Essay Example on Calculating Drink Mix Mass for 0.24L Solution

1. Introduction

The purpose of this lab is to compare the concentration of the drink mix concerning the solvent volume

2. Calculate the molar mass of the drink mix.

Molar mass of drink mix is given by;

Calculating the total molecular mass of the drink mix

Chemical compound, C12H22O11

(12*12+22*1+11*16)

Therefore, molar mass of the drink mix,

Will be 342 g/mol

3. Calculate the mass (in grams and teaspoons) of drink mix to make 0.24 L (1 cup of water) solutions of the following concentrations:

Mass for:

0.05 M

Molar = moles of solute/ volume of the solution

Moles of solute = M*volume of the solution

Moles of solute = (0.05 mol/L) *(0.24L)

Moles of the solute = 0.012 moles

Given molar mass = 342g/mol

Mass = 0.012 moles*M

Mass = 0.012moles *382g/mol

Mass = 4.584 g

1 teaspoonful = 4.1 g

Hence 4.584g/4.1g

Equivalent of one teaspoonful

0.1 M

Molar = moles of solute/ volume of the solution

Moles of solute = M*volume of the solution

Moles of solute = (0.1 mol/L) *(0.24L)

Moles of the solute = 0.024 moles

Given molar mass = 342g/mol

Mass = 0.024 moles*M

Mass = 0.024moles *382g/mol

Mass = 9.168 g

1 teaspoonful = 4.1 g

Hence 9.168g/4.1g

Equivalent of two teaspoonfuls

0.2 M

Molar = moles of solute/ volume of the solution

Moles of solute = M*volume of the solution

Moles of solute = (0.2 mol/L) *(0.24L)

Moles of the solute = 0.048 moles

Given molar mass = 342g/mol

Mass = 0.048 moles*M

Mass = 0.048moles *382g/mol

Mass = 18.336 g

1 teaspoonful = 4.1 g

Hence 18.336g/4.1g

Equivalent of four teaspoonfuls

0.3 M

Molar = moles of solute/ volume of the solution

Moles of solute = M*volume of the solution

Moles of solute = (0.3 mol/L) *(0.24L)

Moles of the solute = 0.072 moles

Given molar mass = 342g/mol

Mass = 0.072 moles*M

Mass = 0.072moles *382g/mol

Mass = 27.504 g

1 teaspoonful = 4.1 g

Hence 27.504g/4.1g

Equivalent of seven teaspoonfuls

e. 0.4 M

Molar = moles of solute/ volume of the solution

Moles of solute = M*volume of the solution

Moles of solute = (0.4 mol/L) *(0.24L)

Moles of the solute = 0.096 moles

Given molar mass = 342g/mol

Mass = 0.096 moles*M

Mass = 0.096moles *382g/mol

Mass = 36.672 g

1 teaspoonful = 4.1 g

Hence 36.672g/4.1g

Equivalent of 9 teaspoonfuls

4. When drink mix is dissolved in water, what is the solute and what is the solvent?

The drink mix becomes the solute; the water becomes the solvent.

Data Table

Concentration	Drink	Mix (teaspoons)	Smell	Taste	Rating (1-5)
0.05	M	1	Fair smell	tasteless	1
0.1	M	2	Fair smell	Less sugary	2
0.2	M	4	Average smell	sugary	3
0.3	M	7	Smells good	Average sugary	4
0.4	M	9	Sweet smell	Too sugary	5

Questions

1. Which concentration of drink did you prefer the most? What was wrong with the other solutions that you made?

Drink with 0.3 M concentration. Other drinks with less concentration, i.e., 0.05M, 0.1M, 0.2M tasted less sugary, drinks with a concentration higher than 0.3M, were too concentrated and tasted too sugary.

2. How is taste related to concentration? Why are they related to this way?

The higher the concentration, the tastier a solution becomes. The concepts are related since the solvent tends to have a higher level of solute molecules with an increase in concentration.

5. You are running a lemonade stand with your friend. You prepared 10 liters of 0.7 M lemonade, but your friend did online research and found that people prefer 0.4 M lemonade. How can you fix the lemonade you made so that it is 0.4 M without starting over? Explain the steps in detail. If you add anything, tell how much!

To make 0.4M concentration, you should add 7.5L of water to your current concentration.

Explanation:

From the Molarity formula

M1×V1=M2×V2

Where M represents molarity and V, volume

Substituting in values

0.7 × 10 = 0.4 × V2

Making the new volume the subject

V2= 17.5L

Therefore, the new volume of water to be added will be given by:

(new volume-initial volume)

Volume of water to be added = 17.5 - 10 = 7.5L

Therefore, you should add 7.5L to 10L to make 0.4 M

Were you able to make solutions with the assigned molarities?

I was able to make solutions with given molarities. Molarity was achieved by first calculating the respective mass needed to make the assigned molarities. Then following the laboratory guidelines to mark the level of the solvent.

Are there any patterns or trends in your data?

The data obtained show a significant trend and relation. The higher the solute molecules, the higher the concentration.

List two sources of error. Remember, a source of error cannot be human error.

An error can occur when using an estimated mass, especially when using a teaspoon to add drink mix to water.

An error can also occur when measuring water to 0.24 l mark hence resulting in inconsistent results.