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molar mass of citric acid, Schemes and Mind Maps of Chemistry

Determination of the molar mass of an acid (and also for citric acid)

Typology: Schemes and Mind Maps

2018/2019

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Skyline College Chemistry 210 Laboratory Manual (August 2013 Revision)
93
Experiment 8. Determination of the Molar Mass of an
Unknown Acid by Acid-Base Titration
In this experiment you will:
Prepare and standardize a solution of sodium hydroxide
Determine the molecular weight of an unknown acid by reacting the acid with standardized sodium
hydroxide solution.
BACKGROUND
An acid reacts with a base to form a salt plus water
(see Scheme 1). Many acids have one proton
available for reaction with a base such as sodium
hydroxide. An acid with one reactive proton per
molecule or formula unit is called a monoprotic acid
or a monobasic acid. A diprotic acid or a dibasic acid
has a maximum of two reactive protons per molecule.
A triprotic acid or a tribasic acid has a maximum of three reactive protons per molecule. There are also examples of
acids, which have four and even more reactive protons per molecule. In contrast, most useful bases have one or two
available hydroxide ions per formula units.
Titration is the process for ascertaining the exact volume of a solution that reacts stoichiometrically according to a
balanced chemical equation with a given volume of a second solution. One reagent is added by means of a burette
until the endpoint is reached. The endpoint occurs when stoichiometric quantities of reagents have been mixed. The
endpoint of a titration for reactions of acids and bases is usually indicated by a third reagent, the indicator, which has
an abrupt and distinctive color change at the hydrogen ion concentration which is present after the stoichiometric
reaction has occurred. The typical indicator for titrations of strong acids and bases is phenolphthalein.
Phenolphthalein is colorless in acidic solution and red (pink in dilute solutions) in basic solution. Since it is much
easier and distinctive to see a color change from colorless to pink rather than from pink to colorless, sodium
hydroxide is added by means of the burette to the acid, usually contained in an Erlenmeyer flask.
Phenolphthalein = In
HIn
In-
Colorless Fuchsia
+ H2O
H2SO4(aq) + 2 NaOH(aq) ! 2 H2O(l) + Na2SO4(aq)
Strong
acid
Strong
base
Water Salt
Acid/Base Reaction Scheme 1
HA(aq) + H2O(l) H3O+(aq) + A
(aq)
H2A(aq) + H2O(l) H3O+(aq) + HA
(aq)
HA
(aq) + H2O(l) H3O+(aq) + A2
(aq)
H3A(aq) + H2O(l) H3O+(aq) + H2A
(aq)
H2A
(aq) + H2O(l) H3O+(aq) + HA2
(aq)
HA2
(aq) + H2O(l) H3O+(aq) + A3
(aq)
monoprotic acid
diprotic acid
triprotic acid
pf3
pf4
pf5
pf8
pf9
pfa

Partial preview of the text

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Experiment 8. Determination of the Molar Mass of an

Unknown Acid by Acid-Base Titration

In this experiment you will:

  • Prepare and standardize a solution of sodium hydroxide
  • Determine the molecular weight of an unknown acid by reacting the acid with standardized sodium hydroxide solution.

BACKGROUND

An acid reacts with a base to form a salt plus water (see Scheme 1). Many acids have one proton available for reaction with a base such as sodium hydroxide. An acid with one reactive proton per molecule or formula unit is called a monoprotic acid or a monobasic acid. A diprotic acid or a dibasic acid has a maximum of two reactive protons per molecule. A triprotic acid or a tribasic acid has a maximum of three reactive protons per molecule. There are also examples of acids, which have four and even more reactive protons per molecule. In contrast, most useful bases have one or two available hydroxide ions per formula units. Titration is the process for ascertaining the exact volume of a solution that reacts stoichiometrically according to a balanced chemical equation with a given volume of a second solution. One reagent is added by means of a burette until the endpoint is reached. The endpoint occurs when stoichiometric quantities of reagents have been mixed. The endpoint of a titration for reactions of acids and bases is usually indicated by a third reagent, the indicator, which has an abrupt and distinctive color change at the hydrogen ion concentration which is present after the stoichiometric reaction has occurred. The typical indicator for titrations of strong acids and bases is phenolphthalein. Phenolphthalein is colorless in acidic solution and red (pink in dilute solutions) in basic solution. Since it is much easier and distinctive to see a color change from colorless to pink rather than from pink to colorless, sodium hydroxide is added by means of the burette to the acid, usually contained in an Erlenmeyer flask. Phenolphthalein = In HIn In- Colorless Fuchsia

  • H 2 O H 2 SO4(aq) + 2 NaOH(aq)! 2 H 2 O(l) + Na 2 SO4(aq) Strong acid Strong base Water Salt Acid/Base Reaction Scheme 1

