Table 1. Titration dataTrial 1Trial 2Trial 3Initial burette reading (mL)1.432.501.33Molarity of NaOH (M)0.1000.1000.100Volume of vinegar sample(mL)5.005.005.00Final burette reading (mL)48.9850.6249.60 Average moles of acetic acid (mol)Average molarity of acetic acid (M)Average mass of acetic acid (g)Average mass of vinegar (g) (assume the density of vinegaris 1.00 g/mL)Average mass % of acetic acid in vinegarKnown mass % of acetic acid in vinegar is 5.45%Percent Error

Given: Trial-1 Trial-2 Trial-3 Initial burette reading 1.43 2.50 1.33 Molarity of NaOH…

Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.43 2.50 1.33 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.98 50.62 49.60

Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.43 2.50 1.33 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.98 50.62 49.60

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...

See similar textbooks

Related questions

Q: Part B A310 ml sample of a KOH solution of unknown concentration requires 12.1 ml of 0. 100 M H,SO,…

A: Formula used: Normality: no of equivalent*1000/ volume in ml So number of equivalent= Normality*…

Q: How do I find what the mL of NaOH added and the pH at the equivalence point?

A: AT EQUIVALENCE POINT THERE WILL SUDDEN JUMP IN pH.

Q: Calculate the number of millimoles of acetic acid in Trial #2? Round your final answer to 4…

A: In the given question, NaOH is titrated with acetic acid.

Q: Data Drawer Number Part I. Standardization of the Sodium Hydroxide Solution Mass of weighing bottle…

A: Mass of oxalic acid sample is calculated as the difference in the weight between mass of weighing…

Q: Analysis: 1. Determine the concentration of acetic acid in the flask 2. Write the neutralization…

A: Given : Volume of CH3COOH = 25.00 ml Molarity of NaOH = 0.18 ml Volume of NaOH = 20.22 ml

Q: During titration experiment, you were required to prepare solution for: 2.00M HCl (32% stock…

Q: QUESTION 3 If 14.36 mL of 0.4832 M NAOH is needed to fully titrate a solution made with 0.5829 g of…

Q: 3. At what point in the graph is there a greater amount of boric acid than sodium borate, provided…

A: Buffer solution usually resist change in their pH. Buffer solution consists of a weak acid and it's…

Q: When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH, 32.50 ml of…

A: The given data contains, Volume of H2SO4 =20 mlMolarity of NaOH=0.1249 M Volume of NaOH =32.50 ml.

Q: Sample Site C Final reading (mL) 1 accurate titration 2nd accurate titration 41.00 mL 40.10 mL…

Q: 2. 15.0 mL HNO3 was titrated to equivalence with 60.0 mL of 0.020 NAOH, What is the concentration of…

A: Given : Volume of HNO3 = 15.0 mL Molarity of NaOH = 0.020 M Volume of NaOH = 60.0 mL To…

Q: Analysis of unknown sample. Find the molarity of NaOH (M) using the given values below. Show your…

A: Molarity of the standardized HCl solution used for the titration of the unknown sample = 0.1090 M

Q: Which is the correct order of steps in the preparation of a hydrochoric acid standard solution with…

A: Standard solution is a solution containing a precisely known concentration of an element or a…

Q: 2. Propose three types of procedural error that may impact the results that were experimentally…

A: Answer. Errors generally occur while conducting experiments which can effect our results but with…

Q: Would adding extra distilled water to the Erlenmeyer flask during the titration affect the molarity…

A: Addition of water to titrant or anlyte changes the concentration of the solution. When water is…

Q: can you generate the unknown concentration using this information?

