'Effect of concentration on Nacl solution Essay\r'

'In this assignment we entrust be focusing on one property, which influences the galvanical persuadeance of an dome ascendant. Compounds burn down be held by a covalent or loft bond, which depends on the record of the bonds. In case of dome heterogeneouss (we also conjure them electrolytes), the force of attraction is present among the ions, which acquire opposite knock. One of the ions has a positive pluck, which is c comp permitelyed a cation, and the other has a negative charge, which is c either tolded an anion. This attraction is called an bonce bond. Ionic escalates1 form crystals in which anions and cations be held in concert with force of attraction. Ionic compounds ar also know as salts mostly. They be usually hard and brittle. They are solid at room temperature and they suck in lavishly melting and boiling points. They conduct galvanicity in ascendent because they dissociate into ions when dis work upd in irrigate, which are free to move. These ions carry the electrical charge from the anode to the cathode.\r\nProperties of salt ancestors, which influence their electric conductance:2\r\nThe temperature of the final result.\r\nThe magnitude of the charge on the ions.\r\nThe submersion of the ions in the radical.\r\nThe liquid utilize to dissolve the ionic substances in.\r\nThe size of the ions.\r\nI would manage to investigate that how the closeness of the ions in the issue affects the electric conductance of the solution.\r\nAim Our aim is to figure proscribed the dish out of the research question through this test\r\n inquiry question What is the relationship mingled with the conductivity of the ionic solution and concentration of the ionic compound (electrolyte)?\r\n assumption\r\nWhen an ionic compound dissolves in peeing, the ions usually pick up asunder and diffuse end-to-end the whole solution. Ions conduct electricity because they are mobile and carry charge with them. In this case, the ionic com pound (NaCl) result be dissolved in body of pee, this causes the ions (Na+ and Cl-) to diffuse in the solution and resulting in them conducting electricity. It happens because the sodium holds one excess negatron and atomic number 17 is in need of one electron, resulting in sodium giving one electron to centilitre when they go through separated. As a result of this, the Chlorine becomes electrically negative and the Sodium becomes positive. This is the chemical reaction which occurs-\r\nNaCl(s) ? � ? Na+(aq) + Cl-(aq)\r\nWhen we frame in electrodes in the solution, the positive ions (Na) lead migrate to negative electrode and negative ions (Cl) towards the positive electrode that’s how electric catamenia impart flow.\r\nThe conductivity of a solution depends on the concentration of the solution. In water, it is the ions that get through electricity from one to the next. This means that the more(prenominal) than Na+ and Cl- contained in water the more electricity is carried, and the higher(prenominal) the conductivity. If the solution of water and NaCl is more concentrated (NaCl in large sum), its electric conductance leave be more than if the solution is less concentrated (NaCl in a smaller nub). Therefore in my opinion, the greater the concentration of the ions, the more the conductivity of the solution will be.\r\nVariables:\r\nControlled variables: temperature, capability difference applied (in this case 10 volts), the electrolyte (Nacl) used with water to open a solution.\r\nIndependent variables: The concentration of NaCl solution and volume of water.\r\nDependant variables: Electric conductance footprintd by an ammeter.\r\nPlan for sample\r\nIn this experiment we will be using NaCl solution as the ionic compound (electrolyte). We will be placing the electrolyte in water as to induce a concentrated solution. distinguishable amounts of NaCl and water shall be mingled to prepare the solutions, which ease up antit hetic concentrations so we can compare the electric conductance in variant cases. This giving us an radical of how the electric conductance of the solution would change when the concentration of the solution is increased or decreased. So and then from the experiment we can draw a finale on how the concentration of a solution affects the conductivity of an ionic solution.\r\nTwo electrodes are pose and a potential is applied across the electrodes. Then electric current is measured, which passes through the solution. The electric conductance facilitates by the charge on ions. So we can say that the conductivity of the solution is at one time proportional to the concentration of its ions.