Conclusion about ph value
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The purpose of this lab was to determine the pH of several different salt solutions through the
use of acid-base indicators and then determining the value of the equilibrium constant for each.
The tables attached contain all the observations and calculations made during this lab. Table 2
shows the colors and pH transitions of indicators that were determined by me and my lab group.
Table 3, shows the colors of salt solution with different indicators which was done individually
and shows the pH level and concentrations of the salt solutions. Then next, table 4 shows which
of the salt solutions went through a hydrolysis reaction and which ions were spectators if there
were any. Then, based on my determination in table 4, table 5 shows the salt solutions that went
through the hydrolysis reaction and the dissociation constant expression for each as well as the
values of the k’s.
Bronsted-Lowry acids are species that donate the H
+
ion, while Bronsted-Lowry bases are
species that accept the H
+
ion. Some salts have acidic or basic properties when added to water
because they ionize with water to go through a process called hydrolysis. The magnitude of K
a
or
K
b
tells you that the primary species that is present in the aqueous salt solution at equilibrium is
mostly acidic, basic or neutral.
The primary source of error in this experiment is due to the adding of the indicators to the wells
and the possibility of some contamination and mixture of different salt solutions which would
alter the pH levels of each of the salt solutions when the indicator is added. How to minimize this
error could be thoroughly rinsing the well after each use and conducting multiple trials of
determining what the color of the salt solution is after adding the indicator. It is important to use
only a few drops of indicator when testing solutions is because at a certain point when the color
changes is half of the indicator is in acid form and the other half is in basic form and if you go
beyond that point the pH of the salt solution could be determined not accurately.
Because we are trying to abide by the 12 principles of green chemistry it was very important to
be precise and accurate when performing this experiment because the large amount of waste
produced and that is why multiple trials for the testing of each salt solution would not be
conducted.
Thus this experiment shows the importance of being precise and accurate as well as
calculating correctly to try and accomplish a true or accepted value of the pH and concentrations
of the salt solutions.
use of acid-base indicators and then determining the value of the equilibrium constant for each.
The tables attached contain all the observations and calculations made during this lab. Table 2
shows the colors and pH transitions of indicators that were determined by me and my lab group.
Table 3, shows the colors of salt solution with different indicators which was done individually
and shows the pH level and concentrations of the salt solutions. Then next, table 4 shows which
of the salt solutions went through a hydrolysis reaction and which ions were spectators if there
were any. Then, based on my determination in table 4, table 5 shows the salt solutions that went
through the hydrolysis reaction and the dissociation constant expression for each as well as the
values of the k’s.
Bronsted-Lowry acids are species that donate the H
+
ion, while Bronsted-Lowry bases are
species that accept the H
+
ion. Some salts have acidic or basic properties when added to water
because they ionize with water to go through a process called hydrolysis. The magnitude of K
a
or
K
b
tells you that the primary species that is present in the aqueous salt solution at equilibrium is
mostly acidic, basic or neutral.
The primary source of error in this experiment is due to the adding of the indicators to the wells
and the possibility of some contamination and mixture of different salt solutions which would
alter the pH levels of each of the salt solutions when the indicator is added. How to minimize this
error could be thoroughly rinsing the well after each use and conducting multiple trials of
determining what the color of the salt solution is after adding the indicator. It is important to use
only a few drops of indicator when testing solutions is because at a certain point when the color
changes is half of the indicator is in acid form and the other half is in basic form and if you go
beyond that point the pH of the salt solution could be determined not accurately.
Because we are trying to abide by the 12 principles of green chemistry it was very important to
be precise and accurate when performing this experiment because the large amount of waste
produced and that is why multiple trials for the testing of each salt solution would not be
conducted.
Thus this experiment shows the importance of being precise and accurate as well as
calculating correctly to try and accomplish a true or accepted value of the pH and concentrations
of the salt solutions.
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