H A(aq) + H 2 O(l) H 3 O+(aq) + A(aq)

H 2 A(aq) + H 2 O(l) H 3 O+(aq) + HA(aq)

HA(aq) + H 2 O(l) H 3 O+(aq) + A^2 (aq)

H 3 A(aq) + H 2 O(l) H 3 O+(aq) + H 2 A(aq)

H 2 A(aq) + H 2 O(l) H 3 O+(aq) + HA^2 (aq)

HA^2 (aq) + H 2 O(l) H 3 O+(aq) + A^3 (aq)

monoprotic acid

diprotic acid

triprotic acid

In this experiment, you will standardize (determine precisely the concentration) a solution of sodium hydroxide, NaOH, using oxalic acid dihydrate, H 2 C 2 O 4 " 2 H 2 O, as a primary standard acid. A primary standard acid is a solid with high degree of purity and large molar mass. The solid acid whose mass is an accurate measure of the number of moles of protons the acid will furnish. Oxalic acid, H 2 C 2 O 4 "2H 2 O, is a diprotic acid and provides two reactive protons per molecule according to the following net equation for the neutralization reaction. H 2 C 2 O 4 "2H 2 O(s) + 2 NaOH(aq) $ Na 2 C 2 O4(aq) + 4 H 2 O(l) We must standardize the NaOH solution as sodium hydroxide reacts with carbon dioxide (CO 2 ) from the air to produce NaHCO 3. The concentration of NaOH is then decreased. We must standardize it against a compound that does not easily react with air or decompose, such as oxalic acid. In the second part of the experiment you will titrate an unknown acid with your standardized NaOH solution using phenolphthalein as the indicator. Your goal will be to calculate the molecular mass of your acid. Your instructor will tell you the number of protons your acid furnishes for reaction with base.

PRE-LAB ASSIGNMENT Titration Experiment Name:

  1. Identify and describe the function of each piece of equipment shown below:
  2. Name the primary standard (name and formula) for this experiment and define the function.
  3. Write the net ionic equation for the following reaction. Please note that oxalic acid is a weak acid and is not fully dissociated when dissolved in water. H 2 C 2 O4(aq) + 2 NaOH(aq) $ Na 2 C 2 O4(aq) + 2 H 2 O(l)
  4. Explain why it is a good technique to wash the sides of the Erlenmeyer flask during the titration.
  5. If we assume that the NaOH solution that we will prepare for standardization is approximately 0.12 M , calculate the number of moles and the mass of oxalic acid dihydrate, H 2 C 2 O 4 • 2 H 2 O, required to neutralize approximately 35 mL of the NaOH solution. Write this in your lab book. NaOH ? M Phenolphthalein a! b! c! d! e! " f " g h!

