What H 3O + concentration corresponds to each pH value: (a) 13; (b) 7; (c) 3? Label each solution as acidic, basic, or neutral.

What is the pH of a solution prepared by adding 18.0 mL of 1.51 M nitric acid to 180.0 mL of 0.150 M dimethylamine solution (CH3)2NH? Round your answer to 2 decimal places.

(a) What is the pH of 0.75 M NaF?(b) What is the pH of 0.88 M pyridinium chloride, C₅H₅NHCl?

6.)Calculate the pH of a 0.400M solution of phosphoric acid, H3PO4.

What volume of water must be added to a 26.33 mL solution of a pH = 1.17 solution of HClO4 to raise the pH to 3.53?

8. Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH-]= 0.00045 M; (b) [OH-]= 8.8 X 10-9 M; (c) a solution in which [OH-] is 100 times greater than [H+]. Group of answer choices A.) (a)[H+]= 2.2 x 10-11M, basic (b) [H+] = 1.1 x 10-6 M, acidic (c) [H+]= 1.0 x 10-8 M, basic   B.) (a)[H+]= 2.2 x 10-11M, basic (b) [H+] = 1.1 x 10-6 M, acidic (c) [H+]= 1.0 x 10-4 M, acidic   C.) (a)[H+]= 2.2 x 10-11M, basic (b) [H+] = 1.1 x 10-6 M, basic (c) [H+]= 1.0 x 10-8 M, basic   D.) (a)[H+]= 2.2 x 10-11M, acidic (b) [H+] = 1.1 x 10-6 M, basicic (c) [H+]= 1.0 x 10-8 M, acidic

Calculate the concentration of HNO3 in a solution at 25°C that has pH (a) 2.06, (b) 1.77, and (c) 6.01.

What is the pH of a 0.680 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺], [OH⁻], and pH in a solution with a pOH of 4.33?