A 1.00 L buffer solution is 0.150 M in HC7H5O2 and 0.250 M in LiC7H5O2. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HC7H5O2 is 6.5 × 10-5.   For the last few problems, partial credit is available if you email me your work immediately after submission.

A solution is prepared by dissolving 0.23 mol of nitrous acid and 0.27 mol of sodium nitrite in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of NaOH to this buffer solution causes the pH to increase slightly. The pH does not increase drastically because the NaOH reacts with the ________ present in the buffer solution. The Ka of nitrous acid is 4.5 × 10-4.

What is the pH of a 0.040 M Ba(OH)2 solution?

What is the Kw of pure water at 50.0°C, if the pH is 6.630?

If one perfectly competitive firm is the only one to raise its price above the market price, it will:

Which list has market structures in the correct order from the most to the least market power?

When a monopoly operates in a contestable market:

26). Which do you think arose/lived first?

If a firm converts a previously competitive industry into a monopoly without any changes in the cost curves, it will:

31). Why are cyanobacteria one of the largest and most important groups of autotrophic bacteria?