Calculate the pH of a solution made with 0.300 M of HF (Ka = 6.8 × 10-4) and 0.200 M of NaF after the addition of 15.0 mL of 1.00 M of HCl to the original buffered solution volume of 1.0 L?

2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.

A buffer solution is prepared by dissolving 0.10 mol of acetic acid and 0.10 mol of sodium acetate in 1 L of solution. A 10-mL portion of 1 M HCl is then added to the solution. How much does the addition change the pH of the buffer? [Ka (CH3COOH) = 1.8 x 10-5]

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What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to 0.200 L of a buffer solution is prepared from equal volumes of 0.200 M acetic acid and 0.600 M sodium acetate. (The Ka for acetic acid is 1.80 ×10-5.)

You are given a 1.00 L buffer solution that is 0.250 M in HF and 0.250 M in LiF.  Find the pH of the solution after the addition of 0.150 moles of solid LiOH.  Assume no volume change upon the addition of base.  The Ka for HF is 3.5 × 10-4.

A 25.0-mL sample of 0.250 M HA is titrated with a 0.150 M LiOH solution. What is the pH after 10.1 mL of base is added? The Ka of HA is 2.2 × 10-6.

To create a buffer solution, 40.00mL of a 0.100M benzoic acid (Bz) solution are mixed with 20.00mL of 0.100M sodium hydroxide solution. What is the pH of the resulting solution if the Ka of benzoic acid 6.5 x10 -5 and the pKa = 4.19? (Use the Henderson Hasselbach Equation with mmol). Reaction: HOBz + OH-  --->  H2O + OBz-   From the buffer solution above, youo take a 10.00mL portion of the buffer. Using all of the information provided, how much conjugate acid and conjugate base are in the 10.00mL portion that you took out? Group of answer choices 0.167mmol 0.500mmol 0.222mmol 0.333mmol