B. The remaining brown-black precipitate is now acidified with 6 M HCI, heated and then centrifuged. A colorless solution is decanted from the brown-black precipitate. The solution is made basic with 6 M NH3, thioacetamide is added and it is heated. No change is observed. Which cation IS NOT present in the unknown? Select all answer choices that apply. A. Cu2+ B. Cd2+ C. Sn4+ D. BI3+

B. The remaining brown-black precipitate is now acidified with 6 M HCI, heated and then centrifuged. A colorless solution is decanted from the brown-black precipitate. The solution is made basic with 6 M NH3, thioacetamide is added and it is heated. No change is observed. Which cation IS NOT present in the unknown? Select all answer choices that apply. A. Cu2+ B. Cd2+ C. Sn4+ D. BI3+

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

1. The Ksp of gold (I) chloride is 2.0 x 10-13. The Kr of the gold (I)-cyanide complex ion is 2.0 x 103%. A. Write the balanced net ionic equation for the reaction between AuCl and NaCN that produces the gold (I)-cyanide complex ion. B. Determine the value of K for the above chemical reaction. C. Determine the solubility of AuCl in a 0.20 M solution of NaCN.
QUESTION 24. Acetic acid is a convenient buffer system in the slightly acidic range. What mass of sodium acetate (NaCH3CO2) must be added to 0.750 L of 0.116 M solution of acetic acid to make a buffer of pH = 5.00? The Ka of acetic acid is 1.8E-5. How many moles of acid are required to change the pH of the solution in part a by 0.05 pH units?
Part B: Calculate the molar solubility of Ca(OH)2 in the presence of the dissolved CaCl2 for each trial. Thank you!!
During the Volhard titration method: A. Fe(III) serves as the indicator. B. An organic compound serves as the indicator. C. Chromate- serves as the indicator. D. A weak acid/base serves as the indicator. E. Cr(VI) serve as the indicator. F. No indicator is needed.
Why we have to use the KHP as a primary standard solution? A. Pure crystals B. Mono protic acid C. High molar mass D. All
Titration of 0.1 M HCl against a 25mL liquor mixture of NaOH and Na2CO3 using phenolphthalein indicator requires 17.5mL of the acid for the endpoint. After this, methyl orange was added and 3.5mL of HCl was again required for the next endpoint. A. Write separate equations for reactions for the two endpoints B. Calculate the amount in milligrams of NaOH and Na2CO3 in the mixture
1. Calculate the final [Ag1+] concentration in solution when 0.035 moles of AgNO3 are added to 500. mL of 0.21 M NaCN. Assume the volume remains constant. Ksp = 1.2 ✕ 10-16 for AgCN. 2. What [Ag1+] is required to start precipitation of AgOH from a saturated solution of Mg(OH)2? Ksp = 3.0 ✕ 10-8 for AgOH and Ksp = 2.7 ✕ 10-11 for Mg(OH)2. 3. If 13.0 mL of 0.19 M MgCl2 are mixed with 21.9 mL of 0.54 M NaOH, what will be the final concentration of Mg2+ in solution when equilibrium is established? Assume the volumes are additive. Ksp = 1.2 ✕ 10-11 for Mg(OH)2.
Concerning EDTA titrations, which of the following is incorrect? 1. OEDTA forms 1:1 complexes with metal ions. 2. OThe most widely used indicators are murexide and Eriochrome Black T. 3. Oln presence of NaOH, EDTA reacts only with Mg2 ions, using murexide indicator. 4. OThe water hardness is usually expressed as CACO3 mg /L water. 5. OEDTA solution was standardized using Zinc Sulfate.
-Why is there a need to standardize the NaOH solution? -Why is there a need to use CO2-free water in this analysis? -Discuss the principle behind why phenolphthalein changes color.
In this experiment, the color change from pink/violet to colorless during the titration is caused by: Group of answer choices a.change from MnO4– to Mn2+ b.change from Fe2+ to Fe3+ c.change from H+ to H2O d.the addition of an indicator.
Explain every statement... With good hand writing.
Spectroscopic or (spectrophotometery) determination of an equilibrium constant experiment A) Mention the steps to prepare a 50.0 ml of 0.15 M [ FeSCN 2+ ] solution from a 0.4 M [FeSCN 2+ ] stock solution? B) Why the nitric acid is added in the preparation?