How much Iron (II) in 100 grams of Spinach Oleracea?

How much Iron (II) in 100 grams of Spinach Oleracea? Spinach Oleracea Name : Jade Taylor Candidate Number : 3689 Centre Number : 58203 Year of Entry : 2004 Contents Plan Aim To found out how much Iron (II) is present in 100 grams of Spinach Oleracea. The factors that I am going to investigated in this experiment include finding the best method to determine the concentration of an Iron (II) Ammonium Sulphate (aq) by trying colorimetry, an electrochemical cells experiment and a redox titration with Potassium Manganate (aq). After this I will extract Iron (II) from Spinach Oleracea using various methods (i.e. boiling the Spinach Oleracea for a range of times in different solutions) and use this spinach extract solution to determine the volume of iron extracted. I will take into account the presences of Oxalate ions and change my experiment accordingly (i.e. heating the spinach extract solution before titration's). Introduction It is important to know the Iron (II) content in 100 grams of Spinach Oleracea, as this allows people to calculate how much Spinach Oleracea needs to be eaten in order to obtain the Recommended Daily Allowance (RDA) of Iron (II). As shown in the table below the Recommended Daily Allowance for Iron (II) varies with age and sex (2) The Recommended Daily Allowance of Iron (II) (2) Age Amount (mg) Youth -3 6 4-12 8 Males 3-18 0

  • Word count: 20005
  • Level: GCSE
  • Subject: Science
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Investigating the effects of changing the concentration of different solutions on the refractive index and the conductivity

Physics Investigation --- Investigating the effects of changing the concentration of different solutions on the refractive index and the conductivity Content Aim P.2 Summary P.2 Risk assessment P.2 Information on errors / uncertainties P.2 Background P.3-7 Refractive index P.3-7 Diary P.7-13 Day 1 P.7 Day 2 P.7 Day 3 P.8 Day 4 P.9-10 Day 5 P.10-11 Day 6 P.11-12 Day 7 P.12 Day 8 P.12-13 Analysis P.13 Background P.14-15 Conductance P.15 Dairy P.15-16 Day 9 P.15 Day 10 P.16 Analysis P.16 Evaluation P.17 Conclusion P.17 Bibliography P.18 Appendix P.19-24 1 P.19 2 P.20 3 P.21 4 P.22 5 P.23 6 P.24 Aim The main aim of this investigation is to find out how some of the properties of solutions change when their concentration is altered. Summary When I was told that we were going to do this practical investigation, I struggled for a while not knowing what to do. But as I searching more and reading more about A Level experiments, they conjured up lots of different ideas in my head. When it came to the time for our plan, I decided to investigate the effect of changing the concentration of different solutions on the refractive index. At the beginning, I had some troubles in choosing suitable equipment. When I tried out some trials, they seemed alright. However due to a few problems arose, I had to change my idea slightly. So instead, I investigated the

  • Word count: 7812
  • Level: GCSE
  • Subject: Science
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To investigate the rate of reaction between different concentrations of hydrochloric acid with metal carbonates using calcium carbonate as an example.

To investigate the rate of reaction between different concentrations of hydrochloric acid with metal carbonates using calcium carbonate as an example. Aim We are going to investigate how concentration affects the rate of reaction; we will be reacting calcium carbonate (CaCO3) with hydrochloric acid (HCl). We will make this a fair test by keeping all the variables the same except the one we are investigating. The products of the reaction between the two are water (H2O) and carbon dioxide (CO2). The equation for this reaction is: Calcium + Hydrochloric › Calcium + Carbon + Water Carbonate Acid Chloride Dioxide Solution CaCO3 (s) + 2HCl (aq) › CaCl2 (aq) + CO2 (g) + H2O (l) To measure the rate of the experiment, I could measure the amount of carbon dioxide (CO2) produced by the experiment at timed intervals (gas syringe experiment), or the decreasing mass of the reactants (mass reduction experiment). Alternatively, I could, measure the time to which the reactants react completely. The size of the calcium carbonate (CaCO3) available is either in granules (at an average) of ˜ 0.5 cm measured lengthways (weight ˜ 0.4-0.7 gm) or in powdered form. The highest concentration of acid available for use in the experiment is 2 mol dm-3. Variables Many different variables can affect the rate of reaction, below is a list

  • Word count: 7291
  • Level: GCSE
  • Subject: Science
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The aim of this experiment is to answer the following question: What is the effect of temperature on the equilibrium constant for the hydrolysis of an ester?

Scott Mabbutt Individual Investigation Aim: The aim of this experiment is to answer the following question: What is the effect of temperature on the equilibrium constant for the hydrolysis of an ester? The reaction I aim to investigate is a reversible reaction where an ester (an organic compound with RCOOR group) is produced and. Esters are generally insoluble in water but are soluble in other solvents. Esters are formed in an esterification reaction where and carboxylic acid (RCOOH group) and an alcohol (ROH), react to form an ester. Below is the esterification reaction/ester hydrolysis reaction. Alcohol + Carboxylic acid Ester + Water The Equipment and apparatus I will be using in my investigation are as follows: * Safety Goggles * Test Tube x 5 * Test tube stoppers x 5 * Water Bath with thermostatic control * Test tube holder (suitable for use in water baths) * Burette * Clamp stand with clamp fixings * Safety Mat * Funnel * 250ml Beaker * 250ml Conical Flask * 10ml Measuring cylinder * Thermometer * White tile Safety goggles will be worn so that the risk of chemicals coming into contact with the eyes is lessened (see risk assessment). Test tubes are being used as the environment for the reaction to take place, they are glass so can be monitored and can be easily stored in a test tube holder in the water

  • Word count: 7186
  • Level: GCSE
  • Subject: Science
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Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress Seeds

Investigating the Effects of Increasing Copper Sulphate Solution Concentrations on the Germination of Cress Seeds Hypothesis: I think that as the copper concentrations in the solution rise above natural levels (0.06mg/l), then the seeds will suffer from copper toxic levels, and germination will be stopped. Factors affecting the investigation: * Light availability * Micronutrients availability: copper, zinc, boron, chlorine * Macronutrients availability: nitrogen, sulphur, phosphorus, potassium, calcium, iron, magnesium * Water availability * Temperature * Oxygen availability * Enough time for germination to occur * Enough space for the seeds to germinate Method: Equipment needed (for doing experiment once): * 500ml of copper sulphate stock solution of 60mg/dm-3 * 500ml of pure distilled water * Micropipette * 7 Large Beakers * Stirring rod * 168 clean plant pots, diameter 20cm (7x24) * Cling Film * Filter paper, diameter 20cm * 2520 cress seeds (168x15) * Ruler with millimetre measurements * Glass screen * Needle * Gloves * Digital Thermometer * Magnifying glass Method For Changing Independent Variable: I will change the independent variable, copper concentration, by using a stock solution of 60mg/l. With this stock solution I will use ten fold serial dilutions to make 5 new concentrations of copper sulphate and then I will make a solution of

  • Word count: 6884
  • Level: GCSE
  • Subject: Science
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The Rates of Reaction of Metals with Acid.

"A" Level Chemistry (Nuffield) IN1: The Rates of Reaction of Metals with Acid Student Number 5122 By Anthony Parker Introduction I plan to study and experiment on two different aspects of chemical kinetics. These include. * Activation energy. Activation energy is the amount of energy; it takes for a known substance to collide (collision theory) with another and react to form product(s). * Order of reaction. By the meaning of 'order of reaction', we mean what the rate of the reaction is. We study this because there are several factors that can affect the rate of a reaction. These include concentration/pressure, temperature or the presence of a catalyst. * What is an acid? The definition of a strong acid is an acid that almost fully ionises (donates its proton/hydrogen atom) in water, a weak acid is an acid that only partially ionises (donates its proton/hydrogen atom) in water. Activation Energy. Reactions can only happen when the reactants particles collide, but most collisions are not successful in forming product molecules. The reactant molecules must collide with enough energy to break the original bonds so that new bonds in the product molecules can be formed. At a particular temperature the energy of each individual molecule are distributed according to the Boltzmann's distribution. There would then, theoretically, be a set number of molecules with

  • Word count: 6869
  • Level: GCSE
  • Subject: Science
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Enthalpy of Neutralisation.

TITLE: Enthalpy of Neutralisation. AIM AND HYPOTHESIS: My aim in this experiment is to compare the enthalpy change of neutralisation by titration, for each reaction between the following 3 acids: Sodium hydroxide (NaOH) and hydrochloric acid (HCl) - pH 1 Sulphuric acid (H2SO4) and NaOH - pH 1 NaOH and Ethanoic acid (CH3COOH) - pH 2.88 - 3 I predict the reaction between the above-mentioned acids would be exothermic because heat will be given off during the reactions and the temperatures will be rising due to the heat evolved. I also predict the reaction between the chemicals is exothermic because the energy content of the products is less than that of the reactants, resulting to heat being given out from the system. These predictions show that the stronger the acid used in neutralization, the more energy is released per mole of water. I will be able to compare these predicted energy changes with my actual results after my experiment. When I have my results- the temperature change from beginning to end of the experiment - I can use the equation Energy change = mass of solution x temperature change x specific heat capacity of water to work out the actual energy change. In neutralization, we assume that the density of the acid/alkali is the same as that of water, so volume of acid = mass of acid. We know that the specific heat capacity of water is always 4.2 Jk - 1 g

