Calculate the pH of a 1.00 L solution that is 0.250 M in trimethylamine and 0.350M in trimethylammonium chloride. Calculate the pH AFTER 0.100 moles of NaOH are added to the solution in 10.

1. For each of the solutions in part 3, calculate an expected pH. The Ka for HC₂H3O2 is: 1.8 x 10¹5 and the Kb for NH3 is 1.76 x 10. Remember to account for the dilution factor. a. 10.0mL of 0.10 M HC₂H₂O2 + 5.0mL of 0.10M HCI b. 10.0mL of 0.10M NH₂ + 5.0mL of 0.10M NaOH c. 10.0mL of 0.10M HC₂H₂O₂ +10.0mL 0.10M NaC₂H₂O₂ d. 10.0mL of 0.10 M NH3 + 10.0mL of 0.10M NH₂CI 2. Which solution(s) in question 1 would be considered a buffer solution? 3. Complete the calculation for K, from the earlier discussion of the amphoteric salt. Will this ion be acidic or basic? Predict the expected pH for the 0.050M solution. (1) H₂PO4 (aq) + H₂O → H3O*(aq) + HPO42(aq); Ka2 = 6.2 x 10-8 (2) H₂PO4 (aq) + H₂O → Kw H3PO4(aq) + OH(aq); Kb = ??? Kal 4. Similarly, the HPO4 ion is also amphoteric. The two possible reactions are: (1) HPO4² (aq) + H₂O → H3O*(aq) + PO4³(aq); Kas = 4.2 x 10-¹3 (2) HPO4 (aq) + H₂O Kw → H₂PO4 (aq) + OH(aq); Kb = <= ??? K₁2 Complete the calculation for Kb. Will this ion be acidic or…

16.

- Calculate the pH of the solution after the addition of each of the given amounts of 0.0513 M HNO3 to a 60.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04.

A 15.00 mL solution of phosphoric acid (H-PO,) is titrated with 17.50 mL of 0.155 M sodium hydroxide. What is the concentration of the acid?

Calculate the pH of the solution after the addition of each of the given amounts of 0.0691 M HNO, to a 50.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? pH 10.457 What is the pH of the solution after the addition of 6.19 mL HNO,? 9.32 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to half the equivalence point volume? 8.04 pH What is the pH of the solution after the addition of 51.1 mL HNO,? 6.58 pH = Incorrect What is the pH of the solution after the addition of a volume of HNO, equal to the equivalence point? pH = 4.76 What is the pH of the solution after the addition of 57.7 mL HNO,? 2.87

Acids and Bases Chapter 17 Non-Algorithmic Question 21 Part A You wish to prepare an HC2H3O2 buffer with a pH of 5.14. If the pKa of is 4.74, what ratio of C2H3O2 /HC2H3O2 must you use? O 0.40 O 6.0 O 2.51 O 0.40 O 0.10

When 1.3 g of C4H9NO is dissolved in 150 mL water, the resulting solution is 0.50% ionized at equilibrium. a. Calculate the pkb for C4H9NO. Answer: b. 5.5 mL of 1.5 M HCl is added to the solution. Calculate the equilibrium [C4H9NO], [C4H9NOH+], [H3O+], [OH-], and [Cl-] in the solution.

Nn.144. Subject:- Chemistry

Given the structures of cocaine (right) and its free base (left) below: a. Would you expect K for the cocaine to be greater or less than 1.0?  Explain. b. Would K for the free base be higher or lower than for cocaine?  Explain. c. To favor the equilibrium towards the free base, would you make the aqueous solution acidic or basic?  Explain. (Hint: think of Le Chatelier’s principle).