Acid-Base Titrations & Standard Solutions | A-level Chemistry | OCR, AQA, Edexcel
Summary
TLDRThis video series educates viewers on titrations, a volumetric analysis technique to determine chemical unknowns like concentration and molar mass. It covers the titration process, using standard solutions, and calculations involved. The script guides through preparing standard solutions, conducting titrations, and analyzing results. It also includes practical examples, such as making a sodium hydroxide solution and calculating unknown concentrations or molar masses, enhancing understanding of titration applications.
Takeaways
- 🔬 **Titrations Defined**: Titrations are a form of volumetric analysis used to determine unknown chemical properties by reacting a known volume and concentration of one solution with a measured volume of another.
- 📊 **Standard Solutions**: Standard solutions, with known concentrations, are crucial in titrations for calculating unknowns such as concentration, molar mass, and chemical formulas.
- 🧪 **Titration Process**: The process involves adding a measured volume of substance X to a flask, adding an indicator, and then adding substance Y from a burette until the endpoint is reached, allowing for the calculation of unknowns.
- 💧 **Indicator Role**: Indicators, chosen based on the chemicals involved, are added to the flask to signal the endpoint of a titration.
- 🔋 **Burette Usage**: A burette is used to add the solution Y into the flask containing X, with careful control over the addition until the endpoint is reached.
- 🔎 **Calculating Unknowns**: By analyzing titration results, one can calculate various unknown chemical properties, guided by the principles of stoichiometry.
- ⚖️ **Making Standard Solutions**: The creation of a standard solution involves dissolving a weighed amount of solute in a solvent, transferring to a volumetric flask, and making up to the mark with solvent.
- 📐 **Concentration Concept**: Concentration measures how much solute is dissolved in a given volume of solvent, which is fundamental to understanding titration calculations.
- 🔄 **Solution Mixing**: After preparing a standard solution, it is thoroughly mixed by inverting the flask to ensure homogeneity.
- 📚 **Titration Calculations**: Calculations in titration involve determining the concentration of unknown solutions, molar masses, and other properties using the reaction stoichiometry and volumes measured.
- 📉 **Error Identification**: The script highlights common errors in preparing standard solutions and suggests improvements, such as using a weighing boat and a volumetric flask for accuracy.
Q & A
What is a titration?
-A titration is a form of volumetric analysis where a known volume and concentration of one solution reacts with a measured volume of another solution to determine chemical unknowns such as concentration, molar mass, formula, and water crystallization.
What is a standard solution?
-A standard solution is a solution with a known concentration used in titrations to calculate chemical unknowns.
How do you make a standard solution?
-To make a standard solution, you first weigh the required mass of the solute, dissolve it in a solvent in a beaker, then transfer the solution into a volumetric flask. Rinse the beaker and add the washings to the flask. Add solvent to the flask without exceeding the graduation line, then adjust the volume by adding solvent drop by drop until the meniscus is at the graduation line. Finally, mix the solution thoroughly by inverting the flask.
What is the purpose of an indicator in titration?
-An indicator in titration is used to signal the endpoint of the reaction, indicating when the titration is complete.
How do you calculate the number of moles required for a standard solution?
-The number of moles required is calculated by multiplying the desired concentration by the volume in decimeters cubed.
What is the molar mass of sodium hydroxide?
-The molar mass of sodium hydroxide (NaOH) is approximately 40 grams per mole, calculated by adding the atomic masses of sodium (23), oxygen (16), and hydrogen (1).
How do you calculate the mass of a solute needed for a standard solution?
-The mass of the solute needed is calculated by multiplying the number of moles by the molar mass of the substance.
What is the reaction between hydrochloric acid and sodium hydroxide?
-The reaction between hydrochloric acid (HCl) and sodium hydroxide (NaOH) produces sodium chloride (NaCl) and water (H2O).
How do you find the concentration of an acid using titration?
-To find the concentration of an acid using titration, you calculate the moles of the base that reacted, use the reaction stoichiometry to find the moles of acid, and then divide the moles of acid by the volume of acid used to get the concentration.
What is the significance of the meniscus in making a standard solution?
-The meniscus is significant in making a standard solution because it indicates the correct volume of solution in the volumetric flask. The bottom of the meniscus should align with the graduation line to ensure the accurate volume.
Why is it important to mix the solution thoroughly after making a standard solution?
