a) dil HCl; forms a white precipitate of silver chloride
b) hot water; In hot water, PbCl2 will dissolve while AgCl remains insoluble
c) H2S in acidic media; black ppt of CuS is formed.
d) 6 M NaOH. A dark precipitate forms will confirm the presence of Fe3+
e) excess NaOH, zinc hydroxide will form a colorless solution of zincate ion: Zn(OH)2 + 2 OH− → Zn(OH)42-
whereas ferric Hydroxide will not.
f) 3M Sulphuric acid; barium ions forms white precipitate of barium sulphate.
POST LAB QUESTIONS Answer the following questions in your lab notebook: 1. Give the chemical formula...
(1) Write the step-wise net ionic equations for all the cations that show amphoteric behavior in excess NaOH solution. (include Al^3+ ion) (2) Write the balanced net ionic equations for all the cations which exhibit complex formation with ammonia. (include Ni^2+ and Co^3+)
i need help with this lab please. can i get someone to answer the entire thing. thank you Instructor Equilibria of Coordination Compounds OBSERVATIONS AND DATA 1. The formation of complex ions with ammonia The net ionic equation for the reaction of excess Cuso, with NH, is 24 Cu2+ + 4NH3 [cu (NH3)4] The predicted effect on the reaction above of adding excess NH, (based on Le Châtelier's principle) is The reaction will shift to the night and product formation...
Questions 1-5 For #1 - #5 questions of Exp. 16, complete the following chemical reaction equations (1 point each). For example, Ag+ (aq) + Cl - (aq) + AgCl (s, I white) 1. For another example, silver precipitation, AgCl (s), reacts with 15 M ammonia aqueous solution. Complete this chemical reaction equation. AgCl (s) + 2NH3 (aq) → Ag(NH3)2 + (aq) + Cl(aq) 2. The silver complex ion, one of the products from above chemical reaction equation, reacts with 6...
Total ionic equation: Net ionic equation: Post-lab: 1. Explain how it is possible for two reactants that are each strong electrolytes to react and form products that are nonelectrolytes. by double replacement reactions. 2. Balance the equations and then write total and net ionic equations for each of the following: a. FeCl(aq) + 3NaOH(aq) → Fe(OH), (s) + 3NaCl (aq) Total ionic equation: Fe mg Bet Can + 3 Ath Tha) + 30th Fe (on), a + Station 3 tan...
Sect. Date Name Prelaboratory Assignment: Qualitative Analysis Group III Cations 1. Prepare a complete flow chart for the procedure and put it on your data sheet. 2. Write balanced net ionic equations describing each of the following reactions: Dissolution of Ni(OH), in nitric acid. Oxidation of Cr'to Cr by CIO in alkaline solution (CIO is converted to CI') The confirming test for Fe 3. A solution that may contain any of the group II cations. Treatment of the solution with...
LAB VII. PRACTICE PROBLEMS - CHAPTER 4 NAME: SECTION: b) How many grams of strontium nitrate, Sr(NO), are needed to prepare 3.40x10 ml. of a 0.925 M solution? c) To what volume should 50.0mL of a 6.00M HCI stock solution be diluted to obtain a 1.50M HCl solution? How much water should be used? d) A 38.5ml sample of 0.875M AgNO, solution is mixed with 51.0mL sample of 0.744M NaCl solution. The AgCl precipitated has a mass of 2.06g. Calculate...
Group 1 Flowchart Use the following chemical facts to construct a flow chart for this lab: 1 Group 1 cations are Ag, Hg, and Pb 2. AgH a and Pbare given to you in lab as their nitrates which are soluble in water (denoted by as) 3 AgHgand Pb are the only common ions that form a precipitate (denoted by with the Cl ion, presented as Hcl They all form white precipitates. 4. These Group 1 precipitates are separated from...
1IC LUDOUCO 1. Complete and balance the following net ionic equations. If no reaction occurs, write NR. a. Mg?+ + OH (imited -- b. Cu²+ + SCN" - c. Co2+ + NH3(aq) limited + H20 - d. Ba2+ + so; - e. Pb2+ + NH3(aq) excess + H20 – f. Fel+ + SO-- 2. Complete and balance the following net ionic equations. If no reaction occurs, write NR. Tables 4 and 5 of Experiment 7 list amphoteric metal hydroxides that...
1. Write balanced net ionic equations for the following oxidation-reduction reac- tions: a. Hydrogen sulfide is added to a solution of Fe(NO3)3. b. Hydrogen peroxide is added to an acidic solution of an iron(II) salt c. The Mn2+ ion is oxidized to MnO2 by KCIO3 in acidic solution (assuming reduction of ClOs to CI-), e Cr20,2 complex ion is reduced to Cr3+ by H2S in acidic solution. e. The compound Co(OH)2 is oxidized to Co(OH)s upon standing in contact with...
POST-LAB QUESTIONS 1. Balance the following equations and indicate the type of chemical reaction that each represents: a. ___ NH.CI() → ___ NH3(g) + __HCl(g) Type: b. __C(s, graphite). __Ha(e) → _CH(8) Type: c. _ Zn(s) + - FeCl(aq) → ___ ZnCl2(aq) + __Fe(s) Type: d. __C.He(s) - 02(g) → _CO2(g) + __ H2O(1) Type: e. AICI: (aq) + __Hz () Al (s) + HCl(aq) →_ Type: 1. Write balanced chemical equations for each of the following: a. Sodium sulfate...