Buffer capacity is a measure of a buffer solution's resistance to changes in pH as strong acid or base is added. Suppose that you have 105 mL of a buffer that is 0.260 M in both benzoic acid (CH₂COOH) and its conjugate base (CH₂COO¯). Calculate the maximum volume of 0.270M HCl that can be added to the buffer before its buffering capacity is lost. volume: mL

Consider a buffer consisting of 1.0 M HNO2 and 2.0 M NaNO. Write the (net ionic) chemical equation for the reaction that occurs when 0.10 mol HNO3 is added to the buffer.

ion The following table shows data from the titration of four 25.0 mL samples of a perchloric acid solution, HCIO4(aq), using a 0.225 mol/L sodium hydroxide standard solution. Bromothymol blue is used as an indicator to detect when the endpoint is reached. Titration of 25.0 mL of HCIO4 with 0.225 mol/L NaOH(aq) final burette reading (mL) initial burette reading (mL) volume of NaOH(aq) added (mL) colour at endpoint Trial 1 Use the data in the table below to answer the next two questions. Trial 2 Trial 3 Trial 4 Trial mL . . . mL mL 1 mL 19.9 0.4 2 Using the chart above, provide the volume of NaOH added for each of the trials. 38.8 3 19.3 19.9 0.2 4 38.4 19.3 blue green green green DELL

A chemistry student weighs out 0.315g of ascorbic acid H2C6H6O6 , a diprotic acid, into a 250.mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.0700M NaOH solution. Calculate the volume of NaOH  solution the student will need to add to reach the final equivalence point. Be sure your answer has the correct number of significant digits.