Biochemistry
8th Edition
ISBN: 9781464126109
Author: Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr., Lubert Stryer
Publisher: W. H. Freeman
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Chapter 1, Problem 15P
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Consider the following pH titration curve of a diprotic acid. What is the approximate values for pka 1 and pka 2?
the curve is attached below.
Given the titration curve of the hypothetical polyprotic acid X at 0.100 M concentration (pKa1=4.0, pKa2=8.0, pKa3=12.0) titrated with 0.600 M NaOH, identify the pH at point C, H, E, and M.
What mass of sodium glycolate (NaC2H3O3) should be added to 400.0 mL of 1.00 M glycolic acid to produce a buffer solution with a pH of 4.00? Ka = 1.47 x 10-4.
Please indicate the full solutions.
Chapter 1 Solutions
Biochemistry
Ch. 1 - Prob. 1PCh. 1 - Prob. 2PCh. 1 - Prob. 3PCh. 1 - Prob. 4PCh. 1 - Prob. 5PCh. 1 - Prob. 6PCh. 1 - Prob. 7PCh. 1 - Prob. 8PCh. 1 - Prob. 9PCh. 1 - Prob. 10P
Ch. 1 - Prob. 11PCh. 1 - Prob. 12PCh. 1 - Prob. 13PCh. 1 - Prob. 14PCh. 1 - Prob. 15PCh. 1 - Prob. 16PCh. 1 - Prob. 17PCh. 1 - Prob. 18PCh. 1 - Prob. 19PCh. 1 - Prob. 20PCh. 1 - Prob. 21PCh. 1 - Prob. 22PCh. 1 - Prob. 23PCh. 1 - Prob. 24PCh. 1 - Prob. 25PCh. 1 - Prob. 26PCh. 1 - Prob. 27PCh. 1 - Prob. 28PCh. 1 - Prob. 29P
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- Describe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NAOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pK, of glycine is 9.6.arrow_forwardExample The reference range for blood pH is 7.35 – 7.42. What is this range expressed as [H+] in nmol l-1? Calculation: pH = - log [H+] 7.35 = - log [H+] [H+] = antilog -7.35 = 4.47 x 10-8 mol.l-1 = 44.7nmol.l-1 similarly: pH 7.42 = 38.0 nmol.l-1 Range [H+] = 38 – 44.7 nmol.l-1 If the blood pH decreases in an acidosis from 7.42 to 7.15, what is the change in [H+] in nmol.l-1? so this is example on the worksheet, but i still understand how to answer the question.arrow_forwardNormal arterial pH is 7.35 to 7. 45. Both metabolic and respiratory alkalosis have pH more basic compare to the normal arterial pH. The difference is 0.5 units. What is pH value in alkalosis? Niemann-Pick type C disease is a progressive neurological disease; symptoms include unsteady walking with uncoordinated limb movements, slurred speech, a difficulty in swallowing, epilepsy and tremor. This condition is due to the abnormal functioning of a lysosome. State the normal functions performed by this organelle.arrow_forward
- Quinine ( C20 H24 N2 O2) is the most important alkaloid derived from cinchona bark. It is used as an antimalarial drug. For quinine, pK, = 5.1 and pK, = 9.7 ( pKp = – log Kp). Only 1 g quinine will dissolve in 1920.0 mL of solution. Calculate the pH of a saturated aqueous solution of quinine. Consider only the reaction | Q+ H2O= QH+ + OH- described by pK, where Q = quinine. pH =arrow_forwardIdentify the acid and conjugate base in each reaction. Calculate the pKa for each acid. List them in order from the strongest to weakest acid. The acid-ionization constants, Ka, at 25°C are listed for each. a. HC2H3O2 + H2O ↔ H3O+ + C2H3O2-acetic acid, KA = 1.7 x 10-5 b. HC7H5O2 + H2O H₂O+ + C7H5O2-benzoic acid, KA= 6.3 x 10-5 c. HC6H4NO2 + H2O ↔ H3O++ C6H4NO2-nicotinic acid, KA = 1.4 x 10-5arrow_forwardDescribe the preparation of 2.00 L of 0.100 M glycine buffer, pH 9.0, from glycine and 1.00 M NaOH. What mass of glycine is required, and what volume of 1.00 NaOH is required? The appropriate pKa of glycine is 9.6arrow_forward
- amino glycine pka is 2.4, 9.8 Calculate the most effective buffering range. if there is two pka, since there are 2 buffer region, is the buffering range 1.4~3.4 and 8.8~10.8? i would like to know the correct answer and detailed solution/reason.arrow_forwardA 0.200 M solution of a weak monoprotic acid (HA) has a pH of 2.35. What is the value of K of this acid? a K =2.011e-4 a What is the percent ionization of this acid? Percent Ionization = .10 %arrow_forwardHow is Ka defined? Write the equation for Ka for the generalized acid HA.arrow_forward
- The pH of normal human blood is in the range of 7.35 to7.45. Compute the range of the concentration of H3O+and the range of the OH- concentration in normal blood.arrow_forwardCalculate the theoretical pH of a Tris buffer (pH 8.0) at 0 ºC. Assume that room temperature is 22 ºCarrow_forwardPotentiometric titration curve is given below, which is obtained during the potentiometric titration between strong base KOH (0.2 M) with strong acid HI, label the point in the curve from the following options. If more than one points are present than write as x, y(means separate by using comma) a)The point where pH is because of excess OH - ions. b) The point where pH is only because of HI in water. c)The point where [HI]= [I] in water. d)The point where pH=pka e) The point where all HI is neutralized. f) The point where pH corresponds to solution of [I- ] in water. 14 13 12 11 10 9 pH 6. TITIT TITarrow_forward
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