EXPERIMENT – O1
TOPIC: ACIDS BASES AND SALTS
AIM: 1. To classify substances as acids, bases and salts using their characteristic
properties.
2. To determine the PH value of the given substances.
MATERIALS: 1. Red & blue litmus paper 2. Test tubes 3. Indicators
(universal, phenolphthalein, methyl orange) 4. pH test paper 5. Dropper
6. Substances (HCl, CH3COOH, H2SO4, NaOH, Ca (OH)2, KOH)
PROCEDURE: 1. Take different types of substances like HCl, CH3COOH, H2SO4, NaOH,
Ca (OH)2, KOH in different test tubes.
2. Drop a sample of all substances on different indicators. And record your
observations
In following table.
Effect on Indicators
RED BLUE METHYL UNIVERSAL pH
S.NO SUBSTANCE LITMUS LITMUS PHENOLPHTHALEIN ORANGE INDICATOR VALUE NATURE
01 HCl
02 CH3COOH
03 H2SO4
04 NaOH
05 Ca(OH)2
06 KOH
07 NaCl
08 Glucose
09 Baking
soda
OBSERVATION: 1. Acids turn blue litmus to red, no colour in phenolphthalein indicator
and have a pH value from 0-7.
2. Bases turn red litmus to blue, pink colour in phenolphthalein indicator
and have a pH value from 7-14.
3. Neutral substances does not affect the indicators, and they have pH
value 7.
CONCLUSION: Hence we separated substances into acids and salts based on their
characteristic properties.
EXPERIMENT -02
TOPIC: ACIDS BASES AND SALTS
AIM: 1. To prepare as Acids, Bases and testing their nature on different
indicators.
MATERIALS: 1. Sulphur powder 2. Dry Ice 3. Magnesium ribbon 4. Calcium Oxide
5. Indicators (red & blue litmus papers, Phenolphthalein, pH paper)
PROCEDURE: PREPARATION OF SULPHUROUS ACID (H2SO3)
1. Heat a little amount of sulphur powder in a deflagrating spoon and
dissolve the gas which is released, in a water.
Step 1: S + O2 ------------ SO2 (on burning)
Step 2: SO2 + H2O------- H2SO3 (On dissolving in water)
PREPARATION OF CARBONIC ACID (H2CO3)
1. Add a small amount of dry ice (solid C02) in water, Bubbles will form
and misty White Fog will be produced. Since the water is much warmer
than the dry ice, Energy is transferred from water to dry ice, causing it to
change from a solid to a gaseous state and bubbles through the water.
On dissolving CO2 gas in water, it produces carbonic acid (H2CO3).
Step 1: CO2 + H2O-------------- H2CO3
Solid + Liquid Carbonic acid
PREPARATION OF MAGNESIUM HYDROXIDE (Mg (OH)2)
1. Burn a small piece of magnesian ribbon (hold with a pair of tongs) in
air (in the presence of Oxygen), It burns with a dazzling flame and
produces ash (Magnesium oxide, Mgo).
Step 1: 2 Mg + O2------------- 2 MgO (On burning)
2. Dissolve Ash (magnesium oxide) in a water, it produces its hydroxide
called magnesium hydroxide, a base.
Step 2: MgO + H2O-------------- Mg (OH)2 (on dissolving in water)
PREPARATION OF CALCIUM HYDROXIDE (Ca (OH)2)
1. react a little amount of calcium with Oxygen, it produces Calcium
Oxide (CaO).
Step 1: 2 Ca + O2----------- 2 CaO
2. Dissolve Calcium oxide (CaO) in water, it produces hydroxide called
Calcium hydroxide, Ca (OH)2, a Base.
Step 2: CaO + H2O--------- Ca (OH)2
Test the nature of prepared substance on different indicators and record
the observations in following table.
OBSERVATIONS:
RED BLUE METHYL pH NATURE
S.NO SUBSTANCE LITMUS LITMUS PHENOLPHTHALEIN ORANGE value
01 H2SO3
02 H2CO3
03 Mg (OH)2
04 Ca (OH)2
CONCLUSION: Hence, we prepared acids from non-metals and bases from metals and
tested their nature on different indicators.
EXPERIMENT – 03
TOPIC: ACIDS BASES AND SALTS
AIM: To prove that salt and water produces in a reaction between an Acid and a
Base (Neutralization reaction).
MATERIALS: 1. Hydrochloric acid (HCl), strong acid
2. Sodium hydroxide (NaOH), a strong base
3. Conical flask 4. Dropper
PROCEDURE:
1. Take 5 ml of Strong Hydrochloric acid (HCl) in a conical flask.
2. Then add 5 ml of Strong base, Sodium hydroxide (NaOH).
3. Observe the reaction between an Acid and a Base.
OBSERVATIONS: We observe that a salt, water and heat energy is produced due to
chemical reaction between a strong acid and a strong base.
HCl + NaOH ----------------- NaCl + H2O + heat
Hydro chloric acid Sodium hydroxide Sodium chloride water
CONCLUSION: Hence, we proved that Salt & water is produced in a reaction between
an acid and a base. As heat is released. So, it is an Exothermic reaction.
EXPERIMENT – 04
TOPIC: PHYSICAL AND CHEMICAL CHANGES
AIM: To study the reaction of acid with Metals (Zinc & Magnesium).
Materials: 1. Zinc metal (granules) 2. Magnesium ribbon
3. Hydrochloric acid (dil. HCl) 4. Sulphuric acid (dil. H2SO4)
PROCEDURE: 1. Takee some Zinc granules in a dry test tube and then add dil. Sulphuric
acid (dil. H2SO4) to it. Set the apparatus as shown in below.
2. Observe the surface of Zinc granules. Take a burning candle, place
near the soap bubbles filled with the gas and observe.
3. Repeat the same procedure with hydrochloric acid (dil. HCl) and other
acids and observe the result in each case.
Zn + H2SO4------------- ZnSO4 + H2
Mg + H2SO4------------ MgSO4 + H2
Zn + 2HCl-------------- ZnCl2 + H2
Mg + 2HCl------------- MgCl2 + H2
OBSERVATION: 1. Some effervescence is observed near zinc surface and the soap
bubbles which burst with pop sound.
2. A burning match stick or candle put off with a POP sound.
CONCLUSION: Hence, we proved that metallic salt and hydrogen gas is liberated on
reacting a metal with an acid.
EXPERIMENT – 05
TOPIC: PHYSICAL AND CHEMICAL CHANGES
AIM: To study the reaction of acids with Metal carbonates (CaCO 3 & MgCO3).
MATERIALS: 1. CaCO3 2. MgCO3 3. Dil. HCl 4. Test tubes
5. Single holed rubber cork
PROCEDURE: 1. Take a little amount of calcium carbonate (CaCO3 or MgCO3) in a
boiling test tube and the add dilute hydro chloric acid.
2. Set the apparatus as shown in below.
3. Observe the reaction between dil. HCl and CaCO3 or MgCO3, and we
can observe the brisk effervescence, represents the liberation of a gas.
4. repeat the same procedure with sulphuric acid and observe the result
in each case.
CaCO3 + 2HCl --------------- CaCl2 + H2O + CO2
MgCO3 + 2HCl---------------- MgCl2 + H2O + CO2
OBSERVATION: 1. Some effervescence is observed in reaction and formation of bubbles
seen in lime water.
2. When the released gas is turned into the lime water, it turns lime
water into Milky white due to formation of CaCO3.
3. When a burning match stick is placed the near mouth of the test tube,
it extinguished the fire.
CONCLUSION: Hence, we proved that acids react with metal carbonates and produces
metallic salt and liberates the CO2 gas.
EXPERIMENT: 06
TOPIC: PHYSICAL AND CHEMICAL CHANGES
AIM: To prove that a precipitation reaction is a reaction that yields an
insoluble product- a precipitate- when two solutions are mixed.
MATERIALS: 1. NaCl solution 2. AgNO3 solution 3. Boiling test tube
4. Dropper 5. Filter paper.
PROCEDURE: 1. Take 10ml of NaCl solution into a boiling tube and then add 10 ml of
silver nitrate solution (AgNO3) solution.
2. Observe the reaction between NaCl and AgNO3 Solution.
NaCl + AgNO3 ---------------- AgCl + NaNO3
OBSERVATION: 1. Aqueous sodium chloride and silver nitrate react to form a white
precipitate of silver chloride; it settles at bottom of the boiling tube.
2. Pour a mixture into a filter paper cone, AgCl precipitate left an filter
paper as residue and NANO3 solution collects in a beaker, placed below
the filter paper.
CONCLUSION: Hence, we proved that an insoluble solid is formed due to a reaction
between two solutions.
EXPERIMENT- 07
TOPIC: PHYSICAL AND CHEMICAL CHANGES
AIM: To study the extraction of pure metal from solution by displacement reaction.
Materials: 1. Two beakers 2. Iron nails (Fe)
3. Copper sulphate solution (aq. CuSO4)
PROCEDURE: 1. Dissolve a few crystals of copper sulphate in water in a beaker.
2. Drop a clean iron nail in the beaker and wait for about one hour and
observe the reaction.
OBSERVATION: CuSO4 + Fe------------ FeSO4 + Cu (Fe > Cu)
Sky blue iron green brown
1. As Iron is more reactive than Copper, Iron displaces the copper from
its aqueous solution and form ferrous sulphate (FeSO4) solution, green in
colour and a brown colour copper particles are settled at bottom of the
beaker.
CONCLUSION: Hence, we extracted a pure metal (copper) from its solutions by
displacement reaction with iron.
