You need to prepare 500 ml PBS buffer, a solution commonly used in biological research. The buffer helps to maintain the pH, and the osmolarity, as well as ion concentrations of PBS buffer, match those of the human body. PBS buffer consists of the following components: 137 mM NaCl, 2.7 mM KCl, 10 mM Na2HPO4, 1.8 mM KH2PO4. How would you prepare the buffer?
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You need to prepare 500 ml PBS buffer, a solution commonly used in biological research. The buffer helps to maintain the pH, and the osmolarity, as well as ion concentrations of PBS buffer, match those of the human body. PBS buffer consists of the following components: 137 mM NaCl, 2.7 mM KCl, 10 mM Na2HPO4, 1.8 mM KH2PO4. How would you prepare the buffer?
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- A solution is prepared by dissolving 64.92 g of Magnesium chloride in sufficient water to make 600 mL of solution. The density of the solution is 1.082 g/mL. (At. wt.: Mg = 24.31, Cl = 35.45) Calculate:a. molality b. mf of solutec. mole % solvent d. %bywt.e. Osmolarity “THE SUB-PARTS TO BE SOLVED (LETTER D & E)”1. (a) Molar solubility is its molarity in a saturated aqueous solution the solubility in molarity for supersaturated solution its molarity in an unsaturated solution its solubility in grams solute per liter of solution for saturated solution (b) Slightly soluble substances are those that completely ionize in water but have limited solubility completely ionize in water and have complete solubility partially ionize in water but have limited solubility partially ionize in water but have complete solubilityIf the osmolarity of a solution of NaCl is 2.4 OsM, what would it be as a percent solution? MW of NaCl = 58.44 g/mole
- The osmolarity of a solution of 100 mM CaCh, is closest to the osmolarity of which of the following solutions? a. 50 mM NaCI b. 100 mM glucose c. 150 mM urea d. 150 mM NaCI e. 75 mM NaCI + 100 mM KCIThe normal range of the sodium electrolyte in the body is 134 to 145 mEq/L. The term mEq is dependent on the charge of the ion. Since sodium is a +1 ion, 134 mEq/L is the same as 134 mmol/L. An ion that has a greater positive or negative charge; however, will have 1 mEq for each positive or negative charge of the ion for every 1 mmol. For example, for Ca+2, 2mEq/1mmol. If the standard range of Magnesium in the body is 0.70 to 0.95 mmol/L, convert this value into mEq/L for the Mg2+ ion. (Use dimensional analysis to figure this out)Complete the table: Solute Mass of solute Moles of solute Volume of solution Molarity of solution MgSO4MgSO4 0.638 gg _____ 27.0 mLmL _____ NaOHNaOH _____ _____ 125.0 mLmL 1.35 MM CH3OHCH3OH 13.5 gg _____ _____ 0.480 M
- Table 2. Volume of BSA, protein content, and absorbance readings of reference solutions Solution Volume of BSA standard solution (μL) Protein content(μg/mL) Absorbance value At 595 nm 1 0 0 0 2 10 1 0.022 3 30 3 0.065 4 50 5 0.106 5 70 7 0.178 6 100 10 0.299 7 120 12 0.380 Make a graph by plotting the absorbance values versus the BSA protein content (in μg) for theseven reference solutions. When constructing the graph, be…When you dissolve Sodium Phosphate Dibasic in water, the resultant solution is ____________, because _____________. Basic; the dibasic phosphate ion further takes up a H+ from the solution, thereby lowering the pH of the solution. Basic; the dibasic phosphate ion further takes up a H+ from the solution, thereby increasing the pH of the solution. Acidic; the dibasic phosphate ion further dissociates to lose a H+, thereby lowering the pH of the solution. Acidic; the dibasic phosphate ion takes up one H+ from the solution, thereby reducing the pH of the solution.What is the effect of adding a small amount of a strong acid or strong base to the acidity of a buffer? How would this compare to an unbuffered solution of the same acidity?
- How is a mixture of ions separated using qualitative analysis? Group of answer choices Electrolysis of ions by variable voltage. Selective precipitation under acidic/basic conditions and electrolysis of ions by variable voltage. Selective precipitation under acidic/basic conditions. Selective precipitation under acidic/basic conditions and formation of complex ions. Selective precipitation under acidic conditions. Selective precipitation under acidic/basic conditions, formation of complex ions and electrolysis of ions by variable voltage. Formation of complex ions. Selective precipitation under basic conditions.Calculate the pH of a dilute solution that contains a molar ratio of potassium acetate to acetic acid (pKa 5 4.76) of (a) 2:1; (b) 1:3.hosphate buffered saline (PBS) is a buffer solution commonly used in biological The buffer helps to maintain a constant pH. The osmolality and ion concentrations of the solution usually match those of the human body. You need to prepare a stock solution at pH 7.00 with NaH2PO4 and Na2HPO4 (pKa =7.21). What would be the respective concentration of these substances if you wish to obtain the final phosphate concentration [HPO4 −2] + [H2PO4 −] = 0.3 M? What will be the pH of the solution after adding 0.18 L of 0.2 M NaOH? What is the ratio of HPO4−2 of H2PO4 – is part b, and what is the significance? NON GRADED PRACTICE QUESTION FOR BIOCHEM