CHEM 110 Lecture Notes - Lecture 3: Magnesium Sulfate, Calcium Sulfate, Calcium Chloride

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greywildebeest28

16 Jul 2018

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There are many soluble minerals in the ocean. Ater on the shores of new jersey have 3. 5% of salt in 60ml of water. E can find this out by boiling the water and letting it evaporate, so that there is only salt left. The salt content is different in different oceans. In the galapagos islands the water has a higher salt content (3. 8%) because there is little freshwater there, and it is warmer over there. In dead sea there is 32% of salt, and people can easily float in it. Elements in salts: sodium, potassium, magnesium, chlorine/chloride. Calcium, sodium, and magnesium have outer electrons that can be easily removed, and they then have positive charges. They can then be combined with negatively charged species like bicarbonate, chloride, and sulfate. How ionic species combine to make salt. Gypsum= calcium + sulfate (ca++ and so4=) Calcium has two positive charges, and sulfate has two negative charges, so they balance each other out.

Related Questions

Need help answering the pre - lab questions

Chemistry 1010 Laboratory Fall 2016 Lab: Percent Sugar Content of Beverages ave you ever been to the ocean? Does it seem that you can float or swim much easier in the ocean than in a swimming pool? Seawater is more dense than freshwater due to the presence of dissolved salt in the cean As a result, our buoyancy-ability to float-is greater in salt water than in plain water. What factors of a particular substance is dissolved in it? Background The density of a pure substance is a characteristic physical property that can be used to identify the substance does not depend on the amount of the substance. The density of any material is determined by measuring its mass and volume and then dividing the mass by the volume. The mass of a substance can be measured directly using a balance. The volume of a liquid can be measured directly using special laboratory glassware, such as a graduated cylinder, buret, or pipet. In this experiment, liquild volumes will be measured using a graduated cylinder Density is defined as the ratio of mass per unit volume. It is an "intensive" property, that is, it The density of a solution depends on its concentration, that is, how much solid is dissolved in the liquid. The higher the concentration of solid, the greater the density of the solution. A convenient way to express concentration is in units of weight percent, which corresponds to the number of grams of sollid that are present in 100 g of solution. A 20% salt solution is prepared by dissolving 20 g of sodium chloride (table salt) in 80 g of water to give a final mass of 100 g of solution. When the density of a solution is plotted on a graph against the concentration of the solution, a regular pattern becomes evident, specifically that density is directly proportional to the concentration of solid in the solution. A 20% salt solution, for example, has a higher density and higher concentration of solid than a 10% salt solution. If the densities of several solutions of known concentration are determined experimentally and plotted on a graph, a calibration curve can be drawn to show a straight-line relationship between the density of a solution and the concentration of solid (note: the calibration curve in this lab reveals a linear (straight-line) relationship, but not all calibration curves are linear). The calibration curve can then be used to find the concentration of solid in an unknown solution simply based on experimentally measuring the density of the solution. Experiment Overview The purpose of this experiment is to determine the percent sugar content in beverages. The density of five reference" solutions will be determined in Part A. The reference solutions contain known amounts sugar " of sugar (0-20%). Their densities will be plotted on a graph to obtain a calibration curve of density versus nt sugar concentration. In Part 8, the densities of two beverages will also be determined, and the The results will be compared against the information provided on the nutrition labels for these beverages 1. if the following mass and volume data are used to calculate the density of solution, how many cal libration curve, created from the data in Part A, will be used to find the percentage of sugar they contain. Pre-Lab Questions significant figures are allowed in the calculated density? Mass of solution 12.53 g: volume of solution = 8.27 mL Calculate the density of the solution described in Question #1 (Hint: This is a 2-step problem. Then calculate the percent sugar in the beverage.) According to its nutrition label, orange soda 2. 3. First, use the density to convert the 355-mL serving size to grams. Lab: Percent Sugar Content of Beverages

Seperation lab: Will rate question

Separation lab - will choose best answer

Seperation lab: will choose best answer

Separation of a Mixture Laboratory

In this experiment we will separate the different components of a mixture made up of sand (SiO2) and sodium chloride (NaCl, commonly known as salt). Both of these compounds are solid white crystals, so it is difficult to tell them apart with the naked eye. However, each component exhibits different physical properties that can be used to separate one from the other. There are several physical separation techniques that can be used to determine the percent composition of the original mixture.

Materials & Apparatus:

Sand/salt mixture provided in your Lab Kit

2 - Erlenmeyer Flasks

Scale

Water

Graduated Cylinder

Background:

It is important to know how to separate mixtures because many reactions carried out in the laboratory produce mixtures of different compounds. It is often necessary to separate the components of these mixtures, which can be done using several techniques. We will explore a few of these techniques: sublimation, filtration, evaporation and decantation.

Sublimation is the process of a substance passing from the solid to the gaseous state without first passing through the liquid state. Not all substances possess this characteristic. In fact, most substances to NOT sublime under normal conditions, but must be placed under low pressure and low temperature. Ammonium chloride (NH4Cl) and iodine (I2) are both substances that do sublime under normal conditions.

Filtration is the process used to separate the components of a mixture of solid substances that differ in solubility in a certain solvent. You can separate a mixture of solid substances by adding a liquid to the original mixture in which only some of the components of the mixture will dissolve. The resulting mixture, which contains both the dissolved and undissolved substances, is then poured through a filter paper--a porous paper that allows liquids to pass through while retaining any solids. The liquid that has passed through the filter paper is called the filtrate; the solid on the paper is the residue.

