Titration Experiment 1: Acid-Base Titration: Unknown HClWrite chemical equation*+ HClcags N s→ Naclceg) + H,OWrite NIEOH c) + HEogs → H2OC)Enter the data into the table and choose three titrations to find the molarity of the unknown HCI.Unknown # HCITitration 1 Titration 2 Titration 3 Titration 4 Titration 5Volume NaOH used to titrateunknown HCI solution17.43ml 16.5O ml662 mll16.57ml16.6dmLMolarity of NaOH used foreach titration0.25640.1787/01692/0.1704/oiado1703Molarity of HCIAverage M HCI (avg ±standard deviation)10.17171.63% PrecisionCalculations1. Provide one representative calculation that you used to determine the molarity of HCI. Besure to show all units and use proper sig figs!V HCI-25mLMHCI =?VN2OH = 16.6lmLMNAOH=0.2564MHCI VHCI=MNAOH VAa OHMHCI 25=O. 1564 16.61MHCI= 0.2564.16.6125MHCI=0.17032. Average molarity of three titrations.6.1787+0.1692+0.1704+0.1619+ O.1703MACI= 0.117 3. Standard deviation across three titrations (put your data in Excel. Write your stdev formulabelow)4. Percent Precision for three titrations

Acid-base titration is a quantitative analytical method to determine the concentration of the…

Titration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation + H2C NaCHcay"+ Noclag) HClcog> Nacog tOH cop) + H Ceg) + Cl →Na ta) + Clan+ Write NIE Enter the data into the table and choose three titrations to find the molarity of the unknown He Unknown # HCI Titration 1 Titration 2 Titration 3 Titration 4 Titration 5

Titration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation + H2C NaCHcay"+ Noclag) HClcog> Nacog tOH cop) + H Ceg) + Cl →Na ta) + Clan+ Write NIE Enter the data into the table and choose three titrations to find the molarity of the unknown He Unknown # HCI Titration 1 Titration 2 Titration 3 Titration 4 Titration 5

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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D How is the pka determined in a titration for the removal of a proton in an acid? It is the pH at the equivalence point It is the initial pH of the acid solution It is the pH halfway between equivalence points O The pKa cannot be determined in a titration Question 4 The volume of sodium hydroxide required to reach the equivalence point is 35.69 mL for a monoprotic acid. What is the volume at which the pKa is determined? Report your answer to one decimal place. Question 5 The final equivalence point in the cola titration cannot be determined because the sodium hydroxide pH is too low. True False
Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K of pyridine is 1.7 x 10-⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution pH at the equivalence point? (Two decimal places) Type your answer...
1.00 x 10-² A student was titrating a solution of HC4H7O₂ with a Sr(OH)2 solution. Determine the pH at a particular point in the titration. Do this by constructing a BCA table and determining the pH. Complete Parts 1-2 before submitting your answer. Before (mol) Change (mol) After (mol) NEXT > 40.0 mL of a 0.200 M HC4H7O2 solution was titrated with 100 mL of 0.100 M Sr(OH)2 (a strong base). Fill in the ICE table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. 0 -1.00 x 10-² 1 HC4H-O₂(aq) + 0.100 1.20 x 10-² 0.200 OH-(aq) -1.20 x 10-² 2.00 x 10-³ 2 2.00 x 10-² H₂O(l) + -2.00 × 10-³ -2.00 x 10-² C4H7O₂ (aq) 8.00 x 10-³ RESET -8.00 x 10-³
Hi, im writting a practice titration lab. The purpose lab is to determine the concentration and Ka of a weak monoprotic acid (HA). You will also determine the identity of the acid. HA(aq) + NaOH(aq) → H2O(l) + NaA(aq) My question is:What volume of NaOH (titrant) was required to reach the equivalence point according to te table.
a) In a NaOH and HCl titration lab: Suppose you add 40 ml of water instead of the 45 mL. How will this affect the calculations for the molarity of the HCI? (In this case, the molarity of HCl turned out to be 0.559 mol/L). While being specific. Explain why it will not matter or it will make the molarity high or it will make the molarity low. b) if you disregard the instructions to titrate until a persistent blue endpoint is reached and instead conclude the titration at the initial appearance of blue, describe the impact on the reported molarity of the CoC12 solution. Provide specific details and specify whether the reported molarity will be higher, lower, or remain unaffected.
Questions 15-20 refer to the same weak base/strong acid (WB/SA) titration. The K of pyridine is 1.7 x 10-⁹. A 40.00 mL solution of 0.700 M pyridine (C5H5N) is being titrated with 1.05 M hydrochloric acid (HCI). What is the solution pH before the titration begins? (Two decimal places) Type your answer...
Question 17
Consider the titration of 80.0 mL of 0.100 M Ba (OH), by 0.400 M HCI. Calculate the pH of the resulting solution after the following volumes of HCI have been added. a. 0.0 mL pH = b. 20.0 mL pH = c. 30.0 mL pH= d. 40.0 mL PH= e. 90.0 mL pH = Submit Answer Try Another Version 1 item attempt remaining
14 Given the hypothetical titration curves below, determine what curve has a stronger acid. 14 a. b. C. d. 12 10 8 6 4 () 0 Curve A Curve B Curve C Cannot be determined A B and C 10 20 30 40 50 60 Volume of 0.1000 M NaOH, mL
QUESTION 5 When titrating a strong monoprotic acid and KOH at 25°C, the O pH will be equal to 7 at the equivalence point. titration will require more moles of base than acid to reach the equivalence point. O pH will be less than 7 at the equivalence point. pH will be greater than 7 at the equivalence point. titration will require more moles of acid than base to reach the equivalence point.
In a titration of a weak acid with a strong base, what is the pH of the solution at the equivalence point?