This document appears to be a lab report for an experiment on the properties of water. It includes procedures conducted on tap water, distilled water, and sodium chloride solution. The document contains questions about why distilled water is used in lab solutions, the differences in lead nitrate solutions, whether distilled water is soft or hard, and the color change of copper sulfate with heating and rehydration. However, it is missing the results and conclusions from the experimental procedures and properties tested.

1. Name: Xemelle Lou Suello
Yr and Sec: BSPharmacy B
LABORATORY ACTIVITY NO.15b
GASEOUS STATE (BOYLE’S LAW)
DATE PERFORMED:
DATE FINISHED:
OBJECTIVE OF THE ACTIVITY:
SUMMARY PROCEDURE:
DATA:
TRIALS VOLUME OF ENTRAPPED AIR (cm3/ mL) PRESSURE + BAROMETRIC AIR
PRESSURE (mmHg)
1
2
3
4
5

2. P
R
E
S
S
U
R
E
VOLUME
QUESTIONS:
1. What is the relationship between the volume of the gas and its pressure?
The relationship between the gas and pressure is that absolute pressure and
volume of a given mass of a confined gas are inversely proportional, if
temperature remains unchanged within a closed system.
2. What kind of graph is obtained?
As the pressure increases the volume decrease, graph obtained is inversely
proportional
( L shape)
3. Is Boyle’s Law applicable to liquids?
Boyle’s Law is not applicable to liquids because the pressure of that applied on the
liquid is the one to be measured not the liquid itself.
4. Is Boyle’s Law applicable to solids? Why?
Boyle’s Law is only applicable in gas, because the formula of the Boyle’s Law is
P1V1=P2V2 where: “P” is equal to pressure and “V” is equal to volume. Which is
refering to gas.
CONCLUSION:
I conclude that barometric air pressure is often also referred to as atmospheric
pressure. In Boyle’s Law P1V1=P2V2 the relationship between the pressure and
volume is that absolute pressure and volume is inversely proportional and also
Boyle’s Law is only applicable in gas.
REFERENCE: www.wiki.answer/Q/is_boyles_law_applicable_to _liquids?
www.wikipedia/Boyle’s_Law

3. Name: Xemelle Lou Suello
Yr and Sec: BSPharmacy B
LABORATORY ACTIVITY NO.16b
PREPARATION AND PROPERTIES OF OXYGEN
DATE PERFORMED:
DATE FINISHED:
OBJECTIVE OF THE ACTIVITY:
SUMMARY OF PROCEDURE:
QUESTIONS:
1. What evidence did you observe that oxygen is not very soluble in water?
One indication that oxygen is not very soluble in water is that you will/we collect it
over. If it is soluble in water, then it would dissolve and we wouldn’t have any to__
test._______________________________________________________________
2. What is the source of oxygen in the procedure you used?
NAME: Hydrogen Peroxide FORMULA: H2O2_____________
3. What purpose does the manganese dioxide serve in this preparation of oxygen?
Manganese dioxide acts as a catalyst which increases the speed of breakdown of
H2O2 to release oxygen (O2)___________________________________________
4. What gas was in the apparatus before you started generating oxygen? Where did itgo?
Probably an Air, composition of air is: Nitrogen 79%, Oxygen 20% , Carbon dioxide,
Helium, Neon and Methane 1%
.______________________________________________________

4. 5. Why are the bottles of oxygen stored with the mouth up?
It is more dense than air mouth up, It stays in the flask upside down, it pours.
6. (a) What is the symbol of element oxygen? __O__
(b) What is the formula for oxygen gas? __O2_
7. Write the word and formula equation for the preparation of oxygen from hydrogen
peroxide.
Word equation: Hydrogen Peroxide  Water + Oxygen__________________
Formula equation: 2H2O2  2H2O + O2__________________________________________________
8. What substances, other than oxygen, are in the generator when the decomposition of
H2O2 is complete?
MnO2 is the catalyst that is used so Mno2 will be left and also H2o(water)_______
C. Properties of Oxygen
2. Write word equations for the chemical reactions that occurred:
C.1. Combustion of wood. Assume carbon is the combustible material
C.2. Combustion of Sulfur.
C.5 Combustion of Steel wool (iron). Call the produce (iron dioxide)
C.6. Combustion of Magnesium
3. Write formula equations for these four chemical reactions.
C.1 (CO2 is the formula for the oxide of carbon that is formed.)
C.2 (SO2 is the formula for the oxide of sulfur that is formed.)

5. C.5 (Fe3O4 is the formula for the oxide of iron that is formed.)
C.6 ( MgO is the formula for the oxide of magnesium that is formed.)
5. Describe the material that is formed when magnesium is burned in air.
When magnesium ribbon is burnt in air, magnesium oxide(MgO) is produce, (but it
is not) produces a white powdery substance. Magnesium reacts with oxygen____
present in the air and produces MgO.____________________________________
6. What elements are in this product?
Magnesium oxide, a little magnesium nitride and bits of magnesium that did not
totally burn._______________________________________________________
7. What is your conclusion about the rate or speed of reaction with respect to he
concentration of the reactants – for example, combustion in a high concentration of
oxygen (pure oxygen) compared to combustion of low concentration of oxygen (air)?
Bright, high and blue flame produces in combusting on a high concentration of
oxygen. While in low concentration of oxygen, is that low flame were produced.
8. What evidences did you observe In the burning of sulfur to confirm your answer in
6(a)?
Sulfur burns in a pure oxygen which produces blue flame/Sulfur dioxide.________
CONCLUSION:
I conclude that the properties of oxygen are: oxygen is a very reactive oxidizing
agent; oxygen is sparingly soluble in water, 30mL of oxygen is one liter of water at
STP with a density of 1.1053 which is slightly heavier that air. Oxygen is a colorless
and odorless gas and it has the ability to support combustion.
REFRENCE: http://www.wikipedia.com/oxygen
http://www.wiki.asnwer/Q/properties_of_oxygen
First Year Science and Technology edition II

