A buffer solution contains 0.53 mol of hydrosulfuric acid (H2S) and 0.10 mol of sodium hydrogen sulfide (NaHS) in 8.70 L. The Ka of hydrosulfuric acid (H2S) is Ka = 9.5e-08. (a) What is the pH of this buffer? pH = ____

Calculate the pH of 2.0 L of a buffer solution that is 0.531 M acetic acid (CH3COOH) and 0.531 M sodium acetate (NaCH3COO) after 0.30 moles of NaOH is added to the buffer. (Ka for acetic acid = 1.8 × 10−5)

You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?

What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4Cl) in enough water to form 2.50L of solution. The K, of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBrO, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBr is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H5O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.