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.
1. Use the pH equation which is: \(pH = -\log[H_{3}O^+]\). 0.055 M HBr, HBr is a strong acid [H 3 O +] = 5.5 X 10-2 M. pH = -\log(5.5 X 10-2) = 1.26. 2. Use the pH equation \(pH = -\log[H_{3}O^+]\) and pK w equation \(pK_w = pH + pOH = 14\). 0.00025 M HCl, HCl is a strong acid [H 3 O +] = 2.5 X 10-4 M. pH = -\log(2.5 X 10-4) = 3.6. Then solve As a result, the pH of the solution will be neutral. #pH_("equivalence point") = "7"# FInally, you add a little more base, 0.20 mL to be precise, to the now-neutral solution. This means that the concentration of the hydroxide ions will determine the pH of the solution. The number of moles of #NaOH# added is 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?
Science. Chemistry. Chemistry questions and answers. Calculate the pH of 100.00mL of 0.20 M HNO3 solution after 43.00 mL of NaOH 0.20 M have been added.

The pKb of ammonia is 4.75 at 25°C. Answer. As shown in part (b) in Figure 17.4.3, the titration curve for NH3, a weak base, is the reverse of the titration curve for acetic acid. In particular, the pH at the equivalence point in the titration of a weak base is less than 7.00 because the titration produces an acid.

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    • calculate ph of hno3