Evaporation can also be used to separate the solvent from the solution. A solution can be slowly heated in an Erlenmeyer flask, and the solute will remain after the solvent has evaporated.

Decantation is the process of separating a liquid from a solid (sediment) by gently pouring the liquid from the solid so as not to disturb the solid.

For this experiment, a practical plan is as follows: First combine the solid mixture of the two compounds, sodium chloride (NaCl) and sand (SiO2), with water. This will dissolve the sodium chloride. The sand will not dissolve into the water. We will "filter" the entire mixture, which allows the water in which the sodium chloride is dissolved to pass through, but not the sand. We will now have separated the sodium chloride and the sand. Then, we must evaporate off the water so that we weigh only the two original solids and not the water we added.

Procedure:

(NOTE: Do NOT dispose of any part of your lab until you are 100% positive you do not need it again. It is good practice to keep all parts of your lab until you are finished.)

Record the letter (A, B, C, or D) of your mixture (on the bag contents label) on the line above Data Table 1 below.

Obtain an Erlenmeyer flask [label it 1] and weigh and record the mass.

Add the entire contents of your unknown mixture bag to the flask and weigh and record the mass of the Erlenmeyer flask and the mixture.

Add 10 mL of water (preferably distilled) to the solid in the Erlenmeyer flask [Erlenmeyer flask 1] and stir gently for 5 minutes.

Weigh a new clean, dry Erlenmeyer flask [Erlenmeyer flask 2].

Decant the liquid from Erlenmeyer flask 1 into Erlenmeyer flask 2. This may work better if you place a utensil against the lip of the pouring flask to encourage a slow steady stream of liquid into the second flask.

Add another 10 mL of water to the solid in Erlenmeyer flask 1, stir for 1-2 minutes, and decant this liquid into the Erlenmeyer flask 2 as before.

Repeat with still another 10 mL of water. This process extracts (dissolves) the soluble sodium chloride from the insoluble sand.

Allow the two flasks to dry. Let them dry until the sand appears dry and freely moves when you shake the Erlenmeyer flask a little and the sodium chloride looks dry.

To speed up the process, you can heat the flasks slowly over a burner set on low on your stove top or in the oven (set at 125-200ËF). I would suggest heating it on top of another pan (NOT nonstick coated) Use a low setting and watch closely as you donât want it to boil over.

Allow the Erlenmeyer flasks to cool to room temperature (if they were heated) and weigh the Erlenmeyer flasks and their contents separately. Record their masses in the appropriate sections of the table.

To ensure that there is no water remaining, heat for another 5-10 minutes oven or 1-2 minutes on the stove. Allow to cool to room temperature and reweigh the Erlenmeyer flask. If it is within 0.3 g of your initial weighing you can stop. If the second weighing is not within 0.3 g of your initial weighing, reheat again, cool, and reweigh. The difference between this mass and the mass of the empty Erlenmeyer flask is the mass of NaCl.

Unknown Mixture Label (A, B, C, or D) ___________

Data Table 1

Measure or calculate and record the following (in grams):
mass of the empty Erlenmeyer flask 1:
mass of the Erlenmeyer flask 1 plus the mixture sample:
mass of the mixture sample:
mass of the Erlenmeyer flask 1 and the remaining contents after drying of sand:
mass of Erlenmeyer flask 1 and dry sand (2nd weighing)
Subtract (a) from (e) to obtain the mass of sand in the sample:
Measure or calculate and record the following (in grams):
mass of an empty Erlenmeyer flask 2:
mass of Erlenmeyer flask 2 and dry NaCl (1st weighing)
mass of Erlenmeyer flask 2 and dry NaCl (2nd weighing)
mass of Erlenmeyer flask 2 and dry NaCl (3rd weighing) if necessary
measured mass of dry NaCl:

Assignment Questions (all work must be shown for all calculations):

Using the results of your lab, complete all the questions below.

Upload one picture that is representative of your experiment with this report to the appropriate D2L Brightspace Assignments folder.

Complete Data Table 1 located in the Procedure. Make sure to include all your work for all the calculations performed.

The amount of sodium chloride in the original mixture may also be determined indirectly by subtracting the SiO2 mass from the initial sample mass. Calculate the expected mass of NaCl using this method.

Calculate the percent difference of NaCl (Note: This is not % Error, but it is a similar calculation. This is an error calculation that checks precision between the results of the two methods from the following equation: (Note: the unit for this calculation is â% differenceâ)

% difference=measured mass-mass by subtractionmass by subtraction x 100

What is the mass percent of each component in your mixture: SiO2, and NaCl? (Note: the units for this calculation are â% SiO2â and â% NaClâ)

mass percent=mass of componenttotal mass of sample x 100

Error Analysis: Was your % difference from Assignment Question 4 within 10%? Why or why not? Did your two mass percentages in Assignment Question 5 add up to 100%? Why or why not? What were your biggest sources of error in this experiment? What would you do differently if you were to repeat this experiment? Explain.

What type of properties (physical or chemical) are we using to separate the mixture in this laboratory. Explain your answer.

A mixture is found to contain 0.69 g SiO2, 1.05 g of cellulose, and 2.17 g of calcium carbonate. What is the mass percentage of SiO2 in this mixture?

Assume you have a mixture of NH4Cl, sand, and salt and access to a regular chemistry laboratory. How would you separate the three?Write out what your procedure would be in numbered steps. Please research the answer to this question and properly cite your source. It is alright to research using the internet. However, Wikipedia, Yahoo Answers, Ask.com, and other non-scientific sources cannot be used.