♫ ♫ ♫ ♫ ♫ ♫ ♫ ♫: 2011

Thursday, September 29, 2011

I hate that I love you so..♥ ♥ ♥

Friday, August 19, 2011

Thousand Thanks

I learned love from you
Watching your caring ways
I learned love from you
In fun-filled yesterdays

You show me how to love and care
Like others that never show'd me well
On how to love and care
and now that I am very well

From you I learned forgiving
Of faults both big and small
I learned what I know about living
From you, as you gave life your all

The example you set is still with me
I'd never want any other
]I'm thankful for all you taught me
And I'm blessed to call you "Mother"

Saturday, June 11, 2011

Wednesday, May 18, 2011

RESSUSCITATING MARAGONDON RIVER
“a degrading river comes back to life”
CAVSCI VIDEO BLOG

(Applied Science)

A Research Paper
Presented to
CAVITE NATIONAL SCIENCE HIGH SCHOOL
Regional Science High School
Maragondon, Cavite

In Partial Fulfillment
of the Requirements in Research 2

by

MARIELLE ANN M. SIGNO
HANS PATRICK B. URSUA
JADE ROLLDIEN G. INDOY

JENNYLOU A. PANGILINAN
Research Adviser

TABLE OF CONTENTS

Content Page

TITLE PAGE............................................................................................................................... i
ABSTRACT................................................................................................................................ ii
APPROVAL SHEET.................................................................................................................... iii
CNSHS MISSION, VISION AND PHILOSOPHY.......................................................................... iv
INTEL ISEF FORMS................................................................................................................... v
TABLE OF CONTENTS............................................................................................................... viii
LIST OF TABLES......................................................................................................................... x
LIST OF FIGURES....................................................................................................................... xi
CHAPTER I – INTRODUCTION................................................................................................... 1
A. Background of the Study....................................................................................... 1
B. Statement of the Problem..................................................................................... 2
C. Hypotheses............................................................................................................ 3
D. Significance of the Study....................................................................................... 3
E. Scopes and Limitations of the Study.................................................................... 3
F. Review of Related Literature................................................................................ 4
G. Definition of Terms............................................................................................... 7
CHAPTER II – METHODOLOGY................................................................................................ 9
CHAPTER III – RESULTS........................................................................................................... 14
CHAPTER IV – DISCUSSIONS.................................................................................................. 19
CHAPTER V – CONCLUSION AND RECOMMENDATIONS...................................................... 21
BIBLIOGRAPHY....................................................................................................................... 23
ACKNOWLEDGEMENT........................................................................................................... 25
Content Page

APPENDICES.......................................................................................................................... 26
A. Ghantt Chart....................................................................................................... 27
B. Calendar of Activities......................................................................................... 28
C. Letters................................................................................................................. 31
D. Photographs of the Experimentation................................................................ 37
E. Evaluation Sheet................................................................................................. 42
F. Statistical Computations..................................................................................... 43
G. Expenses Incurred............................................................................................... 44
H. Certificates of Participation and Merits............................................................. 46
I. Curriculum Vitae................................................................................................. 48

Monday, March 28, 2011

1. Which statement is an identifying characteristic of a mixture?
a) A mixture can consist of a single element.
b) A mixture can be separated by physical means.
c) A mixture must have a definite composition by weight.
d) A mixture must be homogeneous.

2. The presence of which ion usually produces a colored solution?
a) K+
b) F-
c) Fe2+
d) S2-

3. Dissolving 1 mole of KCl in 1000 grams of H2O affects
a) the boiling point of the H2O, only
b) the freezing point of the H2O, only
c) both the boiling point and the freezing point of the H2O
d) neither the boiling point nor the freezing point of the H2O

4. The table below shows the data collected by a student as heat was applied at a constant rate to a solid below its freezing point:

Time
(min)

Temperature
(C)

Time
(min)

Temperature
(C)

0

20

18

44

2

24

20

47

4

28

22

51

6

32

24

54

8

32

26

54

10

32

28

54

12

35

30

54

14

38

32

58

16

41

34

62

What is the boiling point of this substance?
a) 32C
b) 54C
c) 62C
d) 100C

5. Which phase change represents sublimation?
a) NH3(l) NH3(g)
b) KI(s) KI(l)
c) H2O(l) H2O(l)
d) CO2(s) CO2(g)

6. The graph below shows the change in temperature of water in an open container as heat is added at a constant rate:

[Image]

