How metals react with Acids
HOW METALS REACT WITH ACID AND WATER A) How Metals react with Acids: The reaction of metals with acids starts off by the hydrogen being displaced. Mostly in the reaction a Metal becomes a Cation when it looses one or more valence electrons to bond with the acid and so the Acid becomes an Anion. The Result is an ionic bond, ionic compound. Sodium + Sulphuric Acid --> Sodium Sulphate + Hydrogen After the reaction occurs the result is the compound of the acid and metal used and the reaction would also release Hydrogen. We Might have to balance the equation because of the oxidation state and formulae of the Acid After a Metal and Acid react and substance called salt is made that is an ionic compound made from the neutralisation of a Metal and an Acid Different Metals have different rates of reactions, Metals like Sodium react dangerously Fast Acids like nitric acid have such an oxidation state that makes them react violently with other metals and may cause explosive reactions. Its reaction with a metal does not liberate hydrogen and salt produced usually has a very high oxidised state and heavy corrosion may be the result that is there would be a break down in the properties of the metal reacting with it and nitrogen oxide is produced B) How Metals react with Water: When a metal reacts with water it displaces the hydrogen in the water. Metals react with water more
Reactions of the Period 3 elements
Reactions of the Period 3 elements In this essay, I would like to describe the reactions of the Period 3 elements from sodium to argon with water, oxygen and chlorine. Reactions with water For sodium, sodium has a very exothermic reaction with cold water producing hydrogen and a colourless solution of sodium hydroxide. For magnesium, magnesium has a very slight reaction with cold water, but burns in steam. A very clean coil of magnesium dropped into cold water eventually gets covered in small bubbles of hydrogen which float it to the surface. Magnesium hydroxide is formed as a very thin layer on the magnesium and this tends to stop the reaction. Magnesium burns in steam with its typical white flame to produce white magnesium oxide and hydrogen. If you are heating the magnesium in a glass tube, the magnesium also reacts with the glass. That leaves dark grey products (including silicon and perhaps boron from the glass) as well as the white magnesium oxide. The oxide is also produced on heating in steam. Hydroxides are only ever produced using liquid water. For aluminium, aluminium powder heated in steam produces hydrogen and aluminium oxide. The reaction is relatively slow because of the existing strong aluminium oxide layer on the metal, and the build-up of even more oxide during the reaction. For silicon, there is a fair amount of disagreement in the books and on the
Finding the concentration of oxalic acid in a mixture with sulphuric acid
The redox titration will be done between potassium permanganate and ethanedioic acid. This reaction requires acid catalyst because ethanedioic acid is too weak an acid to make the solution acidic enough to react at a reasonable rate. Sulphuric acid is in the mixture and provides the acid catalyst. The ethanedioic acid in the mixture will reduce the manganate(VII) ions (MnO4-) into manganese(II) ions (Mn2+). The potassium permanganate will oxidise the oxalic acid into carbon dioxide. H2C2O4(aq) + MnO4-(aq) ? CO2(g) + Mn2+(aq) Reactants Products H2C2O4: Carbon +3 CO2: Carbon +4 MnO4-: Manganese +7 Mn2+: Manganese +2 To work out the ionic equation, balanced electron-half equations for both the potassium permanganate and the ethanedioic acid have to be worked out. Adding electrons (e-), water (H2O) and hydrogen/hydroxide ions (H+/OH-) depending on the conditions, they can be created. Manganate(VII) ions are reduced to form manganese(II) ions. MnO4- + 8H+ + 5e- ? Mn2+ + 4H2O Ethanedioic acid is oxidised to form carbon dioxide. H2C2O4 ? 2CO2 + 2H+ + 2e- The two equations combine and are
Experiment: Titration Aim My aim is to find the volume of hydrochloric acid needed to neutralise sodium hydroxide.
