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AP Chemistry Summer Assignment

WARNING: AP Chemistry is an ADVANCED PLACEMENT course that will give you the experience of a college course during your high school career. It is the equivalent of taking a full year of a college course at a university.

DO NOT continue with AP CHEM if any of the following criteria apply to you (Be Honest):

• Don’t care about passing the AP Exam

• Don’t have a strong work ethic

• Don’t study or complete assignments on time

• Not willing to seek additional help outside of class when needed

• Not able to handle feeling frustrated with difficult concepts

• Don’t fully read instructions/directions/text

• Cannot manage or prioritize your time

• Not interested in attending college

• Not willing to put in late hours, sacrifice social activities, etc. to succeed

• Blame others for areas that you fail in, do not take ownership of your mistakes

• Not willing/able to seek out/learn information that I do not know on your own

❖ This is not meant to discourage you from challenging yourself with this AP course, but a reality check of the hard work and dedication that will be required of you to succeed.

So Why Summer Work?

This class covers a full year of chemistry at a university.  Let's take a look at an example.  At my college (Cal Poly) Chemistry 127,128, and 129 meets for 3hrs/week for lecture and 3hrs/week for lab.  Each quarter is 10 weeks long (not including finals) so that is 90 hours of lecture and 90 hours of lab for a total of 180 hours in class.

At Laurel High School we start the first week in August and the AP test is on the first Monday in May.  That is 33 weeks not including winter and spring break.  We meet for 4 hours per week (assuming we don't lose time to assemblies, bad weather, holidays, etc. - which we do).  That is a total of 125 hours in class.

The difference is ~55 hours less time – to cover the same amount of material; that has to be made up during the summer, at home, on Saturdays, and during breaks via homework assignments, studying, projects, etc.

CONSEQUENCES for not COMPLETING the summer assignment

- If this is not turned in fully completed by the 1st day of school at the beginning of the AP Chem class period you will be dropped from the course and will have to change your schedule.

- You are expected to have a firm understanding of this material from the first day of school. These topics will be quickly reviewed then used at a deeper, more complex level. We don’t have time for me to teach it to you.

- If you struggle greatly with this assignment you may want to rethink taking this course.

- This assignment will take time to complete, it cannot get done the day or even just the week before school starts.

TO REMAIN IN AP CHEM…

- If you complete this assignment you are still not guaranteed to remain in AP CHEM

- To show that you thoroughly understood the topics in the assignments and are capable of succeeding you must earn a minimum score on the pre test that will be given the first week of school. Those who do not pass with the minimum required score will be dropped from AP CHEM and have to change their schedule.

ATTITUDE IS EVERYTHING!

As I have explained AP CHEM is a tough, challenging course, but it can also be a fun, exciting course that will better prepare you for your college career. The more you are prepared and putting forth effort to comprehend the material the more we can do to enjoy it such as labs, activities, and special projects.

REQUIRED MATERIALS: Paper, pencil, periodic table, calculator, computer/internet access

NO COPYING: if any plagiarized work is used, you will be immediately dropped from the course.

AP CHEM SUMMER ASSIGNMENT CHECKLIST:

READ ALL DIRECTIONS CAREFULLY – it is your responsibility to read and complete all directions as stated. If you skim directions and do something wrong, that is on you!

← PART 1: MEMORIZATION

o Symbols and Names of Elements #1-90

o Polyatomic Ions: formulas, names, and their charges

← PART 2: VIDEO NOTES

Video Notes will be a key component of class – you must WATCH THE VIDEO TO LEARN THE MATERIAL – not just mindlessly write down information.

There will be quizzes on video content.

This allows me to save time in class explaining concepts, and gives you more time to practice skills with my guidance and complete more labs.

o These videos will also help you with part 3

o Use the Cornell Note Taking Style

o hooperslab. Courses(AP Chemistry ( AP Assignments Scroll Down to Summer Assignment

← PART 3: CHEM 1 REVIEW WORKSHEETS (some of the videos from part 2 will help with part 3)

o 1. General Skills

o 2. Basic Math Concepts

o 3. Atoms and the Periodic Table

o 4. Reactions: Types, balancing, net ionic

o 5. Atomic and Molecular Masses and the Mole

o 6. Chemical Equations and Calculations

o 7. Limiting Reactants and Theoretical Yield

o 8. Solutions, Concentration, and Stoichiometry

o 9. Acids & Bases

o 10. Personal Statements

RESOURCES IF YOU NEED HELP/REVIEW/EXAMPLES:

Don’t just say “I don’t know how to do this”, FIGURE IT OUT!

• Videos (search by topic on YouTube): Example: “Khan Academy Acids and Bases”

o Bozeman Science

o Tyler Dewitt

o Khan Academy

o Brightstorm

• Textbook

o Use index to look up location of the material

• Google

o Search topic for how to's

o Search for worksheets for examples/more practice

• Contact me

o Email me: rhooper@ (I should get back to you in a day or two)

o Phone: 601-340-4044

YOU HAVE TO BE SIGNED UP FOR REMIND VIA TEXT MESSAGE OR EMAIL

BY FRIDAY MAY 19TH!

[pic]

PART 1: MEMORIZATION

|Name |Sym | | |

|NO3- |nitrate |ClO4- |perchlorate |

|NO2- |nitrite |ClO3- |chlorate |

|CrO42- |chromate |ClO2- |chlorite |

|Cr2O72- |dichromate |ClO- |hypochlorite |

|CN- |cyanide | | |

|SCN- |thiocyanate |IO3- |iodate |

|MnO4- |permanganate |IO2- |iodite |

|OH- |hydroxide | | |

|O22- |peroxide |CHO2- |formate |

|NH2- |amide |BrO3- |bromate |

|SO42- |sulfate |BrO2- |bromite |

|SO32- |sulfite | | |

|PO33- |phosphite |CO32- |carbonate |

|PO43- |phosphate |HCO3- |hydrogen carbonate |

|HPO42- |hydrogen phosphate |HSO4- |hydrogen sulfate |

|H2PO4- |dihydrogen phosphate |HSO3- |hydrogen sulfite |

|C2H3O2- or |acetate |HS- |hydrogen sulfide |

|CH3COO- | | | |

| | |NH4+ |ammonium |

Name: ________________________________

PART 3

Don’t just say “I don’t know how to do this”, FIGURE IT OUT!

DIRECTIONS: For each problem below show your work. Always use units and box your final answer.

Attach all additional papers with any work shown, clearly numbered.

Anything you get stuck on you can review online via these YouTube channels just type in the topic

Example: “Tyelr dewitt stoichiometry”:

- Khan Academy - Brightstorm - Tyler Dewitt - Bozemann Science

AP Chemistry Worksheet 1: General Skills

1. Round each of the following numbers to four significant figures, and express the result in scientific notation:

a. 300.235800 _______________ c. 0.006543210 _______________

b. 456,500 _______________ d. 0.000957830 _______________

2. Carry out the following operations, and express the answers with the appropriate number of significant figures:

a. 1.24056 + 75.80 _______________ c. 23/67 - 75 _______________

b. 890,000 x 112.3 _______________ d. 78,132 / 2.50 _______________

3. Convert the following to either scientific or standard notation

a. 0.0000532 _______________ c. 6,709,000 _______________

b. 9.23x10-5 _______________ d. 4.44x104 _______________

4. Perform the following conversions: (You need to go online to look up some conversion factors between metric and English units.)

a. 8.60 mi to m _______________ c. 3.00 days to s _______________

b. $1.55/gal to dollars per liter _______________ d. 75.00 mi/hr to m/s _______________

VIDEO NOTES!

5. The density of pure silver is 10.5 g/cm3 at 20oC. If 5.25 g of pure silver pellets are added to a graduated cylinder containing 11.2 mL of water, to what volume level will the water in the cylinder rise? (Water: 1 mL= 1 cm3)

6. The density of air at ordinary atmospheric pressure and 25oC is 1.19 g/L. What is the mass, in kilograms, of the air in a room that measures 12.5 x 15.5 x 8.0 ft?