What is the pressure of the system at the temperature represented by segment DE?
a) 0 torr
b) between 0 and 760 torr
c) 760 torr
d) more than 760 torr

7. Which sample is a homogeneous mixture?
a) NaCl(s)
b) NaCl(l)
c) NaCl(g)
d) NaCl(aq)

8. Which salt contains an ion that forms a colored solution?
a) Mg(NO3)2
b) Ca(NO3)2
c) Ni(NO3)3
d) Al(NO3)3

9. Which solution has the highest boiling point?
a) 1.0 M Ca(NO3)2
b) 2.0 M Ca(NO3)2
c) 1.0 M KNO3
d) 2.0 M KNO3

10. Refer to the phase diagram below:

[Image]

Which point could represent a boiling point for the substance?
a) A
b) B
c) C
d) D

1. b
2. c
3. c
4. b
5. d
6. c
7. d
8. c
9. b
10. a

Colligative Properties of Solutions

Introduction and Summary

Solutions, especially liquid solutions, generally have markedly different properties than either the pure solvent or the solute. For example, a solution of sugar in water is neither crystalline like sugar nor tasteless like water. Some of the properties unique to solutions depend only on the number of dissolved particles and not their identity. Such properties are called colligative properties. The colligative properties we will consider in this SparkNote are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure.

When a nonvolatile solute is dissolved in a solvent, the vapor pressure of the resulting solution is lower than that of the pure solvent. The amount of the vapor pressure lowering is proportional to the amount of solute and not its identity. Therefore, vapor pressure lowering is a colligative property. The equation that describes that phenomenon is called Raoult's law.

Boiling point elevation is a colligative property related to vapor pressure lowering. The boiling point is defined as the temperature at which the vapor pressure of a liquid equals the atmospheric pressure. Due to vapor pressure lowering, a solution will require a higher temperature to reach its boiling point than the pure solvent.

Every liquid has a freezing point--the temperature at which a liquid undergoes a phase change from liquid to solid. When solutes are added to a liquid, forming a solution, the solute molecules disrupt the formation of crystals of the solvent. That disruption in the freezing process results in a depression of the freezing point for the solution relative to the pure solvent.

When a solution is separated from a volume of pure solvent by a semi-permeable membrane that allows only the passage of solvent molecules, the height of the solution begins to rise. The value of the height difference between the two compartments reflects a property called the osmotic pressure of a solution. As you know, if you add more solvent to a solution, the two mix together to form a more dilute solution. The same forces allowing that mixing serve to force solvent molecules from the pure solvent compartment across the membrane into the solution compartment causing the change in volume. The amount of osmotic pressure is directly related to the concentration of the solute. That is because more concentrated the solutions have greater potentials for dilution.

Terms

Colligative Property - A property that depends only on the amount of solute in a solution and not the identity of the solute.

Concentrated - A solution of high concentration.

Concentration - The amount of solute dissolved in a given amount of solvent.

Dilute - A solution of low concentration or the process of lowering the concentration of a solution by the addition of solvent.

Dilution - The decrease of the concentration of a solution by the addition of more solvent.

Dissolve - To become a part of a solution.

Nonvolatile - A substance that does not have an appreciable vapor pressure.

Raoult's Law - The vapor pressure of a solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent.

Solubility - The amount of a particular solute that can dissolve in a given amount of a particular solvent. Solubilities are generally listed in g / L.

Solute - A minor component of a solution.

Solution - A homogeneous mixture.

Solvent - The major component of a solution.

Colligative Properties

What are Colligative Properties?

A we have discussed, solutions have different properties than either the solutes or the solvent used to make the solution. Those properties can be divided into two main groups--colligative and non-colligative properties. Colligative properties depend only on the number of dissolved particles in solution and not on their identity. Non-colligative properties depend on the identity of the dissolved species and the solvent.

