Answered: Calculate the difference in pH upon the…

Calculate the difference in pH upon the addition of 1.00 mL of 0.100 M NaOH to 1.00 L of formate buffer that is composed of 0.10 M formic acid (pKa = 3.745) and 0.20 M sodium formate.

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 8P

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Calculate the difference in pH upon the addition of 1.00 mL of 0.100 M NaOH to 1.00 L of formate buffer that is composed of 0.10 M formic acid (pK_a = 3.745) and 0.20 M sodium formate.

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What mass (in g) of ammonium chloride (NH4Cl) should be added to 2.60 L of a 0.155 M NH3 to obtain a buffer with a pH of 9.45? (Kb for NH3 is 1.8 x 10-5)
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Derive an equation similar to the Henderson–Hasselbalch equation for a buffer composed of a weak base and its conjugate acid. Instead of relating pH to pKa and the relative concentrations of an acid and its conjugate base (as the Henderson–Hasselbalch equation does), the equation should relate pOH to pKb and the relative concentrations of a base and its conjugate acid.
A buffer of what pH is needed to give a Mg2+ concentration of 3.0 * 10-2 M in equilibrium with solid magnesium oxalate?
You find 425.0 mLof 0.350 M sodium oxalate in the lab, and you want to use it to make a buffer with a pH of 1.50. What mass of oxalic acid (MW = 90.03 g/mol, Ka= 5.9 × 10–2) is needed to make this buffer? (Neglect any volume changes due to the addition of solid oxalic acid.)
Derive an equation similar to the Henderson–Hasselbalch equation for a buffer composed of a weak base and its conjugate acid. Instead of relating pH to pKa and the relative concentrations of an acid and its conjugate base (as the Henderson– Hasselbalch equation does), the equation should relate pOH to pKa and the relative concentrations of a base and its conjugate acid.
An industrial chemist studying bleaching and sterilizing pre-pares several hypochlorite buffers. Find the pH of (a) 0.100 M HClO and 0.100 M NaClO; (b) 0.100 M HClO and 0.150 M NaClO; (c) 0.150 M HClO and 0.100 M NaClO; (d) 1.0 L of the solution in part (a) after 0.0050 mol of NaOH has been added.
1. Compare the pH values of boiled and unboiled distilled H2O. 2. The Henderson-Hasselbalch equation relates the pH of a buffer to the relative concentrations of the buffercomponents. According to this equation, under which conditions is pH = pKa? 3. How does the concentration of the buffer affect the buffer capacity?