6. Name: Xemelle Lou Suello
Yr and Sec: BSPharmacy B
LABORATORY ACTIVITY NO.17b
HYDROGEN
DATE PERFORMED:
DATE FINISHED:
OBJECTIVE OF THE ACTIVITY:
SUMMARY OF PROCEDURE:
QUESTIONS:
A.SOURCES OF HYDROGEN
1. Action of Active Metals on Water
Observations:
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
What is the gas evolved?
_____________________________________________________________________________
_____________________________________________________________________________
_____________________________________________________________________________
Equation:_____________________________________________________________________

7. Name two other metals that react with water at ordinary temperature:
The alkali metals react with water at ordinary temperature and these elements are
Sodium (Na) and Potassium (K)__________________________________________
2.Action of less metals on water
Does magnesium powder react with water at ordinary temperature?
Magnesium metals are not affected by water at room or ordinary temperature.
Magnesium generally is a slow-reacting element, but reactively increases with
oxygen levels.____________________________________________________
Does magnesium powder react with boiling water?
Magnesium is very chemically avtive when it takes of hydrogen in boiling water.__
What is the reaction with the litmus of the product of Magnesium powder with
water after boiling?
In hot water, Mg reacts as follows with water(boiling water):__________________
Mg + 2H2O2  Mg(OH2) + H2 So, Mg(OH)2 is basic-all metal hydroxides are basic
– so litmus paper turns into blue. _______________________________________
Equation:_____Mg+H2O2  Mg(OH2) + H2_______________________________
3.Action of metals on acids.
Which of the metals can displace hydrogen from hydrochloric acid?
Metals which are above hydrogen in the reactivity series can displace Hydrogen
from Hydrocholoric acid e.g. potassium, calcium, sodium, and zinc etc._________
What metals cannot?
Metals below Hydrogen series cannot. Examples are Lead and Copper.__________
4. Reactions of Active Metals with different acids.
Equations: H2SO4 + Zn  Zn(SO4) + H2___________________________________
Which of the two acids give off hydrogen gas?
Sulfuric acid is the acid which give off its hydrogen gas._______________________

8. What kind of an acid is nitric acid?
Nitric acid is a monoporic for there is only ibe hydrogen atom._________________
What acids evolve hydrogen when acted upon by metals?
If the metals react with the acid at all some hydrogen will be evolved. Generally a
strong acid such as Hydrochloric Acid or Sulfuric Acid is used for quantitative____
reaction. Even weak acids such as acetic.__________________________________
5.Action of Some metals on Strong Alkali
With Aliminum
Observation:
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Equation:___________________________________________________________
With Zinc dust instead of Aluminum
Equation:___________________________________________________________
Is Hydrogen evolved?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
What metals evovled hydrogen from strong alkali?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
What other hydroxide can be used in place of sodium hydroxide?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________

9. C. Preparation
Write the equation involved in this preparation
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
What is the method of collection H2 gas?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Why can hydrogen be collected in this manner?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
Why are first bubbles allowed to escape?
Because the first bubbles were air and not pure Hydrogen, that is why we should
allow the first bubbles to escape.______________________________________
Why are test tubes of hydrogen kept with their mouths downward?
Because hydrogen gas is lighter than air, so it tends to rise. It would move to the
top of the tube, and then not able to escape.____________________________
D. Properties of Hydrogen
1. Describe the physical properties of hydrogen
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
2.Test for presence of hydrogen
Does this show that hydrogen is still present?
1.__________________________________________________________________
___________________________________________________________________
2__________________________________________________________________
___________________________________________________________________

10. What can you say about the relative density of water?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
3.Density of Hydrogen
What property of hydrogen is shown by this result?
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
CONCLUSION:
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
___________________________________________________________________
REFERENCE:

11. Name: Xemelle Lou Suello
Yr and Sec: BSPharmacy B
LABORATORY ACTIVITY NO.19b
WATER AND ITS PROPERTIES
(HYDRATES, HARD AND SOFT WATER)
DATE PERFORMED:
DATE FINISHED:
OBJECTIVE OF THE ACTIVITY:
SUMMARY OF PROCEDURE:
DATA
OBSERVATIONS AFTER OBSERVATION AFTER
SAMPLE ADDING Pb(NO3)2 EVAPORATION
Test Tube 1
(Tap Water)
Test Tube 2
(Distilled Water)
Test Tube 3
(NaCl Solution)

12. QUESTIONS:
1. Why do analyst use distilled water in preparing laboratory solutions?
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
2. From the results in procedure A, what could be the possible explanations
for any difference in appearance in the various solutions of lead (ii) nitrate?
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
3. Is distilled water soft or hard? Explaine.
Hard water has iron and other minerals which distilled water doest have thus is
soft._____________________________________________________________
4. Does a change in color observe when copper (II) sulfate crystal become
dehydrated? How do you account for the color change when water is added
to the heated copper (III) sulfate.
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
Equation involved:_________________________________________________
CONCLUSION:
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
_________________________________________________________________
REFERENCE: