4. Buffer capacity is a measure of the extent to which a buffer can resist a change in pH upon the addition of a strong acid or strong base. When a strong acid is added to a buffer solution it will react with the weak base to produce wea acid without dramatically changing the mol ratio (mol A-/mol HA). Complete the ICE table below to show the change occurring and calculate the equilibrium for the addition of 0.10 mol of H* added to a buffer consisting of 1.0 mol HA and 1.0 mol A (with a pKa = 9.00 and initial buffer pH of 9.00) The initial values have %3D already been included in the table. A +H* HA mol A mol H* mol HA Initial 1.0 0.10 1.0 Change Equilibrium Using the equilibrium values from the table above and the Henderson-Hasselbalch equation on page 81, calculate the pH after the addition of acid. Neutial s acid to produce we

Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb in order to determine the unknown. Each reaction participant must be represented by one tile. Do not combine terms. Kb = = 5.2 × 10-4 RESET [0] [0.075] [0.10] [5.2 × 10] [x] [2x] [2x]² [0.075 + x] [0.075 - x] [0.075 + 2x] [0.075 - 2x] [0.10+x] [0.10 - x] [0.10 + 2x] [0.10 -2x] < PREV 2 3 Based on your ICE table (Part 1) and the equilibrium expression for Kb (Part 2), determine the pH of the solution. pH = RESET 0 7.86 6.14 0.075 3.9 × 10 3.41 10.59 1.12

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A saturated solution of Cd(OH)2 was found to contain 3.4x 10-6 mol OH- in 100.0 mL. Calculate the Ksp of Cd(OH)2. 4.0

1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water.   2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…

Consider a buffer made by adding 132.8 g of NaC7H5O₂ to 300.0 mL of 1.83 M HC₂H5O₂ (Ka = 6.3 x 10-5) What is the pH of this buffer?

A buffer solution contains 0.201 M CH3NH3 Br and 0.486 M CH3NH2 (methylamine). Determine the pH change when 0.115 mol HBr is added to 1.00 L of the buffer. (Assume Kb (CH3NH₂) = 4.2 × 10-4.) pH after addition change = Submit Answer - pH before addition = pH Retry Entire Group 9 more group attempts remaining D