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  • Level: GCSE
  • Subject: Science
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Rates of Reaction

Rates of Reaction coursework Aim: My aim is to see how the concentration of hydrochloric acid affects the rate of reaction, using marble chips. Prediction: Primarily I state my hypothesis to be; that the increase in concentration (hydrochloric acid) of reactants will increase the collision frequency between the reactants, this and calcium carbonate. Therefore the effective collision frequency also increases. A chemical reaction is where the molecules of reactants either combine or separate, in this case we are looking at the displacement of the between calcium carbonate and hydrochloric acid, below is the formula for this reaction: 2HCl (aq) + CaCO3 (s) ----> CaCl2 (aq) + H2O (l) + CO2 (g) Hydrochloric acid + Calcium carbonate --> Calcium chloride + water + carbon dioxide Reactants: 2HCl (aq): hydrochloric acid (aqueous) CaCO3 (s): calcium carbonate (solid) Products: CaCl2 (aq): calcium chloride (aqueous) H2 O (l): water (liquid) CO2 (g): carbon dioxide (gas) I will now state the principals of the collision theory in order to elucidate the reaction. Max Trautz and William Lewis first proposed this theory in 1916 that qualitatively explains how chemical reactions occur and why reaction rates differ depending on the reactants and reactions. It assumes that for a reaction to be successful the reactant particles must collide, but only a certain fraction of the

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  • Level: GCSE
  • Subject: Science
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Determine the concentration of lime water.

Chemistry concentration of lime water. AS- Assessed Practical Chemistry Aim: To determine the concentration of lime water Plan The aim of this experiment is to find the concentration of a sample of limewater solution in g dm?3. I am required to design my own experiment and choose a range of appropriate equipment and apparatus. The indicator will be supplied to me. I am provided with 250 cm3 of limewater, which has been made such that it contains approximately 1g dm?3 of calcium hydroxide. Also available is hydrochloric acid which has a concentration of 2.00 mol dm?3, this concentration is too much though so it is necessary to dilute it. The apparatus, equipment and chemicals that I will use are as follows: - ) Pipette 25cm3 2) Volumetric flask 500cm3 3) Conical flask 250cm3 4) Burette 5) White tile 6) Clamp and stand 7) Indicator (methyl orange) 8) Limewater (250cm3 with 1g dm?3 of calcium hydroxide) 9) Hydrochloric acid- standard solution (conc. 2.00 mol dm?3) 0) Distilled water Slaked lime dissolved in water is called limewater. Quicklime + Water ? Slaked lime CaO(s) + H2O(l) ? Ca(OH)2(s) Calcium oxide reacts violently with water to produce calcium hydroxide (slaked lime) Addition of further water to Calcium hydroxide produces the saturated aqueous solution known as Limewater. In the experiment it is necessary to react the Hydrochloric acid with the

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  • Level: GCSE
  • Subject: Science
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To investigate the effect of concentration on the temperature rise, heat evolved and heat of neutralization for the reaction between HCl and NaOH.

Aim: - To investigate the effect of concentration on the temperature rise, heat evolved and heat of neutralization for the reaction between HCl and NaOH. Neutralization is the special name given for the reaction between an acid and an alkali leading to the formation of water molecules and a salt. The reactions between basic oxides, or hydroxides, and acids are very important and are called neutralizations. Since the metallic ions and anions from the acid do not change, the essential reaction of neutralization is always the formation of non-ionized molecules of water from the hydroxide and hydrogen ions. H+ (aq) + OH- (aq) H2o (l) The following are examples of neutralizations. The metallic ions and the negative ions from the acids remain to produce the salt. 1/2 H2+So4- (aq) + 1/2 Na+OH- (aq) › 1/2 Na+So4- (aq) + H2o (l) Sulphuric acid Sodium hydroxide Sodium sulphate water H+No3- (aq) + Na+OH- (aq) › Na+No3- (aq) + H2o (l) Nitric acid Sodium hydroxide Sodium nitrate water H+cl- (aq) + Na+OH- (aq) › Na+Cl- (aq) + H2o (l) Hydrochloric acid Sodium hydroxide Sodium chloride

  • Word count: 5717
  • Level: GCSE
  • Subject: Science
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