1. Compare your pKa, Ka and molar mass from your experiment to the expected values for KHP. How well do they compare? What might account for the differences? 2. Based on your results in Part 1, is the method used reliable in determining pKa, Ka and molar mass of a weak acid? Explain. 3. Discuss your thinking on how you determined the identity of your unknown. Were there two (or more) acids that were difficult for you to distinguish between? If so, how did you makeyour final decision?

why are Ka values difficult to evaluate for acids like HBr, HCl, and HNO3?

How do you solve #10?

under these chemical species by increasing pH of an 0.1 M aqueous solution of each. That is, imagine making an 0.1 M solution of each species. Select 1 next to the species that makes the solution with the lowest pH. Select 2 next to the species that makes the solution with the next higher pH, and so on. Notice that some of the rankings have been filled in for you already. Also notice that water is on the list. For that particular case, just compare the pH of pure water to the pH of the other solutions. Note for advanced students: for all charged species, you may assume the necessary counterions act as neither acids nor bases. species CH₂COOH + H₂O* H₂O NO₂ CH₂COO HNO₂ 103 HIO₂ relative pH of 0.1 M aqueous solution 4 (Choose one) 5 (Choose one) (Choose one) 3 (Choose one) 2 X Ś olo 18 Ar

Please show all steps and don't round until the final answer. Thank you!

1. answer correctly or I will leave negative remarks.

1. what is the ph of 0.50 M solution of citric acid? 2. what is the ph of the solution containing 0.50M citric acid and 0.50 M nitric acid. Report your answer to 2 decimal places.

Question Completion Status: A Moving to another question will save this response. Quèstion 2 Identify the Lewis acid and Lewis base in the given reaction *Sample problem: Hydroxyl + Rubidium * Answer (all caps, no space, & arranged based on the given problem): LB+LA 2. C2H5OC2H5 + AICI3 →(C2H5)20AICI3 A Moving to another question will save this response.

3. A solution is 0.5 M NH4OCl. a. Determine the major species in this solution. b. Identify the strongest acid and strongest base in the solution and write the equilibrium reaction between these two. c. Calculate the equilibrium constant for the reaction in (b) using the equilibrium constants from Table 14.2 and 14.3 in your textbook. Note that the reaction for the autodissociation of water may also be helpful here. d. Calculate the equilibrium concentrations of NH4 + , NH3, HOCl, and OCl- . e. Use the equilibrium constant(s) from (c) to calculate the pH of the solution. f. This problem generally reads “Calculate the pH of a 0.5 M NH4OCl solution.” Recap in general terms the steps taken to solve this problem.

The answers are not 1.77E-9 and 1.55E-5. Please help.