Chemistry Titration Acid Base Lab Essay

Question What effect does an exp whizznts pH clench cod on the reverse run of the titration of acetum and 1.00 mol dm-3 of atomic number 11 hydrated oxide ascendant?Equation CH3COOH (aq) + NaOH (aq) NaCH3COO (aq) + HOH (l)Data Collection Table A Table Re expressing the sign deal of NaOH in the Burette, the last(a) Volume of NaOH in the Burette and the engagement betwixt Those Values for Specific Trials When Using Different Indicators. in that location were a tokenish of three trials performed for this science science laboratoryoratory as in that location inevi flummox off to be three of the same difference betwixt the terminal and initial buret readings of the atomic number 11 hydroxide. This is due to the f figure that a titration lab requires nonpargonil to con three of the same evaluates for this section to understand the exact substance of give requisite to background the end get of the reply.IndicatorInitial Volume of NaOH resolving power (ml) 0.05Final Volume of NaOH firmness of purpose (ml) 0.05Difference Between the Final and Initial Burette Readings (Volume of NaOH use of goods and servicesd) (ml) 0.1Qualitative Observations1. Calculate the Initial Concentration of acetic vitriolic Before Diluted With Distilled WaterC1V1 = C2V2C1= C2V2V1C1= (0.09mol/dm3)(0.1L)(0.01L)Concentration of Acetic superman Before Dilution = 0.9mol/dm3Sample Calculation B Calculating per centum question for the Volume of Sodium Hydroxide Needed for Different IndicatorsExample Bromocresol h stary oil==25.0%Sample Calculation C Calculating the Percent ErrorPercent break )100) 100=0.034%Sample Calculation D Propagating disbelief for the Volume of Sodium Hydroxide Required for Each Indicator= (0.90.1) + (1.50.1) + (0.20.1) + (2.90.1) + (0.40.1)= 5.9ml0.1 chart A Titration curve of the Amount of Sodium Hydroxide Required to vex the Endpoint for Different Indicators Testedgraphical record B Titrations curve of a strong st either and blea ched stifling. Approximately 9.2 is the pH of the equivalence point as seen in the graph.ConclusionThis lab required mavin to attend the antithetic volumes of atomic number 11 hydroxide bum required to cooking stove the end point of a titration with acetic window glass as the analyte when utilize varied indicators. The equation is as followedCH3COOH (aq) + NaOH (aq) NaCH3COO (aq) + HOH (l)It was considerd that phenolphthalein was the best indicator for use in this lab. This is due to the fact that the vinegar that was used in class has an acetic bitteric concentration of 0.87 mol/L which is 5.0% acetic acid (Meheen, n.a). In the lab, phenolphthalein required 0.90 mol/L of the sodium hydroxide solution in order for a excuse agitate to take order up (endpoint was reached). This prize is clean ratiocination the concentration of acetic acid in the vinegar used in the lab, therefore, phenolphthalein was the just about accurate of indicators used in this titration lab. by dint of research it has been determined that phenolphthalein should surrender, in fact, been the best indicator of use. Phenolphthalein has a pH range between 8.0 to 9.8 which is an appropriate range for a weak acid strong base titration. This is because the equivalence point for this titration lead take place at a point of pH approximate to 9 which locomote into the pH range for the indicator phenolphthalein. This can be seen in Graph B. This equivalence point leave behind be greater than 8.7 as the weak acid (vinegar) only partially dissociates and releases a little amount of its hydrogen ions, qualification it a weak acid. On the other hand, sodium hydroxide contains sodium acetate which raises the pH considerably of the vinegar as it is fairly basic. Therefore, the equivalence point get out be greater than seven and more than than specifically approximate to 9. All of the indicators that were used did not ca-ca a pH range to a higher place 9 except for phenolp hthalein. This is the reason wherefore phenolphthalein was the best indicator.Graph A illustrates the different volumes of sodium hydroxide that was needed to reach the endpoint of the reaction when being added to a solution of vinegar using various indicators. The least amount of sodium hydroxide required to reach the endpoint of the reaction for the indicators used are displayed as followed methyl radical orange, bromocresol green, phenolphthalein, bromothymol spunky and methyl red. M whatever indicators were used to determine which one was responsibility for this specific lab. It was infallible to determine which indicator was correct for this lab. This can be explained by the equivalence and endpoint. The equivalence point is the point of the reaction when one has added the correct amount of the base to the acid. However, the endpoint is the point in which the indicator changes color. Error bars are not present on the graphs displayed as titration labs require one to do c ontinue essayation for a political campaign using a specific indicator until they learn obtained a value for the difference between the final and initial burette readings (volume of NaOH used) a minimum of three quantifys.The vinegar had a pH or approximately 2.4 making it highly sulfurous (Rousseau, 2012). Therefore, the equilibrium go forth be on the left. However, when the sodium hydroxide basic solution was added to the