Answer to Solved Calculate th pH of 0.00756 M HNO3.. based on rules. This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts.
How would I be able to calculate the pH of a buffer that includes a polyprotic acid and its conjugate base? For example, if I were to add a certain amount of the polyprotic acid H2A and a certain amount of its conj base A^2- (obviously in the form of a salt, say Na2A), how would I find the pH? Assume I know the ka1 and ka2 values. Now what?
d. 3.3 × 10-10 M. In deciding which of two acids is the stronger, one must know: a. the concentration of each acid solution. b. the pH of each acid solution. c. the equilibrium constant of each acid. d. all of the above. e. both A and C must be known. c. the equilibrium constant of each acid. HNO 3 + H 2 O -> H + + NO 3-. This means that for every 1 mole of HNO 3 that dissociates, 1 mole of H + is produced. Thus, every 0.0040M of HNO3 produces 0.0040M of H+. Perfect! Now we can plug our [H+] into the formula for pH: pH = -log [H+] pH = -log [0.0040M] pH = 2.397940009. We have 2 significant figures (sig figs) in our given value 0 Chemistry. Chemistry questions and answers. Calculate the pH of the solution after the addition of each of the given amounts of 0.0518 M HNO3 to a 60.0 mL solution of 0.0750 M aziridine. The pK, of aziridinium is 8.04. What is the pH of the solution after the addition of 0.00 mL HNO3? pH = m What is the pH of the solution after the addition of