-It is important to mix the solution thoroughly after making a standard solution to ensure homogeneity and that the concentration of the solute is uniform throughout the solution.
Outlines
🧪 Introduction to Titrations and Standard Solutions
The paragraph introduces a series of videos focusing on titrations, a form of volumetric analysis used to determine chemical unknowns such as concentration, molar mass, formula, and water crystallization. It explains the titration process, which involves reacting a known volume and concentration of one solution with a measured volume of another. The paragraph also discusses standard solutions, which have a known concentration and are crucial for titrations. The process of making a standard solution is outlined, including weighing the solute, dissolving it in a solvent, transferring it to a volumetric flask, adding solvent up to a graduation line, and mixing thoroughly. The calculations involved in preparing a standard solution are also covered, such as determining the number of moles required and calculating the mass of the solute needed.
🔍 Calculating Concentration and Molar Mass in Titrations
This paragraph delves into titration calculations, explaining how to find unknowns like concentration and molar mass. It provides a step-by-step guide to calculating the concentration of hydrochloric acid when titrating sodium hydroxide, emphasizing the importance of understanding the reaction equation and the stoichiometry involved. The paragraph also demonstrates how to calculate the molar mass of an acid using titration data, showing the process of determining moles of acid in a solution and then using that to find the molar mass based on the mass of the acid used.
📚 Improving Standard Solution Preparation
The focus of this paragraph is on improving the method of preparing standard solutions. It points out errors in a student's approach, such as measuring sodium hydroxide directly on a balance, and suggests using a weighing boat to ensure no residue is left behind. It also recommends using a volumetric flask for accurate solvent volume measurement and inverting the flask to mix the solution, rather than stirring with a glass rod, to prevent residue on the rod.
📈 Determining Chemical Quantities in Titration
The paragraph discusses how to calculate the amount of sodium hydroxide and sulfuric acid used in a titration reaction. It explains the stoichiometry of the reaction and how to use the concentration and volume of the solutions to calculate moles. The summary also covers calculating the concentration of sulfuric acid used in the titration, emphasizing the importance of understanding the reaction's stoichiometry and applying it to find the unknown concentration.
🧐 Writing Reaction Equations and Calculating Concentrations
This paragraph instructs on writing balanced chemical equations for titration reactions, using the example of barium hydroxide reacting with nitric acid. It covers how to balance the equation and calculate the initial concentration of the acid based on the volume and moles of barium hydroxide used. The paragraph also highlights the importance of using appropriate apparatus like a burette and pipette for accurate volume measurements and the necessity of adding an indicator to determine the endpoint of a titration.
🎓 Engaging with A-Level Chemistry Tutorials
The final paragraph serves as a call to action for viewers to join the tutorial series for A-Level chemistry. It emphasizes the engaging and bite-sized nature of the video tutorials, aiming to make understanding A-Level chemistry more accessible and enjoyable.
Mindmap
Keywords
💡Titration
💡Standard Solution
💡Concentration
💡Molar Mass
💡Volumetric Flask
💡Moles
💡Indicator
💡Burette
💡End Point
💡Conical Flask
💡Molarity
Highlights
Introduction to the concept of titrations and their role in volumetric analysis.
Explanation of how titrations can be used to determine chemical unknowns such as concentration, molar mass, formula, and water crystallization.
Definition and importance of standard solutions in titration processes.
Description of the titration process involving a pipette, conical flask, and buret.
The role of indicators in titration and their dependence on the chemicals used.
Step-by-step guide on how to make a standard solution.
Explanation of concentration in terms of solute and solvent.
Instructions on weighing out the solute for making a standard solution.
Details on transferring the solution to a volumetric flask and the importance of not wasting any solution.
The correct method for filling a volumetric flask to the graduation line.
The necessity of thoroughly mixing the solution in a volumetric flask.
Initial calculations required before making a standard solution, including the number of moles and molar mass.
Worked example of calculating the mass of sodium hydroxide needed for a standard solution.
Titrations analysis and the calculations involved to find unknowns such as concentration and molar mass.
Calculation of an unknown concentration using the titration data of sodium hydroxide and hydrochloric acid.
Determining the molar mass of an acid using titration with sodium hydroxide.
Common errors in making a standard solution and suggestions for improvement.
Correct method for making a standard solution of magnesium hydroxide.
Titration between sulfuric acid and sodium hydroxide with calculations for moles of reactants.
Writing a balanced chemical equation for a titration reaction between barium hydroxide and nitric acid.