AP Chemistry Worksheet 2: Basic Math Concepts

Literal/Linear Equations

1. Solve A = P + Prt for t. 4. Solve 3x – 4y = 12 for y.

2. Solve 2(a-c) = 4a for a 5. Solve cx-d = a( x – y ) for y.

3. Solve [pic] = 3a – 2x for x 6. Solve 3x – 2a = 7a for x

Substitution (solve for the missing variable)

7. 2x + 8y = 20 y = 2 10. x = 5 2x + y = 10

8. 5x – 2y = 3 y = 2x 11. 2y + x = -15 x = 3y

9. 2x – 8y = 6 y=-7 - x 12. x = 2y – 1 3x – 2y = -3

Graphing

. Graph the following information in a LINE graph. Label and number the x and y-axis appropriately.

|# of Days |# of Bacteria |

|1 |4 |

|2 |16 |

|3 |40 |

|4 |80 |

|5 |100 |

|6 |200 |

1. What is the independent variable?

2. What is the dependent variable?

3. What is an appropriate title?

Solve each equation for y and then graph each equation.

4. 6x + 7 = -14y

a. Determine the x itnerecept

b. Determine the y intercept

c. What is x when y = 19.5

d. What is y when x = 0.0043

AP Chemistry Worksheet 3: Atoms and the Periodic Table

1. Fill in the gaps in the following table, assuming each column represents a neutral atom:

|Symbol |3919K | | | | |

|Protons | |25 | | |82 |

|Neutrons | |30 |64 | | |

|Electrons | | |48 |56 | |

|Mass # | | | |137 |207 |

2. Give the name and the common charge for elements found in each of these groups of the Periodic Table:

a) Group 1 (b) Group 2 (c) Group 7 (17) (d) Group 8 (18)

3. Describe where each type of element is found on the periodic table

(a) Metals (b) Nonmetals (c) Transition metals

4. Give the name for each of the following ionic compounds:

a. AlF3

b. Fe(OH)2

c. Cu(NO3)2

d. Ba(ClO4)2

e. Li3PO4

f. Hg2S

g. Ca(C2H3O2)2

h. Cr2(CO3)3

5. Write the chemical formula for each of the following compounds:

i. copper (I) oxide l. potassium peroxide o. aluminum hydroxide

j. zinc nitrate m. mercury (I) bromide p. iron (III) carbonate

k. sodium hypochlorite n. nickel (III) acetate q. calcium phosphide

6. Give the name or chemical formula, as appropriate, for each of the following acids:

l. HBrO3

r. HBr

s. H3PO4

t. hypochlorous acid

u. iodic acid

v. sulfurous acid

7. Give the name or chemical formula, as appropriate, for each of the following molecular substances:

w. SF6 z. IF5 bb. XeO3

x. dinitrogen tetroxide aa. hydrogen cyanide cc. tetraphosphorous hexasulfide

8. Rank each of the following in order of INCREASING ionization energy

a. O, S, Ge b. C, Pb, F c. Be, Ba, B

9. Rank each of the following in order of DECREASING atomic radius

a. Cl, Br, Ga b. Ne, Rn, Pb c. Ca, Rb, C

10. Rank each of the following in order of DECREASING electronegativity

a. As, Se, Sn b. Xe, Ru, Hf c. Sb, N, He

AP Chemistry Worksheet 4: Reactions: Types, balancing VIDEO NOTES!

Write the balanced chemical equation for each reaction given below. Remember the diatomics!

a. Zinc carbonate can be heated to form zinc oxide and carbon dioxide

b. On treatment with hydrofluoric acid, silicon dioxide forms silicon tetrafluoride and water.

c. Sulfur dioxide reacts with water to form sulfurous acid.

d. Liquid butane fuel (C4H10) burns in the presence of oxygen gas.

e. Perchloric acid reacts with cadmium to form cadmium perchlorate and a gas.

f. A solution of sodium bromide reactions with a solution of vanadium (III) nitrate to form a brightly colored precipitate.

1. Please complete the following reactions, balance and show the total ionic and net ionic forms of the equation:

a. AgNO3 (aq) + KCl (aq) ( AgCl (s) + KNO3 (aq)

b. strontium bromide (aq) + potassium sulfate (aq) ( strontium sulfate (s) + potassium bromide (aq)

c. Mg(NO3)2 (aq) + Na2CO3 (aq) ( MgCO3 (s) + NaNO3 (aq)

d. chromium(III) nitrate (aq) + iron(II) sulfate (aq) ( chromium(III) sulfate (aq) + iron(II) nitrate (aq)

2. Predict the products for the following reactions, balance the equation, then classify the type of reaction:

a. ____ Na + ____ FeBr3 (

b. ____ NaOH + ____ H2SO4 (

c. ____ C2H4O2 + ____ O2 (

d. ____ NH3 + ____ H2O (

e. ____ PbSO4 + ____ AgNO3 (

 

AP Chemistry Worksheet 5: Atomic and Molecular Masses and The Mole

For each problem below, write the equation and show your work. Always use units and box in your final answer.

1. Determine the molar mass of each of the following compounds:

a. N2O5 FeCO3 Ca(C2H3O2)2 (NH4)3PO4

b. sodium nitrate copper (II) sulfate disilicon hexabromide

2. Calculate the percentage by mass of oxygen in the following compounds:

a. NO2 b. CH3COOCH3 c. Cr(NO3)3 d. (NH4)2CO3

3. The molecular formula of aspartame, the artificial sweetener marketed as NutraSweet, is C14H18N2O5.

a. What is the molar mass of aspartame?

b. How many moles of aspartame are present in 1.00 mg of aspartame? (1000 mg = 1g)

c. How many molecules of aspartame are present in 1.00 mg of aspartame?

d. How many hydrogen atoms are present in 1.00 mg of aspartame?

4. A sample of glucose, C6H12O6, contains 2.03 x 1021 atoms of carbon.

e. How many atoms of hydrogen does it contain?

f. How many molecules of glucose does it contain?

g. How many moles of glucose does it contain?

h. What is the mass of the sample in grams?

5. Calculate the following amounts:

i. How many moles of chloride ions are in 0.0750 g of magnesium chloride?

j. What is the mass, in grams, of 3.50 x 10-3 mol of aluminum sulfate?

k. What is the mass, in grams, of 1.75 x 1020 molecules of caffeine, C8H10N4O2?

l. What is the molar mass of cholesterol if 0.00105 mol weigh 0.406 g?

For each problem below, write the equation and show your work. Always use units and box in your final answer.

VIDEO NOTES!

1. Determine the empirical formula of each of the following compounds if a sample contains

a. 0.104 mol K, 0.052 mol C, and 0.156 mol O

b. 5.28 g Sn and 3.37 g F

c. 87.5 percent N and 12.5 percent H by mass

2. What is the molecular formula of each of the following compounds?

a. empirical formula CH2, molar mass = 84 g/mol

b. empirical formula NH2Cl, molar mass = 51.5 g/mol

3. Determine the empirical and molecular formulas of the following substance:

a. Ibuprofen, a headache remedy contains 75.69 percent C, 8.80 percent H, and 15.51 percent O by mass; molar mass about 206 g

4. any homes in rural America are heated by propane gas, a compound that contains only carbon and hydrogen. Complete combustion of a sample of propane produced 2.641 g of carbon dioxide and 1.442 g of water as the only products. Find the empirical formula of propane. (Hint: Figure out how many moles of C and H were produced. They all came from the fuel.)

5. (This is probably the hardest problem in the whole packet!) Menthol, the substance we can smell in mentholated cough drops, is composed of C, H, and O. A 0.1005 g sample of menthol is combusted, producing 0.2829 g of CO2 and 0.1159 g of H2O.

a. What is the empirical formula for menthol?

b. If the compound has a molar mass of 156 g/mol, what is its molecular formula?

AP Chemistry Worksheet 6: Chemical Equations and Calculations

1. Why is it essential to use balanced chemical equations in solving stoichiometry problems?

2. The fermentation of glucose, C6H12O6, produces ethyl alcohol, C2H5OH, and CO2 as shown here:

C6H12O6 (aq) --> 2 C2H5OH(aq) + 2 CO2 (g)

a. How many moles of CO2 are produced when 0.300 mol of C6H12O6 reacts in this fashion?

b. How many grams of C6H12O6 are needed to form 2.00 g of C2H5OH?

c. How many molecules of CO2 form when 2.00 g of C2H5OH are produced?

3. Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide.

a. Write the balanced chemical equation for this reaction.

b. How many grams of aluminum hydroxide are obtained from 10.5 g of aluminum sulfide?

4. Automotive air bags inflate when sodium azide, NaN3, rapidly decomposes to its component elements:

2 NaN3 (s) --> Na(s) + 3 N2 (g)

a. How many moles of N2 are produced by the decomposition of 1.50 moles of NaN3?

b. How many grams of NaN3 are required to form 5.00 g of nitrogen gas?

c. How many grams of NaN3 are required to produce 10.0 L of nitrogen gas if the gas has a density of 1.25 g/L?

5. A piece of aluminum foil 0.550 mm thick and 1.00 cm square is allowed to react with bromine to form aluminum bromide.

a. How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

b. How many grams of aluminum bromide form, assuming that the aluminum reacts completely?

AP Chemistry Worksheet 7: Limiting Reactants & Theoretical Yield VIDEO NOTES!

1. A manufacturer of bicycles has 50 wheels, 30 frames, and 24 seats.

a. How many bicycles can be manufactured using these parts?

b. How many parts of each kind are left over?

c. Which part is like a limiting reactant in that it limits the production of bicycles?

2. The fizz produced when an Alka-Seltzer tablet is dissolved in water is due to the reaction between sodium

bicarbonate, NaHCO3, and citric acid, H3C6H5O7:

3 NaHCO3 (aq) + H3C6H5O7 (aq) --> 3 CO2 (g) + 3 H2O(l) + Na3C6H5O7 (aq)

In a certain experiment 1.00 g of sodium bicarbonate and 1.00 g of citric acid are allowed to react.

a. Which reactant is the limiting reactant? You must show work to support your answer.

b. How many grams of carbon dioxide form?

c. How much of the limiting reactant is left when the reaction is complete?

d. How much of the excess reactant remains after the reaction is complete?

3. When hydrogen sulfide gas is bubbled into a solution of sodium hydroxide, the reaction forms sodium sulfide and water. How many grams of sodium sulfide are formed if 2.50 g of hydrogen sulfide is bubbled into a solution containing 1.85 g of sodium hydroxide, assuming that the limiting reagent is completely consumed?

4. Solutions of sulfuric acid and lead (II) acetate react to form solid lead (II) sulfate and a solution of acetic acid. If 10.0 g of sulfuric acid and 10.0 g of lead (II) acetate are mixed, calculate the number of grams of sulfuric acid, lead (II) acetate, lead (II) sulfate, and acetic acid present in the mixture after the reaction is complete.

5. A student reacts benzene, C6H6, with bromine, Br2, to prepare bromobenzene, C6H5Br, and HBr.

a. What is the theoretical yield of bromobenzene in this reaction when 30.0 g of benzene reacts with 65.0 g of bromine?

b. If the actual yield of bromobenzene was 56.7 g, what was the percent yield?

AP Chemistry Worksheet 8: Solutions, Concentration, and Stoichiometry

Concentration (Molarity)

1. Calculate the molarity of 0.060 moles NaHCO3 in 1500. mL of solution.

2. What is the molar concentration of 1.0 mol of KCl dissolved in 750. mL of solution?

3. Calculate the molarity of 29.25 grams of NaCl in 2.0 liters of solution.

4. Calculate the molarity of 34.2 grams of sugar, C12H22O11 in 500. mL of solution.

5. Calculate the number of grams of NaCl contained in 0.500L of a 1.5M solution.

Dilutions VIDEO NOTES!

6. If I add 25 mL of water to 125 mL of a 0.15 M NaOH solution, what will the molarity of the diluted solution be?

7. If I add water to 100 mL of a 0.15 M NaOH solution until the final volume is 150 mL, what will the molarity of the diluted solution be?

8. How much 0.05 M HCl solution can be made by diluting 250 mL of 10 M HCl?

9. I have 345 mL of a 1.5 M NaCl solution. If I boil the water until the volume of the solution is 250 mL, what will the molarity of the solution be?

Solution Stoichiometry (These will be tough, but take your time and think it through…) VIDEO NOTES!

