The colorless solution of an unknown solid turned blue litmus red and emitted an odor of ammonia upon addition of NaOH. A pale yellow precipitate was observed upon reaction with AgNO, and a white precip- itate was observed upon addition of Pb(NO,),. Bubbles were not evident upon addition of HCI. Identify the unknown from the list of possibilities in the Introduction to this experiment.
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- 2. A saturated solution of an unknown solid reacted with AGNO, to give a pale yellow precipitate, and also reacted with Pb(NO,), to give a white precipitate. Based on only these two test results, you can conclude that the unknown solid contains which anion? Write the correct balanced equations for reaction of the anion with each of these reagents. Resl of flae teeperfore wunkm Reaction of HICth onken 7 Reastie of ARNO wi nksovny ion cridn of PoNO Waown selcv encity of3. To verify the existence of silver in your solution, one should first form a white precipitate by addition of NaCl. Next, the precipitate should dissolve in aqueous ammonia. Silver can re- precipitate by addition of 6M HNO,. Using chemical equations, describe the identity of the product formed in each step. E (Your three steps should be after addition of NaCl, after addition of ammonia and after addition of HNO,.) 3° 3° it in mirod with sodium chloride3. The colorless solution of an unknown solid turned blue litmus red and emitted an odor of ammonia upon addition of NaOH. A pale yellow precipitate was observed upon itate was observed upon evident upon addition of HCI. Identify the unknown from the list of possibilities in the Introduction to this experiment. reaction with AgNO, and a white precip- 3 addition of Pb(NO),. Bubbles were not 2°
- A solution containing a mixture of metal cations was treated as outlined. 1. Dilute HCl was added and a precipitate formed. The precipitate was filtered off. 2. H, S was bubbled through the acidic solution. No precipitate formed. 3. The pH was raised to about 9 and H, S was again bubbled through the solution. A precipitate formed and was filtered off. 4. Finally, sodium carbonate was added to the filtered solution and no precipitate formed. What can be said about the presence of each of these groups of cations in the original solution? Cation group Description Present in the original solution? Ag*, Pb²+, Hgž+ form insoluble chlorides Bi3+, Cd2+, Cu²+, Hg²+, form acid-insoluble sulfides Pb2+, Sb³+, Sn²+, Snª+ Al3+, Co+, Cr³+, Fe²+, form base-insoluble sulfides Fe+, Ni?+, Mn²+, Zn²+ or hydroxides Ba?+, Ca2+, Mg²+, Sr²+ form insoluble carbonates Lit, Na+, K*, completely soluble Answer Bank None of these ions were present. unknown At least one of these ions was present. All of these ions…1. The color of Na,CO3 solution on adding Bromo cresol green indicator changes from to in absence and excess of HCl respectively. (A Yellow; Blue (B) Blue; Yellow Green; Yellow D) Yellow; GreenA solution containing a mixture of metal cations was treated as outlined. 1. Dilute HCl was added and a precipitate formed. The precipitate was filtered off. 2. H,S was bubbled through the acidic solution. No precipitate formed. 3. The pH was raised to about 9 and H,S was again bubbled through the solution. A precipitate formed and was filtered off. 4. Finally, sodium carbonate was added to the filtered solution. A precipitate formed and was filtered off. What can be said about the presence of each of these groups of cations in the original solution? Cation group Description Present in the original solution? Ag+, Pb?+, Hg3+ ,2+ form insoluble chlorides Bi3+, Cd²+, Cu²+, Hg²+, Pb2+, Sb3+, Sn²+, Sn++ Al3+, Co2+, Cr3+, Fe2+, Fe3+, Ni2+, Mn2+, Zn²+ form acid-insoluble sulfides form base-insoluble sulfides or hydroxides Ba2+, Ca2+, Mg²+, Sr²+ form insoluble carbonates Lit, Na*, K*, NH completely soluble Answer Bank unknown At least one of these ions was present. All of these ions were…
- A samp;e of sodium sulfate solution is added to a solution of silver nitrate casusing a white solid to appear. Which is the precipitate formed in this reaction?A solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H,S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Cd²+ Ag* Ba2+ Mn2+ Mg2+ Fe2+ A13+ Pb2+ Sn2+ Lit Hg3* Hg²+ Sb3+ Answer BankA solution containing a mixture of metal cations was treated with dilute HCl and no precipitate formed. Next, H, S was bubbled through the acidic solution. A precipitate formed and was filtered off. Then, the pH was raised to about 8 and H, S was again bubbled through the solution. A precipitate again formed and was filtered off. Finally, the solution was treated with a sodium carbonate solution, which resulted in no precipitation. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it is possible they were present in the original mixture. Definitely present Definitely absent Possibly present Answer Bank Hg3+ Pb2+ Lit Bj³+ Sn2+ Ni2+ A13+ Ag* Zn2+ Ba2+ Mg2+ Hg²+ Cu?+
- Which of the following statements is true regarding permanganimetry? a) Permanganate solution can oxidize water which is catalyzed by the presence of manganese dioxide or manganese ion. b) The light pink endpoint color for permanganimetry tends to fade with time due to the catalytic reaction. c) Standardization of the permanganate titrant is carried out at elevated temperature with sodium oxalate. d) all of these e) none of theseA solution containing a mixture of metal cations was treated with dilute HCl and a precipitate formed. The solution was filtered and H,S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 8 and H2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in the formation of a precipitate. Classify the metal ions based on whether they were definitely absent from the original mixture or whether it is possible they were present in the original mixture? Definitely absent Possibly present Ag+ Cu2+ Ba2+ Mn2+ Ni2+ AB+ Lit Sn++ Mg2+ Hg2+ Sb3+ Hg2+ Pb2+Determination of Chloride lon by the Mohr Method Introduction: Objectives: Methods & Materials: Discussion and Conclusion 1. What is the role of chromate ions in chloride determination? 2. Why pH range is important in chloride determination? 3. Would the analytical results by the Mohr method for chlorides be higher, lower or the same as the true color value if any excess of indicator were accidentally added to the sample? Why?