Na2SO4
i) Na2SO4 + Ba2+(aq) ----> BaSO4(s) + 2Na+(aq)
Note: The formation of precipitate occurs.
ii) Na2SO4 + Mg2+(aq) ----> MgSO4(aq) + 2Na+(aq)
Note: The precipitation doesn't occur.
iii) 3Na2SO4 + 2Al3+(aq) ----> Al2(SO4)3(aq) + 6Na+(aq)
Note: The precipitation doesn't occur.
Na2CO3
i) Na2CO3 + Ba2+(aq) ----> BaCO3(s) + 2Na+(aq)
Note: The formation of precipitate occurs.
ii) Na2CO3 + Mg2+(aq) ----> MgCO3(s) + 2Na+(aq)
Note: The formation of precipitate occurs.
iii) 3Na2CO3 + 2Al3+(aq) ----> Al2(CO3)3(s) + 6Na+(aq)
Note: The formation of precipitate occurs.
NaOH
i) 2NaOH + Ba2+(aq) ----> Ba(OH)2(aq) + 2Na+(aq)
Note: Precipitation doesn't occur.
ii) 2NaOH + Mg2+(aq) ----> Mg(OH)2(aq) + 2Na+(aq)
Note: Precipitation doesn't occur.
iii) 6NaOH + 2Al3+(aq) ----> 2Al(OH)3(s) + 6Na+(aq)
Note: The formation of precipitate occurs.
NH4OH
i) 2NH4OH + Ba2+(aq) ----> Ba(OH)2(aq) + 2NH4+(aq)
Note: Precipitation doesn't occur.
ii) 2NH4OH + Mg2+(aq) ----> Mg(OH)2(aq) + 2NH4+(aq)
Note: Precipitation doesn't occur.
iii) 6NH4OH + 2Al3+(aq) ----> 2Al(OH)3(s) + 6NH4+(aq)
Note: The formation of precipitate occurs.
Experiment 17 Observations and Report Sheet: Development of a Scheme for Qualitative Analysis Table of Solubility...
Having trouble figuring the equations
REPORT SHEET EXPERIMENT Abbreviated 32 Qualitative Analysis Scheme PART IV: GROUP 4 CATIONS equations for each precipitation reaction. Record the reagent used in each step, your observations, and the Mark + if observed in unknown Equations Observations Procedure Reagent G1tel Forme G4-2 4-3 1-4 tions in group 3 unknown
IUL JUU pe ns, use the solubility generalizations in Table given below. Table Solubility Rules for lonic Compounds Usually Soluble Li, Na, K, Rb, All Group 1A (alkali metal) and ammonium salts are | C, NH, soluble. Nitrates, NO, All nitrates are soluble Chlorides, bromides, All common chlorides, bromides, and iodides are soluble iodides, Cl-, Br, I except AgCl, HgCl, PCl, AgBr, Hg,Brg, PbBr, Agl, Hgal, PbI Sulfates, 50, Most sulfates are soluble except Caso. Srso. Baso, PbSO, Acetates, CH,COO...
Qualitative Analysis of Metal Cations Qualitative analysis can determine the metal cations that are present in a sample based on their solubility characteristics. One such scheme is shown in the flow diagram. Some ions that are soluble in all of the test solutions can still be identified based on flame tests. Certain ions impart characteristic color to the flame.Part AA solution contains some or all of the ions Cu2+, Al3+, K+, Ca2+, Ba2+, Pb2+, and NH4+. The following tests were performed, in...
Part A.
Use the attached flow chart of a qualitative analysis separation
and identification scheme to answer the following question.
What ion is present in solution if the following observations
were seen (enter your answer as the chemical symbol without the
charge)
Addition of HCl: no precipitate
Addition of NH3/NH4Cl: a precipitate
forms
Addition of NaOH and H2O2: no
precipitate
Heat to remove H2O2 and addition of HCl: a
colorless solid is formed
Addition of HCl, Aluminon and NH3: a...
[24]Following questions are based on Experiment #17 "General ation unknown analysis The data and results provided pertain to a specific unknown analysis. Provide Answers to the following for this analysis 1 (a) To separate Qualitative Analytical (QA) Group I from the other groups tested in the general cation unknown you must add (b) The precipitate obtained in (a) above was centrifuged and the supernatant liquid decanted. The The warm test tube contained no precipitate. Based on this observation, provide the...
Lab Section: 1 Prelab: Inorganic Group I Ions 1. On the report sheet, complete the flow diagram for the separation and identification of the ions in Group I 2. Write balanced net ionic equations for the following reactions: The precipitation of the chloride of Pb a. in Step 1. The formation of a yellow precipitate in Step 4. b. The formation of a complex ion in Step 5. c. d. The reaction that forms a white precipitate in Step 5....
help please?
this was the only other information given
REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
please, I need assistance with this Laboratory Report
on the periodic table.
Part A 1. Place 9 clean small test tubes in a test tube rack. The test tubes should be clean but do not have to be dry because aqueous solutions will be used. 2. To cach test tube add 5 drops of the solution (0.1 M) indicated in the data table. 3. Next add 5 drops of silver nitrate (0.5 M) to each of the 9 test tubes....
I concluded that my unknown was Pb2+. since yellow
precipitate formed. can you help me answer the questions for the
Known and unknown report
Qualitative Analysis: Group I Cations 10 ORECTIVES A Leam some chemistry of Group I cations, R Analyze an unknown for Group I cations. THEORY AND DISCUSSION Group I cations are precipitated as insoluble chlorides: Ag, Pb, Hg2 +Cr-AgCl, PbCh, HgCla The colors of the following species will be helpful in the analysis for Group I cations....
Experiment 8 Double Replacement Reactions Background: Some reactions have the net effect of causing the cation of each reactant to trade places, forming a compound with the other anion. These reactions are known as double replacement reactions. In the example below (unbalanced equation), the barium and sodium cations switch places so that barium forms a product with sulfate while sodium forms a product with chloride. Note that the formula of each product is determined by the charges of the ions,...