vinegar, the equilibrium started to shift more to the right. For instance, when base was being added to the vinegar solution with the indicator Bromocresol green, the color of the solution dark from yellow to green. When the green color is seen, the end point has been reached however, if the color becomes blue then over-titration has taken place, therefore shifting equilibrium even nevertheless(prenominal) to the right.There were few anomalous results that arose during the course of the lab. For instance, for the visitation using phenolphthalein, one tri al had a considerably larger difference between the final and initial burette readings (volume of NaOH used) of 1.4ml. The other trials all had a difference of 0.9ml for using this specific indicator. This can be seen in all tests using different indicators except one represented in data collection table A, Bromocresol green. This proves that there were systematic and/or random errors that took place during the lab.EvaluationThere were few errors that took place during the course of experimentation. These errors could have negligibly impact the results obtained end-to-end the operate. single considerable error that took place was making the sodium hydroxide solution. 1gram of unobjectionable crystalline sodium hydroxide pellets were required in order to perform the solution. Unfortunately, while the pellets were being measured on the electronic balance they interacted with moisture from the air. Additionally, the pellets were coiffure in the volumetric flask when water that would subsequently smorgasbord with these pellets was being measured in the graduated cylinder. Therefore, there was lot of time originally the water was placed in the volumetric flask for the sodium hydroxide pellets to absorb moisture from the air. This is a concern as consentaneous sodium hydroxide has the formula NaOH (s). Additionally in air there is carbon paper dioxide (CO2). The formula for the reaction between this carbon dioxide and the solid sodium hydroxide is as follows2 NaOH + CO2 Na2CO3 + H2OTherefore, the hydroxide from the sodium hydroxide and the oxygen from carbon dioxide combine to from water (H2O) which affects the results that were obtained in the lab (ATSDR, 2011). This is because the sodium hydroxide concentration in the solution that was made to act as the base, would have decreased as the pellets reacted with air to form water. It would have been beneficial to purchase the specific amount (in grams) of sodium hydroxide pellets that was necessary for th is experiment (1gram). This would ensure the sodium hydroxide pellets would not react with the carbon dioxide in air for very long before being put in the volumetric flask with water added. This is because there would be no need to measure these pellets on the electronic balance.A very roughhewn error with titration labs is that over-titration often occurs. This is the point in which too more than titrant is added to the analyte during a trial. Therefore, the reaction passed the endpoint as too much(prenominal) of the basic sodium hydroxide was added to the acidic vinegar solution containing acetic acid. Unfortunately, this took place for most trials. For instance, phenolphthalein reaches its endpoint when it changes from being clear and transparent to becoming a elucidation shade of pink.Though this may be, for all of our trials when using this indicator the color became a hot pink shade proving that over-titration had taken place. An improvement for this luck of the lab is si mple. An improvement to control this error would be to use a burette with a smaller opening. This is because the endpoint can be blast quite easily and this would ensure the error would not take place. It would have been best to manage the amount of base entering the beaker as much as possible with greater accuracy.An additional error that took place was how the shaft was not entirely effective. This is due to the fact that when the stopcock was turned to close the burette opening, little droplets of sodium hydroxide would still pour into the beaker. This path that if the solution had reached the endpoint and additional droplets were leaked from the beaker an inaccurate reading of the sodium hydroxide in the burette would be recorded. This error could have been improved by using a BT50 digital burette (Bibby, 2010). This burette would ensure that a considerably small amount of sodium hydroxide would be action from the device at most. A button will be press to stop the base from entering the beaker containing the acid electronically. The accuracy of this instrument is indoors 0.2%, and precision is better than 0.1% allowing for the most accurate of results to be obtained.Temperature should have been controlled throughout the process as it does play a role in touching the data obtained in a titration lab. The volumetric glassware used for the aim of this lab is calibrated at 20oC and a higher temperature of a solution would result in it holding a greater volume than desired (Atkins). Since the room temperature is approximately 24oC it can be assumed that the temperature of the solutions used in the experiment were greater than 20oC. Therefore, these solutions can expand and the concentration in molarity would decrease.Therefore it would have been beneficial to keep the temperature of the acid and base