Calculating the initial concentration of an acid using titration with barium hydroxide.
Identification of apparatus used for accurately measuring volumes in titration, such as a burette and pipette.
Explanation of the necessity of adding an indicator for successful titration.
Transcripts
hi guys in the next series of videos
we're going to take a look at what are
titrations looking at the titration
process an introduction to standard
solutions looking at how we make
standard solutions titration
calculations an exam style question and
finally a summary
so let's have a look at what titrations
are
well titrations are a form of volumetric
analysis
where a known volume and concentration
of a solution is reacted with a measured
volume of a solution the results the
titration can be analyzed and can be
used to find chemical unknowns
these unknowns can include concentration
molar mass
formula
and water crystallization
so before we have a look at the
titration process let's have a look at
what we use
we use something called a standard
solution this is a solution with a known
concentration and is used in our
titrations
we'll take a closer look at the method
used in making a standard solution in a
later part to this video
let's first of all take a brief look at
the titration process
the first step is to use a pipette to
add a measured volume of your first
substance x to a conical flask
we then add a suitable indicator to the
flask
this indicator depends on the chemicals
you're using
we then fill the buret
with the other solution y
we then open the valve on our buret to
allow a small quantity of white to flow
into our flask of x
you can see here that we're turning that
valve to allow y to flow out and into
our conical flask of x
we repeat this process until the end
point is reached
and we can then measure the volume of y
that has been added
we can then calculate the unknowns by
analyzing the results of our titration
so what are standard solutions well
standard solutions as we mentioned in
the previous part of this video are
solutions of a known concentration
they're used in titrations which allow
us to calculate chemical unknowns
so first of all let's quickly recap the
concept of concentration and battle
solvents and solutes
the solute is dissolved within our
solvent and the concentration is a
measure of how much solute is dissolved
in a given volume of the solvent
so now we've recapped the idea of
concentration let's take a look at the
steps involved in making a standard
solution
the first step is to carefully weigh out
the required mass of our solute
the second step is to dissolve the
solute in our chosen solvent in a beaker
the third step is to transfer the
solution that we've made into a
volumetric flask
we then rinse the beaker with our
initial solvent that's the solvent that
we've chosen
and we add the washings into the
volumetric flask making sure nothing is
washed away or poured down a sink and
wasted
in the fourth step we add some of our
solvent to the volumetric flask making
sure not to fill up to the graduation
line that's a line that you'll see on
the neck of a volumetric flask
the fifth step is to add the solvent
drop by drop until the bottom of the
meniscus is sitting on that graduation
line ensuring we have just the right
volume of solution
it's important to not allow the solution
to fill above the line if you do you'll
have to start the process all over again
the final step is step six to mix the
solution thoroughly and this is done by
inverting your flask multiple times
making sure you put the stopper in
tightly first of all
so we've had a look at the method of
making a standard solution let's have a
look at the calculations we do before we
start making our standard solution
the first step is to work out the number
of moles required that's the number of
moles of our solute required
we then calculate the molar mass of the
required substance and we can calculate
the mass of the substance that is
required that's the mass we're going to
weigh out
so let's have a look at a worked example
so you can really understand these
initial calculations
we want to make a 250 centimeter cubed
solution of sodium hydroxide with a
concentration of 0.1 mole per decimeter
cubed
so the first step is to work out the
number of moles required
so
using our equation pyramid the number of
moles is equal to the concentration
multiplied by the volume we want to know
the number of moles so that's the
concentration multiplied by the volume
is the arrangement we're going to use
the information we're given was that the
concentration required as 0.1 moles per
decimeter cubed and the volume was
250 centimeters cubed that's equal to
0.25 decimeters cubed
so that'll be the number of moles is
equal to 0.1 multiplied by 0.25
giving us
0.025 moles required
now to calculate the molar mass
we're producing a solution of sodium
hydroxide so the molar mass of sodium
hydroxide is what we're going to have to
calculate
if we look at our periodic table we can
see sodium has a molar mass of 22.99
which we can round to 23.
hydrogen 1 and oxygen 15.99 which are
round to 16.
so that will be 23 plus 16 plus 1 a
molar mass of 40.
in our final step we're calculating the
mass required we know the number of
moles is equal to
0.025 moles and we know the molar mass
is equal to 40.
