2. In the same way, complete the columns for the initial concentrations of [Fe3+ Ji and [SCN-]I for Table 2 in Part C. Don't forget to show your work before filling the table in. Keep in mind that the total volume of each standard after dilution to the mark on the volumetric flask is 50.00 mL. Table 2 Calculations for reagents at Equilibrium с C Table 2 Calculations for reagents at Equilibrium Sample 0.00200 M 0.00200 M [Fe³+li [SCN-] i Fe(NO3)3 (mL) KSCN (mL) 1 2.0 8.0 2 4.0 6.0 3 5.0 5.0

2. In the same way, complete the columns for the initial concentrations of [Fe3+ Ji and [SCN-]I for Table 2 in Part C. Don't forget to show your work before filling the table in. Keep in mind that the total volume of each standard after dilution to the mark on the volumetric flask is 50.00 mL. Table 2 Calculations for reagents at Equilibrium с C Table 2 Calculations for reagents at Equilibrium Sample 0.00200 M 0.00200 M [Fe³+li [SCN-] i Fe(NO3)3 (mL) KSCN (mL) 1 2.0 8.0 2 4.0 6.0 3 5.0 5.0

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 5P

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In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)
Construct an "I-C-E" table that describes the equilibrium system of HCOOH with a nominal concentration of 0.50 M. Define clearly what is meant by "x" in the table. Use a squiggly li (~) to indicate approximate values. I - C E
II. Math Based Problems: (Show Work! You may write out on paper, scan in as a picture and use the insert signature function in Acrobat Reader DC to insert the picture) Use this equation to answer the following questions. H2PO4 (ag) + H20 (1) +→ H30* (ag) + HPO4 (ag) 1. Tadded 0.005 M solutions of each reactant together. At equilibrium, I found a 0.003 M concentration of HPO4?. (Hint: Does NOT require use of the quadratic equation) A. What is the Ka of my solution? B. What is the pH of my solution at equilibrium?
Calculate the value of the equilibrium constant for each of the following reactions in aqueous solution. a) HC2H3O2 + OH- <--> C2H3O2- + H2O b) C2H3O2- + H+ <--> HC2H3O2 c)HCl + NaOH <--> NaCl + H2O and I need an actual value for Kc not just the Kc formula which I already know. thanks.
Type your numerical answers in the box provided in three significant figures (e.g., 0.123). Do not report your answer in scientific notation. No need for units. If Canvas drops your last zero digit/s, it is OKAY. (e.g. 1.20 to 1.2). Consider a solution of 0.00500 M HBr for numbers 22-24. Determine the following: 22. equilibrium molar concentration of H3O = M. M. 23. equilibrium molar concentration of Br = %3D 24. pH =
For 0.10 M aqueous solutions of each of the following acids, which one will have the fewest number of product ions at equilibrium? O CH3COOH (K = 1.8 x 10-5) %3D O HF (Ka = 3.5 x 10-4) O HCIO2 (K, = 1.0 x 10 2) O HCIO (K, = 3.0 x 10 8) « Previous t (9).docx BluebeardBrothers.pdf Discussion week.docx upd wnkep ype here to search
3. Calculate the [Zn²+] in two solutions and compare the results (ZnS, Ksp = 2.5 X 10-22). (a) a solution that is in equilibrium with ZnS(s) and in which [H3O+] = 1.0 X 10-5 M and [H₂S] = 0.10 M. (b) a solution that is in equilibrium with ZnS(s) and in which [H3O+] = 1.0 X 10-³ M and [H₂S] = 0.10 M.
MISSED THIS? Read Section 18.8 (Pages 829 - 833). Part A A solution is made that is 1.0x10-3 M in Zn(NO,), and 0.130 Min NH3. After the solution reaches equilibrium, what concentration of Zn?+ (aq) remains? Express your answer using two significant figures. Zn]= 5.1• 10- M Submit Previous Answers Request Answer X Incorrect; Try Again; One attempt remaining
Review the reversible reactions given, along with the associated equilibrium constant Kat room temperature. In each case, determine whether the products or reactants are favored. A +B= CK=4.9 x 103 Choose... AgCl F Ag+ + Cl¯ Ksp=1.6 x 10-10 Choose.. CH3COOH CH3COO¯ +H* Ka=1.8 x 10-5 Choose... Al(OH)3 A1³+ Al* + 3 OH Ksp=3.7 x 10-15 Choose...
4. From smallest to biggest value of solubility, order the following salts with their Ks.p between brackets. a- Al(OH) (1.6 × 10-³³) b-BaCO (8.1×10) d- AgCl(1.8×10-10) c-Cu₂S(8.5×10-45) 5. Equilibrium constant for the synthesis of ammonia at 500C", is 6x102 .The reaction will shift to right in: a-[NH]-1×10 M. [Na]-1×10 M. [H.].-2×10 M b-[NH] 2x10 M. [Na].-1.5×10 M. [H.].-3.54x10 d-more than one choice. c- [NH] 1x10 M. [Na] 5M. [H₂]-1×10 M 6. What is the volume of 0.05M HCl that is required to neutralize 50 ml of a 0.10M Mg(OH); solution? a- 100ml c- 300ml b-200ml d-400ml e-500ml 7- On what electrode and What mass (in gram) of chlorine gas could be released from a solution of nickel(II) chloride by a current of 0.25 amperes flowing for 10 hours? (At. Wt Cl-35.5g/mol). a-3.311gm on cathode b- 6.603gm on anode c-3.311gm on anode d- 6.603gm on cathode 8- The reaction PCls (PCI+ Cl2, Drive to prove that the relationship between K, and K. is: a- K, K,RT b- K₁-K₁/RT c- K₂ K₂ RT d-K₂ K/RT…
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16. Calculate the solubility of Hg2Cl2 in grams per 100 ml of water. The solubility product constant of Hg2Cl2 = 1.3 x 10-13. You need to show your works.