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

Neutralisation - How much acid is required to neutralise a base Introduction ============ Neutralisation is the reaction of a base with an acid to form a neutral solution; which contains salt and water. Acid + Base Salt + Water --------------------------- In my experiment I am trying to find out how much acid it takes to neutralise a base to form a neutral solution. I will use one molar of Nitric Acid as the acid and one molar of Ammonium Hydroxide as the base. So this will be a 1:1 ratio. (Molarity = how many molecules of the acid or alkali per 1000 cm3 (1 litre) of water.) Nitric Acid + Ammonium Hydroxide à   Ammonium Nitrate + Water ----------------------------------------------------------- HNO + NH OH NH NO + H O Ionic bonding must take place to form the salt and the water. Ions have been formed because the original atoms have lost or gained electrons. These ions then have electrical charges because they do not have the same amount of positive protons and negative electrons. Atoms that loose electrons are called cations and have a positive charge. Atoms that have gained an electron and have a negative charge are called anions. The General equation for making water is: H + OH H O --------------- In this equation the Hydrogen ion has lost and electron and has become a cation with a positive charge. The Hydroxide ion has gained an electron and has become a negatively charged anion. Ionic bonds are created when ions combine in order to share and thus become electrically stable. From the main neutralisation equation I have circled the parts to make water: HNO + NH OH à   NH NO + H O Equipment Ammonium 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 measure out the acid and the base) Preliminary Before we began our practical our teacher performed the experiment as an example to our class. The teacher set up the equipment as shown above. She informed us of the safety precautions and then began the experiment. She used 20ml of Ammonium Hydroxide (base), placing that in the conical flask. Then she added 6 drops of Methyl Orange (indicator). From the Burette she added 12ml of Nitric acid and swilled the conical flask. After this point she decided to control the amount added to the base and indicator by using the burette. Neutralisation - How much acid is required to neutralise a base :: GCSE Chemistry Coursework Investigation Neutralisation - How much acid is required to neutralise a base Introduction ============ Neutralisation is the reaction of a base with an acid to form a neutral solution; which contains salt and water. Acid + Base Salt + Water --------------------------- In my experiment I am trying to find out how much acid it takes to neutralise a base to form a neutral solution. I will use one molar of Nitric Acid as the acid and one molar of Ammonium Hydroxide as the base. So this will be a 1:1 ratio. (Molarity = how many molecules of the acid or alkali per 1000 cm3 (1 litre) of water.) Nitric Acid + Ammonium Hydroxide à   Ammonium Nitrate + Water ----------------------------------------------------------- HNO + NH OH NH NO + H O Ionic bonding must take place to form the salt and the water. Ions have been formed because the original atoms have lost or gained electrons. These ions then have electrical charges because they do not have the same amount of positive protons and negative electrons. Atoms that loose electrons are called cations and have a positive charge. Atoms that have gained an electron and have a negative charge are called anions. The General equation for making water is: H + OH H O --------------- In this equation the Hydrogen ion has lost and electron and has become a cation with a positive charge. The Hydroxide ion has gained an electron and has become a negatively charged anion. Ionic bonds are created when ions combine in order to share and thus become electrically stable. From the main neutralisation equation I have circled the parts to make water: HNO + NH OH à   NH NO + H O Equipment Ammonium 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 measure out the acid and the base) Preliminary Before we began our practical our teacher performed the experiment as an example to our class. The teacher set up the equipment as shown above. She informed us of the safety precautions and then began the experiment. She used 20ml of Ammonium Hydroxide (base), placing that in the conical flask. Then she added 6 drops of Methyl Orange (indicator). From the Burette she added 12ml of Nitric acid and swilled the conical flask. After this point she decided to control the amount added to the base and indicator by using the burette.