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How to test the Na+ in the original solution? and NH4+?
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- 1. A 0.0450 M Ca(X), has a pH of 11.079. CaX), is composed of a Ca cation and an unknown anion X, which undergoes hydrolysis. A. Write the balanced dissociation reaction of Ca(X), into its ions. Write your answer on your solution sheet B. Write the balanced hydrolysis reaction of the unknown anion, X. Write your answer on your solution sheet C Calculate the Kor K of X D. Given the following K, values of different weak acids, determine the identity of X Weak acids KI HIO 2.00 x 10-11 HCN 6.17 x 10-10 CH₂COOH 180 x 10-5 HNO₂ 4.00 x 10-48. We mix 200 mL of a solution (S1) of caustic potash of pH1=10.7 with 30 mL of a solution (S2) of caustic potash of pH2 = 11.3. a. Calculate the concentration of HO ions in Sj and S2. b. Calculate the concentration of HOʻ ions in the final solution. c. Deduce pH of the final solution.A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.072 M KOH. What volume KOH must be added to give a pH of 5.56? Ka1 = 1.42 × 10–3 and Ka2 = 2.01 × 10–6. Show all of your work on your scratch paper and upload it as a comment to this quiz assignment. Correct!
- Do you always have to use a primary standard in the standardization of titrant? Why or why not?Which is the correct order of steps in the preparation of a hydrochoric acid standard solution with sodium bicarbonate standard solution. I. Dissolved sodium carbonate (13.25 g) in about 150 mL of distilled water in a beaker II. Solution of sodium carbonate was transferred into a volumetric flask and diluted to mark before mixing. III. Weigh the appropriate amount of the primary standard. IV. Titrate with enough volume of the acid to completely neutralize the base. V. Transfer 10.00 ml primary standard into an erlenmeyer flask and add indicator III, I, II, V, IV III, II, I, V, IV V, III, I, II, IV V, IV, III, I, IIA student titrated CH3COOH with NaOH and stopped the titration when the color of the analyte changed from clear to pink. Choose the correct picture that represents the analyte solution. 3 QLOOOH O a. 3 b. 2 O c. 4 O d. 1 CHOOO 2. 4. OH
- Consider the titration of 300.0 mL of 0.500 M NH3 (Kb = 1.8 x 105) with 0.500 M HNO3. What is the pH of the solution when 11 mL of 0.500 M HNO3 has been added with the base? **Report your answer to two decimal places. DO NOT worry about significant figures.**A student titrates 10.0 mL of 2.0 M formic acid, HCO,H (K.= 1.8 x 10-4), using 1.0 M sodium hydroxide, NaOH. 1. What volume of NaOH solution would be needed to reach the equivalence point? a. 10.0 mL b. 20.0 mL c. 30.0 mL d. 40.0 mL1. Molarity of the NaOH solution 0.238 mol/L Trial 1 Trial 2 Trial 2. Volume of H;PO4 added to flask 22.0 mL 22.0 mL 22.0 mL 3. Initial NaOH volume _0.25_ mL _0.75_ mL 0.55 mL 4. Final NaOH volume 17.60_ mL 18.20_ mL _17.90_ mL 5. NAOH volume used for titration to reach green end point mL mL mL 6. NaOH volume used for titration 7. Moles of NaOH used for titration mol mel mel 8. Moles of H;PO4 that reacted mol mel mol 9. Volume of H;PO4 added to flask L 10. Molarity of H3PO4 mol/L mol/L mol/L
- What is the methodology of acid base titration for sodium hydroxide and hydrochloric acid.a. A 1.00 liter solution contains 0.45 moles nitrous acid and 0.35 moles potassium nitrite .If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase. b. A 1.00 liter solution contains 0.38 M ammonia and 0.49 M ammonium bromide. If 0.120 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase. E. The ratio of [NH3] /…1. What process is responsible for the increase in the total negative charge as soil pH increases? a.Protonation b. Dehydration reaction c. H+ bond formation d. Deprotonation 2. What ionic form of nutrient would most likely be easily leached/washed out from the soil? a. Cation b. Conjugate ion c. Anion d. Spectator ion 3. When a soil with cation-Ca complexed is poured with distilled water, what would you expect if the leachate will be reacted with ammonium oxalate? a.The leachate will be negative for calcium b. The leachate will manifest a false negative c. The leachate will be positive for Calcium d. The leachate will manifest a false positive
