A buffer is made by combining 20.0 ml. 0.250 M NHACl with 30.0 mL 0.250 M NH3. A) Calculate the pH of the buffer after 1.00 mL of 6.00 M HCI is added and equilibrium is re- established. B) Calculate the pH of the buffer after 1.00 mL of 6.00 M NaOH is added and equilibrium is re- established. Please help with both parts

A buffer is prepared by mixing 43.2 mL of 0.196 M NaOH with 141.2 mL of 0.231 M acetic acid. Calculate the pH of this buffer after the addition of 0.166 g of solid NaOH. (The pKa for acetic acid is 4.75.) (please type answer not write by hend)

How many moles of potassium hydroxide would have to be added to 250 mL of a 0.385 M hydrocyanic acid solution, in order to prepare a buffer with a pH of 9.360? moles

ave to.) The K of acetic acid is 1.8 | 10. (Note: solid sodium acetate comes as a hydrate NaC2H3O2 3H2O), and thus has a molar mass of 135.08 g/mol.) Buffer A: Calculate the mass of sodium acetate that must be added to make 100.0 mL of an acetic acid/acetate buffer at pH 4.10, given that you will use 5.00 mL of 1.0 M acetic acid.

The addition of hydrofluoric acid, HF and to water produces a buffer solution? NANO3 NaCl NaF NaBr HCI

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 10-6 a) Based on the Ka, 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. d) What would the pH be if 0.0020 mol of HCl was added to 100.0 mL of pure water without the presence of the buffer. Assume NaX and HCI completely dissociate.

An aqueous solution contains 0.32 M potassium fluoride.One liter of this solution could be converted into a buffer by the addition of:(Assume that the volume remains constant as each substance is added. More than one answer maybe required.) a) 0.32 mol HNO3 b) 0.15 mol HNO3 c) 0.31 mol HF d) 0.31 mol KI e) 0.15 mol KOH

3. What is the pH of a buffer produced by mixing 225 mL of 0.305 M HCOOH with 175 mL of 0.141 M KCOOH? Be sure to first find the new concentration of each compound in the mixed solution (M₁V₁ = M₂V₂ remember V₁ = total volume), then apply equilibrium.

Calculate the pH for a buffer with 0.20 M NH3 and 0.20 M NH4Cl, then calculate the pH after 10.0 mL of 0.10 M HCl is added to 75.0 mL of the buffer.

Calculate the pH of a buffer solution that has concentrations of 0.25 M of [NH4]+ and 0.50 M of NH3. The pKa of [NH4]+ is 9.24 Provide two decimal places. pH =   NaOH was added to this solution, the concentration of [NH4]+ will increase decrease remain unchanged