Answered: Vinegar Titration Curve 14.00 13.00…

Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 E 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.1QAP

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

Based on the graph, what is the pK_a of vinegar?

Vinegar Titration Curve
14.00
13.00
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9.00
8.00
E 7.00
6.00
5.00
4.00
3.00
2.00
1.00
0.00
0.00
5.00
10.00
15.00
20.00
25.00
30.00
35.00
Volume NaOH (mL)

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If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
C. Titration of acid by a base Standardization of NaOH Volume of NaOH Mass of KHP Initial buret Final buret Trial used Molarity of NaOH (g) reading (mL) reading (mL) (mL) (1) (2) (3) (4) (5) 1.2075 0.7 25 24.3 0.243 (6) (7) (8) (9) (10) 1.2062 16.4 40.9 24.49 0.2412
Volume of acetic acid (HC2H3O2) in the first titration (L) 10 mL Volume of acetic acid (HC2H3O2) in the second titration (L) 10 mL Normality of sodium hydroxide (NaOH) (N) 0.1 N Volume of sodium hydroxide (NaOH) in the first titration (L) 10 mL = ……..L Volume of sodium hydroxide (NaOH) in the second titration (L) 10 mL = ……..L Normality of acetic acid (HC2H3O2) in the first titration (N) Normality of acetic acid (HC2H3O2) in the secondtitration (N) Average normality of acetic acid (HC2H3O2) (N) Mass % of acetic acid (HC2H3O2) (%)
10. Which refers to the difference between the end point and the equivalence point? A. indicator error B. end point error C. titration error D. personal error
Table 1. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 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) 49.32 49.06 49.93 Table 2. Titration data Table view List view Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.48 1.89 1.95 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) 49.32 49.06 49.93 Expected color at end point Choose... Choose... Choose... Volume of NaOH used (mL) 1. Average Volume of NaOH used in liters 2. Average moles of NaOH used (mol) 3. Average moles of acetic acid (mol) 4. Average molarity of acetic acid (M) 5. Average mass of acetic acid (g)…
Match each term with its definition or description. 0000000 The point in a titration when the added amount of standard reagent is equal to the amount of analyte being titrated. A volumetric analysis technique used to determine the unknown concentration of a solution by using the known concentration of another. A solution of unknown concentration. The standard reagent of known concentration that is added from a buret to the analyte solution. A common concentration unit - moles per liter. The point in a titration when a change in the analyte solution is observed, indicating equivalency. It is added to the analyte solution and aids in the observation of the completion of the reaction. molarity equivalence point Answer Bank end point titration titrant analyte indicator
You are given 3.56 grams of unknown acid. You dissolved it in 50.0mL of DI water and titrate it with 1.00M NaOH. The end point volume of NaOH was 19.7mL. What is the molar mass of the unknown? a. 276 g/mol b. 362 g/mol c. 198 g/mol d. 72.3 g/mol e. 181 g/mol
4.What will be the change in pH after adding 13.4ml of the titrant? * Present your answer to the 2ⁿᵈ decimal place for convenience in graphing. 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 .
6. What do we call reagents of known concentration that is used to carry out a volumetric titration?A. standard titrateB. standard analyteC. standard titrantD. standard reagent7. What has the analyte reached when the amount of added titrant is chemically equivalent to the amount of the analyte in the sample?A. equivalence pointB. end-pointC. titration pointD. Dilution point8. In an acid-base titration, what indicator does an analytical chemist add to indicate chemical equivalence?A. bromophenol greenB. phenolphthaleinC. iodineD.methyl orange9. These are factors in the environment that causes exposure to the emission of electromagnetic waves.A. BiologicalB. ChemicalC. PhysicalD. Radiation10. What concentration unit measures the number of chemical equivalents of reagent in the same volume?A. MolalityB. FormalityC. MolarityD. Normality
What is standard solution ? Why is a standard solution necessary for titration?
A 25.0mL acetic acid sample was titrated using exactly 69.72 mL of a 0.30M sodium hydroxide solution until the endpoint was achieved. What is the molar concentration of the acid sample? A. 0.02 M B. 0.98 M C. 1.95 M D. 3.90 M E. 9.76 M
2. Below is a titration curve generated by a similar titration to the ones simulated, Vinegar Titration Curve 14.00 13.00 12.00 11.00 10.00 9.00 8.00 * 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 15.00 20.00 25.00 30.00 35.00 Volume NaOH (mL) We can use this curve to estimate the pka of our weak acid by what is called the "half equivalence point method". The equivalence point is the middle of the steepest part of this graph. Estimate the volume of NaOH added to the titration at that point by using a rule or other straight edge to follow that point down to the x-axis. Divide that volume by 2 (half the equivalence point) and estimate the pH at that volume of NaOH using your straight edge again. pKa = pH at the half equivalence point. What do you estimate the pka to be? 3. The pka of acetic acid is 4.76. Calculate percent error between the true value and your estimated value from question 2.