5. A common solvent for diluting biochemical samples like the protein you are using in this lab is a buffered 0.05 M Tris solution buffered at pH 7.4 that contains 0.15 M NaCl. Considering your answers to the previous questions, explain why this solvent is suitable for diluting your samples.
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- First read the text sections 10.5 and 10.6 on pH. This is a Dry Lab since we cannot meet on Campus. After calibrating a pH meter you would have measured the pH of four different Basic Aqueous Solutions and examined the data for trends. You would have calculated the expected pH of each of the strong base solutions by assuming that for every NaOH formula unit that dissolves, one OH- ion is released. Thus, we can assume that the OH- Molarity equals the NaOH Molarity. Using the OH- Molarity and the water ionization equilibrium expression (Kw= 1.0 X 10 to the -14 power = H+ Molarity X OH- Molarity), we can calculate the H+ Molarity of the solution. Using the H+ Molarity, we can calculate the solution's pH. Thus a 1.0 X 10 to the 4 power NaOH solution has a pH of 10. The calculated pH value is arrived at as follows. By rearranging the water ionization equilibrium expression and plugging in the OH- Molarity, we can solve for H+ Molarity. H+ M = 1.0 X 10 to the -14 power divided by 1.0 X 10 to…Suppose you want to prepare a solution with a pH of 4.00 using acetic acid, CH3COOH, and sodium acetate, CH3CoOONa. What should the ratio of sodium acetate to acetic acid, CH3CO0-| : [CH3COOH], be in your buffer solution? Hint: The Ka for acetic acid is 1.8x105. 0.18:1 O 1.9:1 0.84:1 O 5.5:1 O 1:1Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CIO₂ H₂O HCIO, H₂S CHÍNH, CH,NH, H₂O HS relative pH of 0.1 M aqueous solution 6 (Choose one) ▼ (Choose one) Y (Choose one) 8 (highest) (Choose one) Y 1 (lowest)
- Order these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of 0.1 M aqueous solution species ? 103 |(Choose one) ▼ OH |(Choose one) ▼ H,0 4 HC,04 6. HIO, 1 (lowest) NO2 |(Choose one)1.) In a 0.100M aqueous solution of a weak acid, the acid is 3.7% dissociated. What is the Ka for this acid? 2.) What is the pH of a 0.010M solution of pyridine, C2H5N, a weak base? It's Kb is 1.5x10-9. 3.) Calculate the pH and percent ionization of a 15.0 M solution of a weak base. (pKa=9.26) SHOW ALL WORK!!A solution is a mixture of 0.100M weak acid and 0.020M of its conjugate base. The pH of the resulting solution is 5.20. What is the pKa of the weak acid? a. 7.00 b. 4.50 c. 5.90 d. 4.74 e. 8.24
- under these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CH₂COOH + H₂O* H₂O NO₂ CH₂COO HNO₂ 103 HIO₂ relative pH of 0.1 M aqueous solution 4 (Choose one) 5 (Choose one) (Choose one) 3 (Choose one) 2 X Ś olo 18 ArOrder these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. relative pH of species 0.1 M aqueous solution HC₂04 7 + H₂O* 1 (lowest) H₂PO4 (Choose one) H₂PO4 4 103 (Choose one) HIO₂ H₂C₂O4 (Choose one) H₂O (Choose one)Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M C6H5NH₂. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) 0.060 Initial (M) Change (M) Equilibrium (M) 0 -X 0.700 - x 1 -0.060 C6H5NH3*(aq) + OH (aq) 0 1 0.040 0.140 0.500 + x CoHşNHz(aq) + 0.300 + x 2 0.500 0.500 - x -0.040 0.300 - x -0.140 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your…
- 23a. Calculate the PH of a HCN 0.04M solution (Ka = 6.2x10−10). *Please show all work! 23b. Explain what is a catalyst.Calculate the pH of a buffer solution prepared by dissolving 0.150 mol of benzoic acid and 0.300 mol of sodium benzoate in water sufficient to yield one liter of solution. The Ką of benzoic acid is 6.30 x 10-5 O 2.516 3.892 4.502 10.158 4.1951. The pKa of HX is 9.34. Calculate the pH of a 0.418 M solution of HX. 2. A weak monoprotic acid, HA dissociates by 2.416 % and has a pH of 3.61. Calculate the Ka value for the acid HA. Record your answer in scientific notation to 3 sig figs.