Your Name:
Date:
Class:

Formula of a Hydrate

Parts of the text on this lab will not print out. This is by design. The parts that won’t print are notes for teachers. Students don’t need those notes and they are automatically excised from the printout.

Objective

The lab work has two objectives: first, confirm the formula of a hydrate with known formula and second, find the formula of a hydrate in which the salt formula is known but not the molar amount of water.

Overview

This lab activity combines in-class problem-solving with lab work. Students will be introduced to the concept of hydrated salts, anhydrous salts, hydrate nomenclature, and the molar mass of hydrates. The lab portion of this work conists in confirming the formula of a hydrate of known formula (CuSO₄·5H₂O) and finding the formula of a hydrated salt of known formula but unknown water content (MgSO₄·XH₂O).

Background

Some chemical compounds, especially inorganic salts, incorporate water into their crystalline structures. Water has a polar structure: it has positively and negatively charged parts within each molecule. This gives it a strong attraction toward ions. The ions in some salts attract and form strong bonds with water molecules. These salts, when they have absorbed water, are called hydrates. Anhydrous salts are salts that can form hydrates but which have had all the water driven off, usually by heat. Hydrated salts are characterized by the number of moles of water molecules per mole of salt. The so-called water of hydration of nickel (II) chloride (NiCl₂) is six moles H₂O for every one mole of NiCl₂. The hydration reaction is shown below. The hydrate in this reaction is called nickel (II) chloride hexahydrate.

The formula of this hydrate shows the molar amount of water incorporated into the crystal matrix. For most hydrates the amount of water included in the formula is only important when trying to measure molar amounts of the salt. You need to know the true formula weight (molar mass) in order to measure out the mass needed to give a certain number of moles.

The way that the water is bound is normally not important since it can be driven off by heat or simply dissolve away if the salt is dissolved in water. For example, for nickel (II) chloride hexahydrate (NiCl₂·6H₂O) the molar mass is 237.69 g/mol not 129.60 g/mol. The figure 129.60 g/mol is the molar mass of the anhydrous salt.

 

Formulas for hydrates are written using a dot convention: conventionally, a dot is used to separate the formula of the salt from the formula of the water of hydration. A numerical coefficient gives the molar amount of water included in the hydrate. Hydrates are named using prefixes for the word hydrate (at right). For example, CuCl₂·2H₂O is copper (II) chloride dihydrate and CuSO₄·5H₂O is copper (II) sulfate pentahydrate. One key point: the dot is not a multiplication sign. When calculating the molar mass you add the molar mass of water (multiplied by the coefficient).

An everyday example of hydration is concrete. Concrete is made by mixing Portland cement with water and aggregate materials. The aggregate materials are the gravel and sand that add strength to the final concrete. The Portland cement is a mixture of calcium silicates, calcium aluminate, calcium aluminoferrite and gypsum. All of these chemicals absorb water by hydration. This means that concrete does not ‘dry’ in a conventional sense. Instead the water mixed with the concrete combines chemically with the materials in the cement and the resulting hydrates form a strong matrix that holds the concrete together and makes it strong.

Another interesting example of the value of hydration is the incorporation of hydrated building materials (such as concrete, gypsum wall board and plaster). The building materials will not rise above the 100°C boiling point of water until all of the water of hydration has been driven off. This can help keep damage to a minimum until the fire can be put out. In the construction business this is known as passive fire protection.

Pre-lab Problems

The following problems will help you to be able to do the math required for the analysis of your lab results. An example problem with an animation can be found at http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/animationsindex.htm under Stoichiometry. The relevant animation is called Percent composition of a hydrate simulation.

Find the molar mass of the following hydrated and anhydrous salts.

1. FeCl₂·2H₂O ____________
2. FeCl₂ ____________
3. CaCl₂·2H₂O ____________
4. CaCl₂ ____________

5. CuSO₄·5H₂O ____________
6. CuSO₄ ____________
7. MnSO₄·4H₂O ____________
8. MnSO₄ ____________

Example:
Given 0.62 g CuSO4·5H2O find the mass of water that would be driven off by heating
          1 mol
0.62 g · ——————— = 2.48 × 10-3 mol          reaction: CuSO4·5H2O --> CuSO4 + 5H2O 
         249.69 g
                   5 mol H2O 
2.48 × 10-3 mol · ————————————— = 1.24 × 10-2 mol H2O = 0.22 g H2O (18.02 g/mol)
                 1 mol CuSO4·5H2O
So the anhydrous salt in the sample accounts for 0.40 g 
and the mass of the water of hydration is 0.22 g

9. Find the mass of the anhydrous salt in a 142.3 g sample of MnSO₄·4H₂O. This might be found in the lab by heating the sample until its mass does not decrease any further.
10. Find the mass of the anhydrous salt and the mass of water in a 10.9 g sample of FeCl₂·2H₂O.

