Calculate the pHof (a) a solution that is 0.060 M in potassium propionate(C2H5COOK or KC3H5O2) and 0.085 M in propionic acid(C2H5COOH or HC3H5O2); (b) a solution that is 0.075 M in trimethylamine, (CH3)3N, and 0.10 M in trimethylammoniumchloride, (CH3)3NHCl; (c) a solution that is made bymixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.20 Msodium acetate.

An analytical chemist is titrating 106.0 mL of a 0.1800M solution of piperidine (C5H₁NH) with a 0.7800M solution of HIO3. The pK, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 15.4 mL of the HIO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO3 solution added. Round your answer to 2 decimal places. pH = X B Ar

2.44 moles of HNO3 is added to water and the final volume is 330mL. The pH of this solution was measured to be 1.47, what is the pKa of HNO3?

15D.5.What is the difference between (a)monoprotic acid and a diprotic acid,(b) a weak acid and a strong acid, (c)an acid and a base? HCl, HBr, and HI are strong acids,yet HF is a weak acid. What does thismean in terms of the extent to whichthese substances are ionized insolution?Label each of the followingsubstances as an acid, base, salt, ornone of the above. Indicate whetherthe substance exists in aqueoussolution entirely in molecular form,entirely as ions, or as a mixture ofmolecules and ions. (a) HF; (b)acetonitrile, CH3CN; (c) NaClO4; (d)Ba(OH)2.