10. Calculate the number of mL of 2.00 M HNO3 solution required to react with 216 grams of Ag according to the equation.

3 Ag(s) + 4 HNO3(aq) ---------> 3 AgNO3(aq) + NO(g) + 2 H2O(l)

11. Calculate in mL the volume of 0.500 M NaOH required to react with 3.0 grams of acetic acid. The equation is:

NaOH(aq) + HC2H3O2(aq) -------> NaC2H3O2(aq) + H2O(l)

12. Calculate the number of grams of AgCl formed when 0.200 L of 0.200 M AgNO3 reacts with an excess of CaCl2. The equation is:

2 AgNO3(aq) + CaCl2(aq) -------> 2 AgCl(s) + Ca(NO3)2(aq)

13. Calculate  the mass of AgCl formed when an excess of 0.100 M solution of NaCl is added to 0.100 L of 0.200 M AgNO3.

14. Calculate:

a. the mass of BaSO4 formed when excess 0.200 M Na2SO4 solution is added to 0.500 L of 0.500 M BaCl2 solution, and

b. the minimum volume of the Na2SO4 solution needed to precipitate the Ba2+ ions from the BaCl2 solution.

15. A sample of impure sodium chloride weighing 1.00 grams is dissolved in water and completely reacted with silver nitrate solution. The dried precipitate of AgCl has a mass of 1.48 grams . Calculate the percentage of NaCl in the original impure sample.

AP Chemistry Worksheet 9: Acids and Bases VIDEO NOTES!

What are the conjugate bases and acids of following?

|original acid |conjugate base |original base |conjugate acid |

|HNO3 |  |OH- | |

|H2O |  |H2O | |

|H3O+ |  |HCO3- | |

|H2SO4 |  |SO42- | |

|HBr |  |ClO4- | |

1. Calculate the [H+] in a solution in which [OH-] = 2.0 x 10-2 M. Is this solution acidic, neutral, or basic?

2. Calculate the [OH-] in a solution in which [H+] = 3.99 x 10-5 M. Is this solution acidic, neutral, or basic?

3. Convert each of the following into pH. Identify each as an acidic, neutral, or basic.

a. 0.0015 M H+

b. 5.0 x 10-9 M H+

c. 3.27 x 10-4 M OH-

d. 1.00 x 10-12 M OH-

4. Convert each of the following into pOH. Identify each as an acidic, neutral, or basic.

a. 0.783 M OH-

b. 6.87 x 10-12 M OH-

c. 1.1 x 10-9 M H+

d. 0.0032 M H+

9. What is the pH, pOH, [H+], or [OH-] for a 0.156 molar solution of hydrochloric acid?

10. What is the pH, pOH, [H+], or [OH-] for a 3.2 molar solution of sodium hydroxide?

11. What is the pH, pOH, [H+], or [OH-] for a 0.92 molar solution of sulfuric acid?

12. Calculate the volume of 0.300 M HCl needed to titrate 75.00 mL of 0.1500 M KOH.

Personal Statement

1. Write a paragraph to tell me about your Chemistry experience. What did you like and dislike? What were you good at and not so good at? What teaching and learning techniques work well for you?

2. Write another paragraph to tell me about your hopes for AP Chemistry. What made you decide to take this class? How much effort are you willing to give to the class? What do you hope to take away from it?

AP CHEMISTRY FRAME OF MIND CHECK

Write a 2-3 sentence response to each statement about what it means and how you can apply it to how you have approached lasses and what changes you can make in the future (for this class and preparing for college).

3. Until you stop doing homework for the sake of a grade and START attacking assignments with the intent to learn and understand the material you will struggle and suffer through advanced courses. Learning will continue to be a chore whether than a valuable experience and privilege.

4. Students who attack a class for the sake of learning and not for a grade have a better understanding and perform better on assessments which results in better grades. They understand it won’t be easy, they understand it will be difficult and require more of them. However they do not let that stop them and use excuses.

5. These students aren’t satisfied with just a right answer they want to KNOW WHY each answer is correct. They view their instructor as a valuable resource in learning the material BUT they do not view their instructor as the ONLY resource.

6. These students don’t spend only 30 minutes on a topic and then say, “Oh well, I either got it or I didn’t.” They reevaluate their time to understand the topic. You won’t understand every little detail of every topic, but you must have a firm foundation to build on and go somewhere. Without it you are guaranteed to go nowhere.

7. These students will look at all practice problems (assigned or not), attempt each to the best of their ability; review the answers to understand the topic (not just see what the answer was). They will seek out additional help ON THEIR OWN TIME to get further assistance and understanding.

8. No matter what strategies your instructor uses if you are going to accept mediocrity even though you are capable of more, then your grades and performance will reflect your choice.

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@lhsapchem

lhsapchem@mail.

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