Example:
A 140.5-g sample of NiSO4·XH2O is heated until no further decrease in mass.
The mass of the anhydrous salt is 77.5 g. Find the number of water molecules 
in the formula of this hydrate of nickel (II) sulfate.
          1 mol
77.5 g · ——————— = 0.50 mol NiSO4         reaction: NiSO4·XH2O --> NiSO4 + XH2O 
         154.76 g
                               1 mol
140.5 g - 77.5 g = 63 g H2O · ——————— = 3.5 mol H2O
                              18.02 g 
3.5 mol H2O
—————————— = 7 mol H2O per mol anhydrous salt so formula is NiSO4·7H2O
  0.5 mol
nickel (II) sulfate heptahydrate

Problems, cont.

11. Given that a 40.14-g sample of hydrated NiSO₄ is reduced in mass to 22.14 g upon heating show that the formula of the hydrate is NiSO₄·7H₂O.
12. Given that a 139.4-g sample of hydrated MnSO₄ is reduced in mass to 94.38 g upon heating find the empirical formula of the hydrate. Also, write the name of the hydrate of manganese sulfate.

Materials

Procedure

Part I

1. Weigh your crucible after you have ensured that it is clean and dry
2. Obtain about 1 g of CuSO₄·5H₂O in your crucible and weigh it, recording the mass to the hundredth’s place
3. Before proceeding any further make a prediction about the amount of mass that will be lost when you heat the sample of copper (II) sulfate pentahydrate. Specifically, calculate the mass of the anhydrous salt and the mass of water that will be driven off. Show this to your instructor before proceeding.
4. Once you have your instructor’s approval, place the crucible containing the CuSO₄·5H₂O on the clay triangle.
5. Light the bunsen burner and adjust for a hot flame.
6. Heat the crucible as gently as possible with the burner by moving the burner under the crucible for a few seconds at a time. Note the release of any steam from the crucible.
7. Remove the heat source and use a pair of lab spatulas to occasionally stir the copper sulfate. Carefully scrape all of it back into the crucible. Be careful not to do this while heating!
8. Continue heating gently until the salt turns completely white. Be careful not to overheat! The heat can become so intense that the sulfate in the salt begins to break down. If this happens the salt will turn yellow and produce a sulfurous smell. It will also ruin your data since it will reduce the mass more than expected due to the decomposition of the salt.
9. Stop heating when the salt has lost all water of hydration. Allow the crucible and its contents to cool completely.
10. Once the crucible is cool, find its mass. Calculate the mass of the contents of the crucible by subtracting the mass of the crucible. Compare your result with the calculations you performed earlier. Were your predictions correct?
11. If your measured mass is larger than your predicted mass of anhydrous salt then you may not have driven off all of the waters of hydration. Heat the crucible and its contents one more time.
12. Empty the anhdrous salt onto a large watch glass. Use the dropper to add a very little water to the anhydrous copper (II) sulfate. Describe what happens in your lab notebook. For your report think about what is happening at the molecular level when you add water.
13. When you finished this part of the lab empty the re-hydrated CuSO₄·5H₂O into the beaker provided by your instructor for this purpose. Then begin Part II.

Part II

In this part of the lab you will repeat the same procedure performed for the salt of known formula with a salt for which you do not know the hydrate formula. The salt is magnesium sulfate (MgSO₄). Your correct identification of the hydrate formula is worth 5 points on your lab report. To ensure better chances of getting the correct result you may want to consider doing at least two (and perhaps three) trials. For each trial use a minimum of 2 g. The magnesium sulfate is not nearly so hazardous as the copper (II) sulfate and a larger amount will help to reduce errors due to small lab balance inaccuracies.

By the way, magnesium sulfate is the chemical name for Epsom Salts. Epsom Salts were discovered by a farmer in Epsom, England. Every day his cows waded through water containing naturally high amounts of magnesium sulfate. He found that the cows showed evidence of diarrhea but also that the incidence of small wounds near their hooves was reduced. Epsom Salts are used as a laxative and in foot soaks and bath salts. It soothes tired muscles and can help to heal skin problems, including acne.

The Report

Each individual student must write their own formal lab report. The report must include your raw data, calculations and a detailed analysis. The procedure portion of your report must be given in your own words and must describe what you actually did in the lab. Include descriptions of your observations in the procedure section. Be sure to show your work for all important calculations: partial credit toward the 5 points of accuracy of your hydrate formula cannot be awarded if you do not show your work. Work must be included in the typed portion of the report. Data should be presented in neat tables. Some questions to help focus your analysis:

1. What was the expected mass of anhydrous copper (II) sulfate? The expected mass of water to be lost by heating?
2. How well did your prediction match up with your results for copper (II) sulfate pentahydrate?
3. If the mass-loss was greater than that expected due to the loss of the mass of water how can you explain this? (See step 8 in Part I). What other explanations can you offer for unexpected results?
4. What is the formula of the hydrate of magnesium sulfate? What is the name of this hydrate?