2. For the solutions that will be prepared in Step 2 of Part I below, calculate the [FeSCN2+].If the calculations done for question 1 give ratios of [Fe3+]: [SCN] greater than 100 : 1 it canbe presumed that the reaction runs with SCN as the limiting reactant and therefore, it can beconcluded that [SCN] = [ FeSCN2+]. Record these values in the table below.Beaker number1[FeSCN²+]234

step: 1Since SCN- is a limiting reagent. So [FeSCN+2] = [SCN-]To calculate diluted concentrationuse…

Answered: 2. For the solutions that will be…

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 4RQ: Consider the equation G = -nF. What are the four terms in this equation? Why does a minus sign...

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Consider the equation G = -nF. What are the four terms in this equation? Why does a minus sign appear in the equation? What does the superscript o indicate?
What mass of solid AgBr is produced when 100.0 mL of 0.150 M AgNO3 is added to 20.0 mL of 1.00 M NaBr?
You are given four different aqueous solutions and told that they each contain NaOH, Na2CO3, NaHCO3, or a mixture of these solutes. You do some experiments and gather these data about the samples. Sample A: Phenolphthalein is colorless in the solution. Sample B: The sample was titrated with HCl until the pink color of phenolphthalein disappeared, then methyl orange was added. The solution became pink. Methyl orange changes color from pH 3.01 (red) to pH 4.4 (orange). Sample C: Equal volumes of the sample were titrated with standardized acid. Using phenolphthalein as an indicator required 15.26 mL of standardized acid to change the phenolphthalein color. The other sample required 17.90 mL for a color change using methyl orange as the indicator. Sample D: Two equal volumes of the sample were titrated with standardized HCl. Using phenolphthalein as the indicator, it took 15.00 mL of acid to reach the equivalence point; using methyl orange as the indicator required 30.00 mL HCl to achieve neutralization. Identify the solute in each of the solutions.
In Questions 1 through 6, you will be calculating the initial concentrations of Fe³+ ([Fe³+10) and SCN ([SCN]o) for each of the reactions you will perform. You should transfer the answers to these questions to the appropriate ICE table(s) on the "Data and Calculations" sheet. In all five reactions, you will be using 5.0 mL of 0.0020 M Fe(NO3)3. Each reaction mixture will be diluted to a final volume of 10.0 mL. What is [Fe³+]o in all five of the reactions you will study? Type your answer, WITHOUT UNITS, in the box below. Include 2 significant figures. If you want to enter your answers in scientific notation, use the format that Blackboard recognizes: 1.5 x 10-3 would be entered as 1.5E-3 (no spaces). QUESTION 2 In Test Tube 1, you will be using 1.0 mL of 0.0020 M KSCN. Each reaction mixture will be diluted to a final volume of 10.0 mL. What is [SCN ] in Test Tube 1? Type your answer, WITHOUT UNITS, in the box below. Include 2 significant figures. QUESTION 3 In Test Tube 2, you will be…
A7
4. During Part 1, which reactant (Fe3+ or SCN-) is in excess and which is limiting? What is the purpose of making one reactant in excess? (Connect to Le Chatelier's Principle) How will you know the concentration of Fe(SCN)2+?
Which of the following is the correct solubility product constant expression for PBSO4? O Kp = [Pb2]°[So,212 %3D Kp = [Pb2*][SO,2 ] O Ksp = 2[Pb2'12[SO,2] %3D Ksp = 2[Pb2']² 2[So,212 %3D
part b
Question 93.
Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+₁ (aq) (Kf = 4.8e+12) A solution is made by mixing 15.0 mL of 0.90 M CuSO4 and 1.00 L of 0.530 M NH3. Assume additive volumes to answer the following questions. Give all answers to three sig figs. a) What is the concentration of NH3 in the resulting solution? [NH3] = .47 M b) What is the concentration of Cu(NH3)42+ in the resulting solution? [Cu(NH3)4²+] = 5.3e-2 X M c) What is the concentration of Cu²+ in the resulting solution? [Cu²+] = 5.3e-2 X M
3a. Cd2[Fe(CN)6] is sparingly soluble: Cd2[Fe(CN)6](s) ↔ 2Cd²+ + [Fe(CN)6]ª¯ with the solubility product L 5.0 × 10-18 M³. Calculate the mass of Cd2 [Fe(CN)6] that == can dissolve in 2.0 liters of water? Molar mass/g·mol‍¹: Cd₂[Fe(CN)6]: 436.8. 3b. Cd2[Fe(CN)6] reacts with chloride due to complex formation: 2- 4- K = 1.0 × 10-14 M¯5 Cd2 [Fe(CN)6] (s) + 8C1¯¯ ↔ 2[CdC14] ²¯ + [Fe(CN)6] 4 Taking this equilibrium into account, calculate the mass of Cd2 [Fe(CN)6] that can dissolve in 2.0 liters of 1.5 M KCl.

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