Consider a buffer solution in which [H₂PO4] = 0.130 M and [HPO4) = 0.0260 M. The pH of this solution is 6.50. Suppose 0.
Posted: Thu Jun 30, 2022 6:17 pm
- Consider A Buffer Solution In Which H Po4 0 130 M And Hpo4 0 0260 M The Ph Of This Solution Is 6 50 Suppose 0 1 (43.75 KiB) Viewed 58 times
- Consider A Buffer Solution In Which H Po4 0 130 M And Hpo4 0 0260 M The Ph Of This Solution Is 6 50 Suppose 0 2 (76.72 KiB) Viewed 58 times
- Consider A Buffer Solution In Which H Po4 0 130 M And Hpo4 0 0260 M The Ph Of This Solution Is 6 50 Suppose 0 3 (53.15 KiB) Viewed 58 times
0.00100 moles of OH are added to 100 mL of solution. If the OH did not undergo any reactions, what would be the concentration, [OH]? (Give you answer to 3 significant digits.) M OH undergoes a strong reaction in the buffer solution. What is this reaction? Once you identify the reaction, fill in the table below. (Give your answers to 3 significant digits.) Initial Buffer Select Add NaOH Change Selet New conc. Sele pH OH- pk. Select + log ( Selec Now that we know the final concentrations for [H₂PO4] and [HPO4], we can use the Henderson-Hasselbach equation to determine the final pH. (Please use three significant figures, without scientific notation, i.e. use 0.0230 instead of 2.30e-2.) A- + H₂O Ha All units are in M (moles/L)
red Question 1 Not yet graded / 5 pts Calculate the Ka of a 0.40 M HA (weak acid) solution whose pH is 2.57. (Hint: Do not use the Henderson- Hasselbach equation). Show your work for credit!! Your Answer: