Quick Blog Question

Quick Blog Question

In this lab, we will be making graphs to compare graphs and look for regularities or patters among the values. Any major irregularity in the data may suggest problem related to the water factor being evaluated. Group hydrogen will find an explanation or scenario that accounts for the observed data and for the resulting Riverwood fish kill.

1SCS 9-19 p.

1SCS 9-19 p. 82-83

9. 11 grams of sugar, 44 grams of water

10. 15, 000 ppm

11. What makes a water molecule polar is that oxygen is more electronegative than is hydrogen; thus, electrons are partially pulled away from the two hydrogen atoms toward the oxygen atom. This results in a polar molecule.

12.

13. a. Oxygen molecule
      b. Hydrogen molecules

14. Heavy metals are called heavy are because their atoms have greater masses than those of essential metallic elements.

15. The effects of heavy-metal poisoning are damage to the nervous system, brain, kidneys, and liver, which can even lead to death.

16. Lead: in paint, cooking vessels
     Mercury: "silent" light switches, medical and weather thermometers

17. Sodium hydroxide is found in many bases.

18. Most acids are made up of molecules including one or more hydrogen atoms.

19. a. basic
      b. basic
      c. acidic
      d. chemically neutral

Practice Questions For Review

Practice Questions For Review

1. pH: an expression of the acidic or basic character of a solution: at 25 ^oC, solutions with pH values lower than 7 are acidic, solutions above 7 are basic, and neutral solutions equal 7; pH is based on a solution's hydrogen ion (H^- or H₃O⁺ ) concentration. 1 vinegar acid, 7 water, 9 ammonia base pg. 70
2. 100 km/hr : 100,000m/360,000,000s
3. 905 mg: King Henry died unusually drinking chocolate milk .000905 kg
4. Electrons: a particle possessing a negative electrical charge; electrons surrounding the nuclei of atoms. Barely weighs anything. Protons: a particle possessing a positive electrical charge that is found in the nuclei of all atoms; the total protons in an element's atom equal its atomic number. Weighs the same as a neutron. Neutrons: a particle without electrical charge; found in the nucleus of an atom. Weighs the same as a proton.
5. Cation is positively charged. Anion is negatively charged. Loosing or gaining an electron.
6. The first column of the tends to lose one electron and have a positive charge. (Na, K, Rb)
7. The second column of the periodic table tends to lose 2 electrons and have a positive charge. ( Mg, Ca, Sr)
8. The sixth column of the periodic table tends to gain 2 electrons and have a negative charge. (O, S, Se).
9. The seventh column of the periodic table tends to gain 1 electrons and have a negative charge. ( F, Cl, Br.)
10. The eighth column of the periodic table tends to not loose or gain any electrons and has a neutral charge. Noble gases. ( He, Ne, Ar).
11. Negative ions: Cl, O; Positive ions: H, K
12. Atom : composed of electrons, protons, and neutrons
13. There is always dissolved minerals and gasses 
14. Heating the water, under pressure
15. K⁺ + I^-= KI        Ba²⁺ + OH^_ = Ba (OH)₂           Al³⁺ +O² = Al₂O₃
16. Cd, 80 atomic number, 200 atomic weight, 120 neutrons, 80 protons, 80 electrons
17. Unsaturated solution is a solution that contains less dissolved solute than the amount the solvent can hold at a specific temperature while a saturated solution has as much dissolved solute that it can hold at a specific temperature.
18. While the water is heated keep adding salt, and then cool it
19. Define the following terms.
20. Chroline and ozone are added to kill bacteria. 
21. MgCl_2: Magnesium has +2 charge so Cl- needs 2. 
22. Ph
23. H: 1
    Mg: 12
    Na: 11
    Cl: 17
24. The temperature was not high enough. It was saturated. Not enough pressure.
25. If a solution exhibits the Tyndall effect what kind of solution is it.

