IB
KYAW WAI IB1I
KYAW WAI IB1I
CHEMISTRY IA (2)
TITRATION OF ACID & ALKALI
Name: KYAW WAI
Date: 5th February 2013
IA CRITERIA ASSESSED: DCP, MS
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Aim of the experiment:
The aim is to determine the water of crystallization of a diprotic acid by titration against a base.
Background:
Many substances that we use are either acidic or basic. Because acids and bases can neutralize each other, that gives us a strategy for finding the unknown concentration of an acid or base when we react
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Tabulate the results in a neat tabular column.
Data Collection:
(a) Qualitative Data:
Materials | Color/Observations | 1) Sodium Hydroxide | Colorless liquid | 2) Sodium Hydroxide after two drops of phenolphthalein | Pink to colorless liquid | 3) After titration with {(COOH)2.xH2O} | Change from black to colorless liquid |
Table 1:Observation
(b) Quantitative Data: Trials | Amount of NaOH in conical flask/cm3 | Amount of Oxalic Acid used in titration/cm3 | - | (±0.06 ml) | (±0.1) | 1st | 25.0 | 20.60 | 2nd | 25.0 | 21.30 | 3rd | 25.0 | 21.05 | 4th | 25.0 | 20.60 |
Table 2:Collection of raw data
Average amount of {(COOH)2.xH2O} used:
=20.8875
≈20.9 (2 d.p)
Neutralization Equation:
(COOH)2 (aq) + 2NaOH(aq) (COONa)2(aq) + 2H2O (l)
Use N1 = M1V1 when M is in mol/dm3 N2 M2V2 1) n(NaOH)=0.025x0.1=0.0025mol 2) n(COOH)2 =0.00125mol 3) N1=M1V1
N2 M2V2
4) 1 = M1x0.0125
2 0.10.025 M1=0.58mol/dm3 5) Mol(COOH)=0.058x0.25= 0.0145mol 6) Mass(COOH)=0.0145x2(12+16+16+1)=0.841g 7) Mass(H2O)=1.5-0.841=0.659 8) Mol(H2O)=0.659 (1.01+1.01+16)
= 0.0366mol 9) Total Number of X= 0.0366 0.0145 =2(approx..)
Discrepancies: 1)We definitely had errors in many areas, such as we cannot really tell at which volume did the color change occurred.
2) The phenolphthalein indicator might be overly
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Chemistry 102 is the study of kinetics – equilibrium constant. When it comes to the study of acid-base, equilibrium constant plays an important role that tells how much of the H+ ion will be released into the solution. In this lab, the method of titrimetry was performed to determine the equivalent mass and dissociation constant of an unknown weak monoprotic acid. For a monoprotic acid, it is known that pH = pKa + log (Base/Acid). When a solution has the same amount of conjugate base and bronsted lowry acid, log (Base/Acid) = 0 and pH = pKa. By recording the pH value throughout the titration process and determining the pH at half- equivalence point, the value of Ka can be easily calculated. In this experiment, the standardized NaOH solution has a concentration of 0.09834 M. The satisfactory sample size of known B was 0.2117 g. The average equivalent mass of the unknown sample was found to be 85.01 g, pKa was found to be 4.69, which was also its pH at half-equivalence point and Ka was found to be 2.0439×〖10〗^(-5). The error was 1.255% for equivalent mass and 0.11% for Ka. In other word, the experiment was very precise and accurate; the identity of the unknown sample was determined to be trans-crotonic by the method of titrimetry.
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I hereby declare that this submission is my own work and that, to the best of my knowledge and belief, it contains no material previously published or written by another person nor material which to a substantial extent has been accepted for the award of any other degree or diploma of a university or other institution of higher learning, except where due acknowledgment is made in the acknowledgments.
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