TUTOR Concentration of Unknown via Titration I 44.58 mL of a solution of the acid H₂C₂O4 is titrated, and 42.80 mL of 0.6900-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution. XM Show Approach Show Tutor Steps Resubmit Incorrect You can work though the tutor steps and submit your answer again,

TUTOR Concentration of Unknown via Titration I 44.58 mL of a solution of the acid H₂C₂O4 is titrated, and 42.80 mL of 0.6900-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution. XM Show Approach Show Tutor Steps Resubmit Incorrect You can work though the tutor steps and submit your answer again,

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.92QE

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TUTOR Concentration of Unknown via Titration I 45.33 mL of a solution of the acid HNO3 is titrated, and 56.00 mL of 0.6900-M NaOH is required to reach the equivalence point. Calculate the original concentration of the acid solution. M Submit Show Approach Show Tutor Steps
1) What is the pH of the 0.66 M NAOH stock solution, to the appropriate number of sig figs? I perform a titration of 350 mL of an unknown concentration solution of HNO3 using the 0.66 M NAOH stock solution and reach endpoint when 530 mL of the basic solution has been added. 2) What was the initial concentration of the HNO3 solution? Please show as much work as possible for partial credit. HTML Edito B IUA A I E E 3 E E X x, E E 回 P 深 T T 12pt Paragraph V> TO DEC 6. 18 atv員 MacBook Pro イ

This is about determinition of acid content in vinegar through titration, please answer the questions. Please answer only the items nummber 4-5. i only put other questions for guide. 1. What is the purpose of standardization? 2. What is the primary standard used (name and formula)? ANS: KHP 3. Suppose that the KHP is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be higher, lower, or unaffected? Explain. 4. In preparing the buret for titration the final rinse is with the NaOH titrant rather than with distilled water. Explain. 5. The procedure suggests the addition of only 2 drops of phenolphthalein. What will be the effect to the analysis if larger amount of phenolphthalein is added?
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO3 after 100.0 mL of the strong acid has been added. The value of Kb for H,NNH, is 3.0 × 10-6. ( PREV 1 Based on the result of the acid-base reaction, determine the pH of the solution. pH RESET 6.21 7.79 11.3 2.70 1.85 1.70 3.91 10.1 12.3 3.70 17.7
Determine the pH at the point in the titration of 40.0 mL of 0.200 M H2NNH2 with 0.100 M HNO: after 10.0 mL of the strong acid has been added. The value of Kb for H2NNH2 is 3.0 x 10-6. 1 2 3 4 NEXT > Use the table below to determine the moles of reactant and product after the reaction of the acid and base. H2NNH2(aq) H*(aq) H2NNH:*(aq) + Before (mol) Change (mol) After (mol) RESET 0.200 0.100 1.00 x 10-3 -1.00 x 103 2.00 x 10-3 -2.00 x 10-3 6.00 x 10-3 -6.00 x 10-3 7.00 x 10-3 -7.00 x 10-3 8.00 x 10-3 -8.00 x 10-3
A titration is carried out for 25.00 mL of 0.100 M HCl (strong acid) with 0.100 M of a strong base NaOH (the titration curve is shown in Figure 14.18 (Links to an external site.)). Calculate the pH after the addition of 30.00 mL base. Answer Choices: 11.959 2.04 12.959 9.595
Consider the titration of 26.0 mL of 0.180 M Na A (a weak base) and 0.140 M H CI. Calculate the pH of the solution after 20.0 mL of H CI has been added. The Kb of the base is 1.41E-4 To avoid rounding errors report your answer with two decimal places. Your Answer: Answer
Consider the titration of a 26.0 – mL sample of 0.180 M CH, NH, with 0.150 M HBr. Determine each of the following. Part A Part B Part C Part D Part E Part F the pH after adding 6.0 mL of acid beyond the equivalence point Express your answer using two decimal places. pH = 1.92 Submit Previous Answers Request Answer X Incorrect; Try Again; 4 attempts remaining
[References] CHEMWORK Consider the titration of 130.0 mL of 0.100 MHI by 0.250 MNAOH. Part 1 Calculate the pH after 25.0 mL of NaOH has been added. pH = Part 2 What volume of NaOH must be added so the pH = 7.00? mL NaOH Submit Show Hints Try Another Version 9 item attempts remaining Submit Answer Visited
ANSWER ALL PLEASE 13) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution before the addition of any KOH. The K aof HF is 3.5 × 10-4. 14) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 150.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5. 15) A 100.0 mL sample of 0.10 M NH3 is titrated with 0.10 M HNO3. Determine the pH of the solution after the addition of 200.0 mL of HNO3. The Kb of NH3 is 1.8 × 10-5. 16) A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 200.0 mL HBr. 17) A 100.0 mL sample of 0.10 M Ca(OH)2 is titrated with 0.10 M HBr. Determine the pH of the solution after the addition of 300.0 mL HBr. 18) A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 400.0 mL of KOH. The Ka of HF is 3.5 × 10-4. 19) A 100.0 mL sample of 0.10…
Part D Consider the titration of a 26.0 – mL sample of 0.180 M CH,NH2 with 0.150 M HBr. Determine each of the following. the pH at one-half of the equivalence point Express your answer using two decimal places. ? pH = 7.00 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining • Part E the pH at the equivalence point Express your answer using two decimal places, pH - 7.00 Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining
Given for nos. 10-11: In an acid-base titration, you were given with a 0.1050 M sodium hydroxide solution placed in a buret and is needed to neutralize 20.0 mL of 0.1500 M sulfuric acid. 10. How much moles of sulfuric acid is found in the 20.0 mL solution of a 0.15M H2SO4? Answer: Computation: 11. What volume of 0.1050 M sodium hydroxide solution is needed to neutralize 20.0 mL of 0.1500 M sulfuric acid? Answer: Computation: 12. Draw and label a complete laboratory set-up of acid-base titration using phenolphthalein as the indicator, using HCl as the analyte/sample, and using NaOH as the standard solution. Cite complete source/(s) if picture will be copied from the internet.