Neutralisation - How much acid is required to neutralise a base :: GCSE Chemistry Coursework Investigation

Neutralisation - How much acid is required to neutralise a constituteIntroduction============Neutralisation is the reaction of a alkali with an acid to form aneutral solution which contains salt and water.Acid + Base Salt + Water---------------------------In my experiment I am toilsome to find out how much acid it takes toneutralise a base to form a neutral solution. I will use one wedge ofNitric Acid as the acid and one submarine sandwich of Ammonium Hydroxide as thebase. So this will be a 11 ratio. (Molarity = how many molecules ofthe acid or alkali per 1000 cm3 (1 litre) of water.)Nitric Acid + Ammonium Hydroxide Ammonium Nitrate + Water-----------------------------------------------------------HNO + NH OH NH NO + H OIonic bonding must take place to form the salt and the water. Ions entertain been formed because the original atoms learn lost or gained negatrons. These ions then have electrical charges because they do nothave the same amount of positive protons and negative electrons. Atomsthat loose electrons are called cations and have a positive charge.Atoms that have gained an electron and have a negative charge arecalled anions.The General equation for making water isH + OH H O---------------In this equation the hydrogen ion has lost and electron and has becomea cation with a positive charge. The Hydroxide ion has gained anelectron and has become a negatively charged anion. Ionic bonds arecreated when ions ruffle in order to share and thus becomeelectrically stable.From the main neutralisation equation I have circled the parts to makewaterHNO + NH OH NH NO + H OEquipmentAmmonium Hydroxide (base)Nitric Acid (acid)Methyl Oxide - (to show the pH of the solution)Clamp (to hold the burette safely and securely in place)Burette - (to hold the acid)White Tile Funnel (to pour the acid into the burette)Goggles - (to protect the eyes)Conical Flask (to hold the base)Measuring Cylinder (to ginmill out the acid and the base)PreliminaryBefore we began our practical our teacher performed the experiment asan example to our class. The teacher set up the equipment as shownabove. She informed us of the safety precautions and then began theexperiment. She used 20ml of Ammonium Hydroxide (base), placing thatin the cone-shaped flask. Then she added 6 drops of Methyl Orange(indicator). From the Burette she added 12ml of Nitric acid andswilled the conic flask. After this point she decided to control theamount added to the base and indicator by using the burette.Neutralisation - How much acid is required to neutralise a base GCSE Chemistry Coursework InvestigationNeutralisation - How much acid is required to neutralise a baseIntroduction============Neutralisation is the reaction of a base with an acid to form aneutral solution which contains salt and water.Acid + Base Salt + Water---------------------------In my experiment I am difficult to find out how much acid it takes toneutralise a base to form a neutral solution. I will use one molar ofNitric Acid as the acid and one molar of Ammonium Hydroxide as thebase. So this will be a 11 ratio. (Molarity = how many molecules ofthe acid or alkali per 1000 cm3 (1 litre) of water.)Nitric Acid + Ammonium Hydroxide Ammonium Nitrate + Water-----------------------------------------------------------HNO + NH OH NH NO + H OIonic bonding must take place to form the salt and the water. Ionshave been formed because the original atoms have lost or gainedelectrons. These ions then have electrical charges because they do nothave the same amount of positive protons and negative electrons. Atomsthat loose electrons are called cations and have a positive charge.Atoms that have gained an electron and have a negative charge arecalled anions.The General equation for making water isH + OH H O---------------In this equation the henry ion has lost and electron and has becomea cation with a positive charge. The Hydroxide ion has gained anelectron and has become a negatively charged anion . Ionic bonds arecreated when ions commix in order to share and thus becomeelectrically stable.From the main neutralisation equation I have circled the parts to makewaterHNO + NH OH NH NO + H OEquipmentAmmonium Hydroxide (base)Nitric Acid (acid)Methyl Oxide - (to show the pH of the solution)Clamp (to hold the burette safely and securely in place)Burette - (to hold the acid)White Tile Funnel (to pour the acid into the burette)Goggles - (to protect the eyes)Conical Flask (to hold the base)Measuring Cylinder (to card out the acid and the base)PreliminaryBefore we began our practical our teacher performed the experiment asan example to our class. The teacher set up the equipment as shownabove. She informed us of the safety precautions and then began theexperiment. She used 20ml of Ammonium Hydroxide (base), placing thatin the conical flask. Then she added 6 drops of Methyl Orange(indicator). From the Burette she added 12ml of Nitric acid andswilled the conical flask. After this point she decided to control theamount added to the base and indicator by using the burette.