1.48 L buffer solution consists of 0.332 M propanoic acid and 0.178 M sodium propanoate. Calculate the pH of the solution following the addition of 0.062 mol HCl. Assume that any contribution of the HCl to the volume of the solution is negligible. The ?a of propanoic acid is 1.34×10−5. PH =  A buffer with a pH of 4.22 contains 0.27 M of sodium benzoate and 0.26 M of benzoic acid. What is the concentration of [H3O+] in the solution after the addition of 0.056 mol HCl to a final volume of 1.6 L? Assume that any contribution of HCl to the volume is negligible. H3O+ =

How does a buffer solution prevent larger change in pH? What does it mean when a solution has exceeded the buffer capacity?

8b.

1.  all the aqueous solutions that are good buffer systems 2.  a buffer solution is 0.421 m in hcn and 0.281 m in kcn, if Ka for Hcn is 4.0 * 10^-10. what is the PH of this buffer solution. b. a buffer solution is 0.495 m in h2s and 0.354 m in khs, if Ka1 for H2s is 1.0 * 10^-7. what is the PH of this buffer solution. c. a buffer solution is 0.455 m in NaHSO and 0.299 m in Na2SO3, if Ka for HSO3 is 6.4 * 10^-8. what is the PH of this buffer solution.  3. A 28.9 ml sample of a 0.385 m aqueous hydrocyanic acid solution is titrated with a 0.372 m aqueous sodium hydroxide solution. what is the ph at the start of the titration, before any sodium hydroxide has been added. b. A 31.9 ml sample of a 0.599 m aqueous hydrofluoric acid solution is titrated with a 0.242 m aqueous barium hydroxide solution. what is the ph after 15.8ml of base has been added. c. when a 23.8 ml sample of a 0.357 m aqueous acetic acid solution is titrated with a 0.459 m aqueous barium hydroxide solution. what is the ph…

Suppose 90.00 mL of 0.200M HCl is added to an acetate buffer prepared by dissolving 0.100 mol of acetic acid and 0.110 mol of sodium acetate in 0.100 L of solution. What are the initial and final pH values? What would be the pH if the same amount of HCI solution were added to 190 mL of pure water? Initial pH = Final pH pH after HCl is added to water =

The K, for NH3 is 1.8 x 10-° at 25°C. Calculate the pH of a buffer solution made by mixing 45.7 mL of 0.493 M NH3 with 62.0 mL of 0.438 M NH4 Cl at 25°C. Assume that the volumes of the solutions are additive. pH =

a) A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol)  b) 10 mL is accidentally spilled into the buffer solution from part a. Determing the new pH of the solution.

Formic acid, HFor, has a K, value of 1.8 x 104. You need to prepare 125 mL of a buffer hav- ing a pH of 3.25 from 0.10 M HFor solution and a 0.10 M NaFor solution. How many mL of NaFor and HFor should be mixed to make the desired buffer?

100. mL of 0.200 M HCl is titrated with 0.250 M NaOH. What is the pH of the solution after 50.0 mL of base has been added? What is the pH of the solution at the equivalence point?