Describe how to prepare 250 mL of a 150 mM phosphate buffer to model E. coli pH of 7.6, given the following: water, H3PO4 MW 98, pKa 2.2; NaH2PO4 MW 120, pka 6.8; Na2HPO4 MW 142, pKa 12.5; Na3PO4 MW 164. You may type or upload your response.
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- What Cc E My Home x D Activity O Dashboard x Alabame is hbr ac O (123) Ne x + iln/takeAssigunent/takeCovalentActivity.dollocatorassignment-take Constant (Review Topicsl (References) pts 2req Use the References to access important values if needed for this question. pts 2reg A student ran the following reaction in the laboratory at 498 K: PCI3(g) + Cl2(g) PCI5(g) pts 2reg When she introduced 0.171 moles of PCI,(g) and 0.190 moles of Cl,(g) into a 1.00 liter container, she found the equilibrium concentration of Cl,(g) to be 5.04x10 2 M. pts 2reg pts 2req Calculate the equilibrium constant, Ke, she obtained for this reaction. Kc %3D Submit Answer Retry Entire Group 1 more group attempt remaining (Previous Next ENG e 40 5 5/5/2 US Home End Ansert 7. Y RVernon was asked to isolate a storage protein from Saba banana (Musa balbisiana Colla). According to the protocol given by his laboratory instructor, the storage protein must be stored in a 0.750 M citric acid buffer solution pH 6.21. Citric acid is a triprotic acid that follows a dissociation equilibrium shown below: H3CH₂O7 H₂CH₂O7 = z → Ka, = 8.32 x 10-4 Ka₂ = 1.82 x 10-5 HC₂H5O72- C₂H50,³- COMPOUND/SALT H3C6H5O7 NaH₂C6H5O7 Na₂HC6H5O7 Na3C6H5O7 Ž Ka3 = 3.98 x 10-6 Help him prepare the buffer by answering the following questions: 1. Based on the chemical equation above, which species will be the (a) acidic and (b) basic component of the buffer to be prepared? 2. Write the complete equilibrium reaction involved in the buffer system. 3. Write the pertinent chemical equations to illustrate what happens upon the addition of small amounts of (a) strong base and (b) strong acid to the buffer system. 4. Based on your answer in number 1, choose among the salts given in the table below and…Salts containing the phosphate ion are added to municipal water supplies to prevent the corrosion of lead pipes. Based on the pKa values for phosphoric acid (pKa1 = 7.5 * 10-3, pKa2 = 6.2 * 10-8, pKa3 = 4.2 * 10-13) what is the Kbvalue for the PO43- ion?
- A 1.5000-g sample of cereals was analyzed for nitrogen using the Kjeldahl procedure. The receiving flask contained 69 mL of 0.02 M HCl. After the ammonia was collected, the solution was titrated with 0 M NaOH, requiring 11.72 mL to reach the methyl red endpoint. Calculate and percent protein in the sample (f=5.70). Ans. in 3 SFsPrepare 1.0 L of a 0.1 M histidine buffer, pH 7.0, starting with histidine dihydrochloride (C3H11N3O2Cl2, FW 228), 0.5 N NaOH, and water. pKa values for histidine are 1.8 (α-COOH), 9.3 (α-NH3+), and 6.0 (-R).6. i Look up and list the size of the following proteins; then predict in what order they would be eluted from a Sephadex G-100 column eluted with 100 mM Tris buffer, pH 7.0? Myoglobin Chymotrypsinogen Serum albumin
- Calculate the pKb for the following: Novocain, Kb = 7 x10-6 methyl red, Kb = 3 x 10-12 Calculate the pH and % ionization for the following: 0.10 M CH3NH2; pKa = 10.657 0.02 M C6H5NH2; pKa = 4.63Consider an amino acid (A) with no ionizable side chains, and call the three species involved in the acid/base equilibria H2A+, HA, and A- (see scheme below). Assume that pKa(1) = 2.0 and that pKa(2) = 9.0. Suppose that the total concentration of the amino acid is 1.0 mM. Report to two significant digits. pH [H2A+] (mM) [HA] (mM) [A-] (mM) 10.0 11.0 12.0what is the pH of a 50 mg mL-1 solution of ascorbic acid (MW 176.1, pKa 4.17)?
- After digesting a 2.6824g stake sample the nitrogen is oxidized to NH4; converted to NH3 with NaOH and distilled in a collection flask containg 50.0ml of 0.7867 M HCl.The excess HCL is then back titrated with 0.8094 M NaOH and required 20.24 ml to reach bromothymol blue end point. Report the percentage w/w protein in the steak given that there is 3.39g of protein for every gram of nitrogen in the steakAn enzyme is needed to be stored in a buffer solution with a pH of 10.00. Unfortunately, only three buffer systems are available in their laboratory: Buffer System Weak Acid Component Ka Conjugate Base Salt PAH Benzoic acid, C6H5COOH 6.25 x 10-5 NaC6H5COO SAD Boric acid, H3BO3 5.81 x 10-7 NaH2BO3 DOH Hydrogen cyanide, HCN 6.20 X 10-10 NaCN In what buffer system (PAH, SAD, or DOH) will Phoebe store the enzyme? (show calculations and briefly explain) Write the equilibrium reaction involved in the buffer system. Calculate the amount (in mL) of the 2.00 M stock solution (pH 10.00) of the same buffer system needed to prepare 250 mL of a 0.650 M buffer pH 10.00.Arginine has ionizable groups with pKa values of 2.17, 9.04, and 12.48. A researcher makes up 73 mL of a 0.125 M solution of arginine at a pH = 8.5. He then adds 35 mL of 0.24 M NaOH. What is the pH of the resulting solution? %3D