X and Y in the following equation represent * CH₂=CH₂ + HOCI CICH₂CH₂OH Ca(OH)₂ H₂C O Calcium chloride and water -CH₂ + X + Y Calcium oxide and hydrochloric acid Calcium hydroxide and hydrochloric acid O Calcium hydroxide and water
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- The Tris buffer system is commonly used in biochemistry as its pKa of 8.1 allows it to buffer close to physiological pH. (CH2OH)3CNH2 + H+ Û (CH2OH)3CNH3+ What concentrations of Tris and Tris H+ are obtained in a 200 mL solution at pH 8.20 containing 6.1g of Tris? The molecular mass of Tris is 121.1 gmol-1 Please do this step by step thank you!calculate the ph of a 0.465 M solUTION OF ethylamine CH3CH2NH2 and 0.211 M ethylammonium bromide CH3CH2NB3Br. the base dissociation constant kb is 6.31 x 10 -4. what is the pH if 76.0 ml of 0.150 M of a strong acid like HCI is added to 100 ml of buffer solution. what if a strong base like NaOh is added with the same ammount insteadCalculate the ratio of dissolved benzoic acid to benzoate ion that will exist in solution at equilibrium at a pH of 2.00. The acid equilibrium constant (K a ) for benzoic acid is 6.46 * 10 ^ (- 5) . Note that this calculation doesn't account for the benzoic acid that has precipitated from solution, but you can assume that the higher the ratio, the more benzoic acid will precipitate. Then, Carry out the same calculation for a pH of 4.00, and explain why it was important to reduce the pH to below 4 in this experiment.
- 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?Standard solution : 0.201 grams of acetylsalicylic acid was combined with 10 mL of 0.5 M NaOH, then transfered to a 100 mL flask and filled the rest of the way with water Then 0.500 mLs of the standard solution was transfered to a 10.00 mL flask and diluted to the 10 mL mark with 0.02 M of buffered iron chloride. Number of moles of NaOH = 0.005 moles Since the reaction between acetylsalicylic acid and NaOH is a 1:1 reaction, the number of moles of acetylsalicylic acid used in the reaction is also 0.005 moles. the concentration from analysis question 5: acetylsalicylic acid in the 100.00 mL volumetric flask is 0.050 M. From your plot, what is the value of εb? From the Beer- Lambert law For the aspirin sample, calculate the concentration of acetylsalicylic acid present using the value of εb that you found The concentration from analysis question 5 represents the concentration in the 10.00 mL sample that was prepared in the volumetric flask using an aliquot of the solution in the…You are conducting a biochemical experiment with an enzyme that has optimal activity at pH = 6.50. You decide to use carbonate (pKa1 = 6.38, pKa2 = 10.30) as the buffer to keep the pH stable throughout the enzymatic reaction. (Recall that the formula for carbonic acid is H2CO3.) You prepare a 0.4 M solution of carbonate buffer at pH = 10.50. Calculate the concentrations of the major carbonate species in your solution. Show your calculations.
- Write the equilibrium constant expressions for the following reactions and determine the value for the equilibrium constants AgCl + 2NH3(aq) ⇌ Ag(NH3)2+ +Cl-(aq) BaCO3 +2H3O+(aq) ⇌ Ba2+(aq) + H2CO3(aq) +2H2O(l) The basic dissociation of aniline, C6H5NH2 The acidic dissociation of methyl ammonium hydrochlorideAlizarin yellow R, Ka=7.9×10−12, is yellow in its protonated form (HX) and red in its ionized form (X−). At what pH will alizarin yellow R be a perfect orange color?Calculate the pH of 640. mL of a 0.280-M solution of hydrocyanic acid before and after the addition of 0.116 mol of sodium cyanide.pH befor addition = pH after addition =
- At 25oC, Ka for acid dissociation of lactic acid (HC3H5O3) is 1.0 x 10-4. Calculate ΔGo for the reaction HC3H5O3 (aq) + H2O(l) H3O+(aq) + C3H5O3-(aq)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?10.0 mL of 0.100 M HCl solution was added to 20.0 mL of 0.100 M (CH3CH2)3N (triethylamine). Kb (CH3CH2)3N = 5.2 x 10–4 Determine the following: a) Concentration of (CH3CH2)3N that did not react with acid. b) Concentration of (CH3CH2)3NH+ formed from the reaction with acid. c) pOH.