How does the mass percentage of citric acid available from citrus fruits (lemon, lime, oranges) depends on the storage time and the types of citrus fruits and fresh lime taken?
Citrus fruits are a regular part of my diet and during this Covid-19 a lot of health experts had advised to consume more of the citrus fruits as they used to build our immunity. Therefore, I had made it a habit to prepare these juices and store it in the refrigerator so I could drink it whenever I want. However, I observed that the flavor of the juice is changing over time which made me curious, “Why does the flavour of the juice change over time ?” and “What are the sources for citric acid ?” . I wanted to understand why this change in flavour took place; is this also affecting the nutritional value. I also investigate whether this change in nutritional value is the same for all citrus fruits or varies among fruits. This would help me understand what is the best citrus fruit which is safest to store for longer periods of time and which has least change in flavour, proving the best fruit juice to be consumed. As I had so many questions about this topic I decided to do some research to help me understand this, I came across an article which discusses the key ingredient in citrus fruits, which is citric acid itself and the article explained how there are different amounts of citric acid in the different fruits. I made the connections to the concept learned during Chemistry class like the concept of titration as an analytical procedure for quantitative estimations of acids and bases. I realized I wanted to connect something I learned from class and to understand how to apply it to real life applications and planned to use it in an experiment.
Citric acid
Citric acid is a weak organic acid that has the molecular formula C6H8O7. It occurs naturally in citrus fruits. It belongs to the functional group carboxylic acid group. It is naturally found in citrus fruits like lemon, lime, orange, grapefruits, pomelos and is used widely in industry as an acidifier, as a flavoring and chelating agent. Citric is soluble in Water and dissolves in absolute (anhydrous) ethanol. Citric acid is a weak organic acid present naturally in living cells. Citric acid is an alpha-hydroxy acid with a three carbon skeleton, which has three carboxylic acid groups (COOH), and one hydroxyl group (OH). It is used as a cleaning agent which is used on a daily basis in the kitchen. It is used to add a sour taste to soft drinks and other food items, in shampoos, food coloring. It is a natural preservative. It is used to remove the chalky deposit from evaporators, kettles, boilers.
Word Equation: Citric Acid Sodium Hydroxide → Sodium Citrate Water
Chemical Equation: C6H8O7 (aq) + 3NaOH (aq) → C6H5O7Na3 (aq)+ 3H2O4 (aq)
When you look at the structure of citric acid, you can see that there are three carboxylic acid groups, which mean that there need to three NaOH for each of the atoms to react with each one of them
Titration is a qualitative analysis technique that can be used to calculate the concentration of an unknown solution with the use of a solution with a known concentration. The process is usually carried out by gradually adding a standard solution ( solution of known concentration) of titration titrant with a burette essentially a long, graduated measuring tube with a stopcock and a delivery tube at its lower end until the color change at the end point. The change in color occurs due to use of indicator, usual phenolphthalein3
The citric acid percentage content of each fruit (lemon lime, orange will does not depend on storage time.
The citric acid percentage content of each fruit (lemon lime, orange will does not depend on storage time.
20.00 ± 0.05 cm3 of juice extracts, diluted in distilled water of 100cm3 and then taking 20cm3 n
A constant of 0.01 mol/dm3 was taken on all the trials.
±0.01 cm3
50cm3
±0.5 cm3
±0.5 cm3
100cm3
±0.01 cm3
100cm3
±0.01 cm3
50cm3
±0.01 cm3
-Chemicals were used in a manner that avoids wastage.
-All chemicals were disposed off into a chemical waste bin to avoid interaction with the environment.
-Unused chemicals were returned to the laboratory, safely.
Minimal amount of chemicals were used to conduct trials, keeping in mind the economic concerns and environmental effects.
Preparing 100 cm3 of 0.1 mol.dm-3 NaOH solution
Molar The solution made has to be a volume of 100 cm3 and concentration 0.1 mol dm-3 -3.
Thus, the number of moles can be calculated from the formula:
Number of moles (n) = molar concentration ( C) X volume in dm3 (V ) =\((0.010 X\frac{100}{1000})\)= 0.001
Mass of NaOH to be used
= number of moles X Molar Mass= 0.001 X 39.997
= 0.039997 g
= 0.04 g (rounded of two decimal places)
-For lemon, squeeze it to remove the juice into a beaker. For lime and lemon use a machine to remove the juice and pour into a beaker.
-Filtrate the juice using a funnel with filter pare, empty the filtrate in another beaker.
-First rinse the pipette with some distilled water.
-Take 20.00 ±0.05 cm3 of the juice from the filtrate using a pipette into a 100cm3 flask
-Juice should be diluted by adding distilled water until the mark reaches 100 cm3, start it using a glass rod.