Experiment: Titration Aim My aim is to find the volume of hydrochloric acid needed to neutralise sodium hydroxide. Theory Titration is a laboratory method used to analyse a chemicals concentration. In this experiment 10cm3 of sodium hydroxide should be neutralised by 10cm3 of hydrochloric acid. Phenolphthalein is used in this experiment as an indictor where the base is a pink colour and acid as a cloudy white colour. When they are use to neutralise each other the mixture goes clear at the endpoint. The endpoint is where the number of moles in both solutions is equal. Different types of titration: * Acid based titration - neutralisation between an acid and a base * Redox titration - form of oxidation reduction * Complexometric titration - used to find certain ions Equipment The equipment I am going to use in this experiment; * Funnel * Hydrochloric acid * Sodium hydroxide * Bosshead / clamp * Stand * Conical flask * Burette * White tile * Goggles * Measuring cylinder * Phenolphthalein Funnel Diagram Bosshead / clamp Burette stand Sodium hydroxide Phenolphthalein White tile measuring cylinder hydrochloric acid Conical flask Method . First I have to collect the equipment, Funnel, hydrochloric acid, sodium hydroxide, bosshead / clamp, stand, conical flask, burette, white tile, goggles, measuring cylinder and
Titration Lab Report
CHEMISTRY LAB Titration Curves of Strong and Weak Acids and Bases Processing the Data: Questions: . Examine the time data for each of the Trials 1-4. In which trial(s) did the indicator change color at about the same time as the large increase in pH occurred at the equivalence point? In which trial(s) was there a significant difference in these two times? In all the 4 trials, the time taken for color change and the time taken for a large increase in pH was the same, leaving no significant difference between the two values. 2. Phenolphthalein changes from clear to red at a pH value of about 9. According to your results, with which combination(s) of strong or weak acids and bases can phenolphthalein be used to determine the equivalence point? The combination of a Strong Acid and Base will give us the equivalence point: there will be a color change of phenolphthalein at pH 9. It is also observed that the reaction between a Weak Acid and Strong Base can be used to obtain a pH of 9. 3. On each of the four printed graphs, draw a horizontal line from a pH value of 9 on the vertical axis to its intersection with the titration curve. In which trial(s) does this line intersect the nearly vertical region of the curve? In which trial(s) does this line miss the nearly vertical region of the curve? For Trials 1 and 3, the horizontal line from pH 9 intersects the S curve. For
Calculating the DHc of the combustion of alcohols.
Sam Forshaw Calculating the ?Hc of the combustion of alcohols. Aim: To work out the ?Hc of the alcohols: ethanol, methanol, pentan-1-ol, butan-1-ol and propan-1-ol by using calorimetry. The idea in this experiment is that if you burn a substance to heat water there is a link between the rise in temperature of the water and the amount of energy the substance contains. For this you need to know the amount of the substance you have burned and the volume and mass of the water you are heating. For this experimant I wil use a copper container for the water, place an aluminium lid on top (to prevent heat loss) and a spirit lamp containing the alcohol that I will be burning. There are however problems with this experiment. Not all of the heat from the reaction will go into the water, much of this energy will be lost to the surroundings and the copper container and aluminium also absorb some of the heat and rise in temperature also. Both of these factors greatly reduce the amount of heat energy produced by the combustion of the alcohol that is available to heat the water. The standard definition for enthalpy change is 'Enthalpy change is the amount of heat energy taken in or given out during any change in a system, provided the system is kept at constant pressure'. Standard enthalpy changes (?H?) are these that occur under standard conditions of 100kPa, 298K and 1 mol dm-3 and
Application of Hess's Law to determine the enthalpy change of hydration of Magnesium sulphate