A: The relationship between the concentration (c) and absorbance (A) is identified as follows-Here, ε…

Q: Question 6 Listen If Mohamed Jama titrated 25.0 mL of an unknown concentration of H2SO4 solution and…

Q: From the 3 trials, determine the average Molarity concentration of the H2SO4 to 3 significant…

Q: When 2.61 g of solid Na,cO, is dissolved in sufficient water to make 250 mL of solution, the…

A: Molar mass of Na = 23g/mol Molar mass of C = 12g/mol Molar mass of O = 16g/mol

Q: During the titration process if a drop of standardized NaOH adheres to the inside of the titrand…

A: Since you have posted a question with multiple questions, we will solve first one for you. To get…

Q: 8. The following titration data was collected in a lab. Based on the results, determine the…

A: Acid base titrations are a good way to determine the unknown concentration of an acid or base. It is…

Q: Calculate the concentration of SCN in each of the following standard solutions. Use 0.0500 M Fe3+…

A: a) Initial molarity of SCN-, M1 = 0.002 M Initial volume, V1 = 1.00 mL Final molarity of SCN-, M2 =…

Q: Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity…

A: To calculate ,we would use the give data values.

Q: Titration Experiment 1: Acid-Base Titration: Unknown HCl Write chemical equation + H2C NaCHcay"+…

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

Q: 2. An old bottle of sulfuric acid is found in the lab. The concentration of this bottle is unknown…

A: To determine the concentration of the sulfuric acid solution, we can set up a balanced chemical…

Q: you take 5 mL of of Stock solution and mix it with 5 mL of water to make solution A. You then take…

A: Given 5 mL of of Stock solution

Q: A 45.0 mL sample of a 0.486 M aqueous hydrocyanic acid solution is titrated with a 0.324 M aqueous…

A: Volume of HCN = 45.0 mL Concentration of HCN = 0.486 M Concentration of Ba(OH)2 = 0.324 M pH of…

Q: Briefely explain the meaning of the following terms as they relate to this experiment. a) Titration…

A: The brief explanations are given below -

Q: An aqueous solution of hydroiodic acid is standardized by titration with a 0.146 M solution of…

A: Given, volume of barium hydroxide = 20.2 mL = ( 20.2 mL × 1 L/1000mL) = 0.0202 L molarity of barium…

Q: Final volume ( 18.66 37.42 55.98 Volume of NaOH added ) 18.66 18.66 18.66 scussion/Analysis: Answer…

A: Average can be expressed as the sum of each measurement values divided by the number of…

Q: Questions 11-14 refer to the same strong base/strong acid (SB/SA) titration. A 15.00 mL solution of…

Q: What is Analyte and Titrant? Explain each in 3-5 sentences.

Q: Identify the different techniques used to standardize a solution (Acid-Base Titration)

A: Answer - Standardization is the process of determining the exact concentration (molarity) of a…

Q: Determine the initial concentrations of the species below, after the solutions are mixed. Volume…

A: Formula used M1 V1 = M2 V2 V2 = total volume = 20ml

Q: Find the molarity of HCl (M) using the given values below. Show your complete solution.…

A: Given that - Mass of Na2CO3 (99.98%) = 0.1510 g Final volume of Na2CO3 = 27.5 mL Volume corrected…

Q: Experiment 1 Data Table 2: Experimental Results HCI available 0.1823 for neutralization (g): Moles…

A: Given :A) Calculate the initial amount (grams) of HCl available for neutralization by the antacid.B)…

Q: What is the concentration of an HNO3 solution in percent by mass that was determined to have a…

A: Given : Concentration of HNO3 = 0.669 M And density of solution = 1.00 g/mL. Assuming 1 L i.e 1000…

Q: 36. Titrating a 10.00 mL aliquot of 0.150 M NaOH with 0.120 M HCl will require a. 8.00 mL b. 0.18…

A: Calculation is given as follows

Q: You collected the following data from a titration experiment using a 0.129M standardized NaOH…

A: Please have a look on the solution:

Q: 1

A: Given: volume of HCl=12.0 mLmolarity of HCl=0.24 Mmolarity of NaOH=0.40 M To find: pH before…

Q: What is the concentration of an HNO3 solution in percent by mass that was determined to have a…

Q: Suppose you are performing a titration. At the beginning of the titration, you read the titrant…

A: Approach to solving the question: I analyzed the question before answering it. Key…

Question

100%

Table 1. Titration data
Trial 1
Trial 2
Trial 3
Initial burette reading (mL)
1.43
2.50
1.33
Molarity of NaOH (M)
0.100
0.100
0.100
Volume of vinegar sample
(mL)
5.00
5.00
5.00
Final burette reading (mL)
48.98
50.62
49.60

Average moles of acetic acid (mol)
Average molarity of acetic acid (M)
Average mass of acetic acid (g)
Average mass of vinegar (g) (assume the density of vinegar
is 1.00 g/mL)
Average mass % of acetic acid in vinegar
Known mass % of acetic acid in vinegar is 5.45%
Percent Error

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Step 5

Step 6

Trending now

This is a popular solution!

