Fusce dui lectus, congue vel laoreet ac, consectetur adipiscing elit. Determining Molarity Through Acid-Base Titration - Lab Report - Studocu Trial mL KHP used; Moles KHP used. \[\ce{H_2SO_4} \left( aq \right) + 2 \ce{NaOH} \left( aq \right) \rightarrow \ce{Na_2SO_4} \left( aq \right) + 2 \ce{H_2O} \left( l \right)\nonumber \]. Potassium hydrogen phthalate, KHC8H4O4 (abbreviated KHP), is a non-hygroscopic, crystalline, solid that behaves as a monoprotic acid. Your email address will not be published. A link to the app was sent to your phone. Conversely, for the titration of a weak base with strong acid, the pH at the equivalence point is less than 7 because only the conjugate acid is present. 2.00 grams was the amount expected to be taken, but the experimental amount was 1.99 grams. 4.Add 4 or 5 drops of phenolphthalein indicator to the flask. The deviation in the volume, however, is not the only indicator of noticeable systematic errors. moles of NaOH used = (0.0131 L)* (0.05 mol/L) = 0.000655 moles The balanced equation is: NaOH (aq) + HCl (aq) NaCl (aq) + H 2O (l) So the mole ratio NaOH:HCl is 1:1. Data Table: Titration Part 1: Use the molar mass of KHP to calculate moles of KHP reacted. Fusce dui lectus, congue vel laoreet ac,gue vel laoreet ac,gue, rem ipsum dolor sit amet, consectetur adipiscing elit. Liters NaOH sol'n used. As the transparent NaOH solution came into contact with transparent phenolphthalein in the KHP solution, it turned pink which on shaking became transparent. Lorem ipsum dolor sit amet, consectetur adipiscing elit. Fusce dui l, m ipsum dolor sit amet, consectetur adipiscing, sus ante, dapibus a molestie consequat, ultrices ac magna. 1.54g of KHP is equivalent to 0.00754 mol of KHP. Unknown Acid Postlab 1 - Chem Lab - Unknown Acid Postlab 1 - Studocu CALCULATIONS molarity of NaOH For each trial calculate the precise molarity of the NaOH solution using the data for the listed trial. \[\text{moles acid} = \text{moles base}\nonumber \] . Nam lacinia pulvinar tortor nec facilisis. The data from the titration is then used to calculate the molarity of the NaOH. Save my name, email, and website in this browser for the next time I comment. eqn. Number of moles of KHP in 2.00 grams = (m/M) = (2/204.22) mol = 0.00979 mol [c] KHP = n/V = (0.00979/0.1) mol dm -3 Number of moles of KHP in 0.01 dm 3 of solution in conical flask = [c] x V = 0.0979 x 0.01 = 9.79 x 10 -4 mol. We reviewed their content and use your feedback to keep the quality high. RAW DATA MASSES Trial #1 Trial #2 Trial #3 mass of KHP weighed out: 0.6096_9 _0.6088_9 0.6022_9 VOLUMES burette reading: FINAL 32.65_ m _33.49_ML_30.47ML burette reading: O INITIAL 3.09 mL 4.29 ML 1.19 mL Volume of NaOH used: minus 0 29.56 mL 29.20 ml 29.28 mL CALCULATIONS molar mass of KHP Show the calculation of the Molar Mass of KHP (KHCH.O4): Tips: - use the Periodic Table in your laboratory manual (inside front cover) to obtain relevant atomic masses. Answered: Data Table: Titration Part 1: Use the | bartleby The expected % uncertainty that was expected was 0.500%, and the uncertainty I obtained was 0.503%. What. A sample of 354.5 mg of KHP is added to water, which is then neutralized by around the world. Related Textbook Solutions If only monoprotic acids and bases are used (those that furnish or react with one H+ per molecule), then at the equivalence point the number of moles of acid equal the number of moles of base (moles acid = moles base). \[\text{M}_A = \frac{\text{M}_B \times \text{V}_B}{\text{V}_A} = \frac{0.500 \: \text{M} \times 20.70 \: \text{mL}}{15.00 \: \text{mL}} = 0.690 \: \text{M}\nonumber \]. moles of NaOH used = moles of KHP moles of NaOH used = (Volume of NaOH used)* (Concentration of NaOH) You have not specified a concentration, so be it, concentration of NaOH = 0.05 mol/L. moles KHP = _____mass KHP_____ MW KHP (204.22 g/mol) 2. Molarity = moles of solute/Liters of solution. questions 6-11 for all other fine trials (not the rough trial) your group completed. When KHP and NaOH combine, a positive hydrogen ion leaves the KHC8H4O4 and a negative hydrogen atom leaves the NaOH. Fusce dui lectus, congue vel laoreet ac, dictum vitae odio. In this case, you are looking for the concentration of hydrochloric acid (its molarity): NaOH is a base with a 1 OH- to 1 NaOH molar ratio so that there are.00278 moles of NaOH. answered 11/20/13, Andre W. Overall, the data obtained, although not completely inaccurate, is not as accurate as it could have been. Nam lacinia pulvinar tortor nec facilisis, cing elit. In order to determine the exact concentration of a sodium hydroxide solution you must standardize it by titrating with a solid acid that is not hygroscopic. 17.56 ml of the above NaOH(aq) solution to titrate the unknown acid solution to its end
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