EXPERIMENTAL PROCEDURE Part A. Standardization of NaOH solution

  1. Prepare a solution of sodium hydroxide that is approximately 0.12 M by adding 100 mL of the 0.8 M stock solution to 500 mL of deionized (DI) water in a clean 1-L plastic bottle. Cap the bottle and shake vigorously to thoroughly mix the material. You do not need to be precise, as we will be determining the precise concentration of the NaOH solution in the next steps.
  2. Rinsing the burette with DI water : Thoroughly clean a burette with DI water. Rinse with DI water three times. If many water spots are observed on the inside of the burette, use soap, water and a burette brush to clean the burette, followed by multiple tap water rinses, and three DI water rinses.
  3. Rinsing the burette with titrant solution : Empty the burette, and then rinse with two 5-mL portions of the NaOH solution. Allow some of the solution to run through the stopcock, draining into a waste beaker, and pour the rest out the large top opening to coat the inside of the burette. This process will prevent dilution of your NaOH solution when you add it to the burette for titration.
  4. Filling the burette : Set up a burette clamp on a ring stand, and put the clean burette on the clamp. Using a funnel rinsed in the same manner as the burette, fill the burette with the NaOH solution (titrant) just below the 0.00 mL mark. Remember there is no need to fill the burette exactly since you will read the difference between the ending and starting volumes to determine the amount of volume delivered. Once the burette is full, remove the funnel. If you overfill the burette, drain a small amount into an empty waste beaker. Always pour fresh solution to the burette prior to each titration.
  5. Remove air bubbles : Air bubbles will be trap in the tip of the newly filled burette. These can be difficult to remove and may alter the volume measurement. Hold the burette over an open beaker an open the stopcock fully to allow solution to flow out of the burette. Your instructor will demonstrate the technique. Refill burette if necessary.
  6. Reading the burette : Practice reading the burette using deionized water in it. Remember to always read the volume to the nearest 0.01 mL. See figure to the left.
  7. Mass out three samples of oxalic acid dihydrate (this is the mass you calculated in the prelab questions) on the analytical balance. Record each mass to the full precision allowed by the balance. Dissolve each in 50 mL of DI water in a 125 or 250-mL flask, and add 2- 3 drops of phenolphthalein. 8. Using the sample with the smallest mass of oxalic acid, prepare to carry out your titration. Place a sheet of white paper under the flask to assist in the visualization of the endpoint. Position the burette such that the glass tip is below the opening to the flask. Record the initial volume. See titration setup figure. 9. Titrate the sample. Because we calculated the mass of oxalic acid to require ~ 35 mL of solution, add 25 mL of the NaOH solution quickly. Then add more slowly, always swirling with one hand, while you control the stopcock with the other. Alternatively, you can set up a magnetic stir bar to stir the solution for you. Occasionally use DI water from your squirt bottle to wash any stray drops on the side of the flask into the solution. 10. When a pink color appears in the solution when a drop hits, but then goes away with swirling, you are near the endpoint and should begin adding the solution very slowly – one drop at a time, always swirling to see if any hint of pink color remains. At this point, wash down any drops on the side of the flask with DI water. If you are very close to the endpoint, and need less than a full drop, allow a drop to start to form on the tip, close the stopcock, then touch the flask to the tip. The partial drop will transfer to the flask; wash it down with DI water.
  8. When the hint of pink remains, you have reached the endpoint. Record the final volume of the solution on the burette.
  9. Repeat this procedure for the other two samples of oxalic acid. Refill the burette between samples. Because you know how much solution was required for the first sample, you can add close to that volume very quickly Titration setup Chemistry 11 Santa Monica College ! "#!! Reading the Buret: ./+!0(/!1%)&2/!34!+!5&./0!6.%2!0(/!!!$%&!'(%&)!+),+-'! 5%00%2!%6!0(/!2/43'7&'!13/,/!+0!/-/! )/1/)!8'//!93:&./!;<#!=!5)+7>!%.!,(30/! 7+.!(/)!&?!5/(34!0(/!5&./0!(/)?'!,30(! 2+>34:!0(3'!./+34:#!@&./0'!+./!+77&.+0/! 0%!AB#BC!2D!+4!+))!./+34:'!'(%&)!5/! ./7%./!0%!0,%!/732+)!?)+7/'#!!@/!'&./! 0%!./7%.!5%0(!0(/!'0+.034:!+4!/434:! 1%)&2/'!,(/4!?/.6%.234:!+!030.+03%4#!! E(/!366/./47/!3'!0(/!1%)&2/!/)31/./#! 5 4 4.62 mL; Eye level !^ Figure 1. Reading a Buret ! Good Titration Techniques E(.%&:(%&0!-%&.!'73/403637!7+.//.'!-%&!,3))!?.%5+5)-!5/!/F?/70/!0%!?/.6%.2!030.+03%4'G!30!3'! 32?%.0+40!0(+0!-%&!)/+.4!?.%?/.!0/7(43H&/#!I4!?/.6%.234:!+!030.+03%4!:/4/.+))-!+4!3437+0%.!0(+0! 7(+4:/'!7%)%.!3'!+/!0%!+!'%)&03%4!0%!5/!030.+0/!8+)0(%&:(!2%/.4!34'0.&2/40'!7+4!4%,! ?/.6%.2!030.+03%4'!+&0%2+037+))-!5-!'?/70.%'7%?37+))-!2%430%.34:!0(/!+5'%.5+47/<#!=!030.+40! 6.%2!0(/!5&./0! dropwise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keeping a hand on the stopcock, !+4!',3.)34:!0(/!'%)&03%4!,30(!0(/!%0(/.!(+4#!!I6!-%&!%!0(3'J!5/! '&./!0(+0!0(/!.+0/!+0!,(37(!.%?'!+./!3'?/4'/!3'!')%,!/4%&:(!0(+0!-%&!7+4!'0%?!0(/!6)%,!5/6%./! 0(/!4/F0!.%?!6%.2'P!!K1/.'(%%034:!+4!/4L?%340! ./?/+0!+4!/403./!030.+03%4#!Q/4/.+))-J!0(3'!,3))!7%'0! by even one drop -%&!2%./!032/!0(+4!-%&!,3))!:+34!6.%2!+!')3:(0)-!!3'!%60/4!7+&'/!6%.!(+134:!0%! 6+'0/.!.%?34:!.+0/#! ! R/63))!0(/!5&./0!5/0,//4!030.+03%4'!'%!-%&!,%4S0!:%!5/)%,!0(/!)+'0!2+.>#!!I6!+!030.+03%4!./H&3./'! 2%./!0(+4!0(/!6&))!1%)&2/!%6!0(/!5&./0J!-%&!'(%&)!/30(/.!&'/!+!)+.:/.!5&./0!%.!+!2%./! 7%47/40.+0/!030.+40#!!R/63))34:!0(/!5&./0!34!0(/!23)/!%6!+!0.3+)!340.%&7/'!2%./!/..%.!0(+4!3'! :/4/.+))-!+77/?0+5)/!6%.!+4+)-037+)!,%.>#! ! Set-up and Preparation of Equipment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itamin-C Analysis Page 4 of 7 4.62 mL Reading the burette

