In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH₂)3 CNH2, often abbreviated as Tris. At 25 °C, Tris has a PKL of 5.91. The hydrochloride of Tris is (HOCH₂)3 CNH3C1, which can be abbreviated as TrisHCI. Part A What volume of 10.0 mol L-¹ NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCI? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 10 Π| ΑΣΦ Submit 3 Previous Answers → O Part B Complete previous part(s) Part C Complete previous part(s) < Return to Assignment X Incorrect; Try Again; 4 attempts remaining ? Provide Feedback mL

In the study of biochemical processes, a common buffering agent is the weak base trishydroxymethylaminomethane, (HOCH₂)3 CNH2, often abbreviated as Tris. At 25 °C, Tris has a PKL of 5.91. The hydrochloride of Tris is (HOCH₂)3 CNH3C1, which can be abbreviated as TrisHCI. Part A What volume of 10.0 mol L-¹ NaOH is needed to prepare a buffer with a pH of 7.79 using 31.52 g of TrisHCI? Express your answer in millilitres to two significant figures. ▸ View Available Hint(s) 10 Π| ΑΣΦ Submit 3 Previous Answers → O Part B Complete previous part(s) Part C Complete previous part(s) < Return to Assignment X Incorrect; Try Again; 4 attempts remaining ? Provide Feedback mL

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 80QAP: Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the...

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. K for copper(II)hydroxide, Cu(OH)2, has a value 2.21020at 25 °C. Calculate the solubility of copper(II) hydroxide in mol/L and g/L at 25 °C.
Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: 2HI(g)H2(g)+I2(g)To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with 3.20 g of HI and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, Na2S2O3. I2(aq)+2S2O32(aq)S4O62(aq)+2 I(aq)It is determined that when equilibrium is reached, 37.0 mL of 0.200 M Na2S2O3 is required to titrate the iodine. What is K at the temperature of the experiment?
Solubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.
To a beaker with 500 mL of water are added 95 mg of Ba(NO3)2, 95 mg of Ca(NO3)2, and 100.0 mg of Na2CO3. After equilibrium is established, will there be â€¢ no precipitate? â€¢ a precipitate of BaCO3 only? â€¢ a precipitate of CaCO3 only? â€¢ a precipitate of both CaCO3 and BaCO3? Assume that the volume of the solution is still 500.0 mL after the addition of the salts.
In a solution with carbon tetrachloride as the solvent, the compound VCl4. undergoes dimerization: 2VCl4V2Cl8 When 6.6834 g VCl4. is dissolved in 100.0 g carbon tetrachloride, the freezing point is lowered by 5.97C. Calculate the value of the equilibrium constant for the dimerization of VCl4 at this temperature. (The density of the equilibrium mixture is 1.696 g/cm3, and Kf = 29.8C kg/mol for CCl4.)
Calculate the equilibrium molar concentrations of trichloroacetic acid in an aqueous solution that contains 284.9 mg of trichloroacetic acid,Cl3CCOOH (163.4 g/mol), in 15 mL (the acid is 73.0% ionized in water). Indicate units
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Mercury (I) chloride, Hg2Cl2, was formerly administer orally as a purgative. Although we usually think of mercury compounds as highly toxic, the Ksp of mercury (I) chloride is small enough (1.3 x 10-18) that the amount of mercury that dissovles and enters the bloodstream is tiny. Calculate the concentration of mercury(I) ion present in a saturated solution of Hg2Cl2.
What is the molar solubility (in M to two decimal places) of copper(II) hydroxide in water (at 25 °C)? Ksp = 2.2 × 10–20
The solubility of borax, which is made up of sodium tetraborate (Na2B4O5(OH)4 8H2O), was analyzed. The dissolution of borax is: Na2B4O5(OH)4 • 8H2O(s) ⇌ 2 Na+(aq) + B4O5(OH)42–(aq) + 8 H2O(l) A 50 mL saturated solution was prepared. After filtration of solution, 5 mL aliquot was transferred to a flask and titrated using 0.432 M HCl. The endpoint was found to be 4.73 mL of the titrant. Tetraborate anion (B4O5(OH)42-) is a weak base which reacts with HCl like the following reaction: B4O5(OH)42–(aq) + 2 H+(aq) + 3 H2O(l) ⇌ 4 H3BO3(aq) What is Ksp expression for the dissolution? What is the tetraborate ions concentration in the filtrate? What is the molar solubility and Ksp of borax if the titration was done at room temperature (298 K)?
Because barium sulfate is opaque to X-rays, it is suspended in water and taken internally to make the gastrointestinal tract visible in an X-ray photograph. Although barium ion is quite toxic, barium sulfate’s Ksp of 1.1 x 10–10 gives it such low solubility that it can be safely consumed. (a) What is the molar solubility of BaSO4? (b) What is its solubility in grams per 100 g of water?
The molar solubility of Ag3PO4 is equal to 1.63 x 10-5 mol/L at a certain temperature. Calculate the Ksp for the compound at this temperature.