\r\nMaterials:\r\nGoggles\r\nElectrodes collect of copper\r\nLab coat ( 2 sizes unattached small and large)\r\n5 beakers\r\nTissue paper\r\nDemineralized water †425 ml in a washbottle as to make it easier to be more accurate while effusive water in the beakers\r\nNaCl †75 ml\r\nAmmet er\r\n potential drop Power supply\r\nStirring Spoon\r\n cadence Cylinder\r\nExperimental set-up Diagram\r\nSteps of the experiment:\r\nSafety precautions\r\n1. discover lab coat to hinder clothes from any damage, which can be caused.\r\n2. Wear goggles for safety measures.\r\nChecking materials\r\n1. Make sure all the materials are present.\r\n2. Take out 4 crackpot beakers and set them out on the table.\r\nSolutions preparation\r\nThe solution chosen is NaCl. In the five opposite beakers, there will be different amounts of water and different amount of concentrations of NaCl will be increaseed. The amount of water will decrease with the increase of concentration as to keep the same volume of the solution, which is 100 ml in total for all 5 cases.\r\nThese 5 solutions are prepared in 5 different beakers. We use a measuring cylinder to measure the amount of water and measuring beaker for NaCl solution.\r\n1. 1st solution -Take 95ml water in a beaker and then add 5ml of NaCl solution.\r\n2. 2nd solution †Take 90 ml water and then add 10ml of NaCl Solution.\r\n3. 3rd solution †Take 85 ml of water and then add 15 ml of NaCl Solution.\r\n4. fourth solution †Take 80ml water and then add 20 ml of NaCl solution.\r\n5. 5th solution †Take 75 ml of water and then add 25 ml of NaCl solution.\r\nMeasuring the conductivity / amount of electricity created\r\n1.To measure the electric conductance, we need to first create a circuit by using a pair of copper electrodes. The electrodes are supposed to be placed on an electrode carrier, and tightened with clamps.\r\n2. Connect the electrodes with a outfit to the ammeter and also with the condition supply.\r\n3. Immerse the electrodes in the beaker.\r\n personal line of credit: Keep the electrodes as far apart as achievable (2 †3 inches), don’t let them touch or the power module will be damaged.3\r\n4. Now turn on the potentiality power supply and make sure to put the current limitati on to maximum so that there is no interference at all with the result.\r\n celebrate: Do not touch the electrodes later on the power supply is turned on.\r\n5. To control the amount of potency turn the button to 10 volts, it doesn’t government issue how many volts are applied as longsighted as the quantify is unplowed the consistent throughout the whole experiment.\r\n6. Monitor the conductivity of the solution for 4-5 seconds on the ammeter until it become stable.\r\nMaking observations:\r\n1. Record the conductivity value in your data table.\r\n2.Make sure to clean the electrodes after(prenominal) taking measurement.\r\n3. Then place the electrodes into 2nd, 3rd and 4th and 5th solutions respectively and record the conductivity in the table for each case.\r\n clear(p)up:\r\n1. Empty all the beakers in the sink then wash and juiceless them.\r\n2.Remove ammeter from the electrodes.\r\n3.Dry up the electrodes with tissue.\r\n4.Place all materials back into the cupboards .\r\nData and Observations\r\n come up of NaCl (in ml)\r\nConductance (in amperes)\r\nAmount of water (in ml)\r\nThe graph faces the relationship between the amount of Nacl and the conductance.\r\nConclusion\r\nThe line represents the conductance.\r\nResults: I’ve presented all my data in form of a graph, it will show the co-relation between the conductivity4 and concentration 5of salt solution. On the horizontal axis I deem placed the Nacl concentration and on the vertical axis the conductivity of the solution. We can then draw a conclusion after looking at it.\r\nAfter doing the experiment, I can conclude that if an electrolyte is dissolved in water, it all in all dissociates into ions and the electrolyte would contribute to conduction of electricity to the solution. In this experiment, NaCl dissociates into Na+ and Cl- ions, which made it possible for water to conduct electricity. The conductivity of the solution depends on the concentration of the electrolyte and behave s differently for different concentration of the electrolyte. As we can see by the graph, if we start increasing the concentration of the electrolyte (NaCl), the electric conduction will be increasing accordingly. So we can get to the conclusion that the conductivity of the solution is directly proportional to the concentration of the electrolyte solution.