FORMULA OF A HYDRATE
Some salts, when crystallized from water solutions, retain definite proportions of water as an integral part of the crystal structure. This type of crystal is called a hydrate. In this experiment, you will determine the whole number proportion of water to salt in a hydrate. This will enable you to write the correct formula for a hydrate (salt · xH2O).
OBJECTIVES
When you have completed this activity, you should be able to:
1. Demonstrate a procedure for determining the amount of water and salt in a hydrate.
2. Compute the smallest whole number ratio of moles of water to moles of salt in a hydrated salt sample.
3. Construct a formula for a hydrate from the whole number ratio of moles of water to moles of salt.
4. Perform an error analysis.
5. Construct a definition for hydrated salts and anhydrous salts.
MATERIALS
• goggles
• crucible tongs (substitute hot pads to protect your hands from heat)
• cooling rack
• balance, sensitive to at least 0.01 g
• small baking dish/ ramekin and cover (substitute any kind of baking dish with lid that can go into the oven)
• burner (substitute an oven to dry your baking dish and its contents)
• Epsom salts (magnesium sulfate hydrate)
PROCEDURE
1. Dry the ramekin or baking dish and cover in an oven overnight. Record the mass of the empty, dry dish and cover in Data Table entry #4.
OR
Place a clean, dry baking dish or ramekin with the cover ajar in the oven and heat for 10 minutes at 250◦F. Discontinue heating and carefully use hot pads remove the dish and cover onto a cooling rack to cool. When cool enough (about 5 minutes), measure the mass of the dish and cover. Record the mass of the empty, dry dish and cover in Data Table entry #2. Repeat the heating, cooling, and measuring procedure until the mass is constant. You have obtained a constant mass when two consecutive masses differ by no more than 0.1 g. Record the mass of the empty, dry dish and cover in Data Table entry #3 and #4.
2. Add about 3.0 g of Epsom salts (magnesium sulfate hydrate) to your dish. Measure and record the exact mass in Data Table entry #1.
3. Determine the mass of the hydrate by subtracting entry #4 from entry #1 in the Data Table. Record this result in Data Table entry #5.
4. Gently heat (250∘F) the dish and contents with the cover ajar for 12 minutes. Cool, measure, and record the mass in Data Table entry #6.
5. Repeat the heating with cover ajar for four minutes. Cool, measure the mass, and record reading in Data Table entry #7. If a third heating is necessary, heat the dish and its contents for one additional minute. Record the mass in the margin next to entry #7. Repeat the heating, cooling, and measuring process until two consecutive masses differ by no more than 0.1 g. Record the constant mass of the dish, cover, and anhydrous salt in Data Table entry #8.
6. Determine the mass of the anhydrous salt by subtracting entry #4 from entry #8 in the Data Table and record in Data Table entry #9.
7. Determine the mass of water lost by subtracting entry #9 from entry #5 in the Data Table and record in Data Table entry #10.
DATA TABLE
1. Mass of ramekin, cover, and hydrated salt g
2. Mass of ramekin and cover (1st heating) g
3. Mass of ramekin and cover (2nd heating) g
4. Constant mass of ramekin and cover g
5. Mass of hydrate g
6. Mass of ramekin, cover, and anhydrous salt (1st heating) g
7. Mass of ramekin, cover, and anhydrous salt (2nd heating) g
8. Constant mass of ramekin, cover, and anhydrous salt g
9. Mass of anhydrous salt g
10. Mass of water lost g
ANALYSIS
1. Calculate the number of moles of water lost. (Take the # of grams in #10 and convert to moles.)
2. Calculate the number of moles of anhydrous MgSO4 (molar mass 120.4 g). (Take #grams in #9 and convert to moles)
3. Calculate the smallest whole number ratio of moles of water to moles of anhydrous salt. (Divide the moles of water by the moles of anhydrous salt.)
4. From your calculated whole number ratio, write the probable formula for magnesium sulfate hydrate. (Use the number from #3, this will be the number of moles of water for the hydrate)
Use this rhyme to help you remember the steps:
1.) Percent Mass – change the percentages you calculated in problem 3 to mass. How do you do that? Simply by changing he % sign to a g (grams)
2.) Mass Mole – Now take each grams and change each one of those to moles. Go back to Portfolio 2 Supplemental Help if you don’t remember how to change mass to moles
3.) Divide by small – Look at each answer (mole) that you just calculated – which value is the smallest? Take that value and divide ALL of the answers (moles) you calculated by it. One of them will be 1 because you are dividing it by itself.
