We can use the rearranged molarity equation to calculate the moles of NaCl needed for the specified concentration and volume: mol NaCl = [ NaCl] × L of solution = 0.800 mol L × 0.250 L = 0.200 mol NaCl. We can then use the molecular weight of sodium chloride, 58.44 g mol , to convert from moles to grams of NaCl : Calculate the pH of a buffer solution that is 1.25 M CH3NH2 and 1.00 M CH3NH3Cl. Kb = 8.85 x 10-4 and what would happen after 35.0 mL of 0.45 M HNO3 is added to 250.0 mL of the buffer solution, what would the pH of the solution be after the HNO3(aq) is added? 1)Calculate the pH of a 0.1M solution of NaOH ,knowing that the volume of the solution is 300mL. 2)Calculate the pH of a 0.3M solution of HCl , knowing that the volume of the solution is 250mL (?) A solution contains #[OH^-] = 4.0 times 10^-5# #M#, what is the concentration of #[H_3O^+]#? What is the pH of a 0.25 M nitric acid (HNO3) solution? a.) 0.602 b.) 2.5 c.) 2.49 d.) 13.40 e.) none of these This problem has been solved! You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Example #5: Equal volumes of a pH = 4.0 and a pH = 6.0 solutions are mixed. What is the pH of the mixed solution that results? The first solution is the more general solution, which MUST be used if the volumes are different. Solution #2 is a shorter calculation that works only if the volumes are equal. Solution #1: The #"pH"# of this solution should be close to that in Part a), because the solution in Part a) is a buffer. c) After adding 0.10 mL NaOH The strong base will dissociate completely. Calculate the pH of a 0.20 M solution of iodic acid (HIO3). JessicaHelena. Apr 22, 2018. Acid Acid base Concentration Ph. In summary, the concentration of [H^+] and [IO_3^-] must be the same for pH to be calculated correctly. When calculating pH, [H+] can be found using the square root of [H^+] and [IO_3^-] can be found using the concentration pH + pOH = 14 (Eq. 3) This relationship can be used to convert between pH and pOH . In combination with Eq. 1a/b and Eq. 2a/b, we can always relate pOH and/or pH to [ OH −] and [ H +] . For a derivation of this equation, check out the article on the autoionization of water. cTyGP7.