? Name: Penguin Chow Cheuk Yan ? ? Class: 6S Class Number: 14 ? ? Date: 04 - 11 - 2002 ? Chemistry Full Report Experiment 5 Title: Application of Hess's Law to determine the enthalpy change of hydration of Magnesium sulphate (VI) Aim: Using Hess's Law to find the enthalpy change of hydration of magnesium sulphate (VI) Theory: Hess's Law can be defined as the heat given off or absorbed by a reaction is independent of the route taken. In this experiment, the enthalpy change of hydration of Magnesium sulphate (VI) cannot be directly measured by calorimetry in the laboratory as hydration is a very slow process. ?H1 = enthalpy change of hydration of MgSO4(S) ?H2 = molar enthalpy change of solution of hydrous MgSO4(S) ?H3 = molar enthalpy change of solution of MgSO4• 7H2O(S) According to Hess's law, the enthalpy of the overall reaction should be equal to the sum of the enthalpies of the two sub-reactions. Thus, this value can be calculated by applying Hess's Law Procedure: A. Determine the enthalpy change of solution of MgSO4(S) . A balance was used to weigh the empty polystyrene foam cup 2. 50 cm3 of deionized water was poured from the measuring cylinder to the polystyrene cup 3. The temperature of the water in the cup was measured using a thermometer 4. 0.025 mole of anhydrous magnesium sulphate (VI) was weighed accurately by the balance and was added into
Organic and Inorganic Fertilisers
Organic and Inorganic Fertilisers A fertiliser is a chemical or natural substance added to soil to increase its fertility. (From The Concise Oxford English Dictionary.) Organic fertilisers are derived from animal or plant remains that decompose on or in the soil, slowly releasing mineral ions. Inorganic fertilisers are manufactured and consist of mineral ions and are usually sprayed onto soil in solution. Fertilisers are needed because in natural ecosystems, decomposition recycles mineral ions whereas with crops the plants are removed at harvest and therefore the minerals are removed and not replaced. All growing crops require nutrients to stimulate photosynthesis and growth throughout the growing season. (Arable Handbook brochure from Kemira Grow-How.) Some of which are more important than others. The major nutrients are nitrogen, phosphate and potassium. The secondary nutrients are calcium, sulphur, magnesium and sodium and the trace elements are manganese, iron, selenium, copper, cobalt, boron, zinc and iodine. (Multi-choice leaflet from Carrs Fertilisers.) Proportions of elements required for healthy plant growth Of the elements required for healthy plant growth, oxygen, carbon and hydrogen account for 96? - 45? carbon, 45% oxygen and 6% hydrogen. Fig 1: - A graph to show proportions of the elements required for healthy plant growth (The Organic Garden Book by
Objective:-To prepare a buffer solution and observe the properties of a buffer
Experiment E5 Preparation and Properties of a buffer Date: 23.3.2011 Name: Leung She Ting Cherry Class: 6A 20 Objective To prepare a buffer solution and observe the properties of a buffer Introduction Buffer is a solution that can resist dramatic pH change when a small amount of acid or alkali is added to it. It is made up of equal amount of a weak acid/alkali and its conjugate base/acid. The working principle of buffer can be demonstrated as below: Ethanoic acid is a weak acid that undergoes slight dissociation, CH3COOH (aq)+H2O(l) CH3CHCOO-(aq) + H3O+(aq) where the equilibrium position mainly lies on the left side. At the same time, sodium ethanoate undergoes complete dissociation, CH3COONa (aq) CH3COO- (aq) + Na+ (aq) in which its equilibrium position lies mainly on the right side. When a small amount of acid is added to the solution, the addition of H3O+(aq) will shift the equilibrium of CH3COOH (aq)+H2O(l) CH3CHCOO-(aq) + H3O+(aq) to the left. The increase of [CH3COOH] does not cause a significant change in pH, thus the pH of the solution is kept almost constant. On the other hand, if a small amount of base is added to the solution, CH3COOH(aq) will react with the base, giving out salt i.e. CH3COONa. This shifts the equilibrium of CH3COONa (aq) CH3COO- (aq) + Na+ (aq) to
Chem Lab report. Standardization of hydrochloric acid by sodium carbonate solution
Laboratory Report: Experiment 1 Standardization of hydrochloric acid by sodium carbonate solution Name: Cheung Chun Hin, Harry Class: 6L (12) Date: 11-9-2009 Objective: To determine the concentration of hydrochloric acid using sodium carbonate solution as a primary standard in volumetric analysis (acid-base titration) Principle of method: The concentration of the hydrochloric acid can be determined by the titration reaction between hydrochloric acid and sodium carbonate solution. Na2CO3 (aq) + 2HCl (aq) H2O (l) + CO2 (g) + 2NaCl (aq) From the above equation, We measure the volume of hydrochloric acid used in the titration (the difference of reading on the burette) and use it in calculating the concentration of hydrochloric acid. So the molarity of the hydrochloric acid Procedures: . The mass of anhydrous sodium carbonate required was weighed to prepare 250.0 cm3 of 0.05M sodium carbonate solution. 2. All anhydrous sodium carbonate was dissolved in a beaker with a suitable amount of deionized water and the mixture was stirred. 3. Sodium carbonate solution was poured into a 250.0 cm3 volumetric flask and it was made up to the graduated mark using deionized water. 4. The volumetric flask was shaken upside down for several times. 5. 25.0 cm3 of sodium carbonate solution was pipetted into a conical flask. 6. 3 drops of methyl orange indicator was added into the