Quick Blog Question

Quick Blog Question

You take the mass of the solute and divide it by the mass of the solution. To get the percentage, you multiply by a 100. The tricky part is learning how to do find the percent of mass.

C.5 1-3

 C.5 1-3

1. a. The solution would become super saturated because the solution was cooled, and because the solution contained more KCl than it contain at a lower temperature.

b.

2. a. 

20g

3.

Diagram b. is diluted so the molecules are more spread out and less saturated than diagram a.

Quick Blog Question

Quick Blog Question

I look at the models and compare how to set up the equations based on the question.

1SCS 1-8 p. 82

1. Three teaspoons of sugar will completly dissolve in a serving of hot tea,  but will not in an equally sized serving of iced tea because as the temeperature rises more solutes are present and can be dissolved.

2. about 132 g

3. a. 200 g
    b. 7000 g
    c. 1892 g

4. a. NaCL, KCl, KNO_{3
     b.} KNO_3,  KCl,  NaCL

5. Saturated: a solution in which the solvent has dissolved as much solute as it can retain stably at a specified temperature.
    Unsaturated solution: a solution containing  a lower concentration of solute than a saturated solution contains at a specified temperature.

6. a. 35 g
    b. saturated
    c. 90 g

7. a. If it is unsaturated it will dissolve.
    b. If it is saturated it will precipitate a lot.
    c. If it is super saturated the crystals will add to the precipitate a little.

8. 23%

C.2 1-3 p. 56

1. a. 105 g
    b. 45g

2. a. 20g
    b. 45g

3. a. 150-90= 60 g
    b. 30 g

Lab Report

Water Testing Experiment

June 25, 2013

Dr. Forman

Kourosh

Julia

Clemmy

Abstract: In this lab, group Hydrogen conducted qualitative tests and confirming tests, and we confirmed ions in different solutions by looking at the precipitate. We tested for the presence of iron and calcium cations, as well as chloride and sulfate anions. Our group worked well together, and we assigned each person a task to do, which made the experiment more productive and less strenuous. 

Procedure: 

Calcium Ion Test

1. Place 20 drops of solution into a well of a 24-well wellplate.

1. Add three drop of sodium carbonate
2. Record your observations

1. Decide whether Ca²⁺  cations are present and record your results
2. Repeat for the remaining samples
3. Discard the contents of the well plate as directed by your teacher.

Iron (III) Ion (Fe³⁺) Test

1. Place 20 drops of solution into a well of a 24-well well plate.

1. Add one or two drops of potassium thiocyanate (KSCN) test reagent to the well.
2. Record your observations
3. Decide whether Fe³⁺ cations are present and record your results
4. Repeat for the remaining samples
5. Discard the contents.

Chloride Ion (Cl^-) Test

1. Place 20 drops of solution into a well of a 24-well wellplate.
2. Add three drops of silver nitrate.
3. Record your observations
4. Decide whether Cl^- anions are present.
5. Repeat for the remaining samples
6. Discard of the contents.

Sulfate Ion (SO₄^2-) Test

1. Place 20 drops of solution into a well of a 24-well well plate.
2. Add thee drops of barium chloride test reagent to the well.
3. Record your observations.
4. Decide whether SO₄^2- anions are present and record your results.
5. Repeat for the remaining samples.
6. Discard the contests of the wellplate.

Results

There was always a reaction in the reference solution testing positive for calcium ions in the first experiment, iron ions in the second, chloride ions in the third, and sulfate ions in the fourth. The blanks did not every show a reaction meaning our team Hydrogen did not mix any substances together that shouldn't be mixed.

The class results help us compare results and look for mistakes using each others data. 

ISBS 25-34 p. 51-52

ISBS 25-34 p. 51-52

25. Qualitative tests: Tests that identify the presence or absence of a particular substance in a sample.
      Quantitative tests: They determine the amount of a specific substance present in a sample.

26. A confirming test is a laboratory test giving a positive result if a particular chemical species is present.

27. a. The purpose of using the reference solution was because it is a solution of know composition     used as comparison, and it is known to have the sought ion.
      b. The purpose of using the distilled water blank was because it is known to not contain any ions of interest.

28. No, the student should not conclude that because some ions are too small and won't show a reaction.

29. a. I would use the Tyndall effect to see if particles are showing when I shine a light through it, and I would observe the unknown mixture to see if there a big solids that can be filtered out to decide whether the mixture is a solution, suspension, or a colloid.

      b. Using the Tyndall effect would help me understand if the mixture is a colloid or solution and observing the mixture, would help me understand if the mixture is a suspension.

30. The possible risks are that in medicine, you would not consume the whole medicine, which could have serious affects.

31. It is useful for element symbols to have international acceptance because anyone can understand the element and there would be no confusion.

32.

33. It isn't possible for water to be 100% "chemical free" because the atmospheric gases nitrogen, oxygen, and carbon dioxide will always dissolve in the water to some extent.

34. H₂O is liquid water. It is composed of 2 Hydrogen atoms and 1 Oxygen atom. When the atoms combined they make liquid at room temperature.

Quick Blog Question

Quick Blog Question

I learned what a confirming test is, the difference between qualitative tests and quantitative tests, how chemists detect certain ions in different liquids, the power of teamwork, and how liquids react when ions are present.

Lab Questions 1-4 p. 45

1. The reference solution and the blank were used so we could compare the results, and see how the reference reacted and the blank solution reacted.

2. Some possible problems associated with qualitative tests are that the solution could get contaminated,  and the ion could still be present but not visible.

3. The tests cannot absolutely confirm the absence of an ion because some ions are too small and won't show a reaction.

4. How my observations may have changed is that the results would be contaminated with other liquids, and for example, the blank could react when it is not supposed to.

Quick Blog Question

Testing water helps us because there are some particles that are too small for us to see and other bacteria that can be harmful to us; therefore, it is very important that we test our water.

ISBS 19-24 p.51

19. a. carbon: 6 electrons
      b. aluminum: 13 protons
      c. lead: 82 electrons
      d. chlorine 17 electrons

20. a. sulfur: no
      b. iron: no
      c. silver: yes
      d. iodine: no

21. a. anion
      b. neutral atom
      c. neutral atom
      d. cation
      e. cation

22. a. lost two protons
      b. neither
      c. neither
      d. lost an electron
      e. lost two electrons

23. a. H
      b. Na ¹⁺

      c. Cl ^1-

      d. Al  ³⁺

^{24. a. KI}

       ^b.  Ca²S²

     c. Fe³Br⁺
     d. Ba²OH^{+
       e.} NH₄PO₄^{3+
       f.} Al³O²⁺

Water Diary

Quick Blog Question

What interested me the most the first week was definitely the foul water lab. It was really interesting how we filtered water enough for us to wash our hands with. I will remember what we filtered out from each step and how to draw the filtration apparatus.

ISBS 13-18 p. 50-52

13.

14.  Represent elements: i, ii, iv, and vi
       Represent Compounds: iii, v

15. A chemical formula represent the elements contained in a substance, together with subscripts that indicate the relative numbers of atoms of each element.

16. a. Phosphoric Acid: 3 hydrogen atoms, 1 phosphorus atom, 4 oxygen atoms
      b. Sodium Hydroxide: 1 sodium atom, 1 oxygen atom, 1 hydrogen atom
      c. Sulfer dioxide: 1 Sulfer atom, 2 oxygen atoms

17.

18. a. NaHCO3 + HCl -----> Nacl + H2O+ CO2
      b. C6H12O6+06-----> 6 CO2 + 6 H20

A.7 1-7 p. 20-21

A.7 1-7 p. 20-21

1. 3591 L

2. Me: 485 L

3.

4. 1493 L is the range

5. 600 L is the mean, 579 is the median. I think the average is a better representation because the median is just the number that is in the middle, but the mean calculates the average, which is a more accurate representation of the water use in our class.

