1S Refer 2. An "iodide/chloride/sulfate" unknown solution gave a white precipitate with aqueous AgNO3, and after centrifuging, the supernate gave a white precipitate with aqueous Ba(NO3)2. The original white precipitate dissolved completely in aqueous NH4OH, and produced a white precipitate after adding aqueous HNO3. State the anion(s) confirmed present and absent in the unknown solution. Anion(s) present Anion(s) absent

1S Refer 2. An "iodide/chloride/sulfate" unknown solution gave a white precipitate with aqueous AgNO3, and after centrifuging, the supernate gave a white precipitate with aqueous Ba(NO3)2. The original white precipitate dissolved completely in aqueous NH4OH, and produced a white precipitate after adding aqueous HNO3. State the anion(s) confirmed present and absent in the unknown solution. Anion(s) present Anion(s) absent

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

Make a complete schematic diagram for the precipitation separation and identification of group lll cations.
None
The % (w/w) I- in a 0.6712-g sample was determined by Volhard titration. After adding 50.00 mL of 0.05619 M AgNO3 and allowing the precipitate to form, the remaining silver was back-titrated with 0.05322 M KSCN, requiring 35.14 mL to reach the endpoint. Report the %(w/w) I- in the sample. [Ans. 17.76 % (w /w)]
Chemistry A 0.3500 g sample of impure KI is treated with 0.1942g of pure K2CrO4 and the solution is boiled to expel all of the liberated iodine. The cooled solution is then treated with excess KI and the liberated I2 titrated with 0.100N sodium thiosulfate, requiring 10.00ml. Find the percentage purity of the original sample of KI
Answer 1 of the following 2 questions. 7.A Consider an aqueous solution of CaF2(ag) with Kg = 4.0x10-11. (a) What is its solubility in water? (b) What is its solubility in the presence of 0.05 M sodium fluoride? (c) Justify any assumptions you made in (a) and (b).
Give a list of laboratory apparatus and equipment that are to be utilized for the preparation of 500 mL of 0.2 M K4 Fe (CN) 6. Also give the procedure of preparation.
Gravimetric Analysis. Please include complete solution, thank you. 4.) A 0.2025 g sample consisting of only BaCl2 and KCl required 20.25 mL of 0.1200 M AgNO3 solution for the quantitative precipitation of chloride. Calculate the %Ba and %K in the sample.
The concentration of sulfate in a solution containing a mixture of sulfuric acid is to be determined. A 25.0 mL portion of the sample is treated with 10.00 mL of 0.0500 M BaCl₂. The resulting precipitate is filtered off and the supernatant solution containing the Ba²⁺ is then titrated with 0.0354 M EDTA which gives an end point at 7.45 mL. (a) Identify the type of EDTA titration method used. (b) Calculate the molar concentration of sulfate in the sample
A 0.5g sample of CaCO3 is dissolved in an acidic solution. The calcium is precipitated as Ca2C2O4H2O and the dry precipitate is found to weigh 0,72. What is the percentage of CaO in the the sample
Kk.468.
[7] please help me answer this question and show your solution/explanation after.
A solution is made by mixing 500.0 mL of 0.02018 M Na, HASO, with 500.0 mL of 0.04078 M NaOH. Complete the mass balance expressions for the sodium and arsenate species in the final solution. (HASO + [HSO,] 1.219 ×10¬4 M [Na*] = 5.304 x10-6 M + Post a new auestion tv O, hulu 14 MacBook Pro 2$ % & 4 5 7 8. de Y U K C V N M. command option .. .- * 00