To explain the difference between the two sets of solution properties, we will compare the properties of a 1.0 M aqueous sugar solution to a 0.5 M solution of table salt (NaCl) in water. Despite the concentration of sodium chloride being half of the sucrose concentration, both solutions have precisely the same number of dissolved particles because each sodium chloride unit creates two particles upon dissolution--a sodium ion, Na⁺, and a chloride ion, Cl^-. Therefore, any difference in the properties of those two solutions is due to a non-colligative property. Both solutions have the same freezing point, boiling point, vapor pressure, and osmotic pressure because those colligative properties of a solution only depend on the number of dissolved particles. The taste of the two solutions, however, is markedly different. The sugar solution is sweet and the salt solution tastes salty. Therefore, the taste of the solution is not a colligative property. Another non-colligative property is the color of a solution. A 0.5 M solution of CuSO₄ is bright blue in contrast to the colorless salt and sugar solutions. Other non-colligative properties include viscosity, surface tension, and solubility.

Raoult's Law and Vapor Pressure Lowering

When a nonvolatile solute is added to a liquid to form a solution, the vapor pressure above that solution decreases. To understand why that might occur, let's analyze the vaporization process of the pure solvent then do the same for a solution. Liquid molecules at the surface of a liquid can escape to the gas phase when they have a sufficient amount of energy to break free of the liquid's intermolecular forces. That vaporization process is reversible. Gaseous molecules coming into contact with the surface of a liquid can be trapped by intermolecular forces in the liquid. Eventually the rate of escape will equal the rate of capture to establish a constant, equilibrium vapor pressure above the pure liquid.

If we add a nonvolatile solute to that liquid, the amount of surface area available for the escaping solvent molecules is reduced because some of that area is occupied by solute particles. Therefore, the solvent molecules will have a lower probability to escape the solution than the pure solvent. That fact is reflected in the lower vapor pressure for a solution relative to the pure solvent. That statement is only true if the solvent is nonvolatile. If the solute has its own vapor pressure, then the vapor pressure of the solution may be greater than the vapor pressure of the solvent.

Note that we did not need to identify the nature of the solvent or the solute (except for its lack of volatility) to derive that the vapor pressure should be lower for a solution relative to the pure solvent. That is what makes vapor pressure lowering a colligative property--it only depends on the number of dissolved solute particles.

summarizes our discussion so far. On the surface of the pure solvent (shown on the left) there are more solvent molecules at the surface than in the right-hand solution flask. Therefore, it is more likely that solvent molecules escape into the gas phase on the left than on the right. Therefore, the solution should have a lower vapor pressure than the pure solvent.

http://img.sparknotes.com/figures/A/a355d48810a7fa33761d1f32c3099d7b/erlenmeyers.gif

Figure %: The Vapor Pressure of a Solution is Lower than that of the Pure Solvent

The French chemist Francois Raoult discovered the law that mathematically describes the vapor pressure lowering phenomenon. Raoult's law is given in :

Figure %: Raoult's Law Describes the Mathematics of Vapor Pressure Lowering

Raoult's law states that the vapor pressure of a solution, P, equals the mole fraction of the solvent, c _solvent, multiplied by the vapor pressure of the pure solvent, P^o. While that "law" is approximately obeyed by most solutions, some show deviations from the expected behavior. Deviations from Raoult's law can either be positive or negative. A positive deviation means that there is a higher than expected vapor pressure above the solution. A negative deviation, conversely, means that we find a lower than expected vapor pressure for the solution. The reason for the deviation stems from a flaw in our consideration of the vapor pressure lowering event--we assumed that the solute did not interact with the solvent at all. That, of course, is not true most of the time. If the solute is strongly held by the solvent, then the solution will show a negative deviation from Raoult's law because the solvent will find it more difficult to escape from solution. If the solute and solvent are not as tightly bound to each other as they are to themselves, then the solution will show a positive deviation from Raoult's law because the solvent molecules will find it easier to escape from solution into the gas phase.

Solutions that obey Raoult's law are called ideal solutions because they behave exactly as we would predict. Solutions that show a deviation from Raoult's law are called non-ideal solutions because they deviate from the expected behavior. Very few solutions actually approach ideality, but Raoult's law for the ideal solution is a good enough approximation for the non- ideal solutions that we will continue to use Raoult's law. Raoult's law is the starting point for most of our discussions about the rest of the colligative properties, as we shall see in the following section.

