Sodium benzoato , NaC7H5O2, is used as a preservative in foods . Consider a 50.0mL sample of 0.250 M NaC7H5O2 being tittated by 0.200M HBr .  A) what is the pH after the addition of 50.0mL of the HBr solution  B) what is the pH at the equivalence point  C) what is the pH after the addition of 75.0mL of the HBr solution?

3. A buffer solution contains 0.125 moles of ammonium chloride added to 500.0 ml of 0.500 M solution of ammonia. A) What is the pH of this buffer? B) What is the pH after the addition of 0.0100 moles of HCI bubbled into 500.0 mL of the buffer?

Determine the pH during the titration of 19.8 mL of 0.302 M hydrobromic acid by 0.117 M barium hydroxide at the following points:(1) Before the addition of any barium hydroxide (2) After the addition of 12.8 mL of barium hydroxide (3) At the equivalence point (4) After adding 33.2 mL of barium hydroxide

For 550.0 mLmL of a buffer solution that is 0.135 MM in HC2H3O2 and 0.115 MM in NaC2H3O2, calculate the initial pH and the final pH after adding 0.020 molmol of HCl.

For an aqueous solution formed by mixing 4.50mL of 0.15M LIOH with 25.0mL of 0.100M C2H5CO2H (propanoic acid), a) determine whether this forms a buffer solution. b) determine the pH of this combined solution. c) state whether the addition of 6.75mL of 0.100M HCl to the solution will have a large or small effect on the pH of the solution. Explain your reasoning (using 1-2 sentences).

A buffer solution contains 0.388 M ammonium bromide and 0.290 M ammonia. If 0.0311 moles of sodium hydroxide are added to 225 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding sodium hydroxide) pH

Help needed please

7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?

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

Determine the pH during the titration of 26.9 mL of 0.112 M hydroiodic acid by 0.130 M barium hydroxide at the following points: (1) Before the addition of any barium hydroxide (2) After the addition of 5.80 mL of barium hydroxide (3) At the equivalence point (4) After adding 14.7 mL of barium hydroxide