-Pouring the solution in a fresh beaker and use a pipette to take 20.00 ±0.05 cm3 again
-Pour this into a conical flask, then add a few drops of phenolphthalein indicator
-Take initial reading of NaOH from the burette (two decimal places)
-Drop NaOH into the juice slowly, drop by drop until the color changes pink
-Check and the record the reading on the burette
-Calculate amount of NaOH (initial reading - final reading)
-Calculate the moles of citric acid reading to the NaOH, use this information to calculate the mass of citric acid.
-Using this information calculate the percentage of mass
-The data was collected in 3 trials and the same procedure was repeated for lemon juice, orange juice.
-All steps were repeated for 5 days, three trials and the same procedure for all three fruits.
Sample calculation
For Day 1, Trial-1
Initial burette reading = 0.00 ± 0.05 cm3
Final burette reading = 7.20 ± 0.05 cm3
Difference in burette reading = Final – Initial = (7.20 ± 0.05 cm3) – (0.00 ± 0.05 cm3) = 7.20 ± 0.10 cm3
As the data collected is of acid base titration, the reading that is repeated (concordant or precise reading) has been chosen as an average instead of calculating arithmetic average to procure more accurate data.
For example, for Day-1, the three trial values for difference in burette readings are 7.20 ± 0.05 cm3, 7.00 ± 0.05 cm3 and 7.00 ± 0.05 cm3 respectively. So, the reading 7.00 ± 0.05 cm3 repeats itself twice and is thus the precise or concordant reading. Thus, the average reading is taken as 7.00 ± 0.05 cm3
For Day-1, Standard deviation (SD)=\(\frac{(7.20-7.00 )^2+(7.00-7.00)^2 +(7.00-7.00)^2}{3}\)=0.12
Sample calculation
Citric acid reacts with NaOH according to the equation
HOCH2CH2OH(COOH)CH2COOH + 3 NaOH → NaOCCH2CH2OH(COONa)CH2COONa + 3H2O
Moles of citric acid ( n citric acid ) =\(\frac{moles\ of \ NaOH}{3}\)\((as\ they \ citric \ acid \ and\ NaOH\ reacts\ in\ the \ ratio\ 1:3)\)
=\(\frac{molar\ concentration \ of \ NaOH\ used× \frac{Average\ volume \ of \ NaOH \ taken \ in\ cm^3}{1000} }{3}\)=\(\frac{0.0×\frac{7.00}{1000}}{3}\)=2.33 × 10-4
Molar concentration of citric acid
\(=\frac{number\ of\ moles\ of \ citric\ acid }{\frac{Volume\ of \ juice\ used\ in \ cm^3}{1000}}\)=\(=\frac{2.33× 10^{-4} }{\frac{20}{1000}}\)\(=\frac{2.33× 10^{-4} }{{20 × 10^{-3}}}\)=0.1165 × 10-1
=11.65 × 10-3 mol dm-3
Moles of citric acid present within 1 dm3 or 1 L of juice = 11.65 × 10-3 mol
Mass of citric acid present within 1 dm3 of juice
= moles × molar mass=11.65 × 10-3 ×192.12
=2238.19 × 10-3=2.238 g ≅2.24 g
Concentration of citric acid = 2.24 g L-1
For Day-1 of lime juice
Average volume of NaOH = Precise reading among the three trial values of difference in burette reading = 7.00 ± 0.10 cm3
Concentration of NaOH solution used (c)=\(\frac{moles }{Volume}\)=\(\frac{mass (m) }{\frac{molar \ mass}{Volume(V)}}\)
\(\frac{∆ \ c}{c}=\frac{∆ \ m }{ m}+\frac{∆\ V }{V}\frac{± 0.01 }{0.40}+\frac{±0.60 }{100.00}±0.03\)
Moles of NaOH (n) = concentration (c) × Volume of NaOH consumed (V)
Fractional error in moles of NaOH\(\bigg(\frac{∆ n }{n}\bigg)=\frac{∆ c }{ c }+\frac{∆ V }{ V }=±0.03+\frac{± 0.10}{7.00}=±0.04\)
Moles of citric acid =\(\frac{moles\ of \ NaOH }{3}\)
Therefore, fractional error in moles of citric acid = fractional error in moles of NaOH
Mass of citric acid = moles of citric acid molar mass
Concentration of citric acid in g L-1\(=\frac{mass\ of \ citric \ acid }{Volume \ of \ juice}\)
Volume of juice used (Vjuice)= 20.00 ± 0.05 cm3
Fractional error in concentration of citric acid
= fractional error in mass of citric acid + fractional error in volume of juice
\(=\frac{∆n }{n}+\frac{∆V }{V}=(± 0.04)+\frac{± 0.05}{20.00}b\)
Percentage error in citric acid concentration = fractional error\( 100 \) × 100 = ± 0.04 × 100 = 4.00
Graph-1 is a scattered plot of mass percentage of citric acid in g/L against the number of days for which the juice was stored.