Boiling Point Elevation

One consequence of Raoult's law is that the boiling point of a solution made of a liquid solvent with a nonvolatile solute is greater than the boiling point of the pure solvent. The boiling point of a liquid or is defined as the temperature at which the vapor pressure of that liquid equals the atmospheric pressure. For a solution, the vapor pressure of the solvent is lower at any given temperature. Therefore, a higher temperature is required to boil the solution than the pure solvent. is a phase diagram for both a pure solvent and a solution of that solvent and a nonvolatile solute that explains that point graphically.

http://img.sparknotes.com/figures/A/a355d48810a7fa33761d1f32c3099d7b/bpel.gif

Figure %: Phase Diagram for a Solvent and its Solution with a Nonvolatile Solute

As you can see in the the vapor pressure of the solution is lower than that of the pure solvent. Because both pure solvent and solution need to reach the same pressure to boil, the solution requires a higher temperature to boil. If we represent the difference in boiling point between the pure solvent and a solution as ΔT_b, we can calculate that change in boiling point from the :

In the we use the units molality, m, for the concentration, m, because molality is temperature independent. The term K_b is a boiling point elevation constant that depends on the particular solvent being used. The term i in the above equation is called the van't Hoff factor and represents the number of dissociated moles of particles per mole of solute. The van't Hoff factor is 1 for all non-electrolyte solutes and equals the total number of ions released for electrolytes. Therefore, the value of i for Na₂SO₄ is 3 because that salt releases three moles of ions per mole of the salt.

Freezing Point Depression

As you may have noticed when we looked at the , the freezing point is depressed due to the vapor pressure lowering phenomenon. The points out that fact:

http://img.sparknotes.com/figures/A/a355d48810a7fa33761d1f32c3099d7b/fpdep.gif

Figure %: Phase Diagram for a Solution and the Pure Solvent Indicating the Freezing Point Depression

In analogy to the boiling point elevation, we can calculate the amount of the freezing point depression with the :

Note that the sign of the change in freezing point is negative because the freezing point of the solution is less than that of the pure solvent. Just as we did for boiling point elevation, we use molality to measure the concentration of the solute because it is temperature independent. Do not forget about the van't Hoff factor, i, in your freezing point calculations.

One way to rationalize the freezing point depression phenomenon without talking about Raoult's law is to consider the freezing process. In order for a liquid to freeze it must achieve a very ordered state that results in the formation of a crystal. If there are impurities in the liquid, i.e. solutes, the liquid is inherently less ordered. Therefore, a solution is more difficult to freeze than the pure solvent so a lower temperature is required to freeze the liquid.

Osmotic Pressure

Osmosis refers to the flow of solvent molecules past a semipermeable membrane that stops the flow of solute molecules only. When a solution and the pure solvent used in making that solution are placed on either side of a semipermeable membrane, it is found that more solvent molecules flow out of the pure solvent side of the membrane than solvent flows into the pure solvent from the solution side of the membrane. That flow of solvent from the pure solvent side makes the volume of the solution rise. When the height difference between the two sides becomes large enough, the net flow through the membrane ceases due to the extra pressure exerted by the excess height of the solution chamber. Converting that height of solvent into units of pressure (by using the ) gives a measure of the osmotic pressure exerted on the solution by the pure solvent. P stands for pressure, r is the density of the solution, and h is the height of the solution.

shows a typical setup for measuring the osmotic pressure of a solution.

http://img.sparknotes.com/figures/A/a355d48810a7fa33761d1f32c3099d7b/osmoticsetup.gif

Figure %: Setup for Measuring the Osmotic Pressure of a Solution

You can understand why more molecules flow from the solvent chamber to the solution chamber in analogy to our discussion of Raoult's law. More solvent molecules are at the membrane interface on the solvent side of the membrane than on the solution side. Therefore, it is more likely that a solvent molecule will pass from the solvent side to the solution side than vice versa. That difference in flow rate causes the solution volume to rise. As the solution rises, by the pressure depth equation, it exerts a larger pressure on the membrane's surface. As that pressure rises, it forces more solvent molecules to flow from the solution side to the solvent side. When the flow from both sides of the membrane are equal, the solution height stops rising and remains at a height reflecting the osmotic pressure of the solution.

The equation relating the osmotic pressure of a solution to its concentration has a form quite similar to the ideal gas law:

Although the above equation may be more simple to remember, the is more useful. This form of the equation has been derived by realizing that n / V gives the concentration of the solute in units of molarity, M.

Problems and Solutions

Problem :
What is the vapor pressure of the pure solvent if the vapor pressure of a solution of 10 g of sucrose (C₆H₁₂O₆) in 100 g of ethanol (C₂H₆O) is 55 mmHg?

