Acetic acid’s pKa is 4.75 and nitrous acid’s pKa is 3.16. If you made one buffer of equal parts acetic acid and its conjugate base, then a second buffer of equal parts nitrous acid and its conjugate base, how would the two buffers’ pHs compare to each other? Why?

Buffers will resist pH changes following the addition of acid or base within about +/-1 pH unit of the pka of a solution. True False

Which of the following is true about the titration curves of solutions of weak acids? A. The pH for optimal buffering power of a weak acid is 7.00. B. You can calculate the pKa of an acid, given the pH and the molar ratio of the acid and its conjugate base. C. The pKa of a weak acid is the pH at which the acid is completely dissociated. D. At a pH below the pKa of a weak acid, its conjugate base will predominate.

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

Cesium buffer helps in determining easily ionizable elements in ICP-MS and ICP-OES. But how? Cesium is easily ionizable element it produces more electrons in the plasma. In principle it should also suppress the ionization of metal of our interest. In that case Cesium buffers interferes our analysis. I don’t understand why Cesium helps to reduce the ionization of sodium and potassium, not the ionization of metal of our interest. Can you please explain how cesium helps to reduce the ionization of only a specific metal not the metal of interest?

Why is the PH of the 0.1M acidic acid-sodium acetate buffer solution different from that 0.1M acetic acid?

Use the Henderson-Hasselbalch equation to calculate the pH of a buffer that is 0.18 M acetic acid and 0.85 M in acetate anion. The pKa value for acetic acid is 4.74. Round your answer to two decimal places.

Compare the size of the change in pH value when HCl and NaOH are added to water vs. the size of the change in pH value for the standard reference buffer . Explain why the change for water vs. buffer was the same or different in size.

A buffer is made with 0.50 M weak acid and 0.50 M sodium salt of the conjugate base. The pKa of the weak acid is 9.30 After the addition of a small amount of strong concentrated acid, the new equilibrium concentrations are 0.6 M weak acid and 0.4 M base. Calculate the new pH. Enter result with 2 decimal places, digits only.

What is the relationship between the buffer range and the buffer-component concentration ratio?