What is the pH of a solution of 0.5 M trimethylamine (N(CH3)3) with pKa for (CH3)3NH+ = 9.48?

3. Which is the stronger acid: (b) Boric acid with a pKa of 9.14 or carbonic acid with a pKa of 6.37?

What percentage of aqueous phenylammonium ion is deprotonated at pH = 8.530? The Ka of phenylammonium ion is 2.51×10-5 M. Be sure to write the chemical equation showing the acid/base equilibrium ofC6H5NH3+ ion.

In which solvent, (CH3)2C=O or [(CH3)3C]2C=O, is NaCl more soluble? Explain.

1. Solve the following problem and fill in all the blanks

Draw the amino acid Asparagine with the biologically-preferred stereochemistry and ionization expected at pH 7.4.

In the following chemical reaction what is the concentrations of [H3O+] in a solution that is 0.00045 M [Al(H2O)6]3+.  Assume that the [Al(H2O)6]3+ dissociates 100% completely and assume 1 Liter of solution. [Al(H2O)6]3+  +  3H2O  ↔  [Al(H2O)3(OH)3]2+  +  3H3O+

Calculate the pH of the solution after the addition of each of the given amounts of 0.0651 M HNO3 to a 50.0 mL solution of 0.0750 M aziridine. The pKa of aziridinium is 8.04. What is pH after adding 62.6 mL HNO3?

An analytical chemist is titrating 234.9 mL of a 0.5100M solution of trimethylamine ((CH3)N) with a 0.5700M solution of HNO3. The pK, of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 251.7 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = -0 X $

6. Calculate the pH of a 1% w/v solution of ephedrine sulfate. pKa of weak base ephedrine is 9.36