This is my lab report on chemistry. 5 g sample of KHP. Adjust the pH of 100 mL (4 deliveries from a 25-mL pipet) to about 10 by addition of 3 mL of the ammonia buffer; check with a pH meter. the data point can be rejected (check with your lab instructor to do a Q-test). Calculate the ratio of mass of KHP (g) to Volume of NaOH (mL) for each trial. hasten solution. Using the total volume of NaOH added to each, and the molarity of your NaOH standard solution,. 0 mL of NaOH left in their original containers. 1M) and volume of NaOH(aq) is known. Calculate the concentration of NaOH, a) From the titrations against HCl and b) From the titrations in which glucose was added to the borax II. Honeywell Burdick Jackson. Standardization. 1 M acid solutions (note that citric acid is triprotic). Get quality assignment writing, essay writing and homework writing with us for as cheap as $10. Standardization of Solution and Titration Lab Report, Preparing a Dilute HCl Solution from a Concentrated One Titrating NAOH Solution with HCl Solution (of Known Concentration) Chemistry lab report(by abdazino abdalla) International College Objective preparing a dilute HCl solution from a concentrated one titrating NAOH solution with HCl solution (of known concentration) Procedure Section A. Reaction 1) Max. The 50% NaOH solution can be added using a graduated cylinder. 47 ml of the naoh for the color to change (neutralization) molarity = moles/liter. Experimental reports, the time for doing so should be long and the task could probably not. Immerse the glass pH electrode in the solution. You'll report the average (or mean) of the three values. Example calculations Standardization of a sodium hydroxide solution What is the molarity of a solution of sodium hydroxide, 25. Calculations for Report. strong baseA strong base is a basic chemical compound that is able to deprotonate very weak acids in an acid-base reaction. Another problem in the preparation of standard NaOH solutions is the need to remove dissolved CO 2 from the water used. Chemistry 1211. volume of base added). Turn on the magnetic stirrer. Swirl to dissolve the KHP completely. KHP is the primary standard, therefore it's concentration is consent and stable. acid and base titrations lab report chm 114 jx abstract this goal was to give us experience finding the standardization of through the use of primary standard. 5"""""©2016"James"Madison"University"and"JMU"Board"of"Visitors" Here is an example calculation that you may follow when calculating your results:. At a certain volume of added NaOH, all the KHP acid will be neutralized due to the large equilibrium dissociation constant (Kb) of the base. The solution turns color after 25. Note the end point. If you eat or drink too much, you may develop heartburn or indigestion. 0 M sodium hydroxide solutions having an initial temperature of 20. Standardisation Procedure. 05 mL of a NaOH solution to completely neutralize it using phenolphthalein as an indicator. Pipette 5 ml of 1. Fill the buret with NaOH standard solution to slightly above the zero mark and set up the buret as demonstrated by the lab instructor. strong baseA strong base is a basic chemical compound that is able to deprotonate very weak acids in an acid-base reaction. Determine the standardized concentration of a NaOH solution based on the following experimental data: mass of KHP = 0. 0°C react in a calorimeter. 1M for the titration). Experiment 5: Standard Solutions; Titration Chemistry 1515L October 2007 In this experiment, you will prepare an approximately 0. An introduction to titration: standardization of HCl and NaOH Introduction: The objective of this experiment is. Draw a molecular representation of the species in the Erlenmeyer flask at this point. 09081 M Conclusion. 64 mL of NaOH titrant to reach the end point, what volume of titrant would be required to reach the end point in a second titration using 0. Include all your repeat readings in the table, and indicate which are the concordant results to be used in the calculation of the mean titre. JOMO KENYATTA UNIVERSITY OF AGRICULTURE AND TECHNOLOGY DEPT: CIVIL ENGINEERING UNIT: CHEMISTRY 1 (SCH 2109) PRACTICAL REPORT EXPT 2: Standardization and Determination of Concentration of Hydrochloric Acid in a Given Solution by ARAKA BRAMWEL MBOGO EN251-0221/2010 TITLE: STANDARDIZATION and DETERMINATION OF THE CONCENTRATION OF. To a very slight extent, it does break into H+ and OH- ions. Standardization of NaOH Solution? Hypothesis: A prediction of what you think the results of the project will be. Concentrated (65%) nitric acid also came in a similar plastic bottle, albeit black plastic, presumably to prevent photo-degradation. Take 20 ml of sodium hydroxide solution into a clean conical flask with addition of 2-3 drops of methyl orange indicator. Titrate with 0. The standard solution must react in a reasonable amount of time in a quantitative reaction setting. So, I could really use some help in here. 2 M NaOH solution standardize it (i. Part 1: Reaction: HCl & NaOH ? NaCl. Solution Pr eparation: Primary and Secondary Standards 1. Introduction. mass of oxalic acid 0. Using the data you obtain and equation 4,. The exact concentration of any hydrochloric acid solution is not known, unless it is prepared from standard ampoules. Report Average Values. 