Problem :
What is the freezing point of a solution of 15.0 g of NaCl in 250 g of water? The molal freezing point constant, K_f, for water is 1.86 ^oC kg / mol.

Problem :
A solution of 0.5 g of an unknown nonvolatile, nonelectrolyte solute is added to 100 mL of water and then placed across a semipermeable membrane from a volume of pure water. When the system reaches equilibrium, the solution compartment is elevated 5.6 cm above the solvent compartment. Assuming that the density of the solution is 1.0 g / mL, calculate the molecular mass of the unknown.

Solution for Problem 1 >>

To solve this problem, we will use Raoult's law:

Then rearrange the equation to solve for the pressure of the pure solvent, P^o. After converting the gram amounts to moles we find that the mole fraction of the solvent ethanol is 0.975. Therefore, the vapor pressure of the solvent is 56.4 mmHg.

Solution for Problem 2 >>

ΔT_f = - i K_f m

For NaCl, i = 2. The concentration of the solution is 1.03 m in NaCl. Therefore, the change in the freezing point of the water is -3.8 ^oC. The freezing point of the solution is, therefore, -3.8 ^oC.

Solution for Problem 3 >>

To solve this problem, we will rearrange the formula for osmotic pressure:

Then we can calculate the pressure from the pressure depth equation, then convert the units into atmospheres.

Next, we can calculate the molarity of the solution. Finally, we will use that molarity to calculate the molar mass of the unknown from the volume of the solution and the mass of the unknown.

Wednesday, February 23, 2011

Informal Theme No.4

Pantomime

Shh! Shh! Hey no sound, that’s what I always hear on the stage.

At first, when Ma’am us that we will have pantomime, our only reaction was “Pantomime, huh?” “What’s that?” It’s very new in our ear. Just then we found out that you will act without talking but we all know that in talking we can communicate. “How is that?” questions are running in our mind. While were practicing we just found the answer “COOPERATION”. Every problem, we can make it! That’s why we are the 3F, united we stand divided we fall. Even though we had mistakes when we are together we can still make it through.

After pantomime, we had a self fulfilment, we proved to ourselves and to others that not only in kalokohan we are solid but we can stand for the good as well. Everything is a job welldone for a beginner like us. Thanks to our English III teacher, Ma’am Mildred C. Atendido for such unforgettable experiences in her class and for the new lesson that we’ve learned.

Informal Theme No. 3

THE CREATION OF THE TEACHER
The Good Lord was creating teachers. It was His sixth day of 'overtime' and He knew that this was a tremendous responsibility for teachers would touch the lives of so many impressionable young children. An angel appeared to Him and said, "You are taking a long time to figure this one out."
"Yes," said the Lord,” but have you read the specs on this order?"
TEACHER:
…must stand above all students, yet be on their level
... must be able to do 180 things not connected with the subject being taught
... must run on coffee and leftovers,
... must communicate vital knowledge to all students daily and be right most of the time
... must have more time for others than for herself/himself
... must have a smile that can endure through pay cuts, problematic children, and worried parents
... must go on teaching when parents question every move and others are not supportive
... must have 6 pair of hands.
"Six pair of hands, “said the angel, "that's impossible"
"Well,” said the Lord, " it is not the hands that are the problem. It is the three pairs of eyes that are presenting the most difficulty!"
The angel looked incredulous, “Three pairs of eyes...on a standard model?"
The Lord nodded His head, “One pair can see a student for what he is and not what others have labelled him as. Another pair of eyes is in the back of the teacher's head to see what should not be seen, but what must be known. The eyes in the front are only to look at the child as he/she 'acts out' in order to reflect, “I understand and I still believe in you", without so much as saying a word to the child."
"Lord, " said the angel, " this is a very large project and I think you should work on it tomorrow".
"I can't," said the Lord, " for I have come very close to creating something much like Myself. I have one that comes to work when he/she is sick.....teaches a class of children that do not want to learn....has a special place in his/her heart for children who are not his/her own.....understands the struggles of those who have difficulty....never takes the students for granted..."
The angel looked closely at the model the Lord was creating.
"It is too soft-hearted,” said the angel.
"Yes," said the Lord, “but also tough, you cannot imagine what this teacher can endure or do, if necessary".
"Can this teacher think?" asked the angel.
"Not only think," said the Lord, "But reason and compromise."
The angel came closer to have a better look at the model and ran his finger over the teacher's cheek.
"Well, Lord, ” said the angel, your job looks fine but there is a leak. I told you that you were putting too much into this model. You cannot imagine the stress that will be placed upon the teacher."
The Lord moved in closer and lifted the drop of moisture from the teacher's cheek. It shone and glistened in the light.
"It is not a leak," He said, "It is a tear."
"A tear? What is that?" asked the angel, "What is a tear for?"
The Lord replied with great thought, " It is for the joy and pride of seeing a child accomplish even the smallest task. It is for the loneliness of children who have a hard time to fit in and it is for compassion for the feelings of their parents. It comes from the pain of not being able to reach some children and the disappointment those children feel in themselves. It comes often when a teacher has been with a class for a year and must say good-bye to those students and get ready to welcome a new class."
"My, “said the angel, " The tear thing is a great idea...You are a genius!!"
The Lord looked sombre, "I didn't put it there."