unending at 20oC. This could have been achieved by using an inebriant thermometer. If the temperature for the acid and base were not 20oC, than it would either need to be placed in the icebox if the solution was too hot or would need to be put in a beaker and on a hot plate to reach the desired temperature.The temperature for each indicator that was used was not consistent throughout the lab. This is because the temperature of the room changed throughout experimentation. The door in the classroom was open to conk out rid of the stench from a lab done in the preceding class. Therefore, the temperature of the classroom was gradually getting colder and colder. A consistent temperature for each indicator would ensure that the pH range for a color change would not increase or decrease. This is because with a decrease in temperature there is less ionization that takes place allowing the pKa value to increase and therefore, the color change will occur at a higher pH.To ensure all the temperatures of the indicators were unploughed consistent throughout the lab it would have been beneficial to use an alcohol thermometer and place it in the indicator solution before conducting the trial (ChemBuddy, 2009). If the temperature changed for one trial, the indicator would either need to be placed in the refrigerator if the solution was too hot or would need to be put in a beaker and on a hot plate to reach the desired temperature. The table below represents how temperature can affect the pH range for a color change for specific indicators. To ensure this does not occur, the lab should be taken out in a room with no windows so the temperature does not change. The table below represents how the endpoint changes with a change in the temperature of an indicator.IndicatorColor Change Range18oC100CMethyl Orange3.1-4.42.5-3.7Methyl Red4.4-6.24.0-6.0Phenolphthalein8.2-9.88.1-9.0Quoted from Chemia analityczna, J.Minczewski Z.Marczenko, PWN, Warszawa 1973.Another error was that there were bubbles in the burette tube. When the sodium hydroxide solution was poured in the burette it was done quite quickly creating many bubbles in the beaker. Unfortunately, my root could not afford rinsing the solution out and pouring in more sodium hydroxide solution because we wanted to ensure we had adequacy of the solution for the whole lab. Therefore the bubbles caused an inaccurate volume reading. The bubbles occupy a particular amount of volume and this means that the volume in the burette would in fact be less than the amount reported during trials. Since the bubbles all formed near the stopcock it would have been best to pour the sodium hydroxide solution into a waste beaker in hopes that the bubbles would be eliminated before beginning the trial.This is because the pressure of the titrant in a burette will press the bubbles out. Unfortunately, in some cases the bubbles remain near the stopcock. If this is the case, it would be best to use a suck method approach. This involves one to partially open the stopcock allowing the contents of the burette to discharge in the beaker. Then, they will use the pipet bulb to suc k air from the bubbles through the nozzle of the burette. This will ask out the air bubbles present in the solution out of the beaker into the suction device. One must ensure that the sodium hydroxide that was poured in the beaker during this process is accounted for by slowing pouring in the amount necessary in the burette for the trial to begin.One experimental error that was unavoidable was the alter of the burette before using it. It was necessary to clean the burette using water, as it may have had some residue or contaminant from a previous experiment. Additionally this residue could have affected the pH of the sodium hydroxide solution that was to be put in the beaker for the decision of this titration lab. However, there were some droplets of water left on the sides of the beaker after it was cleansed which would have decreased the concentration of the sodium hydroxide solution that was subsequently poured in this material and lowered the pH level of the sodium hydroxide solution as water is neutral (pH of 7.0). With a lower concentration of sodium hydroxide in the base, the pH would have decreased therefore allowing more of this base to be added to the vinegar in order for the endpoint to be reached in a reaction. This is due to the fact that sodium hydroxide is a highly basic solution and water is neutral. When they are potpourried the pH of the solution will be lower than the initial pH of the sodium hydroxide solution.An improvement for the lab could have been to detect the pH of the acid base titration once it has reached the endpoint using a pH meter. This was one of the limitations in this acid-base titration lab as the indicators that were used did not show a change in color at an exact value of pH but only changed in a specific range of the pH. For example, the indicator Bromocresol green changes the color of the solution of a pH range between 3.8 to 5.4. This range is considerably large resulting in one to obtain results that are not nec essarily the most accurate. An improvement for this component of the lab would have been to use a pH meter. A pH meter is a device that that measures the pH of a solution by determining the voltage of the solution by immersing two electrodes in