A buffer can protect against changes in pH when hydrogen ion or hydroxide ion is added to a reaction mixture. Explain the reason.
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- 1. Describe how you would go about making up the following solutions. a) 150ml GTE buffer (resuspension solution) containing, 20mM Tris pH 8, 5000µM EDTA, 1M Glucose1. What volumes of 50 mM CH3COOH and 30 mM NaCH3CO0 solutions are needed to prepare 2L of 20 mM acetate buffer pH 3.6? (pka for acetic acid is 4.74)4. A 100.0-mL sample of brackish water was made ammoniacal, and the sulfide it contained was titrated with 16.47 mL of 0.02310 M AgNO3. The analytical reaction is Calculate the concentration of H2S in the water in parts per million, cppm.
- 2. Exactly 600.0 mg of pure sodium oxalate, Na,C,0, was dissolved in acid and titrated with a potassium permanganate solution according to the reaction: MnO, + 5C,0, > Mn²+ + CO,. The end point was reached after adding 34.00 ml of titrant. Calculate the molarity of the KMNO, solution.1. Calculate the pH of a buffer solution made from 0.20 M CH3COOH and 0.50 M CH3COO- that has an acid dissociation constant for CH3COOH of 1.8 x 10-5.2. Calculate the pH of a buffer containing 0.1 M sodium acetate and 0.2 M acetic acid (pKa = 4.76).
- 1. Adding as little as 0.1 ml of concentrated HCl to a liter of H20 shifts the pH from 7.0 to 3.0. Adding the same amount of HCl to a liter of a solution that 0.1 M in acetic acid and 0.1 M in sodium acetate, however, results in a negligible change in pH. Why do these two solutions respond so differently to the addition of HCI?10. Why would it be inaccurate to say that a buffer is a solution that maintains a constant pH? K/U12. What is the pH of a solution in which [OH] = 0.000005 M? )5.3 8.7 O 5 x10
- 4. A 100-mL buffer solution with pH of 4.80 is prepared as a stock solution. Using this stock buffer solution, three buffers are prepared by diluting a given volume of the stock buffer (as shown below) to 100 mL with water. Volume used from Buffer Final volume, mL original solution, mL 1 5 100 2 10 100 20 100 a. Do they have the same pH? Check the box corresponding your answer. O Yes O No HY 47.1 Basic Biochemistry, Laboratory b. Which is true about their absolute concentrations? Check the box corresponding your answer. [Buffer 1] > [Buffer 2] > [Buffer 3] [Buffer 3] > [Buffer 2] > [Buffer 1] [Buffer 3] = [Buffer 2] = [Buffer 1] [Buffer 3] = [Buffer 2] > [Buffer 1] [Buffer 3] > [Buffer 2] = [Buffer 1] c. Which is true about their concentration ratios? Check the box corresponding your answer. [Buffer 1] > [Buffer 2] > [Buffer 3] [Buffer 3] > [Buffer 2] > [Buffer 1] [Buffer 3] = [Buffer 2] = [Buffer 1] [Buffer 3] = [Buffer 2] > [Buffer 1] [Buffer 3] > [Buffer 2] = [Buffer 1] %3! %3D d.…We usually say that a perfect buffer has its pH equal to its pKa. Give an example of a situation in which it would be advantageous to have a buffer with a pH 0.5 unit higher than its pKa.12. A D5NS solution is NaCl 0.9% w/v supplemented with 5 % w/v dextrose. A patient was ordered 1 liter of D5NS with 20 mEq KCl for dehydration. How many milliosmols are in 1 liter of this fluid? MW: dextrose = 198, Na=23, K=39, Cl=35.5) Round to the nearest whole number.