2- Dissolve in small quantity of distilled water and transfer quantitatively to 250ml measuring flask. 954g of disodium hydrogen phosphste. It can therefore be used to determine the molarity of a. NaOH is the most common strong base. Acid base titration lab report conclusion. This is an acid base titration where the titrant is standard HCl, and your sample is a base containing an unknown amount of Na 2 CO 3. If there is time, do your calculations before leaving the lab. However, this lab will NOT require a graph. Acid base titration lab report introduction. Titration Lab Report Essay Titration Lab Introduction The purpose of this lab is reach and be able to calculate the equivalence point when we use titration to neutralize a base with acid. Convert this to a percent citric acid by weight. The standard solution is one whose concentration is already accurately known. Standardization. Acid Base Titration Lab Report. 2 mL of concentrated HCl into a 250 mL beaker containing a little water. Acid-Base Titrations. ) You will react the NaOH solution with a known amount of the solid acid potassium hydrogen phthalate (KHP). 925 mmol x 1/1 = 0. VOLUMETRIC ANALYSIS Volumetric Analysis is a method of analysis based on titration. Background: Far from titanums and titillation, titration establishes a solution's standard strength or degree of concentration. Place the beaker containing the. asked • 03/09/16 If it takes 25. 1st Get the balanced equation NaOH + HCl -> NaCl + H2O Find the number of moles in HCl; n = cv n =. This is a chemistry lab report on an Acid-Base Titration experiment of titration when the number of moles of NaOH (Na) added is equal to the number of moles of KHP (Nb) in the solution. PRACTICAL REPORT EXPT 2: Standardization and Determination of Concentration of Hydrochloric Acid in a Given Solution by ARAKA BRAMWEL MBOGO EN251-0221/2010 TITLE: STANDARDIZATION and DETERMINATION OF THE CONCENTRATION OF HYDROCHLORIC ACID PRESENT IN A GIVEN SOLUTION Aims: To be able to standardize Sodium Hydroxide (NaOH) solution using. Physical Chemistry Laboratory - Conductometric Titration. Transfer 10mL of your diluted HCl to an Erlenmeyer flask, and add 2 drops of indicator solution (BTB). 10 M NaOH using 50% concentrated NaOH and "equilibrium water" in a 1-L volumetric flask. The most common form of VA is the titration, a process whereby a standard solution of known. Before preparing. that should be addressed in a formal lab report. To make things easier, in thediscussion to follow, we will do each of these lab reports separately. Discard the rinse solution. , the original 25 mL) in moles/liter from the known stoichiometry of the acid-base neutralization reaction, the known concentration of the NaOH titrant, and the known dilutions of the HCl solution. Place the beaker on a magnetic stirrer and add 0. Spectrophotometric Determination of Equilibrium Constant page 7 6. Calculate the number of moles of hydrochloric acid left in 100 cm3 of solution Moles in 100cm3 = 0. Four clean 125-mL or 250-mL Erlenmeyer flasks for the HCl ( In the absence of Erlenmeyer Flask Conical flask can use) 3. In this titration, the concentration of acetic acid, HC 2H3O2, in commercial vinegar will be determined by titration against a standard solution of NaOH. 1st Get the balanced equation NaOH + HCl -> NaCl + H2O Find the number of moles in HCl; n = cv n = 0. The titration is the process of determining the specific amount of a standard solution required to react with a certain amount of unknown. 0 mL of a 2. The calculated molarity was too highThe moles of NaOH used would be high. are re- quired. 30 g portions of dry potassium hydrogen phthalate into. 5 N oxalic acid to a conical flask. Fill the buret with 0. Use the same procedure as in the latter experiment. Hydrochloric acid (HCl) is one of the substances found in gastric juices secreted by the lining of the stomach. Abrash Q: What is the purpose of this experiment? NaOH, since you'll be making a finer determination of the amount of NaOH by titration later in the lab. 01 mol kg-1, was titrated by the just standardized NaOH solution. Calculate the molarity of the standard Na2CO3 solution. 