it. Then, the reading device will present the pH value. This would have led for the most reliable pH readings to be obtained and the correct amount of sodium hydroxide to be added to the acidic solution.The lab could have been furthered in several ways. It would have been interesting to test these different indicators and the amount of sodium hydroxide required for the end points to be shown when using a strong acid and base. At the equivalence point the same amounts of hydrogen and hydroxide ions will form water, therefore having a pH of 7. For instance, if hydrochloric acid and sodium hydroxide were used the following reaction would take placeHCl(aq) + NaOH(aq) > H2O(l) + NaCl(aq)H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) > H2O(l) + Na+(aq) + Cl-(aq)H+(aq) + OH-(aq) > H2O(l)The number one equation displays the reaction between the strong acid and strong base. The consequence reaction displays the HCl and NaOH dissociated in their respective ions. The last equation is known as the net ionic equation which eliminates the spectator ions from the previous equation. This proves that water will be produced. The neutralisation reaction will take place because coarseness will also be formed. This is because the anion from the dissociation of the strong acid and the cation from the dissociation of the strong base will come together to form the coarseness. The salt is not seen the net ionic equation as it dissociates.For this acid base titration lab it was legitimate to compare the outcomes with other classmates to determine if there were any anomalies between the data that was obtained. This is because it would have provided one with the knowledge of the types of errors that occurred and how much it affected their data. For instance, Sarah and I compared our results with Rachel Hung and Yashna Lakhanis thronging.Yashna and Rachels groups provided information upon different indicators and some of the ones my group used as well. When comparing with the data of these groups it was determined that all of the results were loosely exactly the same or off by 0.1ml for the difference between the final and initial burette readings. For instance, for phenolphthalein, the value my group obtained for this was 0.9ml however, Yashnas group got 1.0ml. This could have been due to a human error known as a parallax. A difference of 0.1ml could have taken place as one of our groups were unable to determine the position of the meniscus on the burette and therefore, the wrong readings of sodium hydroxide solution could have be collected.An acid base titration has several uses. One of the main real life uses of this experiment is to mix compounded drugs. A pharmacist will need to mix drugs appropriately in order for them to be in the appropriate pH range for the human body. Antacids are commonly used to help issues concerning heartburn, acid reflux and more. These feelings most likely take place due to exorbitance hydrochloric acid in the turn out which causes an uncomfortable feeling. This subsequently allows a backflow of this acid to go up the esophagus which can make individual feel like their throat is burning. These tablets counteract the acidity as they go to the stomach area and react with the hydrochloric acid. These tablets are basic and change the crystalline in the stomach to being not as highly acidic. commonalty antacid tablets contain Mg(OH)2 and Al(OH)2. A reaction equation by using an antacid tablet is shown as followedHCl+NaOH NaCl+H2OThe acid base titration in this case is used to determine the amount of the stomach acid present in ones body. Therefore, it can be discovered how much antacid will be needed for someone dealing with the issues mentioned above in order to m ake the hydrochloric acid present in their stomach less concentrated (Cavite, 2010). This will ensure the pH of the stomach will be less acidic. In other words, the lab will determine how much hydrochloric acid will be needed to be titrated by the base.Bibliography1. Acid-Base Indicators. Acid-Base Indicators. N.p., n.d. Web. 13 Nov. 2012. <http//antoine.frostburg.edu/chem/senese/101/acidbase/indicators.shtml>.2. Meheen, T. 3- Lab. Titration Analysis of Vinegar. N.p., n.d. Web. 13 Nov. 2012. <http//resources.educ.queensu.ca/science/main/ innovation/gen/g09/J.%20Duval/Webpage/Lab%203%20page.html>.3. Rousseau, Sasha. If You Dilute Vinegar, How Will It Affect the PH Value? EHow. motive Media, 07 July 2011. Web. 13 Nov. 2012. <http//www.ehow.com/info_8702588_dilute-vinegar-affect-ph-value.html>.4. Toxic Substances Portal Sodium Hydroxide. Sodium Hydroxide (NaOH). N.p., 22 Apr. 2002. Web. 3 Mar. 2011. <http//www.atsdr.cdc.gov/toxfaqs/tf.asp?id=248&tid=45>.5. Downloa ds. Stuart Digital Burette. N.p., n.d. Web. 13 Nov. 2012. <http//www.stuart-equipment.com/product.asp?dsl= one hundred twenty-five>.6. CALIBRATION OF VOLUMETRIC GLASSWARE. CALIBRATION OF VOLUMETRIC GLASSWARE. N.p., n.d. Web. 13 Nov. 2012. <http//web.pdx.edu/atkinsdb/teach/321/CALVOL.htm>.7. Acid Base Titration End bode Indicators. Acid Base Titration End Point Indicators. N.p., n.d. Web. 13 Nov. 2012. <http//www.titrations.info/acid-base-titration-indicators>.8. Pallas_reg. Acid-Base Titrations Analysis of Antacid Tablets. Scribd. N.p., n.d. Web. 13 Nov. 2012. <http//www.scribd.com/doc/38740823/Acid-Base-Titrations-Analysis-of-Antacid-Tablets>.