so we can look at our equation that the
number of moles is equal to the mass
divided by the molar mass the equation
rearrangement we're going to use is that
the mass is equal to the number of moles
multiplied by the molar mass so that's
0.025 multiplied by 40
giving us a mass of one gram that's
required
so let's have a look at titration
analysis and the calculations that we
can carry out
in general these calculations can follow
certain steps and i'll show you how our
calculations can be broken down in these
easy to follow steps
calculations can be used to find
unknowns
these unknowns could be
the concentration of the solution the
molar mass and many other things
exam questions will usually guide you
through it'll give you small steps to
follow so don't be worried if a big
titration calculation comes up
let's have a look at some of the
calculations that we can do
the first calculation we're going to
look at is the calculation of an unknown
concentration
25 centimeters cubed of a 0.1 mole per
decimeter cubed solution of a base
sodium hydroxide is titrated with 22.5
centimeters cubed of an acid
hydrochloric acid
what is the concentration of the acid
involved in this titration
so we're looking to find out the
concentration of the acid that's our
unknown so let's answer this question
looking at the steps involved
the first step is the reaction equation
we know that our acid hydrochloric acid
is reacting with our base sodium
hydroxide and we know that acids and
bases react together to form a salt in
this case sodium chloride and water now
we can check to see our equation is
balanced and it indeed is
the second step is to calculate the
amount in moles of base that has reacted
so what do we know we know the volume of
base was 25.0 centimeters cubed that's
equal to
0.025 decimeters cubed
we know the concentration of our base
was 0.1 moles
per decimeter cubed
now using our equation pyramid the
number of moles is equal to the
concentration multiplied by the volume
the number of moles is equal to
0.1 multiplied by naught 0.025
to give us 0.0025
moles of base
now to calculate the amount in mole of
acid that was used
looking at the reaction equation up here
we can see that one mole of hydrochloric
acid reacts with one mole of sodium
hydroxide it's a one to one ratio
so one to one means that
0.00025 moles of our base will react
with
0.0025 moles of our acid
meaning that the number of moles was
0.0025
moles
so now to calculate the concentration
again write down what we know we know
the number of moles is equal to 0.025
we know the volume of our acid used was
22.5 centimeters cubed that was given to
us in the question that is equal to
0.0225
decimeters cubed
now if we look at our equation pyramid
the number of moles is equal to the
concentration times by the volume
the rearrangement of this equation we're
going to use is that the concentration
is equal to the number of moles divided
by the volume so that is 0.0025
divided by
0.0225
to give us a concentration of 0.111
moles per decimeter cubed
so now we've had a look at finding an
unknown concentration let's have a look
at a slightly different calculation
calculation to find an unknown molar
mass
1.5 grams of an acid was dissolved in
water in order to make a solution with a
volume of 250 centimeters cubed
25 centimeters cubed of the solution of
this acid hx was titrated with 22.5
centimeters cubed of a base sodium
hydroxide which had the concentration of
0.1 moles per decimeter cubed
what is the molar mass of the acid
involved in this titration
so the first step again is to write out
our reaction equation we have our acid h
x now don't worry that this acid hx
containing x is a general element
isn't specific it's just used to
represent an acid here
it's reacting with a base sodium
hydroxide we know acid plus base equals
salt plus water the salt is going to be
n a
x and we're going to form a water
checking to see our reaction is balanced
which is indeed is
we can then move on to step two which is
quite similar to the step two of our
previous calculation
calculate the amount in moles of base
that has reacted
so let's write down what we know
we know the concentration is equal to
0.1 moles per decimeter cubed as we're
given that in the question
and we know the volume of our base that
was used was
22.5 centimeters cubed that is equal to
naught point naught two to five
decimeters
cubed so we can write out our reaction
pyramid that the number of moles equals
the concentration multiplied by the
volume to see that the rearrangement we
need to use is the number of moles is
equal to the concentration multiplied by
the volume
the concentration is naught point one
moles per decimeter cubed and the volume
is 0.025
giving us no point not not two to five
moles of base that has been used
so now for the third step to calculate
the amount and mole of acid that was
used to make the initial solution
so if we have a look at our reaction
equation we can see that one mole of hx
reacts with one mole of sodium hydroxide
so that's a one-to-one ratio
that means that
0.025 moles of our sodium hydroxide will
react with
0.00225 moles of our acid
hx now importantly this is telling us
that there is
0.0025 moles of hx in the 25 centimeter
