A student must make a buffer solution with a pH of 2.00.Determine which weak acid is the best option to make a buffer at the specified pH.acetic acid, K, = 1.75 × 10-8, 5.00 Mformic acid, Ka1.77 x 10-4, 2.00 Mpropionic acid, K, = 1.34 × 10-5, 3.00 Msodium bisulfate monohydrate, K, = 1.20 × 10-2, 3.00 MDetermine which conjugate base is the best option to make a buffer at the specified pH.sodium sulfate decahydrate, Na, SO, · 10 H,OO sodium acetate trihydrate, CH,COON · 3 H,Osodium formate, HCOONAsodium propionate, CH, CH,COONA The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M.Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pHof 2.00?mass =Enter numeric valueBased on this information, what volume of acid should the student measure to make the buffer solution?volume =mL

A buffer works best at a pH closer to the pKa value of the acid. Closer the pKa value of the acid to…

A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. acetic acid, K, = 1.75 × 10-8, 5.00 M formic acid, K. = 1.77 x 10-4, 2.00 M propionic acid, K = 1.34 × 10-5, 3.00 M %3D sodium bisulfate monohydrate, K, = 1.20 × 10-2, 3.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. O sodium sulfate decahydrate, Na,SO, · 10 H,O sodium acetate trihydrate, CH, COONa · 3 H,O sodium formate, HCOONA O sodium propionate, CH,CH, COONa

A student must make a buffer solution with a pH of 2.00. Determine which weak acid is the best option to make a buffer at the specified pH. acetic acid, K, = 1.75 × 10-8, 5.00 M formic acid, K. = 1.77 x 10-4, 2.00 M propionic acid, K = 1.34 × 10-5, 3.00 M %3D sodium bisulfate monohydrate, K, = 1.20 × 10-2, 3.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. O sodium sulfate decahydrate, Na,SO, · 10 H,O sodium acetate trihydrate, CH, COONa · 3 H,O sodium formate, HCOONA O sodium propionate, CH,CH, COONa

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...

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A student wants to make a pH 4.0 buffer solution. She decides to use a buffer made from formic acid and sodium formate (HCOONa). She adds 50.0 grams of sodium formate to a 1 L volumetric flask. The Ka of formic acid is 1.77×10-4. How many mL of 3.0 M formic acid should she add to the 1 L volumetric flask so that when the flask is diluted to the mark the pH will be 4.00?
A buffer is prepared using 0.085 Mformic acid (HCOOH) and 0.085 Msodium formate (NaHCOO). Which of the following statements is FALSE? O The addition of 0.02 M HCI will decrease the pH slightly O The addition of 0.02 M NAOH will increase the pH slightly The formate ion can neutralize bases added to the buffer The addition of 1.0 M HCI will cause the pH to drop significantly Diluting the solution with pure water won't change the pH of the buffer
A chemistry student is asked to maked a buffer of pH = 4.0. Which of the following acids would be the best choice? Explain your selection to the best of your ability and in your own words. Formic acid -4 Ka = 1.8 x10 Acetic acid Ka = 1.8 x10-5 -5 Chloropropanoic acid Ka 7.8 x10 Benzoic acid Ka = 6.3 x10-5
I. Consider a 1.00 L of 1.50x10 -3 M hydrocyanic acid (HCN,K=4.9×1019) 1. Write the equilibrium expression. 2. Calculate the pH of the solution. 3. If a 9.00x10 mol sodium cyanide, NaCN, is added, what is the pH of the resulting solution? Assume negligible volume change.
A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka’s for KHP are 1.12 x 10-3 and 3.90 x 10-6. a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
A student wants to make a 0.75 mol/L buffer solution using potassium hydrogen sulfate, KHSO4, and a conjugate base. Which of the following options could be used as a conjugate base to make this buffer solution? Answer choices a 0.80 mol/L solution of H2SO4 a 0.50 mol/L solution of K2SO4 a 0.002 mol/L solution of K2SO4 a 9.0 mol/L solution of KHSO4
You need to prepare 100.0 mL of a pH 4.00 buffer solution using 0.100 M benzoic acid (p?a=4.20) and 0.180 M sodium benzoate. How many milliliters of each solution should be mixed to prepare this buffer? benzoic acid: mL sodium benzoate: mL
9 If the dissociation constant of a weak acid is 1.4 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order to prepare a buffer that has a pH of 4.85? a) 0.100 M weak acid with 0.0100 M conjugate base b) 0.0100 M weak acid with 0.100 M conjugate base c) 0.100 M weak acid with 0.200 M conjugate base d) 0.300 M weak acid with 0.300 M conjugate base e) 0.500 M weak acid with 0.250 M conjugate base
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