2. Kinn and Porsche need to store a certain biomolecule in 300 mL of 0.50 M citrate buffer maintained at pH 5.90. Relevant equation: H3C6H507 (aq) Solids Ka1 = 8.4 x 10-4 H3C6H5O7 The available solids in the laboratory are as follows. NaH₂C6H5O7 Na2HC6H5O7 H₂C6H507 (aq) Na3C6H5O7 Ka2 = 1.8 x 10-5 Molar Mass, g/mol 192.124 214.100 236.090 HC6H507² (aq) 258.060 Ka3 = 4.0 x 10-6 -C6H507³- (aq) 2a. Help Kinn and Porsche prepare the buffer by supplying the missing information in the following table. Provide calculations as basis of choosing the identity of each solid. Show your solution on the computation of the mass of each solid needed to prepare the buffer.

2. Kinn and Porsche need to store a certain biomolecule in 300 mL of 0.50 M citrate buffer maintained at pH 5.90. Relevant equation: H3C6H507 (aq) Solids Ka1 = 8.4 x 10-4 H3C6H5O7 The available solids in the laboratory are as follows. NaH₂C6H5O7 Na2HC6H5O7 H₂C6H507 (aq) Na3C6H5O7 Ka2 = 1.8 x 10-5 Molar Mass, g/mol 192.124 214.100 236.090 HC6H507² (aq) 258.060 Ka3 = 4.0 x 10-6 -C6H507³- (aq) 2a. Help Kinn and Porsche prepare the buffer by supplying the missing information in the following table. Provide calculations as basis of choosing the identity of each solid. Show your solution on the computation of the mass of each solid needed to prepare the buffer.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The theoretical pK, of a weak acid is 3.54. Calculate the pK, experimental error of a solution composed of 10 mL of 0.23 M HA, 15 mL of 0.17 M of NaA and 20 mL of water. The measured - of C pH of this solution is 3.17. (Report only the numerical answer of the percent without the % symbol)
How many milliliters of 1.92 M NaOH must be added to 2.00 x 10² mL of 0.20 M H₂PO, to make a buffer solution with a pH of 7.407 Round your answer to 2 significant digits. Note: Reference the pk, of weak acids at 25 °C table for additional information. mL. 0.8
5:51 1 .ll LTE Search Question 16 of 20 Submit Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH, with 0.100 M HNO3 after 80.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 4 Based on the result of the acid-base reaction, set up the unknown. ICE table in order to determine the H2NNH3*(at H2O(1) =H;O*(aq) H2NNH2(aq + Initial (M) Change (M) Equilibrium (M) RESET 0.100 0.200 0.0333 0.0667 +x -X 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x www
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
The pH of a blood plasma is 7.36. Assuming the principle of buffer system is HCO3-/H2CO3, calculate the ratio HCO3-/H2CO3. Is this buffer solution more effective against an added acid or an added base? (Ka1= 4.2 x 10-7 and Ka2 = 4.8 x 10 -11) (Need to show your calculation.).
1. Answer the following, use the data and plot as a reference, answer the following questions:a) What volume of 0.100 M NaOH solution is required to reach the equivalence point, at which the solution is completely neutralized?b) Briefly explain why the pH of the solution drastically increases once the titration proceeds past the equivalence point. c) The end point in a titration of 50.00 mL of aqueous NaOH was reached by the addition of 35.23 mL of 0.250 M aqueous HCl titrant. Calculate the molarity of the NaOH solution. The titration reaction equation is:NaOH (aq) + HCl (aq) → NaCl (aq) + H 2O (l)
2. Calculate the volume of the salt to be used in the preparation of 200 ml of the following buffer solutions. Show computations below. BUFFER DESIRED NUMBER pH 456N 7 8 2.10 SITO 4.40 6.90 7.18 9.45 8.25 0.1M SOLUTIONS QWOL CH3COOH/CH3COONa NaH₂PO4/Na₂HPO4 NaH₂PO4/Na₂HPO4 NH4CI/NH3 NH4CI/NH3 pka 4.70 6.80 6.80 9.30 9.30 VOLUME OF SALT (ml)
A 15.00 ml aliquot of a 0.75 M solution of a weak acid (K, = 1.50E-04 at 25°C) is titrated with 0.500 M NaOH. Determine the pH at the following volumes of NaOH: Volume NaOH = 20.00mL pH = Volume NaOH = 22.50mL pH = Volume NaOH = 30.00mL pH =
What is the pH of a buffer solution made by mixing 50.0 ml of 0.100M potassium hydrogen phthalate with 13.6 ml of 0.100 M NaOH and diuting the miture to 100.0 ml, with water? The Kaz for hydrogen phthalate is 3.1 10-6. O 3.25 O 5.08 O 5.51 O 5.94
You are a formulation scientist preparing a semisolid topical scream. Your formulation requires that a 1000 mL solvent of pH 7.4 phosphate buffer be prepared to suit the pH of the skin. To prepare the buffer, you must use monobasic sodium phosphate (NaH2PO4) and sodium hydroxide (NaOH) since these two ingredients are compatible with your other ingredients in the cream. NaH2PO4 + NaOH → Na2HPO4 + H2O 1. The Ka of NaH2PO4 6.2 x 10-8. Using the Henderson-Hasselbalch equation, calculate the molar ratio of [conjugate base]/[weak acid] that must be used in preparing the buffer. 0.39 B. 0.78 C. 1.56 D. 2.34 2. There is an available 50 mL of 0.2M NaH2PO4 in the laboratory. Convert this first to the moles of NaH2PO4. The molar mass of NaH2PO4 is 119.98 g/mol. 0.005 mol B. 0.010 mol C. 0.025 mol D. 0.045 mol 3. Given the number of moles of NaH2PO4 available as computed above and the molar ratio calculated, which of the following moles of NaOH when added to NaH2PO4 will produce the…
How many moles of B (weak base) would need to be added to 524 mL of 0.209 M BHCl (the acidic salt) to produce a solution with a pH equal to 9.02? Report your answer to the thousandths place. The Kb of the weak base (B) is 3.8 × 10-6.