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MA Review | Constants 1 Periodic Table You may want to reference (Pages 729 - 739) Section 17.3 while completing this problem. Correct A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HC1O4 solution. Calculate the pH after the following volumes of acid have been added. At the equivalence point, the moles of OH from the strong base are neutralized by H+. However, the concentrations of OH and H+ are still governed by an equilibrium. For a neutral solution, 10-7 = [H+] = [OH-]. Part D 26.5 mL of the acid Express your answer using two decimal places. o 2 ? 1 0 Ad pH = 2.10 pH = Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

Answer 1

what you have done wrong.. you didn’t answer it in two decimal places , you answered it just in one decimal place. Thank you

[KOM] → strong base M, = 0.150m, V, = 20.ome in facter (n.) = 1 nim,u = (1 x 0:15+20) meqt = 3 meat (HClOu] → strong Acid M2 = 0.125M , V2 = 26.5ml n-tacter (hz) = 1 n₂M 2U 2 = (180 125 x26.5) met = 3.3125 here nimiu, <h2 M2V 2 TH+] = n2 M2 U2 -nimivi Vi+U2 3.3125 - 3 - (H+] = 0.006720 M - 20 + 265 ) 6 + 20 Jio PM = -log, CH] => -log Co-006720) [PH = 2.17 / Ane