21:051.I what is back titration2. What is the importance of back titration?3. During titration an end point supposed to be reached. What is an end point?What is the difference between an end point and equivalence point if there one?Add a caption...> Status (Custom)+

Answered: 2. What is the importance of back…

Chemistry: Matter and Change

1st Edition

ISBN:9780078746376

Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Chapter18: Acids And Bases

Section18.4: Neutralization

Problem 50SSC

See similar textbooks

Similar questions

Identify which of the graphs represent the given titration experiments best. Graph A Graph B 12 12 11- 11- 10- 10- 9- 9- 8- 8- 7- 7- 6- 6- 5- 5- 4- 3- 3- 2- 2 1 10 15 20 25 30 35 40 45 50 10 15 20 25 30 35 40 45 50 Titrant.volume Cml). Titrant.volume (mL). Answer Bank This graph does not represent a titration. a basic solution titrated with an acid an acidic solution titrated with a base Hd Hd
4.What will be the change in pH after adding 13.4ml of the titrant? * Present your answer to the 2ⁿᵈ decimal place 5.What will be the change in pH after adding 26 ml of the titrant? Present your answer to the 2ⁿᵈ decimal place 6.What is the total volume at equivalence point? Present your answer to the 2ⁿᵈ decimal place 7.What is the pH at equivalence point? Present your answer to the 2ⁿᵈ decimal place 8.Upload a clear and well-lit image of a hand-written, completely plotted and labeled titration curve .
The titration of 5.00 mL of 0.4949 M NH3 with 0.2250 M HNO3. Kb = 1.8×10–5. Fill out chart and list possible indicator. Volume HNO3 (mL) Calculated pH 1 initial 0.00 2 ¼ way to eq. point 3 ½ way to eq. point 4 ¾ way to eq. point 5 0.5 mL before eq. point 6 equivalence point 7 0.5 mL after eq. point 8 well past eq. point 15.00
Titration of Acids and Bases Part B. Determination of the molar concentration of an unknown acid. Molarity of N₂OH = .09M ☆ Volume of unknown acid used (mL) Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mb Moles 9.6 mL 0.5mL 9.1mL (OH) Sample calculations for molarity of unknown acid solution: Trial 2 10mL 18,9 Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 9.6 ml 18.9ml 9,3mL 9.4mL mol NaOH used? M N₂OH = M acid = .1 Gril To multiple decimals
QI/ One of the student wanted to calculate the exact of HCl concentration. He made standardization of 10 ml NaOH with 0.1M H,C,0,2H,0 according to the table: Titration- H2C204 (Burette) Run. No V in. ml V final ml End point 1 2 5 12 Then, he made titration of 10 ml HCl with standard solution of NaOH according to the table: Titration- NAOH (Burette) Run. No V in. ml V final ml End point 1 10.2 2 10 20.3 Was the student successful in the titration ? why? So what is the concentration of HCI?
Which of these apply to Image C (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
10:57 H₂O 0.1 NaCl Solution A Solution B Initial pH 7.0 5.D 3.0 10.0 Acid-Base Titration % acidity from vinegar label Molarity of NaOH 2030 Volume of Vinegar (ml) Initial Volume of NaOH (ml) Final Volume of NaOH (mL) Report Table AB.3: Effect of Adding Base pH after 5 Drops NaOH 11.0 9.0 3.0 11.0 Acid/Base Titration, Buffers, and PH Report Sheet pH after 10 Drops NaOH 5% 0.101 Trial 1 Report Table AB.4: Concentration of Acetic Acid in Vinegar 11.0 12.0 3.0 11.0** 5.00 ML 0.00 ML 41.20 ML Total pH Change Trial 2 5,00 ML 000 ML 38.40mL Buffer? (Y or N) Trial 3 Show your calculations for calculating the %(m/v) for acetic acid in vinegar for Trial 1 in Report Table AB.4. X 5.00 ML 0.01 ML 41.30mL
10:49 1 4 7 +/- Question 6 of 10 In the titration of 69.0 mL of 0.400 M HCOOH with 0.150 M LIOH, how many mL of LiOH are required to reach the equivalence point? 2 5 8 mL 3 60 9 O Submit Tap here or pull up for additional resources XU x 100
[20] ml of [4] M HC2H3O2 is titrated with 2.25 M sodium hydroxide. Ka for HC2H3O2 is 1.8 x 10-5 a. How many mL of sodium hydroxide will be needed to reach the equivalent point? b. What will the pH be at the midpoint to equivalent point (half equivalent)? c. What will the pH be at the equivalent point? d. What will be the pH when an excess 25 mL of sodium hydroxide 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 80.0 mL of the strong acid has been added. The value of Kb for H2NNH, is 3.0 x 10-6. ( PREV 1 2 3 4 NEXT > Based on the result of the acid-base reaction, set up the ICE table in order to determine the unknown. H2NNH3*(aq) + H20(1) - H;O*(aq) + H,NNH2(aq) Initial (M) Change (M) Equilibriu m (M). 5 RESET 0.100 0.200 0.0333 0.0667 +x -x 0.100 + x 0.100 - x 0.200 + x 0.200 - x 0.0333 + x 0.0333 - x 0.0667 + x 0.0667 - x
Which of these apply to the Image (attached)? There should be 4 total answers: A. High End pH B. High Initial pH C. Vertical Line with Equivalence Point Tall D. Equivalence Point Not at pH 7 E. Equivalence point at pH 7 F. low end pH G. low initial pH H. Vertical Line with Equivalence Point Short Using the info identified above, what type of analyte and tirant combo are in the image. Options for Analyte and Titrant: - Weak base - Strong Acid - Strong Base - Weak Acid
5. 50 ml of 0.100 M HC2H3O2 is titrated with 0.25 M sodium hydroxide. Ka for HC2H3O2 is 1.8 x 105 a. How many mL of sodium hydroxide will be needed to reach the equivalent point? What will the pH be at the midpoint to equivalent point? b. c. What will the pH be at the equivalent point? d. What will be the pH when 25 mL of sodium hydroxide is added?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Chemistry: Matter and Change

Chemistry

ISBN:

9780078746376

Author:

Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher:

Glencoe/McGraw-Hill School Pub Co

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

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

Publisher:

Cengage Learning

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

2. What is the importance of back titration? 3. During titration an end point supposed to be reached. What is an end point? What is the difference between an end point and equivalence point if there one?