Error Analysis Questions for Acid-Base Titration Experiment

1. In standardizing the solution of aqueous sodium hydroxide, a chemist overshoots the end point and

adds too much NaOH(aq). Would this error result in a calculated concentration of NaOH that was

overestimated or underestimated? Explain your reasoning.

2. In the titration of the unknown diprotic acid, assume a chemist uses a standardized solution of

NaOH that has been underestimated in its concentration. How would this error affect the final

calculation for the molar mass of the unknown acid? Would it be overestimated, underestimated or

remain unaffected? Explain your reasoning.

3. In the titration of the unknown diprotic acid with NaOH, assume a chemist overshoots the end point

and adds too much NaOH. How would this error affect the final calculation for the molar mass of

the unknown acid? Would it be overestimated, underestimated or remain unaffected? Explain your

reasoning.

LAB REPORT GUIDELINES The lab report section includes work recorded during the lab, your analysis and discussion of data and results, and your conclusions. The discussion and conclusion sections should be word-processed. Other parts of the report - calculations, etc. may be typed. Heading ! Title of experiment and number ! Your name ! Dates of the experiment Data/Observations/ Results ! ORIGINAL QUANTITATIVE DATA (signed data pages from your lab notebook) Calculations Show calculations for the following quantities in your report (use proper format for labeling and showing calculations in a formal report): Part A: ! Calculate [NaOH] based on each titration ! Calculate the average [NaOH] (of the good trials as described in the procedure) ! Calculate the relative range ! Provide a discussion of your choice to omit any bad trials, including any other relative range calculations you may have performed. Part B: ! Calculate the molar mass of the unknown acid for each trial ! Calculate the average molar mass (of the good trials as described in the procedure) ! Calculate the relative range ! Provide a discussion of your choice to omit any bad trials, including any other relative range calculations you may have performed. ! Determine the identity of your unknown acid. Your acid is one of the following: o Oxalic acid dihydrate (H 2 C 2 O 4 • 2 H 2 O) (diprotic) o Succinic acid (C 4 H 6 O 4 ) (diprotic) o Fumaric acid (C 4 H 4 O 4 ) (diprotic) o Tartaric acid (C 4 H 6 O 6 ) (diprotic) o Citric acid monohydrate (C 6 H 8 O 7 • H 2 O) (triprotic) o Based on the molar masses of these compounds (calculate and provide in a table), identify the most likely identity of your unknown. If you cannot definitively determine its identity, suggest the reasonable possibilities. ! Calculate the percent error for the experimental molar mass with the value for the acid you have determined it to be. (If more than one possibility, show the percent error for each of them). Discussion/Theory/ Results/Error Analysis In this section, you will explain the experiment, evaluate, discuss your results, and analyze errors in paragraph form. ! Briefly explain why we standardized the sodium hydroxide

Acid-Base Titration

POST-LAB QUESTIONS Name:

1. KHP, potassium hydrogen phthalate (KHC 8 H 4 O 4 ), is often used to standardize basic solution used

in titration. If a 0.855-g sample of KHP requires 31.44 mL of a KOH solution to fully neutralize

it, what is the [KOH] in the solution?

The reaction is KHC 8 H 4 O4(aq) + KOH(aq) $ K 2 C 8 H 4 O4(aq) + H 2 O(l)

2. The KOH solution standardized above is used to titrate a 20.00-mL sample of sulfuric acid

(H 2 SO 4 ) solution of unknown concentration. Determine [H 2 SO 4 ] for the unknown acid solution if

41.27 mL of the NaOH solution is needed to fully react with it.

3. A 25.00 mL aliquot of a nitric acid solution of unknown concentration is pipetted into a 125 ml

Erlenmeyer flask and two drops of phenolphthalein are added. The above sodium hydroxide

solution (the titrant) is used to titrate the nitric acid solution (the analyte). If 16.77 mL of the

titrant is dispensed from a burette in causing a color change of the phenolphthalein, what is the

molar concentration of the nitric acid (a monoprotic acid) solution? Express the molar

concentration of nitric acid to the correct number of significant figures.