Write out the dominant chemical reaction/equilibrium that wifl determine solution pH when 0.1 mole of each of the following compounds is dissolved in 1 L water. DO NOT CALCULATE pH. a. Na[CH;CH2CO2] b. HC1O4 с. (CН3):N
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![Write out the dominant chemical reaction/equilibrium that wil determine solution
pH when 0.1 mole of each of the following compounds is dissolved in 1 L water. DO NOT
CALCULATE pH.
a. Na[CH3CH2CO2]
b. HC104
c. (CH3)3N
d.
HS
CH2OH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffba53fc5-f280-45c2-b123-0feb9eb35059%2Ffc32860c-a446-40b9-a57d-18a404228dfd%2Fhwapu_processed.jpeg&w=3840&q=75)
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- Hydrogen sulfide (H2S) is an odorous gas that can be stripped from solution by bubbling air through the solution. H2S when dissolved in water is also a weak acid that can deprotonate to bisulfide ions which are not removed by air stripping. That reaction is ?2?--> H^+ + ??^- With equilibrium constant Ka=0.86x10-7.Find the fraction of hydrogen sulfide in the H2S form at pH 6 and pH 8. At which pH would you expect to have an easier time to strip away H2S gas?C10H12NO4N is a weak base and has a Kb of 1.58x10-10. One, 0.650g, is dissolved in 235mL of distilled water. a. What is the initial concentration, in units of molarity, of the zalcitabine? b. Write an expression for Kb for zalcitabine. c. What are the equilibrium concentrations of the products and reactant? d. What is the pH, pOH, and % ionization of this weak base?Tris(hydroxymethyl)aminomethane [(HOCH2)3CNH2—Tris, or THAM] is a weak base frequently used to prepare buffers in biochemistry. Its Kb is 1.2 × 10−6 and pKb is 5.92. The corresponding pKa is 8.08, which is near the pH of the physiological buffers, and so it exhibits good buffering capacity at physiological pH. What weight of THAM must be taken with 100 mL of 0.50 M HCl to prepare 1 L of a pH 7.40 buffer?
- To produce a formate buffer solution that is at a pH of 4.06, what should the concentration of the formate (HCOO-) ion be given 0.366 M of formic acid (HCOOH)? Formic acid has a Ka of 1.8 x 10^4.Considering the equilibrium below, which of the following is/are TRUE? CH3OH + HNO2 = CH3OH2+ + NO2- CH3OH is a base NO2 is a conjugate acid IAM. I only SXY. II only AND. I and II IKI. Neither I nor II Which of the following statements is/are ALWAYS TRUE? A higher Ksp value equates to a higher solubility regardless of the salt type When Qsp = Ksp, the system is at equilibrium CHM. I only EQU. II only LIB. I and II RIA. Neither I nor IIA solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution. The Ka of benzoic acid is 1.36 × 10-3. A) benzoate ion B) benzoic acid C) H3O+ D) H2O E) This is a buffer solution: the pH does not change upon addition of acid or base.
- A. What two compounds would be best to use in preparing a pH 9.0 buffer solution? justify your answer. Assume you have the acids and the sodium salts of their conjugate bases available to you. Answer: The two compounds best fo preparing a buffer solution with a pH of 9.0 would be hydrocyanic (HCN) and phenol (HOc6H5) because their pKa values are 9.40 and 9.80 respectively making their pH levels the closest to 9. B. WHat mass ration of sodium to acid is needed to prepare this buffer? C. Can this buffer solution better resist pH changes from a string acid addition or strong base addition?A solution is prepared by dissolving 0.23 mol of benzoic acid and 0.27 mol of sodium benzoate in water sufficient to yield 1.00 L of solution.The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution. The Ka of benzoic acid is 6.3 ⋅ 10-5. A. H2O B. benzoic acid C. H3O+ D. benzoate E. This is a buffer solution: the pH does not change upon addition of acid or base.Consider the following reactions. Explain how the addition of strong acidinfluences the solubility of CaCO3.CaCO3(s) <----> Ca2+ + CO32-(aq)CO32-(aq) + H3O+(aq) ----> HCO3(aq) + H2O(l)
- A solution is prepared by dissolving 0.23 mol of chloroacetic acid and 0.27 mol of sodium chloroacetate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the __________ present in the buffer solution. The Ka of chloroacetic acid is 1.36 × 10-3.An enzyme-catalyzed reaction is carried out in a 250 mL solution containing 0.1M TRIS buffer. The pH of the reaction mixture at the start was 7.8. As a result of the reaction, 0.003mol of H+ was produced. What is the ratio of TRIS base to TRIS acid at the start of the experiment? What is the ratio at the end of the experiment? What is the final pH?Your research advisor asks you to prepare a buffer solution at pH = 3.50 with capacity of about 0.100 M. Given the following solutions available (of any concentration), determine which species would give the best buffer, and give possible concentrations of the conjugate species. Dimethylamine pKb = 3.27; ethlyamine pKb = 3.35; aniline pKb =9.13; sodium nitrite pKb = 10.60.