Quantity of Acetic Acid in Salad DressingTitration Results: 1000μL aliquots of salad dressing against a sodium hydroxide solutionPlease only fill in 3 concordant results!Titration number:123ErrorFinal burette reading (mL)7.91522.2±0.05 mLInitial burette reading (mL)0.97.917±0.05 mLTitre (mL)77.17.2±0.10 mLAverage (mean) volume of concordant titres: 7.1Concentration of Acetic Acid (M) (to 3 sig figs): 6.88mLIMConcentration of Acetic Acid (as %w/v) (to 3 sig figs):%Note: %w/v = (g/mL) x 100%

The concentration of the NaOH solution is missing from the image, so it's not possible to calculate…

Answered: Quantity of Acetic Acid in Salad…

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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HC2H3O2 (aq) + NaOH (aq) ----> NaC2H3O2 (aq) + H2O(l) Trial Vi (mL) Vf (mL) 1 2.25 15.76 2 3 For their first trial, a student pipettes 5.00 mL of a vinegar solution into an Erlenmeyer flask. The student titrates the vinegar with standardized NaOH with a molarity of 0.317 M. The volume of titrant used was recorded in the table above. Calculate the molarity of the vinegar solution for this trial. Enter a number without units.
According to the reaction below: if 35.48 mL of H2SO4 with an unknown concentration were titrated using 1.122 M KOH, and it required 120.80 mL of the KOH solution to react with all of the H2SO4, what was the initial concentration of the H2SO4 solution in mol/L. H2SO4 +2KOH → 2H2O + K2SO4 Answer to THREE decimal places
Determine which of the following statements is/are FALSE: Statement 1: The endpoint is when all the analyte has reacted with a small excess of titrant Statement 2: At the endpoint, the concentration of analyte will be slightly artificially high Statement 3: According to the image below, the titrant needs to be added dropwise in Figure 2 L L L L 1 2 3 4 Select one: Only statement 2 Only statement 3 Statements 1 and 3 Statements 1 and 2 Statements 2 and 3
Make sure has correct significant di
Determining the % Citric Acid (H3C6H5O7) in Lemon Juice Balanced neutralization reaction: 3NaOH + H3C6H5O7 ------ Na3C6H5O7) + 3H2O (Citric Acid) a) Volume of Lemon Juice = 10.0ml b) Mass of Lemon Juice = 11.1g c) Density of Lemon Juice = _______g/ml d) Amount of NaOH to neutralize = 63.9ml e) Grams of Citric Acid in Lemon Juice = ______grams f) % Citric Acid in Lemon Juice = ________%
A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.
Acid Base Titrations Given the information below, calculate the acid concentration: show work and use correct number of significant figures Unknown acid ID#: ____HCl_____(concentration unknown) Concentration of NaOH: 0.10 M Initial Buret reading (mL) : 4.0 Final Buret reading (mL): 14.2 Volume of NaOH added (mL): 10.2 Calculated acid concentration (M): ???
Calculate the number of Moles of NaOH required to reach equivalence.
A solution of phosphoric acid (H3PO4) with a known concentration of 0.250M H;PO4 is titrated with a 0.800 M NaOH solution. How many mL of NaOH are required to reach the third equivalence point with a starting volume of 72.0 mL H;PO4 according to the following balanced chemical equation: H;PO4 + 3 NaOH Na3PO4 + 3 H2O STARTING AMOUNT ADD FACTOR ANSWER RESET *( ) %3D 43.2 72.0 6.75 x 104 22.5 0.250 1000 0.0675 2 3 7.50 67.5 0.001 0.800 mol H3PO4 L NaOH g NaOH LH;PO4 M H3PO4 M NaOH g H;PO + mL H3PO4 mL NaOH mol NaOH
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
Question Completion Status: QUESTION 3 3. A weak acid was titrated using 0.20 M KOH. The pH at several volumes added was recorded and plotted as shown below. If 175 mg of the weak acid was used, what was the molar mass of the weak acid solution? pH vs Volume of KOH(aq) 13 12 11 10 6. 7. 6. 4. 3 4 5 6 8 9 10 mL KOH(aq) QUESTION 4
A student uses 16.40 mL of 1.500 M NaOH to titrate 11.90 mL of H 2 SO 4 . The theoretical molarity of H 2 SO 4 1.100 M. Write the balanced equation for the reaction, find the molarity of H 2 SO 4 , and determine the student's percent error. a) Balanced equation b) Molarity of H 2 SO 4 c) Percent error

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