The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 3.50? mass= Based on this information, what volume of acid should the student measure to make the buffer solution? volume= g ml.

In general, adding a strong acid or a strong base to a buffer solution _________ neutralizes the solution making a solution that is neither acidic nor basic. drastically changes the pH to be either strongly acidic or strongly basic. causes only a slight change in pH making the solution only a little more acidic or only a little more basic than it already was. has variable results so there is no general trend

Calculate the change in pH that occurs when 1.0 g NaOH is added to 250 mL of each of the following solutions.a. Pure water b. 0.0200 M NH3 c. 0.100 M NaOHd. 0.250 M HCL e. 0.100 M HClO4   Please answer it correctly. Show complete solutions.

Assuming the final solution will be diluted to 1.00 L , how much more HCl should you add to achieve the desired pH?

You add 19.00 mL of 0.600 M NaOH to 50.00 mL of pure water, and to this mixture you then add 8.00 mL of 0.200 M HCl. What will be the pH of the resulting solution?

At the equivalence point of a weak base against HCl, the solution contains only that of the base, and the pH is calculated from the concentration of this product. True or False?

I don't know if it is possible, but I have to make a solution of acetic acid with a pH of 4 and a volume of 250 mL. I have 500 mL of acetic acid 10% and I need to add a certain amount of this acetic acid to the water to have this pH. I was wondering what are the quantities of water and acetic acid I need to "mix" together.  Thank you !

What is a description of the salt that is used in a buffer solution? from the conjugate base from a weak acid O from the conjugate base of a weak base from the conjugate acid of a weak acid O from the conjugate acid of a strong base

Which of the following combinations of chemicals makes a buffer? Mark all that apply. (Identifying solutions as buffers on a quiz or exam is a critical skill. For this chapter, many problems ask you to find the pH of a solution. The challenge is classifying the solution appropriately, and then selecting the right approach to finding its pH.) O solution that is 0.1 M each in hydrochloric acid and sodium chloride O solution made by combining 25 mL of 0.1 M acetic acid with 12.5 mL of 0.1 M sodium hydroxide O solution that is 0.1 M each in ammonia and ammonium chloride O roughly equimolar mixture of acetic acid and sodium acetate

You add 15.00 mL of 0.700 M NaOH to 50.00 mL of pure water, and to this mixture you then add 5.00 mL of 0.400 M HCl. What will be the pH of the resulting solution?