Informal Theme No. 3

Informal Theme No. 2

3 Words of Wisdoms:

1.) She never says take care because as if you are telling that watch out something bad will happen to you. Instead of “take care” say “stay safe”.

2.) Patience is a virtue, like “successful persons do not believe in failure. They believe in their own ability to overcome any obstacle and their faith overcomes every hindrance.

3.) You should have already future plans. “Your life must have direction” that is what Ma’am is always telling us. She will ask us “What course you will take? “ and “What do you want to be someday?” if you haven’t decided yet go and find a high building and jump!

Informal Theme No. 2

3 Words of Wisdoms:

1.) She never says take care because as if you are telling that watch out something bad will happen to you. Instead of “take care” say “stay safe”.

2.) Patience is a virtue, like “successful persons do not believe in failure. They believe in their own ability to overcome any obstacle and their faith overcomes every hindrance.

Informal Theme No. 1

Personality Distinguishes You from Others

An authority may once said “there are 3 types of a person”, a person he think he is, a person others think he is and the person he really is. Personality distinguishes us from one another. We all come in different size and shape. What is important to me may not be important to you, and the one you treasure most is in there I don’t care about at all.

Monday, January 3, 2011

Informal Theme No.6

Our Second First Kiss
We dwell on the past, while living the present
But I admit, the past was unpleasant
Full of ups and downs, less pleasure more pain
We wished for the sun, but only got rain
We both made mistakes, put pain in our hearts
But here we are again, promising to never part
Counting our blessings and letting go of the past
Starting all over and making it last
Feelings and memories flow deep in my mind
Of those days our love was genuine and kind
Holding you close, feeling your skin
You look into my eyes and make my head spin
Those feelings are back, but stronger than ever
I know you're the one I wanna hold on to forever
We both smile again, nothing's better than this

Kissing you again was like our second first kiss.

Informal Theme No.3

                                                   Girl Scout Camping

             The scouting activities for me ever since is exciting because I can meet new friends and learn many things. There are lots of exciting activities like games, orientation and most of all the campfire, here we sing many songs like Campfires Burning, Come, Come Light Up the Fire and so many songs. We had competitions like Cheering, Presentations. I learned new song that most of the scouters love also, MAMA MY HEAD AND MY SELF WHAT IS THIS HERE THIS IS MY
...brain buster                          .....neck breaker
...eye dropper                         .....chest protector
...nose blower                         .....BOY HUGGER
...mouth pusher                        ...fruit basket
...chin chopper                         ...knee bender       ...foot stopper

TIKI TIKI TOO!! that what I learned from the SCOUTS Mama my head and my self^_^

Informal Theme No. 9

Christmas Party

We had a great time in school!!! fun.fun fun. There are lots of exciting games. I joined the trip to jerusalem with the twist. My partner is Robert, the twists are hard like : the boy will carry the girl like a 1 kilo of rice, newly wed like a baby and so many more..,

All sections presented an intermission number. Our president choose 7 representatives in our class and I am included there. We dance the song of Yeng Constantino "Pasko sa Pinas". Everyone is very happy eating!!!

luv.luv

...happy new year to all!!

bye 2010...welcome 2012!!!

