Exercise 1: You got a job as an adjunct instructor at a community college and want to make 320 ml of a 2% maltose solution for one of your students' lab experiments. How much maltose would you need?

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please answer part 1 & 2 of question
Since the number of molecules of a particular solute is impossible to count we can use the Molecular Weight of the
solute to get to it. Each atom and therefore molecule has a particular mass. The mass in grams of one mole of a
substance is its Molecular Weight (MW).
Molecular Weight (the weight of one mole of a particular molecule or atom): MW = g/mole
The Molecular Weight of a chemical is usually given on the bottle, but can also be calculated using the periodic
table of elements. The atomic mass for every element is listed underneath the symbol for that element in the
periodic table, and for a chemical, the atomic mass for each component of that chemical, added together, will give
the Molecular Weight for that chemical.
For example, sodium chloride has a chemical formula of NaCl. According to the periodic table, Na (sodium) has
an atomic mass of 22.99 and CI (chlorine) has an atomic mass of 35.45. NaCl therefore has a Molecular Weight of
22.99 +35.45 = 58.44. Remember that the Molecular Weight is measured in g/mole. 6.022 x 1023 molecules (1
mole) of NaCl thus weigh 58.44 g.
Now, this is not a concentration yet, since we have not dissolved anything in a solvent. Molarity is
a measure of a number of molecules in 1 liter of solution. By definition, a 1 molar solution has 1 mole of the solute
per 1 liter of solvent. To make a solution of NaCl that is 1 molar (1 M), we therefore need to dissolve the 58.44 g of
NaCl from above in a total volume of 1 liter.
If you have the amount of solute (mass) and the volume, but need to know the Molarity, you can use the following
equation:
M (mole/liter) = weight of solute (g)
V (liter) * MW (g/mole)
Generally, to prepare 1 liter of a simple molar solution from a dry reagent you have to multiply the Molecular
Weight by the desired Molarity to determine how many grams of reagent to use. This is the equation above, just
rearranged.
Needed weight in g to dissolve in 1 liter = MW (g/mole) * M (moles/liter)
It is very important that you always use the correct and complete units for these calculations since they can tell you
at a glance whether your formula is wrong. For example, if you want to know how many g of NaCl to weigh out to
make a 1 M solution, your units, when canceled out, should leave you with grams. Don't forget that Molarity
always refers to 1 liter. If you want less or more than 1 liter of your solution this will have to be factored into the
equation.
Needed weight in g to dissolve in desired volume = MW (g/mole) * M (moles/liter)* desired volume (liter)
Example:
If you want to make 250 ml of a 2 M NaCl solution:
58.44 g/mole * 2 moles/liter* 0.25 liter = 29.22. To make this solution properly you would weigh out
29.22 g of NaCl, dissolve it in about 200 ml of water and then fill the total volume to 250 ml with water.
Why would you not pour the 29.22 g directly into 250 ml of water and then dissolve?
Skills Boot Conp /
Transcribed Image Text:Since the number of molecules of a particular solute is impossible to count we can use the Molecular Weight of the solute to get to it. Each atom and therefore molecule has a particular mass. The mass in grams of one mole of a substance is its Molecular Weight (MW). Molecular Weight (the weight of one mole of a particular molecule or atom): MW = g/mole The Molecular Weight of a chemical is usually given on the bottle, but can also be calculated using the periodic table of elements. The atomic mass for every element is listed underneath the symbol for that element in the periodic table, and for a chemical, the atomic mass for each component of that chemical, added together, will give the Molecular Weight for that chemical. For example, sodium chloride has a chemical formula of NaCl. According to the periodic table, Na (sodium) has an atomic mass of 22.99 and CI (chlorine) has an atomic mass of 35.45. NaCl therefore has a Molecular Weight of 22.99 +35.45 = 58.44. Remember that the Molecular Weight is measured in g/mole. 6.022 x 1023 molecules (1 mole) of NaCl thus weigh 58.44 g. Now, this is not a concentration yet, since we have not dissolved anything in a solvent. Molarity is a measure of a number of molecules in 1 liter of solution. By definition, a 1 molar solution has 1 mole of the solute per 1 liter of solvent. To make a solution of NaCl that is 1 molar (1 M), we therefore need to dissolve the 58.44 g of NaCl from above in a total volume of 1 liter. If you have the amount of solute (mass) and the volume, but need to know the Molarity, you can use the following equation: M (mole/liter) = weight of solute (g) V (liter) * MW (g/mole) Generally, to prepare 1 liter of a simple molar solution from a dry reagent you have to multiply the Molecular Weight by the desired Molarity to determine how many grams of reagent to use. This is the equation above, just rearranged. Needed weight in g to dissolve in 1 liter = MW (g/mole) * M (moles/liter) It is very important that you always use the correct and complete units for these calculations since they can tell you at a glance whether your formula is wrong. For example, if you want to know how many g of NaCl to weigh out to make a 1 M solution, your units, when canceled out, should leave you with grams. Don't forget that Molarity always refers to 1 liter. If you want less or more than 1 liter of your solution this will have to be factored into the equation. Needed weight in g to dissolve in desired volume = MW (g/mole) * M (moles/liter)* desired volume (liter) Example: If you want to make 250 ml of a 2 M NaCl solution: 58.44 g/mole * 2 moles/liter* 0.25 liter = 29.22. To make this solution properly you would weigh out 29.22 g of NaCl, dissolve it in about 200 ml of water and then fill the total volume to 250 ml with water. Why would you not pour the 29.22 g directly into 250 ml of water and then dissolve? Skills Boot Conp /
Similarly, for liquid solutes, volume of solute to use = % concentration * volume needed
Example: if you want to make 2 liters of a 10% hydrogen peroxide solution you would mix 10 ml/100 ml x
2000 ml = 200 ml of hydrogen peroxide with 1800 ml of water.
It's your turn..
Exercise 1: You got a job as an adjunct instructor at a community college and want to make 320 ml of a 2%
maltose solution for one of your students' lab experiments, How much maltose would you need?
3. Weight/volume (w/v):
You find this quite often in sciences as well. For analyses where ppm, ppb, % etc. do not apply, this is a good way
to indicate concentration. Solutes dissolved in blood, for example, are often indicated as weight per volume.
Acceptable levels of total cholesterol, for example, are 150-200 mg/dl (a deciliter being 1/10th of 1 liter).
Example: if you take the example from the previous page, your 200 ml of 4% maltose solution (8 g in 200 ml)
can also be expressed as a 40 g/liter sugar solution.
4. Molarity (M)
This measure of concentration is most commonly used for laboratory solutions and often the hardest for students to
master. In chemistry and biology, it is often important to have a measure of the number of molecules in a given
volume of solution, not just a measure of percent or weight/volume. We will encounter this again when we talk
about pH, for example. So what is Molarity? Molarity (M) describes the number of molecules (in this case, a
specific number of molecules or moles) of a chemical in one liter of solution. Similar to the formula for percent
above,
c=n/v
Molarity can be calculated by
where the concentration (c) is Molarity and instead of mass of a chemical we measure the number of moles (n) of
this chemical per volume (v).
Molarity (describes a concentration as a number of molecules/volume): M= moles/liter
So what is a mole? The key word is number and like a baker's dozen, a mole is just that, a number, albeit a very
high one: 6.022 * 1023. A 1 molar solution (1 M) of sucrose therefore would contain 6.022 * 1023 molecules of
sucrose per liter.
1 mole (number of molecules or atoms) = 6.022 * 1023
13
Basic Lahoroen Stills Boot Cany
Transcribed Image Text:Similarly, for liquid solutes, volume of solute to use = % concentration * volume needed Example: if you want to make 2 liters of a 10% hydrogen peroxide solution you would mix 10 ml/100 ml x 2000 ml = 200 ml of hydrogen peroxide with 1800 ml of water. It's your turn.. Exercise 1: You got a job as an adjunct instructor at a community college and want to make 320 ml of a 2% maltose solution for one of your students' lab experiments, How much maltose would you need? 3. Weight/volume (w/v): You find this quite often in sciences as well. For analyses where ppm, ppb, % etc. do not apply, this is a good way to indicate concentration. Solutes dissolved in blood, for example, are often indicated as weight per volume. Acceptable levels of total cholesterol, for example, are 150-200 mg/dl (a deciliter being 1/10th of 1 liter). Example: if you take the example from the previous page, your 200 ml of 4% maltose solution (8 g in 200 ml) can also be expressed as a 40 g/liter sugar solution. 4. Molarity (M) This measure of concentration is most commonly used for laboratory solutions and often the hardest for students to master. In chemistry and biology, it is often important to have a measure of the number of molecules in a given volume of solution, not just a measure of percent or weight/volume. We will encounter this again when we talk about pH, for example. So what is Molarity? Molarity (M) describes the number of molecules (in this case, a specific number of molecules or moles) of a chemical in one liter of solution. Similar to the formula for percent above, c=n/v Molarity can be calculated by where the concentration (c) is Molarity and instead of mass of a chemical we measure the number of moles (n) of this chemical per volume (v). Molarity (describes a concentration as a number of molecules/volume): M= moles/liter So what is a mole? The key word is number and like a baker's dozen, a mole is just that, a number, albeit a very high one: 6.022 * 1023. A 1 molar solution (1 M) of sucrose therefore would contain 6.022 * 1023 molecules of sucrose per liter. 1 mole (number of molecules or atoms) = 6.022 * 1023 13 Basic Lahoroen Stills Boot Cany
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