) Determine the mass (in grams) of sodium formate that must be added to 1.00 L of 0.180 M formic acid to prepare a buffer with a pH = 3.50. Assume there is no change in volume upon addition of the sodium formate. b) Write the predominant chemical reaction that occurs when 0.050 mol of HClO4 is added to 1.00 L of the buffer prepared in part a and calculate the pH of the solution.

A buffer contains 0.035 mol of boric acid (pKa = 9.15) and 0.015 mol of sodium borate per liter. (a) Calculate the pH of the buffer.(b) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of the buffer.(c) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of pure water.

A chemistry graduate student is given 450. mL of a 0.50M methylamine (CH, NH,) solution. Methylamine is a weak base with K,=4.4 × 10 *. What mass of CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH = 10.96? You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. olo x10 Ar Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility .........................................

An analytical chemist is titrating 198.6 mL of a 0.7200M solution of formic acid (H₂CO₂) with a 0.7700M solution of KOH. The p K of formic acid is 3.74. Calculate the pH of the acid solution after the chemist has added 209.6 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places.