A 100.0 mL buffer solution is constructed using 0.035 M HX, a weak acid, and 0.045 M NaX. Ka, HX = 4.7 x 106 a) Based on the K,, what is the pH range where the buffer should be effective. b) From the given concentrations, what is the actual pH of the constructed buffer. c) What would the pH of the buffer if 0.0020 mol of HCl is added to the buffer solution.

There are 0.250 ml of a Buffer solution, where the concentration is 0.225 M of sodium acetate and 0.225 M of acetic acid. What will the change in pH be if 30 ml of a 0.1 M HCl solution are added?

Without detailed calculation and RICE table, determine whether the following solutions are acidic or basic, buffer or not buffer.Explain your answers by identifying the major speciesand the dominate chemical reaction. (a)1M NaCl + 1M HCl in equal amounts (b)1M NH4Cl + 1M NH3in equal amounts (c)1M Na2C2O4+ 1M HCl in equal amounts  (d)2M H3PO4+ 3M NaOH in equal amounts

An analytical chemist is titrating 102.2 mL of a 0.1400 M solution of dimethylamine ((CH,) NH) with a 0.7900 M solution of HNO,. The pK, of dimethylamine is 3.27. Calculate the pH of the base solution after the chemist has added 19.5 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = Explanation Check 2021 McGraw-Hil Terms of Use