Introduction: Sodium hydroxides‚ NaOH Is a commonly used titrant for determining the concentration of acidic solutions. We also have guidelines and formulas for achieving and measuring the concentration for example concentration = amount per litre i.e. grams/litre (g/L) or mol/L (M = Molarity) Primary standard and its importance can be justified by its accuracy to find the concentration of a solution‚ in this lab report; we will measure the concentration of NaOH and test our titration method as
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finding the concentration of an acetic acid. 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. When that is found‚ we can determine the concentration. HC2H3O2 (aq) + NaOH (aq) H2O (l) + NaC2H3O2 (aq) The above equation is used to neutralize the acetic acid. The acid reacts with a base to produce water and a salt. Because there’s a 1:1 ratio‚ the moles of the acid must equal the moles of the base in order to reach
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Trial | 1 | 2 | 3 | Final Reading HCl (ml) | 35 | 35 | 35 | Initial Reading HCl (ml) | 0 | 0 | 0 | Volume HCl used (ml) | 35 | 35 | 35 | | | | | Final Reading NaOH (ml) | 30.6 | 30.2 | 30.0 | Initial Reading NaOH (ml) | 0 | 0 | 0 | Volume NaOH used (ml) | 30.6 | 30.2 | 30.0 | | | | | Acid to Base Ratio | 0.87 | 0.86 | 0.86 | Average acid/base ratio | 0.86 | | | | | Base to Acid Ratio | 1.14 | 1.16 | 1.17 | Average base/acid Ratio | 1.16 | Name: Jared Philip
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FACULTY OF RESOURCE SCIENCE AND TECHNOLOGY DEPARTMENT OF CHEMISTRY STK 1094 – Analytical Chemistry 1 EXPERIMENT NO : 1 TITLE OF EXPERIMENT : ACID – BASE TITRATIONS DATE OF EXPERIMENT : 27 SEPTEMBER 2013 GROUP MEMBERS & MATRIX NUMBERS : 1. DELVINO DISONNEO ANAK DALIN (44903) 2. GOH CHIA HONG (44927) 3.LINDA CHONG (41889) 4.LIM WHYE KIT LEONARD(41874) 5. LAB FACILITATOR : REPORT DUE DATE : 4 OCTOBER 2013 INTRODUCTION The laboratory
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Acid-Base Titration Pre-Lab Discussion In the chemistry laboratory‚ it is sometimes necessary to experimentally determine the concentration of an acid solution or a base solution. A procedure for making this kind of determination is called an acid-base titration. In this procedure‚ a solution of known concentration‚ called the standard solution‚ is used to neutralize a precisely measured volume of the solution of unknown concentration to which one or two drops of an appropriate acid-base
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recorded for the unknown sample. Titration of KHP with NaOH In this part the molarity of diluted NaOH was determined. After mixing 800 mL of water with 4.2 mL of 19.1 M NaOH‚ the diluted solution of NaOH was poured in a buret until the initial volume on the buret was 30.00 mL. 0.3005g of KHP was dissolved in 40.0 mL of 50% ethanol‚ and a drop of indicator was added to the Erlenmeyer flask containing the KHP solution. When the titration of KHP solution with NaOH reached its endpoint‚ pale pink color was
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207-209 degrees Celsius. Melting point‚ while very helpful in identifying an unknown organic acid‚ is simply not enough. Next‚ a series of titration experiments had to be done. In the first series‚ a titration is completed of sodium hydroxide (NaOH) with KHP. Three reps were completed and the resulting data led to the finding of the molarity of the sodium hydroxide. The second part of the titration series involved titrating the same prepared sodium hydroxide solution with Hydrochloric Acid (HCL)
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known accurately. We will first prepare a standard solution of NaOH. One way to prepare a standard solution is to dissolve an accurately massed amount of the substance and dilute it to a measured volume. In this way; the concentration can be calculated exactly. However‚ it is usually impossible to obtain NaOH of sufficient purity to use it as a primary standard. An indirect method is more practical for obtaining a standard solution of NaOH. We will prepare a solution of an approximate molarity and standardize
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Standardization of a NaOH Solution with Potassium Hydrogen Phthlate (KHP) Name:________________________________________________________________ Period:_____ Prelab 1. A 0.8234-g sample of "KHP" required 38.76 mL of NaOH for titration to the phenolphthalein endpoint. What is the exact molarity of the NaOH solution? 2. A 25.00-mL aliquot of an unstandardized HCl solution is titrated with the previously standardized NaOH solution from #1 above. If 32.55 mL of NaOH titrant is required
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hydroxide solution‚ NaOH. Research question How does different molarity of potassium hydrogen phthalate solution which is prepared by dilution process influence the volume of sodium hydroxide‚ NaOH used during titration process until the colourless phenolphthalein indicator solution turns pink where the volume of potassium hydrogenphthalate used is kept constant at (22.5 ± 0.01) cm³ throughout the process? Independent variable : Concentration of potassium hydrogen phthalate‚ KHP. Dependent variable
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