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Section: ACID-BASE TITRATION: REPORT PAGES Name: Partner's name: PART I. Standardization of NaOH solution DATA TABLE 1 Trial 1 Mass KHP (3) 1.516 a Final burette reading (mL) 13.8mL Initial burette reading (mL) 0 mL Volume of base used (mL) Vbase=Vina-Vinitial 13.8ml Volume of base used (L) 0.0158 L Trial 2 Trial 3 0.500g 0.6029 13 mL 13.1mL 0,1mL 13.OnL 13 mL 0.01L 0,013 L UNKNOWN NUMBER 14 PART II. Titration of the unknown acid DATA TABLE 2 Trial 1 Trial 2 Trial 3 10.00 10,00 10.00 Volume of unknown acid, Vacid (mL) Final burette reading (mL) Initial burette reading (ml) Volume of base used (mL): VbaseVfinal - Vinitial 9.4mL 0.0mL 9.4L 9.3mL 0.0mL 9.3ml 9.4mL 0,0ml qual CALCULATIONS: PART I. Standardization of NaOH solution 1. Calculate the number of moles of potassium hydrogen phthalate (KHP) in each sample. Use dimensional analysis. MMXNP 1 mol KHP Hp = mxnp X where: ner is the number of moles KHP, MHP is the mass of KHP, and MMKHP is the molar mass of KHP Trial 1 NKHP Trial 2 KHP Trial 3 KHP 101 | Pag
VON 2. Calculate the molarity of NaOH (Mr.on) for each sample using: nkaran.o at the equivalence point, and nn.ch - MNOH X Vuon and MaOH = where Mrow is the molarity of NaOH; nkar is the number of moles of KHP, non is the number of moles of NaOH, and VN.ou is the volume of NaOH(L). Trial 1 Mon 0.1931 M Trial 2 Mion-0.1385M Trial 3 Muon= 0, 891 M 3. Calculate the average value of the molarity of your NaOH. This is the value (Mon) you will use to determine the molarity of your unknown acid in part II. M Naon = 0.1868M PART II. Titration of the unknown acid UNKNOWN NUMBER 1. Calculate the molarity of your unknown acid for each sample using: MNOVNO M.cdVacid = MOV naon and Macid = Vacia where Mac is the molarity of acid; M Neon is the average molarity of NaOH (the base). Vson is the volume of NaOH m and Vaca is equal to 10.00 mL. Trial 1 Macid- 0.1756 M Trial 2 Macd= 0.1134 Macid Trial 3 0, 1756m 2. Calculate an average value for the molarity of your unknown acid. Macid = 0.175m 102 Page