05 mol According to the equation, 1 mole of H2SO4 reacts with 2 mole of NaOH to form 2 mole of H2O. In this experiment, a hydrochloric acid solution will be titrated with sodium hydroxide. Add 2 mL of 6 M HCl, and immediately titrate with thiosulfate until the solution becomes pale yellow. For this lab, you will need to use distilled water. An indicator must be used to pin point the equivalence point, the point in which 1 mole of a substance is equal to 1 mole of another. Question options: A week before the lab Day before the lab at 10 pm The morning of lab day at 8 am One hour before the lab Question 2 1 / 1 point Which materials/chemicals belong in the desiccator? Question options: Drying agents such as anhydrous magnesium sulfate silicagel 1 M NaOH aqueous standard solution aqueous extract of your reaction. Results Table. This lab manual. Place the beaker containing the. 0 mL of a 2. The equation for the reaction is. Essay on Acid-Base Titration - Acid-Base Titration I. Turn in a clean 250. Antacid tablets (Tums vs. Add 500 ml of ethyl acetate into the reactor and simultaneously start the stop watch. Zn MW = 65. 1molar NaOH a) from solid b)from liquid 2. Add about 10 drops of bromothymol blue indicator to each solution and titrate the excess NaOH with the standard HCl solution. edu is a platform for academics to share research papers. 2M HCl into the unknown solution and the recording of the solution's pH as each drop was added. Report your results in the usual scientific manner. Sodium hydroxide (), as a solid and in solution, looses strength on exposure and its concentration needs to be determined or standardised by titration, using a hydrochloric acid (HCl) solution of a known concentration (0. Acid-Base Titrations with Balances. 0 M sodium hydroxide solutions having an initial temperature of 20. Preparation of EDTA: 1. Testing for cations using different solutions of NaOH, Ammonia and Sodium Carbonate? Can the cations in a solution be identified by using another solution. Procedure: The flask is filled with 10 mL of unknown concentration of HCl. EXPERIMENT 11 STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION WITH A PRIMARY STANDARD 3 The stoichiometry becomes more complex when the acid and base release unequal number of H3O + and OH− ions. Titrate with sodium hydroxide from the burette. Household ammonia. The titration is the process of determining the specific amount of a standard solution required to react with a certain amount of unknown. Physical Chemistry Laboratory - Conductometric Titration. EDTA Standardization 1. The simplest example of this occurs in the reaction discussed earlier, in which hydrochloric acid or HCl( aq ) reacts with the base sodium hydroxide, designated as NaOH( aq ), in an aqueous solution. Titration of acids and bases lab report - Related to solve complex, hw help; determining molarity lab. Standardization. Using the three values of enthalpy changes measured, it was shown that;. LAB REPORT Kim Hoff Damien Guilband Noah Jabusch 03/09/15 ­ 3/10/2015 Acid­Base Titration Lab INTRODUCTION : The purpose of this acid­base titration lab was to determine the molar concentration of two acid solutions by performing titrations with a strong base, NaOH, of known concentration. Calculate the molarity of the iodine solution. You will first standardize your NaOH solution, and then use it to analyze aspirin tablets for their aspirin content and purity. Potentiometric titration of a HCl–H3PO4 mixture Potentiometry will be used to detect the endpoints of the titration of a mixture containing unknown amounts of hydrochloric (strong) and phosphoric (weak polyprotic) acids. The first lab report is on the Standardization of NaOH (Page 169 of the lab manual). 1559 Words Nov 7th, 2015 7 Pages. Testing for cations using different solutions of NaOH, Ammonia and Sodium Carbonate? Can the cations in a solution be identified by using another solution. Variables Independent variables Mass of KHP (mKHP) Volume of KHP solution Dependent variables Volume of NaOH added [since the colour change will not happen at exactly the same volume of NaOH added (VNaOH)] Controlled…. The calculated molarity was too highThe moles of NaOH used would be high. 00 M aqueous HCl solution with 50. Pipette out 20 ml of Oxalic acid into a conical flask and add 2-3 drops of phenolphthalein indicator and titrate the colourless solution against NaOH till pale. Reaction 3. Standardization of Solution and Titration Lab Report, Preparing a Dilute HCl Solution from a Concentrated One Titrating NAOH Solution with HCl Solution (of Known Concentration) Chemistry lab report (by abdazino abdalla) International College Objective preparing a dilute HCl solution from a concentrated one. Each mole of HCl reacts with the water to NaOH Standardization • It is usually impossible to obtain NaOH of sufficient purity to use it as a primary standard. Acid base titration lab report conclusion. 