Acids, Bases & Salts

ACIDS, BASES & SALTS

SCIENCE HOLIDAY HOMEWORK

INTRODUCTIONAcids are sour in taste and change the colour

of blue litmus to red.Bases are bitter in taste and change colour of

red litmus to blue.Litmus is a natural indicator, turmeric is

another such indicator.

COMMON ACIDS AND BASESHYDROCHLORIC ACID ( STOMACH ACID ) –

“HCL”ACETIC ACID ( VINEGAR ) – “HC2H3O2”CARBONIC ACID ( SODA WATER ) – H2CO3AMMONIA WATER ( CLEANING AGENT ) –

NH4OHALUMINIUM HYDROXIDE ( ROLAIDS ) –

AL(OH)3

REACTION OF ACIDS WITH METALSACID + METAL → SALT + HYDROGEN EX:- HYDROCHLORIC ACID + ZINC → ZINC

CHLORIDE + HYDROGEN

Not applicable for non- reactive metals like copper, silver, gold.....

REACTION OF ACIDS WITH METAL CARBONATESACID + METAL CARBONATE → SALT +

CARBON DIOXIDE + WATER EX:- HYDROCHLORIC ACID + SODIUM

CARBONATE → SODIUN CHLORIDE + CARBON DIOXIDE + WATER

REACTION OF ALKALI WITH AMMONIUM SALTSALKALI + AMMONIUM SALT → SALT +

AMMONIA + WATER EX:- SODIUM HYDROXIDE + AMMONIUM

CHLORIDE → SODIUM CHLORIDE + AMMONIA + WATER

NEUTRALIZATIONACID + BASE → SALT + WATER EX:- HYDROCHLORIC ACID + SODIUM

HYDROXIDE → SODIUM CHLORIDE + WATER

SALTSA salt is formed when a hydrogen of an acid is

totally or partially replaced by a metal.Salts of a strong acid and a strong base are

neutral with pH value of 7. on the other hand, salts of a strong acid and a weak base are acidic with pH value of less than 7 and those of a strong base and weak acid are basic in nature, with pH value more than 7.

pH SCALEFor measuring the hydrogen

concentration in a solution, called pH scale is developed. Where “p” stands for potenz which means power in German.

On the pH scale we can generally measure from 0( very acidic ) to 10 ( very alkaline ).

The pH of a neutral solution is 7. the pH below 7 turns that the solution is acidic and if the pH of a solution is above 7 it is alkali.

IMPORTANCE OF Ph EVERYDAYARE PLANTS AND ANIMALS Ph SENSITIVE?ANS. Our body works within the pH range of

7.0 to 7.8. living organisms can survive only in a narrow range of pH change. If rain water of less than 5.8 pH i.e., acid rain falls into rivers the survival of aquatic life becomes difficult. Thus, plants and animals are pH sensitive.

• pH IN OUR DIGESTIVE SYSTEMANS. Components in saliva help keep the pH in your

mouth between 6.5 and 7 so that the enzyme salivary amylase can start to break down carbohydrates. The enzymes that help digest food in the stomach, such as pepsin, work best at a pH around 2, while those that function in the intestines, including peptidases and maltase, work best at a pH around 7.5.

Antacids increase the pH in the stomach, which might make the enzymes in the stomach less effective. The low pH of the juices in the stomach can cause ulcers if they eat through the walls of the small intestine or stomach. This low pH also kills many microorganisms in the food you eat, helping prevent illnesses.

pH changes as the cause of tooth decay.ANS. Tooth decay starts when the pH of the

mouth is lower than 5.5. tooth enamel, made up of calcium phosphate is the hardest substance in the body. It does not dissolve in water, but is corroded when the pH rate in the mouth is below 5.5. bacteria present in the mouth produce acids by degradation of sugar and food particles remaining in the mouth after eating.

CHEMICALS FROM COMMON SALTSSeawater contains many salts dissolved in it.

Sodium chloride is separated from these salts. Deposits of solid salts are also found in several parts of the world. There large crystals are often brown due to impurities. This is called rock salt. Beds of rock salts were formed when seas of bygone ages dried up. Rock salts are mined a coal.

Some examples of salts are:

COMMOM SALT The common salts thus obtained is an

important raw material for various materials of daily use, such as sodium hydroxide, baking soda, washing soda, bleaching powder and many more.

SODIUM HYDROXIDE When electricity is passed through an

aqueous solution of sodium hydroxide ( called brine ), it decomposes to form sodium hydroxide. The process is called the chlor-alkali process because of the products formed- clor for chlorine and alkali for sodium hydroxide.

2NaCl + 2H2O → NaOH + Cl2 + H2

BLEACHING POWDER Chlorine is produced during the electrolysis of aqueous

sodium solution ( brine ). This chlorine gas is used for the manufacture of bleaching powder. Bleaching powder is produced by the action of chlorine on dry slaked lime [Ca(OH)2]. Bleaching powder is representated as CaOCl2, through the actual composition is quite complex.Ca(OH)2 + Cl2 → CaOCl2 + H2O

BLEACHING POWDER IS USED IN: 1] for bleaching cotton and linen in the textile industry, for

bleaching wood pulp in paper factories and for bleaching washed clothes in laundry.

2] as an oxidising agent in many chemical industries 3] for disinfecting drinking water to make it free of germs.

BAKING SODA The soda is commonly used in kitchen for

making tasty crispy pakoras is baking soda. Sometimes it is added for faster cooking. The chemical name of the compound is sodium hydrogencarbonate ( NaHCO3 ). It is produced using sodium chloride as one of its raw material.

NaCl + H2O + CO2 + NH3 → NH4Cl + NaHCO3

WASHING SODA Another chemical that can be obtained from

sodium chloride is NaCo3.10H2O ( Washing Soda ). Sodium carbonate can be obtained by heating baking soda; recrystallisation of Sodium Carbonate gives washing soda. It is also a basic salt.

Na2CO3 + 10H2O → Na2CO3.10H2O.

ARE THE CRYSTALS OF SALTS REALLY DRY?Copper sulphate crystals which seem to be dry

contain water of crystallisation. When we heat the crystals, this water is removed and the salt turns white.

If you moisten the crystals again with water, the blue colour reappears.

Water of Crystallisation has a fixed number of crystals water molecules present in one formula unit of a salt. Five water molecules are present in one formula unit of copper sulphate.

CaSO4.5H2O

PLASTER OF PARIS ( P.O.P )On heating gypsum at 373K, it loses water

molecules and becomes calcium sulphate hemihydrate [ CaSo4.1/2H2o ]. this is called Plaster of Paris, the substance which doctors use as plaster for supporting fractured bones in the right position. Plaster of Paris is a white powder and on mixing with water it changes to gypsum giving a hard solid mass.

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