6. Our average is 600 L because we have bigger yards, we plants that need a lot of water, and it doesn't rain as often.

7. My daily use of water is close to the national average (370 L) because I personally don't use that much water than the average of the nation.

B.5 1-3 p.33

1.

2. The model represents a heterogeneous mixture because the mixture is not uniform throughout. There are molecules on the top and compounds on the bottom.

3. 

ISBS 1-12 p.50

ISBS 1-12 p.50

1. A physical property is a property  that can be observed or measured without changing the identity of the sample of matter.

2. Three physical properties of water are density, the freezing point, and an aqueous solution.

3. Because ice floats, ice is less dense then liquid water.

4. While at a huge party, I was thirsty and drank water with ice in it, and as I was drinking the water, I thought of all the water vapor around me.

5. Heterogeneous and homogeneous mixtures are different because a heterogeneous mixture is not the same, or uniform throughout, and a homogeneous mixture is uniform throughout.

6. What we will need to know is whether gasoline or water is less dense then another.

7. a. a medicine accompanied by instructions to "shake before using": colloid
    b. Italian salad dressing: suspension
    c. mayonnaise: colloid
    d. a cola soft drink: colloid
    e. an oil-based paint: solution
    f. milk: colloid

8. This demonstrates that the air in the room is a colloid.

9.

Solution: Salt water 

Suspension: Coffee

10. This is a solution because a solution is a homogeneous mixture and you can see a beam of light through the mixture and it is uniform throughout.

11. Substance: an element or a compound; a material with a uniform, definite composition and distinct properties. Ex: an element and compound

12. a. compound
      b. element
      c. compound
      d. element
      e. compound
      f. compound
      g. Element

Quick Blog Question: 

1. Chemistry is, "a science that deals with the composition, structure, and properties of substances and with the transformations that they undergo" Merriam-Webster. Chemistry is important to know because from an educational standpoint, its required by most colleges and universities and it teaches you how to be objective and how to reason and solve problems.  Chemistry also helps you understand the world that you live in and how the objects around you work. It educates you about chemicals and teaches you useful techniques. It makes you a more environmentally educated and a better critical thinker. That is why Chemistry is taught and the pros of taking the course.

Quiz Terms

Matter: anything that occupies space and has mass. Ex: all solids, liquids, and gases

Physical Properties: properties that can be observed and measured without changing the chemical makeup. Ex: density, freezing point of water

Density: the mass of material with a given volume. Ex: density of water is 1.00 g/mL

Freezing point: The temperature at which a liquid turns into a solid; it is the same volume as its melting point. Ex: the freezing point of water is 0°C at normal atmospheric pressure.

Aqueous Solution: a solution in which water is the solvent / water-based solution. Ex: distilled water.

Mixture : a combination of materials in which each material retains its separate identity. Ex: foul water

Heterogeneous Mixture: a mixture that is not uniform throughout. Ex:  coffee grounds settling to the bottom and were not distributed evenly in the foul water. Ex: Suspension

Suspension: a mixture containing large, dispersed solid particles that can settle out or be separated by filtration.  Ex: Water plus coffee grounds and water plus small pepper particles

Tyndall effect: the scattering of a beam of light caused by reflection from suspended particles. Ex: light shined through a sample of purified water

Colloid: a mixture containing solid particles small enough to remain suspended and not settle down. Ex: whole or low fat milk which contains small butterfat particles dispersed in water.

Homogeneous mixer: a mixture that is uniform throughout; a solution

Solution: a homogeneous mixture of two or more substances.

Solute: the dissolved substance. Ex: salt

Solvent: the dissolving agent. Ex water

Unit 1A Vocabulary List

Unit 1A Vocabulary List

Filtration: Solid particles are separated from a liquid by passing the mixture through a material that retains the solid particles and allows the liquid to pass through. 

Filtrate: The liquid collected after it has been filtered.

Percent Recovery: The proportion of sought material recovered in a process.

