▼ Part A - Solution 1 After being given a solution containing a set of unknown ions, you perform the following sequence of tests to determine the identity of the cations in solution: 1. A flame test produces no color 2. You take a small portion of the solution and add NaOH. A vapor is produced that turns red litmus blue. 3. You add HCI to solution, which results in the formation of a white precipitate. The supernatant is separated and used for the remainder of the tests. 4. The addition of buffered NH4*/NH3 to a portion of the supernatant from step 3 does not produce a precipitate. 5. The addition of ammonium oxalate to a portion of the superntant from step 3 does not produce a precipitate 6. The addition of a strong base to a portion of the supernatant from step 3 generates a precipitate. 7. The supernatant from step 6 is separated from the precipitate. The addition of HCI and K4Fe(CN)6 to the solution produces no reaction. Based on these tests, identify which of the following ions must be present, can be present, and cannot be present. Na+, NH4+, Ag+, Fe³+, Al³+, Cr³+, Ca2+, Mg²+, Ni²+, Zn²+

▼ Part A - Solution 1 After being given a solution containing a set of unknown ions, you perform the following sequence of tests to determine the identity of the cations in solution: 1. A flame test produces no color 2. You take a small portion of the solution and add NaOH. A vapor is produced that turns red litmus blue. 3. You add HCI to solution, which results in the formation of a white precipitate. The supernatant is separated and used for the remainder of the tests. 4. The addition of buffered NH4*/NH3 to a portion of the supernatant from step 3 does not produce a precipitate. 5. The addition of ammonium oxalate to a portion of the superntant from step 3 does not produce a precipitate 6. The addition of a strong base to a portion of the supernatant from step 3 generates a precipitate. 7. The supernatant from step 6 is separated from the precipitate. The addition of HCI and K4Fe(CN)6 to the solution produces no reaction. Based on these tests, identify which of the following ions must be present, can be present, and cannot be present. Na+, NH4+, Ag+, Fe³+, Al³+, Cr³+, Ca2+, Mg²+, Ni²+, Zn²+

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The titration on the right was performed by placing 10.00 mL solution in an Erlenmeyer flask and titrating it with 0.1000 M HCl. How would you classify the species being titrated in this titration? diprotic weak base monoprotic weak base triprotic weak acid triprotic weak base diprotic weak acid monoprotic weak acid
Answer both questions regarding Acids and Bases. After adding 50 mL of NaOH solution, the sample in the flask still had not turned pink. What error did the student make? and then, compare your percentage of HCI to the manufacturer’s percentage for the toilet bowl cleaner. We’re your results close? What might account for any differences? (Use the second photo for reference)
If 450 mL of some Pb(NO3)2 solution is mixed with 350 mL of 2.70 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.
If 550 mL of some Pb(NO3)2 solution is mixed with 100 mL of 7.50 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.
C. A solution made by mixing 4.08 g HCI with 6.16 g Ba(OH)2 in 0.600 L total solution. Start by writing a balanced chemical equation for this process, complete with phase symbols: Mass of excess reactant leftover = pH =
A solution contains 7.73×10-3 M potassium carbonate and 8.42x10-3 M sodium hydroxide. Solid magnesium nitrate is added slowly to this mixture. A. What is the formula of the substance that precipitates first? formula = B. What is the concentration of magnesium ion when this precipitation first begins? [Mg?+] =| M
40 mL of LiOH are titrated to the equivalence point with 65 mL of 1.2 x 10-2 M HNO3. Find the concentration (molarity) of the LiOH solution.
M52.
Use the reported molarity For vinegar ( average value) To calculate the percent by mass of HC2H302 and vinegar. Assume the density of the solution is 1.036 g/ml
Please don't provide handwritten solution
Don't provied handwriting solution.
I dont know how to do this question