Help me with number 6. Writing net ionic equations by using the qualitative analysis scheme. 6. For each numbered step in the qualitative analysis scheme, type the net ionicequation associated with each step. Show only the final net ionic equation. Dothis for all reactions. Do not show net ionic reactions for steps that produced noreaction. Some steps have multiple net ionics, therefore it is important that eachstep is clearly labeled. For example:Step 1: addition of AgNO3Net ionic for formation of AgCINet ionic for formation of AgINet ionic for formation of Ag2CO3Net ionic for formation of Ag3PO4Step 2: etc alypis SchemeNOTESmust redo for final draft in reportIconse chutive testing)* Comprehensive testing of all ins* After addition of te sting agent, ions go to the RIĞHT precipitates go to the LEEL* be Sure to write states of matter, vse steps #s as this scheme does* number all separation steps!* You will write NIES for all Steps (1-7), yov will snow onlu the Net lonic, and theymust be typed! Do not show NIE'S if they produced no reaction!mixed Known[1.ar, Sot, POcom"] I [1-4 ions ; worn't have I'aND nog]un known_Sample(7)Observationsfor UNKNOWNANogDe comtNitrateSolidTesthave NitrateComPletene ssPpt.AgClis) feluwAglis)Apt.so4?lag)Ag, Pon es)Selidbeamt(2) Add HNO3 (OM)SolidDecantBa SO4NO3littleNOHz Poybit solidiettCo2NOAgl, AGCISouMolyndatetestO AddNH3DeantNO U zSolöd(AHa)s PZY:12MDs(s) RodoNo PNo, cearptNo pou3-Add HNOSNo IpH (7 ]!SAVE YOURDECANTAg ClHaveyou need to test it!

Answered: Image /qna-images/answer/daed314f-eeda-4d93-a422-9387c8a20c31.jpg

6. For each numbered step in the qualitative analysis scheme, type the net ionic equation associated with each step. Show only the final net ionic equation. Do this for all reactions. Do not show net ionic reactions for steps that produced no reaction. Some steps have multiple net ionics, therefore it is important that each step is clearly labeled. For example: Step 1: addition of AgNO3 Net ionic for formation of AgCI Net ionic for formation of AgI Net ionic for formation of Ag2CO3 Net ionic for formation of Ag3PO4 Step 2: etc

6. For each numbered step in the qualitative analysis scheme, type the net ionic equation associated with each step. Show only the final net ionic equation. Do this for all reactions. Do not show net ionic reactions for steps that produced no reaction. Some steps have multiple net ionics, therefore it is important that each step is clearly labeled. For example: Step 1: addition of AgNO3 Net ionic for formation of AgCI Net ionic for formation of AgI Net ionic for formation of Ag2CO3 Net ionic for formation of Ag3PO4 Step 2: etc

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter7: Reactions In Aqueous Solutions

Section: Chapter Questions

Problem 30QAP

See similar textbooks

Similar questions

The procedures and principles of qualitative analysis are coy cred in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.
Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitrate
ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
Give an example of a polyprotic acid and write equations for the successive neutralizations of the acidic hydrogen atoms of the acid molecule to produce a series of salts.
Write molecular and net ionic equations for the successive neutralizations of each acidic hydrogen of sulfurous acid by aqueous calcium hydroxide. CaSO3 is insoluble; the acid salt is soluble.
42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.
A 0.500-L sample of H2SO4 solution was analyzed by taking a 100.0-mL aliquot and adding 50.0 mL of 0.213 M NaOH. After the reaction occurred, an excess of OH ions remained in the solution. The excess base required 13.21 mL of 0.103 M HCl for neutralization. Calculate the molarity of the original sample of H2SO4. Sulfuric acid has two acidic hydrogens.
Consider the following generic equation OH(aq)+HB(aq) B(aq)+H2OFor which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution? If it is not correct, write the proper equation for the acid-base reaction between the pair. (a) hydrochloric acid and pyridine, C5H5N (b) sulfuric acid and rubidium hydroxide (c) potassium hydroxide and hydrofluoric acid (d) ammonia and hydriodic acid (e) strontium hydroxide and hydrocyanic acid
Working with Concentration (Molarity Concepts) Note: You should be able to answer all of the following questions without using a calculator. Part 1: a Both NaCl and MgCl2 are soluble ionic compounds. Write the balanced chemical equations for these two substances dissolving in water. b Consider the pictures below. These pictures represent 1.0-L solutions of 1.0 M NaCl(aq) and 1.0 M MgCl2(aq). The representations of the ions in solution are the correct relative amounts. Water molecules have been omitted for clarity. Correctly label each of the beakers, provide a key to help identify the ions, and give a brief explanation of how you made your assignments. Keeping in mind that the pictures represent the relative amounts of ions in the solution and that the numerical information about these solutions is presented above, answer the following questions c through f. c How many moles of NaCl and MgCl2 are in each beaker? d How many moles of chloride ions are in each beaker? How did you arrive at this answer? e What is the concentration of chloride ions in each beaker? Without using mathematical equations, briefly explain how you obtained your answer. f Explain how it is that the concentrations of chloride ions in these beakers are different even though the concentrations of each substance (compound) are the same. Part 2: Say you were to dump out half of the MgCl2 solution from the beaker above. a What would be the concentration of the MgCl2(aq) and of the chloride ions in the remaining solution? b How many moles of the MgCl2 and of the chloride ions would remain in the beaker? c Explain why the concentration of MgCl2(aq) would not change, whereas the number of moles of MgCl2 would change when solution was removed from the beaker. As part of your answer, you are encouraged to use pictures. Part 3: Consider the beaker containing 1.0 L of the 1.0 M NaCl(aq) solution. You now add 1.0 L of water to this beaker. a What is the concentration of this NaCl(aq) solution? b How many moles of NaCl are present in the 2.0 L of NaCl(aq) solution? c Explain why the concentration of NaCl(aq) does change with the addition of water, whereas the number of moles does not change. Here again, you are encouraged to use pictures to help answer the question.
Complete and balance each of the following molecular equations (in aqueous solution); include phase labels. Then, for each, write the net ionic equation. a NaOH + HNO3 b HCl + Ba(OH)2 c HC2H3O2 + Ca(OH)2 d NH3 + HNO3
When the following solutions are mixed together, what precipitate (if any) will form? a. FeSO4(aq) + KCl(aq) b. Al(NO3)3(aq) + Ba(OH)2(aq) c. CaCl2(aq) + Na2SO4(aq) d. K2S(aq) + Ni(NO3)2(aq)
Describe in words the titration of an acid with a base. Be sure to use the terms equivalence point, indicator, and end point correctly.