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...

See similar textbooks

Similar questions

buffer consists of 0.30 M ethylamine (C2H5NH2) and 0.40 M C2H5NH3Cl. What is the pH after 5.04 gof HNO3 is added to 2.00 L of the buffer? Kb(C2H5NH2)=5.6×10−4
A 400-mL buffer solution is 0.350 M in ammonia (NH3) and 0.350 M in ammonium chloride (NH4Cl).Kb(NH3)=1.76×10−5Part A:What is the initial pH of this solution? Express your answer using two decimal places.pH = 9.25 Part B:What is the pH after adding 125.0 mL of 0.100 M HBr to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 10.26) Part C:What is the pH after adding 150.0 mL of 0.100 M LiOH to the initial buffer solution in Part A?Express your answer using two decimal places.pH = (not 8.33) --------------------------- Give the formula for tin(IV) hydroxide.
= 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 beaker with 195 mLmL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 MM. A student adds 7.70 mLmL of a 0.440 MM HClHCl solution to the beaker. How much will the pH change? The pKapKa of acetic acid is 4.740. Express your answer numerically to two decimal places. Use a minus ( −− ) sign if the pH has decreased.
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
A beaker with 1.0 x 10^2 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 8.80 mL of a 0.360 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740.
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?
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
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 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.
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