rest we didnt need to do each group was assigned 1 column. Name Section RESULTS: Cloudy NH,OH + precipitate from AgNO, + HCI Precipitate formed Na,Co, + HCI Bubbles are emitted. This is a gas evolution reaftor. Test NaNO, Ba(NO, NH.NO, Fe(NO), AgNO, Ni(NO), Cu(NO) Color Chata Teal-green HCI CoorChang H,SO teal-gman liquidorna H.PO Nazpoy Houdy Teal green Solar formed Chunky Cloudy...
please fill out everything as soon as possible thank you so much! Section Results Testing the Solubility Rules and Reaction of Precipitates with HCI Column A Column B Na2SO4 NaBr Column NH.NO, No reaction no reaction NaOH ColumnD Na.co. no reaction no reaction Ba(NO)2 No reaction reaction no reaction reaction AgNO reaction no reaction reaction reaction Pb(NO3)2 no reaction reaction no reaction reaction NI(NO3)2 no reaction no reaction reaction reaction Unknown Treaction reaction no reaction reaction All compounds used in...
For each reaction in the table above, write the molecular, ionic, and net ionic equations? the unknown had no reaction to any of the chemicals so I put g because it may have been a gas. There was no odor no color etc. I'm not sure what else I need to so to answer the question. We were unable to transcribe this imager e n 1 Grid table of unknown chemicals (ppt - precipitate; g - gas; color, odor) Ow...
Writing Chemical Equations: Results Toto, AtHMED Name Date Partners Instructor Section Results Testing the Solubility Rules and Reaction of Precipitates with HCI Column A Column B Column C Column D NaBr Na SO NaOH Na:CO Aftte dey Sreah to hu le NH4NO NR NR N2 perenetrte anget N cloudy eleely Slegoth Whi'te NA Ba(NO)2 Whute leromegenens Chonks Nhuenytle pretrpitate white Brewn yelle black hatero hikno predpi fake AgNO hetero wery Lte cledy blag ceh hitt uhile eleyly fruritnta white Pb(NOs)2...
Writing Balanced Molecular, Ionic, And Net Ionic Equations Write Balanced Net-Ionic Equations for the following Reactions in Aqueous Solution: 1. Copper metal (Cu(s)) is immersed in an aqueous solution of silver nitrate (AgNO3). The solution turns light blue and a silver coating appears on the copper. 2. Dilute solutions of antimony(III) chloride and sodium sulfide are mixed to give a precipitate. 3. Dilute solutions of silver nitrate and potassium iodide are combined and give a yellow precipitate. 4. Dilute solutions...
Using the Solubility Rules, write the balanced molecular, total ionic, and net ionic equations (including physical states) for the following: Hints: There is no such thing as Na2+ or Na3+. Na is in group 1A, so you know it can only form a +1 charge. (For example, it will form 3 Na+ ions for each Na3PO4.) There is a diatomic molecule Cl2. But when ionic compounds are dissolved in water, they form ions so the dissociation of MgCl2 is to...
write balanced molevular and ionic equations for each reaction that produced percipitation. Post Laboratory Questions 1. Write balanced molecular and ionic equations for each reaction that produced precipitation Compound Molecular Equation Net lonic Equation Ba NO3)2 Na₂504 BalNO3)2 Nach Ba(NO3)2 + rayCD3 | AgNO3 NaBr AgNO3 Ag Noz t NaBr Age Br + 2 Na NO3 AgNO3 + Na +2Br Agt Br + 2 Ag Br + 20 AgNO3 + NaOH - AgoH + Nanoz Agt +N05 + Mat toti...
write balnced molecular and ionic equations for the following reactions. your predictions CaCOs(s) and HCl(aq) a. m=Cocost2HclCaclzt Hz0+Cor -Cacosut 2 2cz c 2ci0 b. Well 5C [Ni(NOs)2 + NaOH] and HCl(aq) o identify acids and c. HCl(aq)+ NHa(aq) paper is affected. d paper is affected. d. CHsCOOH(aq)+ NaOH(aq) you use to test paper yau in tobr ne 5. Which observations are the bases of identifying your unknown? Be specific. you use to test ncte he