elleiramO4i9

Informal Theme No. 4

Divine Comedy

The Divine Comedy is in three parts, one that details his spiritual travels through Hell, one for Purgatory, and the other that takes him through Heaven, guided always by a figure of legend. In “Inferno,” the poet finds himself lost in dark woods, and though he tries to find his way out, he ultimately meets the ancient poet, Virgil. Virgil explains that in order to reach Paradise, Dante must first follow him on a tour of Hell, and then leads him down through the gates. For Dante, there are nine circles of Hell, each tailored to the sinners who go there. The sixth through the ninth circles have inner levels within each of them, and on the fourth level of the ninth circle of hell (where traitors to their masters reside) he finds Satan himself. The two poets exit Hell in time for the sun’s rising on Easter Sunday, and that is where Virgil leads him on to Purgatory. In this place, Dante is marked with seven P’s for each of the sins, and as they climb, these are removed and the climbing becomes easier. Purgatory, too, is terraced like Hell, but here the sinners could climb higher with proper prayer and repentance measures. There are seven terraces to Purgatory, with their corresponding historical and very real figures, and after the seventh he passed through a wall of fire to be guided in Paradise by his Lady, Beatrice, leaving Virgil behind. To pass through the river Lethe, Dante is told to confess his sins, but he instead faints and is carried across to find Beatrice. He finds Heaven has seven Spheres for each virtue and those who lived them so fully they became inhabitants, then Fixed Stars where many Apostles lived, and finally the ninth heaven (space itself) allowed him to witness Christ and the Virgin Mary entering and to gaze upon divinity as the angels sang. He’s left alone, though, to be one with God, and has no words to describe the greatness he finds.

Informal Theme No. 1

Cervical Cancer ; a Feminine Risk

When you get a diagnosis of cancer, it's natural to wonder what may have caused the disease. Doctors cannot always explain why one woman develops cervical cancer and another does not. However, we do know that a woman with certain risk factors may be more likely than others to develop cervical cancer. A risk factor is something that may increase the chance of developing a disease.

Studies have found a number of factors that may increase the risk of cervical cancer. For example, infection with HPV (human papillomavirus) is the main cause of cervical cancer. HPV infection and other risk factors may act together to increase the risk even more:

HPV infection: HPV is a group of viruses that can infect the cervix. An HPV infection that doesn't go away can cause cervical cancer in some women. HPV is the cause of nearly all cervical cancers.

HPV infections are very common. These viruses are passed from person to person through sexual contact. Most adults have been infected with HPV at some time in their lives, but most infections clear up on their own.

Some types of HPV can cause changes to cells in the cervix. If these changes are found early, cervical cancer can be prevented by removing or killing the changed cells before they can become cancer cells. The NCI fact sheet Human Papillomaviruses and Cancer: Questions and Answers has more information.

A vaccine for females ages 9 to 26 protects against two types of HPV infection that cause cervical cancer. The NCI fact sheet Human Papillomavirus (HPV) Vaccines: Questions and Answers has more information.
Lack of regular Pap tests: Cervical cancer is more common among women who don't have regular Pap tests. The Pap test helps doctors find abnormal cells. Removing or killing the abnormal cells usually prevents cervical cancer.
Smoking: Among women who are infected with HPV, smoking cigarettes slightly increases the risk of cervical cancer.
Weakened immune system (the body's natural defense system): Infection with HIV (the virus that causes AIDS) or taking drugs that suppress the immune system increases the risk of cervical cancer.
Sexual history: Women who have had many sexual partners have a higher risk of developing cervical cancer. Also, a woman who has had sex with a man who has had many sexual partners may be at higher risk of developing cervical cancer. In both cases, the risk of developing cervical cancer is higher because these women have a higher risk of HPV infection.
Using birth control pills for a long time: Using birth control pills for a long time (5 or more years) may slightly increase the risk of cervical cancer among women with HPV infection. However, the risk decreases quickly when women stop using birth control pills.
Having many children: Studies suggest that giving birth to many children (5 or more) may slightly increase the risk of cervical cancer among women with HPV infection.
DES (diethylstilbestrol): DES may increase the risk of a rare form of cervical cancer in daughters exposed to this drug before birth. DES was given to some pregnant women in the United States between about 1940 and 1971. (It is no longer given to pregnant women.)

Having an HPV infection or other risk factors does not mean that a woman will develop cervical cancer. Most women who have risk factors for cervical cancer never develop it.

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Cervical Cancer ; a Feminine Risk

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