1. Arsenious acid a weak acid with pKa = 9.22.HASO2 H + AsO₂ K = 10-9.22(a) If 103 M of the herbicide NaAsO2 are added to 1L of distilled water at 25 degrees C, what is theresulting pH? Please list species, list sufficient constraints to solve the system, draw a log C-pH diagram,and solve for the system pH both graphically and algebraically. Assume complete dissociation of the addedsalt. (15 points)

Answered: Image /qna-images/answer/a4084910-d25d-4291-921a-cecd90043c5e.jpg

Answered: 1. Arsenious acid a weak acid with pKa…

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...

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8.An organic compound was analyzed and found to contain 55.8% C, 7.03% H, and 37.2% O. A 1.500 g sample of the compound was vaporized and found to occupy 530 cm 3 at 100°C and 740 torr. Which of the following is the correct molecular formula of the compound? A) C2H30 B) C,H4O2 C) C3H2O D) C4H6O2 E) C2H3O2
A chemist titrates 120.0 ml. of a 0.7695 M trimethylamine ((CH₂)₂N) solution with 0.1789M HNO, solution at 25 °C. Calculate the pH at equivalence. The PK, of trimethylamine is 4.19. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HNO, solution added. PH-0
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The third step is to find the ph
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How many grams of citric acid and sodium citrate dihydrate must be added to 1L of water to produce a solution with pH 3.9 and a total solute concentration of 1 mM? (MW Salt = 294.09; MW Acid = 192.13) I found the answer below, but my calculation does not match it. Can you please show me in detail how the calculation from the image below was done? How did they get the amount of citric acid and citrate? Please make sure that you get the same result and the calculation is completely detailed.
Calculate the pH of a 0.10 M NaCN solution. Ka of HCN = 6.2 x 10-10. Show the following steps: Pertinent Equilibria Definition of unknown Equilibrium constant expressions Mass-balance equations Charge-balance expression Number of independent equations and unknowns Approximations Solution to equation Checking the validity of approximation
A water at a drinking water plant has an alkalinity of 4*10-3 eq/L at a pH of 9.5. a) Find the TOTCO3 of this water, assuming carbonate is the only significant weak acid/base species b) 1.5*10-3 M HOCl is added to the water for disinfection. What will be the final pH and alkalinity of this water?
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For different enzymes, there is an optimum pH at which the enzyme is most active. For example, for enzymes of gastric juice optimum pH 1-2, for duodenal enzymes pH 7.7, for liver enzymes pH 9.5, etc. Determine which medium (a or b) is most favorable for each of the enzymes mentioned above if the following substances are added to 1.0 liter of water: a) 0.040 mol KOH and 0.030 mol HBr; b) 4.0 10-9 mol HNO3. Neglect the change in the volume of the solution. Confirm your answer with calculations.
A 0.0614 M solution of butyric acid, C₂HCOOH is 0.066 % ionized. a) Calculate concentration at equilibrium for each reagent. Report your answer to 4 significant figures. [C₂H₂COOH] = [H₂O¹] = [C₂H,COO]=[ M M b) What is the pH of the acidic solution? c) What is K, of the acid? 2.68-10 06.09-108 pH = 02.57-10 0.0613 01.01-10-10

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