5. You use a 0.1380 M HCl to standardize an NaOH solution. The burets below show initial and final volume readings for the titration to the perfect endpoint. Calculate the appropriate volume ratio (Va/Vb or Vb/Va ratio) and the [NaOH]. Acid Buret Reading (mL) initial final sump)mm HEHI | | | Base Buret Reading (mL) initial final ILI

5. You use a 0.1380 M HCl to standardize an NaOH solution. The burets below show initial and final volume readings for the titration to the perfect endpoint. Calculate the appropriate volume ratio (Va/Vb or Vb/Va ratio) and the [NaOH]. Acid Buret Reading (mL) initial final sump)mm HEHI | | | Base Buret Reading (mL) initial final ILI

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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A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the pH. Complete Parts 1-4 before submitting your answer. 3 NEXT > A 50.0 mL solution of 0.300 M CH3COOH was titrated with 0.300 M NaOH. Fill in the 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.. CH3COOH(aq) + OH (aq) Before (mol) Change (mol) After (mol) 0.150 0 1 -0.150 Initial (M) Change (M) Equilibrium (M) -X 0.300 0.0150 0.0150 - x 0 1 2 -0.300 0.300 + x -0.0150 0.0200 + x CH3COO (aq) + 0.300 0.300 - x A student was titrating a solution of acetic acid with a sodium hydroxide solution. Determine the pH at the equivalence point. Do this by constructing a BCA…
8. You are titrating 50.0 mL of 0.200 M propanoic acid with 0.100 M NaOH. Use the data in the table to answer the questions. Name Propanoic acid Structure CH3CH2CO2H pka 4.874 Ka 1.34 × 10-5 a) Assuming that the equivalence point is considered 100% completion, calculate the pH at the following points: 0%, 10%, 50%, 90%, 100%, and 120%. b) Sketch the titration curve. c) What would be an ideal pKa for an indicator to use in this titration?
Calculate the pH during the titration of 10.00 mL of 0.400 M hypochlorous acid with 0.500 M NaOH. First what is the initial pH (before any NaOH is added)? The Ka for HOCl is 3.0 x 10-8 M.(THE ANSWER IS 4.96) I DONT NEED THIS ABOVE QUESTIONS DONE!!!! THE QUESTIONS BELOW RELATE TO IT THOUGH!!!! What is the pH after 4.80 mL of NaOH are added? What is the pH at the equivalence point? What is the pH after 9.80 mL of NaOH are added?
Explain how the calculation of the molar solubility will be affected if the end point of the titration was surpassed (excess HCl was added). Procedure: . Obtain a sample of saturated Ca(OH)2 solution (without added CaCl2) from your instructor. Pipet 25 mL of the saturated Ca(OH)2 solution into a 125 mL flask and add 2 drops of methyl orange indicator. Titrate the Ca(OH)2 solution to the methyl orange endpoint, where the color changes from yellow to red. Remember, the addition of HCl should stop within one-half drop of the end point. Read and record the final volume of standard HCl in the buret. Titrate two additional 25 mL aliquots of the saturated Ca(OH)2 solution.
How do I determine the volume of NaOH delivered and the molar it’s of the standard NaOH?
2. After dissolving the KHP with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 sec and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared! a) What happened? b) What can the student do to correct for this erTor and salvage this trial? How should the data sheet be modified to reflect this correction? 3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red! a) What happened? b) What can the student do to correct for this error and salvage this trial? How should the data sheet…
Answer the following questions about a titration between 25.0 mL of a weak base (Kb= 6.9*10-5) and 0.100 M hydrochloric acid). A.What is the concentration of the weak base solution if it requires 37.50 mL of the HCl solution to reach the equivalence point (assume 1:1 stoichiometry)? B.What is the initial pH of the weak base solution before any HCl is added? C.What is the pH of the titration at the equivalence point? D.The pKa of ethyl red is ~ 5.4 and the pKa of thymol ~ 8.4. Which indicator would be best to use in the titration?
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. PREV 1 2 4 NEXT Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. 3.0 x 10-6 %3D 5 RESET [0] [0.200] [0.0200] [0.100] [0.140] [0.175] [x] [2x] [0.200 + x] [0.200 - x] [0.0200 + x] [0.0200 - x] [0.100 + x] [0.100 - x] [0.140 + x] [0.140 - x] [0.175 + x] [0.175 - x] II
Part C. Determination of Unknown Balanced chemical equation: Hcl+ Na OH -o Nacl t Hg0 Unknown number NA Trial 1 Trial 2 Trial 3 Volume of unknown HCl titrated 10.00mL NA NA Initial burette reading 0.90mL Final burette reading 30.90mL Volume NaOH added 20 00ML 50.00MLXO.144 m=43.2m moles NaOH added 4.335m (Use average molarity from part B and multiply it by the volume you added) 0.4335 M moles HCl 4.335m 04335m 10.00 mL molarity of HCl Actual Molarity (from instructor) 0.3150M percentage error
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