Histogram: A graph indicating the frequency or number of instances of particular values(or value ranges) within a set of related data.

Range: The difference between the largest and smallest values in a data set.

Average: Adding all the values together and dividing the sum by the total number of values.

Mean: same as average

Median: The middle value.

Electrical Conductivity: The ability to transmit an electric current

Direct Water Use: Water consumed by an end user and can be directly measured. 

Indirect Water Use: Water consumed in the preparation, production, or delivery of goods and services.

Gaseous State: Water vapor in the air.

Liquid State: In lakes, rivers, oceans and clouds

Solid State: Ice

Surface Water: water found on Earth’s surface, such as oceans, rivers, and lakes 

Ground Water: water from an aquifer or other underground source 

Aquifer: a structure of porous rock, sand, or gravel that holds water beneath Earth’s surface

ISAS: pg. 23

3. a. manufacture of the filter paper: This is in indirect use of water because the water used to make the filter paper is water you could not see unless to the factory, people do not usually think of water being used in that way.

b. premoisting of the sand and gravel: This is a direct use of water because when doing the experiment, we directly added water to the sand and gravel, and we were fully aware of the water use.

c. use of water to cool the distillation apparatus: Even though we were aware of the water it did not affect our solution of filtered water so it is an indirect use.

4. To "purify" water is to remove contaminants from water.

5. Three techniques for purifying water is sand filtration, charcoal adsorption and filtration, oil-water separation.

6. Oil was removed from oil-water filtration process. Solid particles were removed from the foul water in the sand-filtration process. Many substances that could give water a bad taste, a cloudy appearance, or an odor was removed in the charcoal adsorption filtration process.

7. The procedure could not because there are still surviving germs in the water. The water needs to be disinfected using disinfecting chemicals and chlorine.


pg. 22

1. Three water uses that I can do without are taking a shower, flushing the toilet, and washing hair.
2. One activity that I cannot do without is drinking water.
3. For taking a shower and watering plants I could reduce my water use. I could take shorter showers and water my plants less.
4. a. Instead of washing the windows at my house, I could wash the windows on the car.
     b. This water would be taking from the window washer container.

Qz: Water from the Foul water lab cannot make suitable drinking water because it still has germs; disinfecting the water by adding disinfecting chemicals and chlorine can make it drinkable.

Lab Report Dirty Experiment

Dirty Experiment

June 18, 2013

Dr. Forman

Kourosh

Julia

Clemmy

Abstract: During our procedure we filtered water in three ways: oil-water separation, sand filtration, charcoal adsorption and filtration. Our group was successful in that we were able to filter enough foul water to a point where it could be used to wash our hands.

Procedure:

       1. Make a data table

       2.  Get 100 mL of foul water

              3. Fill out the first row of data in the chart

       4. Add oil to the water

       5.Let the sample to sit for 1 minute causing to the oil to rise to the top

       6. Remove the oil

      7. Add distilled water to the remove oil

      8. Fill out the second row of data

      9. Dispose of the liquid

      10. Poke holes in the bottom of the disposable cup

      11. Add 1 cm of gravel, 2 cm of sand, 1 cm of gravel

      12.  Gently pour the sample into the cup

      13 Catch the filtrate in a beaker as it pours through

      14. Dispose of the sand and gravel

      15. Place a moist folded piece of paper into the funnel

      16. Place the funnel in a clay triangle supported by a ring with a beaker underneath

       17.  Place one teaspoons of charcoal into the flask, pour the water, then stir

      18. Gently pour the liquid through the paper allowing it to filter through

19. If your filtrate is dark then repeat step 18

20. Record your results

21.  Dispose of the charcoal

Results

The water that we filtered had a salt in it because salt electrically charges a light bulb. From Dr. Forman's demonstration we learned that there are invisible particles in our water, and we did not create pure water.

1. Percent Recovery: 82%

2.  We lost 18mL of foul water

3. We lost 18% of foul water