Determine if the following statements are correct regarding the graph of rate data above? The half-life, t1/2, is independent of the initial concentration The rate constant, k, would have units of M-1 s-1  Doubling the concentration of A would not change the rate of the reaction.

Below is a representation of an acid in water.  Which of the following statements is/are correct about the following image: The percent ionization of the acid would be 100% The acid could be chloric acid The acid could be acetic acid

Determine which of the following statements are True or False about 500.0 mL of buffer consisting of 2.1 M pyruvic acid (HC3H3O3) and 3.6 M sodium pyruvate (NaC3H3O3): The pH slightly decreases when 25.0 mL of 0.50 M hydrochloric acid is added to the buffer but the buffer is still effective 0.250 moles of sodium hydroxide will be neutralized by pyruvic acid and the buffer is still effective 0.125 moles of hydrochloric acid will be neutralized by pyruvic acid and the buffer is still effective

Predict what happens when 0.700 g of K2SO4 is added to 0.500 L of a 0.20 M AgNO3 solution. The Ksp of Ag2SO4 is 1.2 x 10-5. (Assume no change in volume)   

Predict what happens when 0.210 g of K2SO4 is added to 0.500 L of a 0.35 M AgNO3 The Ksp of Ag2SO4 is 1.2 x 10-5. (Assume no change in volume) 

A 0.075 M solution of an unknown weak acid has a pH of 2.38. Determine the percent ionization of that acid.

What is the molar solubility of lead (II) chloride (PbCl2), the Ksp is 1.7 x 10-5?

What is the pH of a solution made of 0.552 M cyanic acid (HCNO) with 0.789 M of sodium cyanate (NaCNO)?

For this question you need to do the work on Honorlock then show the work to the camera.  Immediately Go to Exam 3 Free Response Upload Spring 2025 and submit your work I will look at the time between ending this exam and uploading your work. You will not see this question in the upload so do not submit until you are done with this question.  For Full Credit show all your work including reactions, equations, and math. A 0.0125 M solution of a weak acid (HA) has a pH of 2.48. Calculate the acid ionization constant (Ka) for the acid.  

A 198.6 mL sample of 0.318 M potassium hydroxide, KOH is being titrated against 0.548 M selenic acid, H2SeO4. Determine the volume of H2SeO4 needed to reach the equivalence point.