cubed sample we want to know how much
there was in the initial 250 centimeter
cubed solution now we know that 250
divided by 25 is equal to 10. so looking
at the volume that's 10 times as much
meaning there's going to be 10 times as
many moles so that's
0.00025 times 10
giving us
0.025
moles of acid in the 250 centimeter
cubes initial solution
now the final step to calculate the
molar mass of the acid that we used
well we know the number of moles is
0.025 we've just calculated that and we
know the mass of our acid was 1.5 grams
we were given that in the question so
using our reaction pyramid that the
number of moles is equal to the mass
over the molar mass we can work out that
the molar mass will be the mass divided
by the number of moles that's 1.5
divided by 0.02
to give us a molar mass of 66.667
grams per mole
a student decides to make up a standard
solution of sodium hydroxide she
carefully measures out 10 grams directly
onto a balance she adds this to a
conical flask with a hundred mils of
water and stirs using a glass rod
part a the student made a number of
errors in her method how could she
improve her method
so for three marks we should probably
give about three errors if we can find
them
so let's take a look at her method
it says here that
student measures out 10 grams of sodium
hydroxide directly onto a balance
it's probably better for the student to
use a weighing boat to ensure that no
residue is left behind as a weighing
boat can easily be washed out to ensure
that all of our chemical reactant is
being used
so the first improvement is she could
use a weighing boat
in the method we're then told that she
adds this to a conical flask
the student could instead use a
volumetric flask to ensure that an
accurate solvent volume is measured
and for our third and final suggestion
of improvement the method says the
student stirred using a glass rod
alternatively the student could invert
her flask in this case her volumetric
floss which we said she should use
to ensure that no residue is left on the
glass rod
so for each of those corrections we
receive one mark she could use a
weighing brake she can use a volumetric
flask and she can invert the flask
rather than staring with her glass rod
moving on to part b
having learnt the correct way of making
up a standard solution the student
decides to make up a standard solution
of mgoh2 magnesium hydroxide the student
wants to obtain one liter of 0.1 moles
per decimeter cubed solution
what mass of magnesium hydroxide should
she use
let's first of all draw out the pyramid
that we're going to need we know that
the number of moles is equal to the
concentration multiplied by the volume
so we can go ahead and calculate the
number of moles of magnesium hydroxide
in the solution
so we know the concentration is 0.1
moles per decimeter cubed and we know
the volume is one liter that's one
decimeter
so that gives us naught point one moles
so now we can go ahead and use our
second pyramid
number of moles is equal to the mass
divided by the molar mass
we know the number of moles is equal to
0.1
we want to know the mass and we can
calculate the molar mass if we take a
look at our periodic table we can see
that we can find all the components we
need we want to find out the molar mass
of magnesium hydroxide
mgoh2 we can see that we have hydrogen
over here with a mass of 1
oxygen over here with a mass of 16 and
magnesium over here the mass of 24.3
so the molar mass will be
24.3
plus
sixteen times two as we have two oxygens
plus one times two for our two hydrogen
atoms to give us a total
of fifty eight point three that is our
molar mass of magnesium hydroxide
so putting that into our equation
we can see
that the mass is equal to the number of
moles 0.1 multiplied by 58 58.3 our
molar mass to give us 5.83
grams that we require
so the answer is 5.83 grams of magnesium
hydroxide
so this question holds two marks the
first comes from correctly calculating
the number of moles of magnesium
hydroxide
in our solution and the second from a
correct final answer of the mass of
magnesium hydroxide we
need so let's go ahead and have a look
at question two a titration between
sulfuric acid and sodium hydroxide is
carried out the equation for the
reaction is shown below we're given the
equation here
25 centimeters cubed of 0.04
naught multiple decimeter cubed of
sodium hydroxide is neutralized by 17.5
centimeters cubed dilute sulfuric acid
part a asks us to calculate the amount
in moles of sodium hydroxide used in
titration
this is very similar to the second step
of the equations that we were doing
before
so write down what we know
we know that the concentration is equal
to 0.0440
moles per decimeter cubed and where the
volume is
25.0 centimeters cubed which is
5 0.025
cubed
we can look at our triangle pyramid
which is the number of moles equal to
the concentration multiplied by the
volume so n is equal to c times v
which is
0.044
multiplied by 0.025
to give us 0.0011
[Music]
moles of sodium hydroxide used
so now let's look at part b
calculate the amount in moles of h2so4
sulfuric acid used in the titration
so in order to do this we need to look
at our reaction equation
now we can see that two moles of sodium
