Write balanced net ionic equations for the primary reaction occurring in each of the well plates after the addition of the test reagent. and Indicate in which direction each test reagent shifted the equilibrium. 3 drops of 0.1M iron(III) nitrate and 3 drops of 0.1M potassium thiocyanate in each test tube Tube 3drops of Test reagents Observation 1 0.1M silver nitrate Light yellow with white PPE 2 0.1M sodium nitrate No change 3 0.1M sodium phosphate Light yellow 4 0.25M ammonium oxalate Bright yellow 5 6M ammonium hydroxide Orange with PPE 6 NONE Dark red

Write balanced net ionic equations for the primary reaction occurring in each of the well plates after the addition of the test reagent. and Indicate in which direction each test reagent shifted the equilibrium. 3 drops of 0.1M iron(III) nitrate and 3 drops of 0.1M potassium thiocyanate in each test tube Tube 3drops of Test reagents Observation 1 0.1M silver nitrate Light yellow with white PPE 2 0.1M sodium nitrate No change 3 0.1M sodium phosphate Light yellow 4 0.25M ammonium oxalate Bright yellow 5 6M ammonium hydroxide Orange with PPE 6 NONE Dark red

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter8: Polyfunctional Acids And Bases

Section: Chapter Questions

Problem 3P

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at room temp. 0.00188 g AgCl dissolves in 1L of H2O. what is the ksp of AgCl?
Iron(II) Sulfide has a Ksp of 3.72 E-19, and Lead(II) sulfide has a Ksp of 9.04 E--29. What happens when you add S2- slowly to a solution containing Fe2+ and Pb2+? The Lead and the iron will precipitate out equally. The Lead will completely precipitate out before any of the iron will precipitate. The Iron will completely precipitate out before any Lead will precipitate. Because the Ksp 's are so low neither one will precipitate out.
In following these steps . Complete the table and provide th given chemical reactions in the qualitative analaysis of Group 3 Cations. Procedure 1. Place 20 drops of each of the following aqueous solutions to separate centrifuge tubes: 0.1M Cr (NO3)3, 0.1M Al (NO3)3, 0.1M Co (NO3)2, 0.1M Zn (NO3)2, 0.1M Mn (OH)2, 0.1M Ni (NO3)2, 0.1 M Fe (NO3)3. Make each solution basic by adding few drops of 6M NH4OH. Confirm using a litmus paper. 2. Add 5 drops of freshly prepared 6M (NH4)2S to each centrifuge tube. Place the samples in thecentrifuge machine for 3 mins. After centrifuge record results. Decant the supernatant liquid of all the samples. 3. Add one drop of NH4OH in each centrifuge tubes. Add 20 drops of distilled water in eachcentrifuge tubes. Then add a few drops of 6M HCl in each solution. Place the samples in the water bath for 10 mins. After water bath, centrifuge the samples for 3 mins. 4. After centrifuge, add a few drops of 6M NH4Cl in each sample. Decant the supernatant liquid…
Each equilibria has several disturbances. Each one needs to be addressed separately. For each disturbance to the equilibrium reaction, state how the disturbance affected the equilibrium (shifting it left or shifting it right). Explain specifically what occurred and how it pairs with the observation. Pour about 1 milliliter of deionized water to each of three test tubes. Add 1 drop of 0.1 M Fe(NO3)3 and 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes, and two more drops of 0.1 M KSCN to another of the test tubes. Try to compare the colors of the solutions as quantitatively as possible. Record your observations and explain what happened using Le Châtelier's principle. Part 5: Iron/Thiocyanate Equilibrium Fe,* {pale yellow} + SCNFe(SCN)2²*{deep red) Add 1 drop of 0.1 M Fe(NO₂), to each test tube Add 1 drop of 0.1 M KSCN to each test tube. Add two more drops of 0.1 M Fe(NO3)3 to one of the tubes. Add two more drops of 0.1 M KSCN to the other…
It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?
Give the expression for the solubility product constant for Ca3(PO4)2- Select one: O a. B Ca2+PR PO43-P Ca3(PO4)2 O b. [ Ca2+P[ PO43-P Ca3(PO4)2 O c. R Ca2+P[3 PO43-3 Ca3(PO4)2 O d. [ Ca2+j?[ PO43-73 O e. [Ca2+j³[PO43-12
A precipitate of PbI2 is formed when 5 mL of 0.012 M Pb(NO3)2 is added to 5 mL of 0.030 M KI. It was found experimentally that the final concentration of I- in the 10 mL solution after equilibrium was 8 x 10-3 M 1) What is [Pb2+] at equilibrium? 2) What is Ksp for the formation of PbI2 ?
QUESTION 6 In Test Tube 5, you will be using 5.0 mL of 0.0020 M KSCN. Each reaction mixture will be diluted to a final volume of 10.0 mL. What is [SCN 10 in Test Tube 5? Type your answer, WITHOUT UNITS, in the box below. Include 2 significant figures. QUESTION 7 What is the correct expression for Kc for the reaction you will be studying in this experiment. Assume that all concentrations are measured at equilibrium. The chemical equation for this reaction is: Fe 3+ (aq) + SCN (aq) Z FeSCN 2+ (aq) Kc = ([Fe³+][SCN]) / [FeSCN²+] Kc = [FeSCN²+]/([Fe³+][SCN) Kc = [SCN] / [[Fe³+][FeSCN²+]) Kc = [Fe³+][SCN][FeSCN²+] None of the above QUESTION 8 Why will you be measuring the absorbance of each of your reaction mixtures after they have reached equilibrium? The measured value of the absorbance is identical to the equilibrium concentration of FeSCN2+, [FeSCN²+ Jeq The measured value of the absorbance is directly proportional to the equilibrium concentration of Fe3+, [Fe³+ leq The measured value…
In a reaction mixture 20.0mL of 0.010M KI, 10.0mL of 0.040M KBrO3, 10.0mL of 0.040M Na2S2O3, and 20.0mL of 0.10M HCl were mixed. What is the concentration of [I-], [BrO3-], and [H+]?
4. You have a test tube in which the following equilibrium is established. Fe3+ (ag) + SCN (ag) =FESCN+ (ag) ww. ww Describe how concentrations of Fe3+. SCN and FeSCN²+ will change if a crystal KS CN is added to the mixture above? What would stay constant? ww ww
What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl- and 0.015 M I-? Ksp for Ag2CrO4 is 1.2 x 10-12.
What is the confirmatory reagent of lead sulfide? * OK2CrO4 OKCN SnClz HNO3 What is the name of the red precipitate confirming the presence of nickel ion? Nickel dimethylglyoxime Nickel thiocyanate Ammonium dimethylglyoxime Ammonium thiocyanate

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Tube	3drops of Test reagents	Observation
1	0.1M silver nitrate	Light yellow with white PPE
2	0.1M sodium nitrate	No change
3	0.1M sodium phosphate	Light yellow
4	0.25M ammonium oxalate	Bright yellow
5	6M ammonium hydroxide	Orange with PPE
6	NONE	Dark red