3) How many grams of Na 2 HPO 4· 7H 2 O and how many mls of 1N HCl will you need to add to make the third buffer? In the Questions section of your lab report, answer the following questions. Sodium hydroxide is hygroscopic and absorbs water from the air when you place it on the balance for massing. Concentrated (65%) nitric acid also came in a similar plastic bottle, albeit black plastic, presumably to prevent photo-degradation. NaOH titration of HCl 0 2 4 6 8 10 12 14 0 102030 mL NaOH added p H 40 Titration curve of weak diprotic acid by NaOH(aq). The solution becomes clear again as the hydronium ions from the hydrochloric acid neutralize the added hydroxide ions. However, the endpoint for the titration of the acid solution in Part B. The Standardization of NaOH and KHP Home / Natural Sciences / Chemisty / The Standardization of NaOH and KHP. Stir the sodium hydroxide, a little at a time, into a large volume of water and then dilute the solution to make one liter. You need these materials: 19 M NaOH, potassium hydrogen phthalate (KHP), phenolphthalein solution, citric acid (H 3 C 6 H 5 O 7), distilled water, petroleum jelly, unknown HCl solution. Standardization of NaOH Experiment 18 18-2 Ideally, the preparation of a standard NaOH solution would involve accurately weighing a certain amount and then diluting to some final volume. Measure 16. Titration Experiment Report Sheet. 0 M HCl (instead of water) into the Styrofoam calorimeter. Approximately 125-mL sample of HCl to titrate with your NaOH solution. Lab Report (Conductometric Titration) - Free download as Word Doc (. 1) What, chemically speaking, is the difference between buffer 1 and buffer 3? 2) Calculate the ionic strength of each of the solutions you made. Physical Chemistry Laboratory - Conductometric Titration. 1000 N or M Volume 0. 05 mL of a NaOH solution to completely neutralize it using phenolphthalein as an indicator. Report your determination of. 05 cubic centimeters. 5"""""©2016"James"Madison"University"and"JMU"Board"of"Visitors" Here is an example calculation that you may follow when calculating your results:. known NaOH standard, using a pH meter to track changes in the pH of the acid solution as you add measured volumes of base. 0 mL of which requires 21. Acid and base titration lab report - Secure Term Paper Writing Service - Get Professional Help With High-Quality Assignments For Me Professional Research. Calculate the volume of HCl. H2SO4 in 500 mL reagent grade water, transfer to a 1 L volumetric flask and make up to the mark with water. EXPERIMENT 11 STANDARDIZATION OF A SODIUM HYDROXIDE SOLUTION WITH A PRIMARY STANDARD 3 The stoichiometry becomes more complex when the acid and base release unequal number of H3O + and OH− ions. NaOH Standardization. 925 mmol 50ml Concentration of NaOH= Discussion: NaOH is the secondary standard, therefore it’s concentration varies with time and is unstable. Spectrophotometric Determination of Equilibrium Constant page 7 6. The Standardization of NaOH and KHP. Label the bottle with tape. 00333 x10 =0. Therefore HCL would be highC. There was a little HCl in the Erlenmeyer flask before you began your titration. Muriatic acid is hydrogen chloride (HCl) dissolved in water. Lab Report On Titration 971 Words | 4 Pages. HCl with NaOH: Before NaOH is added, the conductance is high due to the presence of highly mobile hydrogen ions. Temperature measurements were taken at intervals of 30 seconds and were used to generate graph time against temperature in each case. Dilute 12 M of HCl to 100 mL 1. of used in the titration, since the molarity (0. Acids and bases lab report, titration of acids and bases lab report, titrations of acids and bases lab report, acids bases and buffers lab report, lab report for acids. 20 M NaOH, the instructor will refill it for you. So the equivalent weight of NaOH is 40. Standardization of a Sodium Hydroxide Solution. A primary-standard zinc metal ion solution was prepared by dissolving 0. Variables Independent variables Mass of KHP (mKHP) Volume of KHP solution Dependent variables Volume of NaOH added [since the colour change will not happen at exactly the same volume of NaOH added (VNaOH)] Controlled…. SAMPLE INFORMAL LAB REPORT FROM CHEMISTRY 31. How many milliliters of 0. Standardization of Sodium Hydroxide Solution Essay Sample. Turn on the magnetic stirrer. Transfer it to a 250 cm3 flask and make up to the mark with water. Draw dotted perpendicular lines to the x and y axes. unknown bottled water and report the water hardness as ppm CaCO3. Report Average Values. Abrash Q: What is the purpose of this experiment? The purpose of this experiment is to explore two techniques by which we answer the. At a certain volume of added NaOH, all the KHP acid will be neutralized due to the large equilibrium dissociation constant (Kb) of the base. we calculated 10. Report your conclusions P AR T 2. Standardization. That is plagiarism and you will receive no credit for this part of the report. 919 g of KHP and is titrated with a solution of NaOH that is approximately 0. Alternatively : Dissolve 8. 2 Procedure 3. 6 Hydrochloric acid (HCl), 32% AR or Sulphuric Acid (H2SO4), 98%, AR. AP LAB 05d: Enthalpy of Neutralization (∆H° neutralization) Aim To calculate a value for the standard enthalpy of neutralization Apparatus Insulated cups (the calorimeter), thermometer, graduated cylinder Chemicals 2. Run another trial using 50. basic knowledge of lab techniques. Chem 102 Lab Notes Sp97 Chemistry 102 Laboratory Notes. A faint green-yellow color is the ideal end-point. , the original 25 mL) in moles/liter from the and the known dilutions of the HCl solution. 10 M and standardize the sodium hydroxide against the hydrochloric acid. Today's experiment before titrating with 1 M HCl or 1 M NaOH is. Standardization of NaOH Solution? Hypothesis: A prediction of what you think the results of the project will be. In this experiment we’re going to do a titration of a weak diprotic acid (an unknown) by a strong base (NaOH). Please use this example to do your lab report. Begin to titrate your first KHP solution by adding NaOH rapidly until a pink color is noticed. Show your calculations for the molarity of the NaOH from each of the three standardizations. docx), PDF File (. Primary standard - is a highly purified compound that serves as a reference material in all volumetric and mass titrimetric methods. LABORATORY REPORT SHEET(1). 1 N NaOH y 0. This is where you will write a procedure for the creation of X. Another problem in the preparation of standard NaOH solutions is the need to remove dissolved CO 2 from the water used. The moles of NaOH consumed is related, through the stoichiometric factor (of 1/2, based on the balanced equation) to the moles of acid that were contained in the sample. 0 mL of HCl and 90. A pH indicator is used to monitor the progress of the acid–base reaction. Lab Drawer Equipment. Materials: Distilled water, beverages (juice, soda, sport drinks), Sugar reference solutions (0, 5, 15, ad 20%) 25ml each, Balance, centigram (0. Calculate the ratio of mass of KHP (g) to Volume of NaOH (mL) for each trial. C) CONDUCTOMETRIC TITRATION: 10ml of supplied HCl solution (strength in the order of N\10) is pipette out into a 250ml beaker and about 100ml of distilled water is added. The calculated molarity was too highThe moles of NaOH used would be high. Because NaOH and HCl react in 1:1 molar ration, the. Neutralization Neutralization is the process whereby an acid and base react with one another to form a salt and water. Add 2-3 drops of phenolphthalein indicator and titrate with sodium hydroxide present in the burette. Continue to add NaOH to the HCl solution until 45-50 mL of NaOH has been added. pdf form from the lab website and open it using Adobe 7. Describe a simple experiment which would allow you to determine which bottle contains which solution. , the original 25 mL) in moles/liter from the and the known dilutions of the HCl solution. Using your NaOH molarity from last week, determine the molarity of your HCl solution from the volumes of NaOH needed to titrate your flasks of HCl, remembering that you designed it to be ~0. the pH range. Gloves may be worn if available in the lab. Percentage Yield Lab Answers. Prepare one liter of 0. The solution turns color after 25. To compute for the molarity of the standard NaOH: The reported values for the molarity of standard NaOH are 0. value), determine the molarity of your volumetric standard HCl. Make sure you record the purity of the standard. A primary standard is a substance used to determine the concentration of a solution. Lab 2 Titrate your impure KHP sample. Titrate with NaOH solution till the first color change. SAMPLE OF A FORMAL LAB REPORT phenolphthalein, standard 0. Experiment #2 report form instructions. Place sodium hydroxide solution in a 25 mI buret. 12 H 2 O and 3. 05 mL of a NaOH solution to completely neutralize it using phenolphthalein as an indicator. To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. 