(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 cati...
(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+)
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(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 cati...
POST LAB QUESTIONS Answer the following questions in your lab notebook: 1. Give the chemical formula...
POST LAB QUESTIONS Answer the following questions in your lab notebook: 1. Give the chemical formula for a single chemical reagent that would : (a) separate Ag from Cut b) separate AgCl from PbCl2 - separate Cu2+ from Mat (d) separate Fet from Zn2+ (e) Dissolve Zn(OH), but not Fe(OH)3 (f) separate Ba2+ from Mn2+ and Zn2+ 2. Write balanced ionic chemical equations for: a. The dissolution of AgCl in excess ammonia b. The precipitation of Pb * to PbCrO4(s)...
2. Complete and balance the following net ionic equations. If no reaction occurs, write NR. Tables...
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 form complex ions in the presence of excess hydroxide ions and aqueous ammonia. a. Mg(OH)2 + OH excess b. Cu(OH)2 + OH"excess c. Co(OH)2 + OH → d. Fe(OH)3 + NH3(aq) excess → e. Pb(OH)2 + NH3(aq) excess →
1IC LUDOUCO 1. Complete and balance the following net ionic equations. If no reaction occurs, write...
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...
2. How are the Group I cations first precipitated from solution? 3. Write the net-ionic equation...
2. How are the Group I cations first precipitated from solution? 3. Write the net-ionic equation for the initial precipitation of any one Group I cation from your unknown solution. 4. Lead(II) chromate is used as a yellow pigment in paints. Write the net-ionic equation for its formation in this Experiment during the confirmatory test for lead(II). 5. When ammonia is added to a white precipitate of mercury(I) chloride, the precipitate turns grayish-black. Write the net-ionic equation for what happens,...
Write balanced molecular, ionic and net-ionic equations for 10 reactions (8 precipitate (P) and 2 neautralization)...
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...
3. Pb(OH)2 (8) is amphoteric and forms the complex ion Pb(OH)/(aq) with excess OH in solution....
3. Pb(OH)2 (8) is amphoteric and forms the complex ion Pb(OH)/(aq) with excess OH in solution. Write the balanced equilibrium equation of Pb(OH)2 (s) in the presence of excess hydroxide. 4. A solution contains Pb(NO3)2 and Zn(NO3)2. Consult the solubility table and answer the following questions: a. NaOH (aq) is added to the solution. What precipitate (or precipitates) forms? b. Can you separate the two metal ions using NaOH? c. Nat (aq) is added to the solution. What precipitate (or...
In aqueous solution, the Co 2+ ion forms a complex with six ammonia molecules. Write the...
In aqueous solution, the Co 2+ ion forms a complex with six ammonia molecules. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the last step in the formation of the complex.
[HCO 3 Na] NaOH co H.CO] Hc1] Write balanced net ionic equations that show how a...
[HCO 3 Na] NaOH co H.CO] Hc1] Write balanced net ionic equations that show how a buffer containing NaHCO, and Na.co, maintains its pH when a small amount of HCl or NaOH is added. +OHO + H₂O Ho +HO
1. Write balanced net ionic equations for the following oxidation-reduction reac- tions: a. Hydrogen sulfide is...
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...
13. Write the balanced molecular, full ionic and net ionic equations and give the name(s) and...
13. Write the balanced molecular, full ionic and net ionic equations and give the name(s) and formula(s) of the spectator ion(s) in the reaction between an aqueous solution of Cd(NO3)2(aq) and an aqueous solution of K2S(aq) that results in the formation of an insoluble sulfide compound.
POST LAB QUESTIONS Answer the following questions in your lab notebook: 1. Give the chemical formula for a single chemical reagent that would : (a) separate Ag from Cut b) separate AgCl from PbCl2 - separate Cu2+ from Mat (d) separate Fet from Zn2+ (e) Dissolve Zn(OH), but not Fe(OH)3 (f) separate Ba2+ from Mn2+ and Zn2+ 2. Write balanced ionic chemical equations for: a. The dissolution of AgCl in excess ammonia b. The precipitation of Pb * to PbCrO4(s)...
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 form complex ions in the presence of excess hydroxide ions and aqueous ammonia. a. Mg(OH)2 + OH excess b. Cu(OH)2 + OH"excess c. Co(OH)2 + OH → d. Fe(OH)3 + NH3(aq) excess → e. Pb(OH)2 + NH3(aq) excess →
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...
2. How are the Group I cations first precipitated from solution? 3. Write the net-ionic equation for the initial precipitation of any one Group I cation from your unknown solution. 4. Lead(II) chromate is used as a yellow pigment in paints. Write the net-ionic equation for its formation in this Experiment during the confirmatory test for lead(II). 5. When ammonia is added to a white precipitate of mercury(I) chloride, the precipitate turns grayish-black. Write the net-ionic equation for what happens,...
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...
3. Pb(OH)2 (8) is amphoteric and forms the complex ion Pb(OH)/(aq) with excess OH in solution. Write the balanced equilibrium equation of Pb(OH)2 (s) in the presence of excess hydroxide. 4. A solution contains Pb(NO3)2 and Zn(NO3)2. Consult the solubility table and answer the following questions: a. NaOH (aq) is added to the solution. What precipitate (or precipitates) forms? b. Can you separate the two metal ions using NaOH? c. Nat (aq) is added to the solution. What precipitate (or...
[HCO 3 Na] NaOH co H.CO] Hc1] Write balanced net ionic equations that show how a buffer containing NaHCO, and Na.co, maintains its pH when a small amount of HCl or NaOH is added. +OHO + H₂O Ho +HO
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...
13. Write the balanced molecular, full ionic and net ionic equations and give the name(s) and formula(s) of the spectator ion(s) in the reaction between an aqueous solution of Cd(NO3)2(aq) and an aqueous solution of K2S(aq) that results in the formation of an insoluble sulfide compound.
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