Step by step

Solved in 6 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

d) please see attached question concentration KOH=20.8325mL pH solution=2.9 beginning of the titration, Vbase = 0.00 mL
Titrated with 0.3554 M NaOH True molarity of unknown: 0.5018 M Trial 1 Trial 2 trial3 The volume of acid added to flask (mL) 10.00 10.00 10.00 Initial buret reading (mL) 0.00 14.06 28.19 Final buret reading (mL) 14.06 28.19 42.30 Volume of base titrated into flask 14.06 14.13 14.11 calculated molarity of acetic acid in your unknown A) calculate the molarity of acetic acid in your unknown for each trial. b) choose the three trials that have molarities that agree within 1% of one another and use these three molarities to calculate average c)use the true molarity for your acetic acid solution from above. using the average molarity that you calculated above calculate the percent error for your unknown.
If 35.12 mL of 0.4221 M NaOH is needed to fully titrate a solution made with 0.7737 g of a diprotic acid, what is the experimental molar mass of the acid? 91.73 g/mol 120.9 g/mol 53.77 g/mol 104.4 g/mol 41.60 g/mol
Which of the following are TRUE about using a buret? Choose all that apply. Group of answer choices Your eye should be level with the meniscus when reading the buret. The volume of liquid in the buret is read from top to bottom. The initial volume reading of liquid in a buret is a smaller number than the final volume reading after a titration. A buret should always be filled to the top.
Volume NaOH (added). pH of analyte 0.00 mL _1.00 10.00 mL 1.23 20.00 mL _1.54 30.00 mL _2.20 _33.33__ mL (at equivalence point) _5.22 35.00 mL _11.46 40.00 mL _12.04_ 9. Sketch your pH curve below. Place the pH on the y-axis and volume of NaOH added on the x-axis.
Please explain, correct and typed answer please as I can not understand handwriting clearly
If 2 ml of 25 N H2SO4 is transferred to 50 ml volumetric flask and complete to mark with ditilled water, the concentration of acid will be .. M* O 2.5 O 1.5 2 O 0.5 0 1 Non of these
10 Chem101 Postlab Quiz 11: BIOL 122 - Int x + -> A app.101edu.co Apps Canvas MYACU to Chem101 Q Quizlet O Khan Academy E Google Docs YouTube Question 5 of 5 A 20.0 mL solution of NaOH is neutralized with 35.0 mL of 0.200 M HBr. What is the concentration of the original NaOH solution? M 1 6. 7 +/- MacBook Pro esc 888 %23 %24 % & 2 4 7 R P Q W Y tab J K caps lock > V M shift 3. 2. 4,
A student performed a titration on a commercial acid certified to be 0.500 M. Using her data from the titration, the student determined her sample to be 0.487 M. Assuming the certified value was the true value, what was the percent error of her measurement?
SKIP IF YOU ALREADY DID THIS OR ELSE DOWNVOTE ANSWER COMPLETELY AND I WILL UPVOTE
Standardization of 1N H2SO4 Titration 1 Titration 2 Titration 3 Titration 4 Mass of flask and Sodium Carbonate 1.5067 g 1.5098 g 1.5076 g 1.5077 Final buret reading (mL) 22 mL 22mL 21.5 mL 22.5 mL Volume of Sulphuric acid used (mL) 30 mL 30 mL 30 mL 30 mL What is the result of my titration?
Br- X tBuOOtBu (cat.) HBr reflux tBuOOtBu (cat.) HBr reflux Me Br