9mL HCl, and ended with 10. Also you cant make a standard solution of hydrochloric acid as when you open the bottle hydrogen chloride escapes into the air so I will have to find the concentration of HCL by titrating it against a standard alkali. Present your data for the standardization of HCl. and zero or note the burette. Your instructor will indicate which procedure you are to follow (Part I or Part II). Deutsch Chem. PART A: Standardization of a Sodium Hydroxide solution NaOH Sample Code = O Trial 1 Mass of KHP transferred = 0. The reaction of an acid such as HCl with a base such as NaOH in water involves the exothermic reaction HCl(aq) + NaOH(aq) ---> NaCl(aq) + H 2 O In one experiment, a student placed 50. Discard the rinse solution. 0 mL of a standard solution of hydrochloric acid of concentration 0. Standardization of sodium hydroxide. Turn in a clean 250. Here's how to perform the calculation to find your unknown:. Write your hypothesis before you begin the experiment and, if the experiment has more than one part, you will need a hypothesis for each section. 0 M NaOH solution into a graduated cylinder. The total marks for this lab will be 40 marks!!! The questions are worth 12 marks and the 3 part Discussion section is worth 9 marks so be sure to write thorough, elaborate explanations in these two parts of the lab report. 1st Get the balanced equation NaOH + HCl -> NaCl + H2O Find the number of moles in HCl; n = cv n =. 09081 M Conclusion. Read this free Science Lab Report and other term papers, research papers and book reports. 23) for at least 1 hour at 110 o C (DO NOT overdry your sample). 321 g initial volume of NaOH 1. Include a printed graph of the HCl-NaOH data with your lab report and label it. Aim: to determine the quantity and concentration of NaOH to completely neutralize one molar hydrochloric acid till the n point. Aim To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. 2 M NaOH will be needed to titrate the 0. Background: Far from titanums and titillation, titration establishes a solution's standard strength or degree of concentration. 2 was consistently reproduced to to a dark pink color. The labels have fallen off of three bottles thought to contain hydrochloric acid, or sodium chloride solution, or sodium hydroxide solution. Get an answer for 'What would be the independent, dependent & constant variables in an experiment based on determining the molar conc. Repeat Step 3. 1559 Words Nov 7th, 2015 7 Pages. The initial color should be blue and the end-point should be Report the average normality for the standardized solutions. 1M) and volume of NaOH(aq) is known. The concentration of dissolved oxygen can be readily, and accurately, measured by the method originally developed by Winkler in 1888 (Ber. Also you cant make a standard solution of hydrochloric acid as when you open the bottle hydrogen chloride escapes into the air so I will have to find the concentration of HCL by titrating it against a standard alkali. Using the formula C1V1 = C2V2, where C1 is the molarity of the NaOH, the difference in volume is the V1 and the amount of aqueous. Acid-base titrations are lab procedures used to determine the concentration of a solution. with NaOH and cover the top of the buret with plastic wrap until you are ready to use it. Click n=CV button below NaOH in the output frame, enter volume of the solution used, read solution concentration. Present your data for the indicator based titration of the mixture. In the first titration, 0. For this lab, the unknown potassium hydrogen phthalate sample was titrated with a standardized sodium hydroxide solution. Satoshi kishigami, good lab report is the nd. The exact concentration of any hydrochloric acid solution is not known, unless it is prepared from standard ampoules. NaOH solution was slowly added to the HCl solution until a faint pink color persisted for 30 seconds. Valencia Community College. In my reaction 58 cm3 of H2SO4 , c=(1,80 mol/dm3) reacted with 1dm3 NaOH c=0,162mol/dm3. From The Interactive Lab Primer (U of Nottingham), sim of titrations, also has. The molarity of the HCl was then calculated based on the volume and molarity of the NaOH solution and volume of HCl solution used in the titration. 0500 M HCl solution is added. The formula for KHP is KHC 8 H 4 O 4, and it has one ionizable proton. Using the given heat capacity, given densities and measured volumes of the solutions and the measured temperature change, we can analyze the heat exchange, q, and correct for the heat loss to the calorimeter using the Calorimetric constant, C cal, determined in Part 1. Variables Independent variables Mass of KHP (mKHP) Volume of KHP solution Dependent variables Volume of NaOH added [since the colour change will not happen at exactly the same volume of NaOH added (VNaOH)] Controlled…. To save time in this experiment, we will assume that the hydrochloric acid solution concentration is 0. 6, the endpoint was consistently reproduced to a faint pink color.