4.) Multiply till whole – you should get a whole number if you don’t then you must multiply that number until it becomes a whole number.
Examples: 0.5 multiply by 2 = 1 0.33 multiply by 3 to get 1
The trick here though is if you have to multiply a decimal to get “it” to whole, then you need multiply ALL of your answers.
NOTE: STEP #4 is NOT always done, only done if the number of moles is NOT a whole number.
5. Perform an error analysis.
a. Calculate the percent error (Remember to calculate % error= |Experimental value-Theoretical value|/ Theoretical value X 100%).
Compare the molar mass of your experimentally determined hydrate with the theoretical molar mass of hydrate = 246.4 g
b. List several possible sources of error. Include error inherent in the procedure itself.
6. Epsom salts are hydrates of magnesium sulfate. The formula for Epsom salt is MgSO4·7H2O. If a 7.834 g sample is heated until constant mass is obtained, what is the mass of the anhydrous magnesium sulfate? What percent of the hydrate is water?
7. A certain hydrate of potassium aluminum sulfate has the formula KAl(SO4)2·xH2O. When a sample weighing 5.459 g is heated to remove all the water, 2.583 g of anhydrous salt remains. What is the mass % of water in the hydrate? Determine the value of x.
PRE-LAB: FORMULA OF A HYDRATE
Read the introduction and the procedure of the lab activity, highlighting key information as you read. Answer the following questions.
1. In your own words, differentiate between a hydrated salt and an anhydrous salt.
2. Why is it important to heat the baking dish or ramekin and cover in step #1?
3. Why is it necessary to achieve constant mass? How will you know when constant mass is achieved?
4. Why should the ramekin be cooled before taking a mass reading?
5. How might each of the following affect the reliability of your results? Explain.
a) Increased humidity in the room.
b) Eliminating the preliminary heating, cooling, and massing of the ramekin and cover prior to its use.
c) Recording mass measurements to two significant figures.
Have Santa deliver that unknown hydrate sample.to my house and I'll get right on that analytical procedure.
Wow this is... just... beyond my knowledge!!!
what is your question about this?
savage
To determine the formula of a hydrate, you'll need to follow the steps outlined in the procedure provided:
1. Dry the ramekin or baking dish and cover in an oven overnight or heat it for 10 minutes at 250°F. This step ensures that any water or impurities are removed from the dish and cover before starting the experiment. Record the mass of the empty, dry dish, and cover.
2. Add about 3.0 g of Epsom salts (magnesium sulfate hydrate) to your dish and record the exact mass.
3. Determine the mass of the hydrate by subtracting the mass of the empty dish and cover from the mass of the dish, cover, and hydrated salt.
4. Gently heat the dish and contents with the cover slightly open at 250°F for 12 minutes. Cool, measure, and record the mass.
5. Repeat the heating and cooling process for several more cycles until the mass remains constant (differs by no more than 0.1 g).
6. Determine the mass of the anhydrous salt by subtracting the mass of the empty dish and cover from the constant mass of the dish, cover, and anhydrous salt.
7. Determine the mass of water lost by subtracting the mass of the anhydrous salt from the mass of the hydrate.
In the analysis section, you'll complete various calculations using the data obtained from the experiment:
1. Calculate the number of moles of water lost by converting the mass of water lost to moles.
2. Calculate the number of moles of anhydrous salt (magnesium sulfate) by converting the mass of the anhydrous salt to moles using the molar mass of magnesium sulfate (120.4 g/mol).
3. Calculate the smallest whole number ratio of moles of water to moles of anhydrous salt by dividing the moles of water lost by the moles of anhydrous salt.
4. From the calculated whole number ratio, write the probable formula for the hydrate using the number of moles of water for the hydrate.
Performing an error analysis and calculating the percent error can help identify potential sources of error and determine the accuracy of your results.
Finally, in the pre-lab section, you'll answer questions about the concept of hydrated and anhydrous salts, the importance of the heating step, achieving constant mass, cooling before taking mass readings, and how certain factors can affect the reliability of the results.