hydroxide will react with one mole of
sulfuric acid so that's a two to one
ratio
so
if we have 0.0011
moles of our sodium hydroxide
it's going to react with half as much
sulfuric acid so that's
0.0011 divided by 2 to give us 0.00055
moles
of sulfuric acid
part c our final part is to calculate
the concentration in moles per decimeter
cubed of h2so4 sulfuric acid used in
titration
again as we always do write down what we
know we know the number of moles is
equal to 0.00055
moles as we've just worked out and in
the question we're told the volume is
17.5
centimeters cubed that's equal to
0.0175 decimeters cubed
so our equation pyramid shows us the
number of moles equals the concentration
multiplied by the volume we want to know
the concentrations the rearrangement
that we'll use is that the concentration
is equal to the number of moles divided
by the volume so that is 0.00055
divided by 0.01
to give us a concentration of 0.03143
moles
per decimeter cubed
question three a student carries out the
titration using barium hydroxide and
nitric acid
in part a we're asked to write an
equation for the reaction taking place
so we know our two reactants are barium
hydroxide
and
nitric acid
now we're going to form
salt and water our salt being barium
nitrate
so now we've written our equation we
need to go ahead and check to balance it
so on both sides of the equation we have
one barium
on the left hand side we have one
nitrogen on the right hand side in our
product we have two so we can balance
that by putting a two in front of our
nitric acid to check our hydrogen atoms
we have two here and two here that's
four on the reactant side the left hand
side and we have
only two on this side so we'll put a two
in front of our water molecule so now we
have four on both sides to check our
oxygen atoms there's two here and six
here that's eight and we have six here
and two here eight again so that is our
correct and balanced equation and for
that we get one mark
in part b we're told that 50 ml of
barium hydroxide a concentration of 0.5
moles per decimeter cubed are required
to fully titrate 100 ml solution of our
acid
we're asked what is the initial
concentration of the acid
so the first thing we're going to do is
write out the pyramid we're going to
need
we know that the number of moles is
equal to the concentration times the
volume of our solution
so we're going to work out the number of
moles of barium hydroxide that have been
used in the titration so the number of
moles is equal to the concentration
multiplied by the volume the
concentration is 0.5 moles per decimeter
cubed we have 50 mils so we're going to
multiply that by
50 over 1000 converting the mils there
to decimeters cubed
giving us not
.025 moles
now if we take a look at the equation
that we previously wrote we can see that
one mole of barium hydroxide reacts with
two of nitric acid
so that's one to two therefore if we
have
0.025 moles of our barium hydroxide
that's going to react with
0.05 moles of our nitric acid so we know
we have 0.05 moles of nitric acid that's
reacting initially
we know there's a 100 mils of the
solution so let's go ahead and quickly
note down what we know we know the
number of moles is 0.05
we know the volume is 100 ml so that's
100 over 1000 converting to decimeters
cubed giving us 0.1 decimeters cubed
now using the same pyramid we can
calculate the concentration see that the
concentration is the number of moles
divided by the volume so that's
0.05 divided by 0.1 to give us
0.5
moles per decimeter cubed
so this question holds three marks the
first mark is given for correctly
calculating the number of moles of
barium hydroxide
the second for applying that and using
that to calculate the number of moles of
acid
the third and final mark for correctly
calculating the initial concentration of
the acid remembering to give units part
c the last part of our question asked us
to name two pieces of apparatus that are
used to accurately measure the volume of
solutions in a titration and we're asked
what other chemical substance must be
added to the reaction flask for
titration to be successful so if we deal
with the first part of the question to
name two pieces of apparatus that are
used to accurately measure the volume of
solution in a titration this could be a
burette and also a pipette which are two
important pieces of apparatus that you
will have used that are used to
accurately measure volumes of solution
often small volumes
now to deal with the second part of the
question
what chemical substance must be added
well we know that it's important to use
an indicator because this will tell us
when we have reached the endpoint of our
titration
or when we are near it
there are a variety of different
chemical indicators that have been used
we're not asked to give a suggestion of
one here just to explain what chemical
supplements would be added but
some questions may ask you to go into
more detail and suggest an indicator
such as methyl orange or phenolphthalein
this question holds three marks
you get one mark for each suggestion of
a correct piece of apparatus and the
third and final mark comes from stating
it's an indicator that needs to be added
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