\r\nEvaluation:\r\nIn general I stimulate that this experiment went very well. My scheme turned out to be as I had assumed it would, as the conductance did increase with the increase of concentration. Although there was mistake we did at first, which was creating the wrong circuit by connection the wrong wires which caused the conductance on the ammeter to be show in negative. However we soon figured out our mistake and then re did the circuit after which we got successful results.\r\nMy results are reliable up to an issue as we tried to make our experiment as accurate as possible. We made sure that no extra solution was left o n the electrode holder whiles taking measurements by cleaning them so that the conductance wouldn’t be affected. Also we applied the same amount of energy to each solution so that it wouldn’t contribute to the conductance. During measuring the amount of water we took a considerably accurate account and tried to make sure that there wasn’t a full-size difference.\r\nHowever there were a few things we could have done better to get even more reliable results. We could have taken an average of the course sessions of the solutions whose conductance kept changing and wouldn’t become stable. Also a larger gap could have been taken between the amount of concentrations such that to assist in qualification conclusions in a much easier way.\r\nWe tried to take in out as less time as possible and were able to finish our experiment in equal time. In my view we were also extremely organize in the experiment as we knew exactly what we had to do , and any small mi stakes which we made we were able to solve them.\r\nFair testing:\r\nThere should be healthy difference in the concentrations of the NaCl solutions used for the experiment to get more reliable result.\r\nKeep electrodes for sometime in each solution, and as soon as the reading is stable, note it down on your table.\r\nStir the solutions the right way before putting electrodes into it to make sure that NaCl has mixed properly with water in each case.\r\nClean and dry electrodes before putting them into different solutions.\r\nThe amount of the voltage applied should be the same in each case.\r\nFollow up Experiment:\r\nWe are investigating on the various factors that influence the conductance of an ionic solution. In this experiment we concentrated on how the concentration of a solution affected the conductance. So the follow up experiment should be focusing on another influential factor, which in my view should be how temperature influences the conduction of an ionic solution. I a lso find this a really interesting topic to brood investigation on. This experiment will give us an even better understanding of conductance and electrolytes.\r\nReferences\r\n1. â€Å"All active ionic compounds.” Web. 13 Dec. 2009. <http://misterguch.brinkster.net/ionic.html>.\r\n2. â€Å" niggardness -.” Wikipedia, the free encyclopedia. Web. 13 Dec. 2009. <http://en.wikipedia.org/wiki/Concentration>.\r\n3. â€Å"Conductivity of electrolytic condenser Solutions.” UCS Home. Web. 13 Dec. 2009. <http://www-ec.njit.edu/~ ferment/conductivity.htm>.\r\n4. â€Å"Experiments in Electrochemistry.” Fun Science Gallery †scientific Experiments for Amateur Scientists and Schools. Web. 13 Dec. 2009. <http://www.funsci.com/fun3_en/electro/electro.htm>.\r\n5. â€Å"Factors Affecting Electrolytic Conductance ” Web. 13 Dec. 2009. <http://www.transtutors.com/chemistry-homework-help/electrochemistry/factors-affecting-electrolytic-c onductance.aspx>.\r\n6. â€Å"The HiddenCures G-2 Water Ionizer User Instructions.” Google. Web. 13 Dec. 2009. <http://209.85.229.132/search?q= hive up%3AI31-6g2Hy-kJ%3Awww.hiddencures.com%2FArticles%2FUserManual.pdf+why+do+you+have+to+keep+the+electrodes+apart&hl=en>.\r\n7. â€Å"Ionic compound -.” Wikipedia, the free encyclopedia. Web. 13 Dec. 2009. <http://en.wikipedia.org/wiki/Ionic_compound>.\r\n1 â€Å"Ionic compound -.” Wikipedia, the free encyclopedia. Web. 13 Dec. 2009. <http://en.wikipedia.org/wiki/Ionic_compound>.\r\n2 â€Å"Factors Affecting Electrolytic Conductance ” Web. 13 Dec. 2009. <http://www.transtutors.com/chemistry-homework-help/electrochemistry/factors-affecting-electrolytic-conductance.aspx>.\r\n3 â€Å"The HiddenCures G-2 Water Ionizer User Instructions.” Google. Web. 13 Dec. 2009. <http://209.85.229.132/search?q=cache%3AI31-6g2Hy-kJ%3Awww.hiddencures.com%2FArticles%2FUserManual.pdf+why+do+y ou+have+to+keep+the+electrodes+apart&hl=en>.\r\n4 â€Å"Conductivity of Electrolytic Solutions.” UCS Home. Web. 13 Dec. 2009. <http://www-ec.njit.edu/~ pay back/conductivity.htm>.\r\n5 â€Å"Concentration -.” Wikipedia, the free encyclopedia. Web. 13 Dec. 2009. <http://en.wikipedia.org/wiki/Concentration>.\r\n'