A buffer solution is formed by adding 0.200 moles of solid potassium nitrite, KNO₂, to 500.0 ml of 0.500 M Nitrous acid, HNO₂ solution. You may assume that the change in volume is negligible upon addition of the solid. pKa of HNO2 is 3.40 Ka of HNO2 is 4.0E-4 m.w. of HNO2 is 47.01 g/mol pH of the buffer solution is 3.30, so now Calculate the pH of the buffer solution after the addition of 5.00 ml of 2.50 M Ba(OH)₂.

A 1.48 L buffer solution consists of 0.128 M butanoic acid and 0.338 M sodium butanoate. Calculate the pH of the solution following the addition of 0.080 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-5. pH =

A 1.00 L buffer solution is 0.125 M in HF and 0.125 M in NaF. Calculate the pH of the solution after the addition of 0.0500 moles of solid NaOH. Assume no volume change upon the addition of base. The K, for HF is 3.5 x 10 4. O 2.89 3.46 3.82 O 3.34 О 3.63

10. A buffer solution is made of mixture of aqueous methanolic acid, HCOOH. With aqueous sodium methanolate acid NaHCO. The equilibrium reaction takes place in buffer solution is: НСООН < НСОО + Н Small amount of NaOH is then added to that buffer solution. What reaction take places at the buffer solution to resist change of pH caused by addition of base? а. НСООН +H* b. HCOO+H* НСООН НСООН с. НСООН +ОН" d. HCOOH +ОН" НСОО +Н2О НСООН

2. A buffer solution contains 0.15 mol of propionic acid (HC3H5O2) and 0.10 mol of sodium propionate (NaC3H5O2) in 1.20 L of the solution. What is the pH of the buffer after the addition of 0.01 mol of NaOH?

Calculate the pH of the buffers prepared in the following ways: a. by mixing 50.00 mL of 0.200 M ammonium nitrate, NH,NO,, with 25.00 mL 0.200 M NaOH b. by neutralizing half of the acid in 100.00 mL of 0.200 M ammonium nitrate solution with 1.0 M NaOH c. by mixing 60.00 mL of 0.400 M sodium formate (NaCHOO) with 40.00 mL 0.360 M HCI d. by mixing 80.00 mL of 1.00 M NH, with 40.00 mL of 1.00 M HCI e. by mixing equal volumes of 1.00 M NH, and 0.50 M HCI

A buffer solution with a pH of...

Answer using this data for the remaining questions on this page: For 1.0L of an acetic acid solution: Ka = 1.8 x 10-5 and [HA] = 0.250M 2. Calculate the pH of the solution. 3. What is the pka? 4. Calculate the pH of the solution if you make it a buffer by adding enough solid sodium acetate to make the concentration of acetate ion equal to 0.35M. The volume of the solution does not change. 5. What is the new concentration of [HA] if 2.0mL of 5.00M of HCI is added to 1.000L of the solution above? 6. What is the new pH?