Sample calculation
Mean % of citric acid content =\(\frac{Sum \ of\ mass\% of \ all\ five\ days}{5}\)= \(\frac{2.24+1.99+1.76+1.34+1.22 }{5}\)=1.71 gL-1
The y axes values represent the dependent variable percentage content of citric acid present in each type of fruit The x axis values represent the independent variable, which is the type of fruit. As the x axes values (independent variable values) are categorized and not numbers/ figures, it is not possible to make a scatter plot or line graph. Therefore, bar graph being most suited to present this type of data and effectively exhibiting the data collected.
The graph clearly displays that the mean content of citric acid in g/L is maximum for lemon juice (14.86 g/L) followed by orange juice (7.83 g/L) and least for lime juice (1.71 g/L). This claim is in accordance with the results from Graph-1.
Citric acid is an organic tri-carboxylic acid. It can undergo decarboxylation according to the reaction below
HOOC-CH2-C(COOH)(OH)-CH2(COOH) ------🡪 H3C-CH(OH)-CH3 + 3CO2 (g)
As gas is liberated during the reaction, the disorderness of the system increases and thus the change of entropy is positive indicating an increase in entropy of the system. Thus, the reaction is entropically favored and spontaneous in nature. With the increase in storage time, more and more citric acid molecules undergo decarboxylation and thus the mean mass percentage of citric acid decreases. The qualitative observation that more bubbles were formed and the appearance of the juices turned hazy with the passage of time confirms the liberation of CO2 with the passage of time.
How does the mass percentage of citric acid available from citrus fruits (lemon, lime, oranges) depends on the storage time and the types of citrus fruits and fresh lime taken?
The mass percentage of citric acid in g/L (mass of citric acid present within1 L of the juice) is decreasing from 15.47 g/L to 14.15 g/L for lemon juice, 8.74 g/L to 6.79 g/L for orange juice and 2.24 g/L to 1.22 g/L for lime juice. Thus, for all the three kinds of juices, it has been observed that the mass percentage of citric acid decreases with time. Thus, a negative correlation can be claimed between the mass percentage of citric acid and the storage time (measured in terms of number of days).
The citric acid content within the juice must diminish to 0.00 within 49 days for lemon juice, within 20 days for orange juice and within 9 days for lime juice. Thus, it can be claimed that the citric acid content lasts the longest for lemon juice followed by orange juice and the least for lime juice.
The decrease of mass percentage with time is fastest for orange juice as it has the maximum value of gradient and minimum for lime juice as it has the minimum value of gradient.
The mean content of citric acid in g/L is maximum for lemon juice (14.86 g/L) followed by orange juice (7.83 g/L) and least for lime juice (1.71 g/L). This claim is in accordance with the results from Graph-1.
With the increase in storage time, more and more citric acid molecules undergo decarboxylation and thus the mean mass percentage of citric acid decreases. The qualitative observation that more bubbles were formed and the appearance of the juices turned hazy with the passage of time confirms the liberation of CO2 with the passage of time.
Graph-1 shows the values of regression coefficient obtained from Excel for the equation of linear trend line depicting the correlation between the mass % of citric acid in g/L and the number of days. The values are 0.9851 for lemon juice, 0.9723 for lemon juice and 0.9794 for lime juice. This shows that there is a strong correlation between the mass percentage of citric acid in g/L and the storage time (measured in terms of number of days). Moreover, Graph-2 clearly indicates the differences in the values of mean values for the mass percentage of citric acid in juices. Thus, the null hypothesis is rejected and the alternate hypothesis has been accepted.
Citric acid also contains a alcohol group – (OH). This group can also react with NaOH along with the three carboxylic acids. This changes the mole ratio of the citric acid and NaOH to 1:4 from 1:3. Thus, the calculations and data processing in this investigation would become invalid. Alcohol (OH) group is acidic in nature and thus this possibility cannot be averted.
(HOOC)CH2-C(COOH)(OH)-CH2-(COOH) + 4 NaOH -----🡪 (NaOOC)CH2-C(COONa)(ONa)-CH2-(COONa) + 4 H2O
To optimize this, the concentration of citric acid can be monitored by measuring the absorbance of the solution using a UV-Visible spectroscopy at a wavelength at which the molecule shows maximum absorbance.
Apart from storage time, storage temperature is also an important parameter to decide the shelf-life of any processed food. Thus, investigating the effect of temperature on the mean citric acid content of the juices will be a significant research. To do so, we can take the same three kind of juices and heat them to different temperatures using a Bunsen burner or electric heater. After that, the mean citric acid content can be determined using the acid base titration with NaOH.
-Penniston, Kristina L., et al. “Quantitative Assessment of Citric Acid in Lemon Juice, Lime Juice, and Commercially-Available Fruit Juice Products.” Journal of Endourology, vol. 22, no. 3, Mar. 2008, pp. 567–570, www.ncbi.nlm.nih.gov/pmc/articles/PMC2637791/, 10.1089/end.2007.0304.
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