A buffer contains 0.15 mol of propionic acid ( CH₂COOH) and 0.24 mol of sodium propionate (C₂H₂COONa) in 1.20 L Part A What is the pH of this buffer? Express the pH to two decimal places. IVE ΑΣΦΑ Y pH = Submit Part B pH = What is the pH of the buffer after the addition of 0.02 mol of NaOH? Express the pH to two decimal places. [37] ΑΣΦ Submit Part C Request Answer pit Submit Request Answer What is the pH of the buffer after the addition of 0.02 mol of HI Express the pH to two decimal places. 0? AL Best An ? 20 ?

A buffer contains 0.15 mol of propionic acid ( CH₂COOH) and 0.24 mol of sodium propionate (C₂H₂COONa) in 1.20 L Part A What is the pH of this buffer? Express the pH to two decimal places. IVE ΑΣΦΑ Y pH = Submit Part B pH = What is the pH of the buffer after the addition of 0.02 mol of NaOH? Express the pH to two decimal places. [37] ΑΣΦ Submit Part C Request Answer pit Submit Request Answer What is the pH of the buffer after the addition of 0.02 mol of HI Express the pH to two decimal places. 0? AL Best An ? 20 ?

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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= く O Acids and Bases Calculating the composition of a buffer of a given pH 0/5 a A chemistry graduate student is given 300. mL of a 0.70 M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K = 4.9 x 10 10. What mass of NaCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 9.48? You may assume that the volume of the solution doesn't change when the NaCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. x10 ㅁ
A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
Acetic acid has a Ka of 1.8 x 10¬º. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate], B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid]. Match each buffer to the expected pH. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help [acetate] ten times greater than [acetic acid] [acetate] = [acetic acid] [acetic acid] ten times greater than [acetate] pH = 3.74 pH = 4.74 pH = 5.74
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 0.95 M NaH2PO4 and 0.68 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 (5 marks total) a. From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. (2 marks) b. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places (2 marks) c. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis? (1 mark)
How many moles of hydrofluoric acid, HF, must be added to 150 mL of 0.31 M sodium fluoride to give a buffer of pH 3.25? Ignore the volume change due to the addition of hydrofluoric acid. ( Ka for HF is 6.8 x 10-4.)
Consider a buffer made by adding 132.8 g of NaC₇H₅O₂ to 300.0 mL of 2.35 M HC₇H₅O₂ (Ka = 6.3 x 10⁻⁵) a What is the pH of this buffer? b What is the pH of the buffer after 0.750 mol of H⁺ have been added? c What is the pH of the buffer after 0.250 mol of OH⁻ have been added?
You have been given 0.200 Molar solutions of hydrocyanic acid and potassium cyanide. The Ka of HCN = 4.9x10-10. If you wanted to make a buffer with a pH = 9.00, would you add a greater volume of the HCN solution or the KCN solution? More HCN equal amounts of each more KCN
The Ka of acetic acid is 1.76 ×10-5. Determine the pH of a buffer solution prepared by combining same volume of 1.00 M potassium acetate and 2.00 M acetic acid.
How many grams of ammonium chloride must be added to 0.53 L of 1.7 M ammonia to prepare a pH = 10.01 buffer? (See the Acid-Base Table.)
How many grams of dry NH4Cl need to be added to 1.80 L of a 0.800 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.53? Kb for ammonia is 1.8×10−5. Express your answer with the appropriate units.
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
Which is true about buffer solutions? -they hold the pH close to the pKa -they contain comparable moles of a weak acid and a strong base - they hold pH constant at pH=7 -they prevent acids and bases from reaching equilibrium -they hold the pH close to the equivalence point pH