adding NaOH. We had to do a standardization test because the NaOH has a high reactivity and that could cause a small change. The NaOH solution was supposed to have a molar concentration of .5 however when we standardized the solution we found the actual molarity of the solution to be .4761. This may be due to the fact that NaOH is almost impossible to have pure because it reacts with CO2 in the air. Strong bases are generally very reactive and it makes it hard to have a pure solution of NaOH
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Chemistry. Chapter 4‚ Acid-Base Reactions‚ Titration Lab for procedure‚ or see worksheet. Data Standardization of Base with Solid Acid | PART I | Solid Acid | Base (NaOH) | Ratio: volume base/ mass acid | Final mass or volume | .70g | 38 ml | 38 ml / .70g | Initial mass of volume | .70g | 0.0 ml | | Mass or volume | .70g | 38 ml | | Titration of HCL | PART II | Acid (HCL) | Base (NaOH) | Ratio: volume base/ volume acid | Final volume | 10 ml | 4.8 ml | 4.8ml / 10ml | Initial
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EXPERIMENT V POTENTIOMETRIC TITRATION These files are in Adobe Acrobat format‚ if you are using Netscape Navigator or Internet Explorer and have Adobe Acrobat Reader installed (If you do not; Acrobat Reader can be downloaded for free from Adobe) these files should open directly in your browser. INTRODUCTION Many Acid-Base titrations are difficult to accomplish using a visual indicator for one of several reasons. Perhaps the analyst is color-blind to a particular indicator color
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vinegar in question through titration. After standardization of our titrant‚ which in this case will be NaOH‚ we will use this along with the indicator Phenolphthalein‚ to titrate the vinegar to determine the concentration of Acetic Acid in the sample. Equipment and reagents- We will use a 50mL beaker‚ a graduated buret‚ spatula‚ droplet applicator‚ 125mL Erlenmeyer flask‚ hot plate‚ and a container of snow. The reagents we will use are KHP‚ NaOH‚ distilled water‚ Vinegar sample and Phenolphthalein
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Introduction The goal of this lab was to correctly prepare a 0.2M solution of NaOH‚ identify highly acidic household cleaning chemicals‚ and determine their concentration (molarity) through titrations using the previously prepared 0.2M NaOH solution. Experimental First‚ to create 0.5L of 0.2M solution of NaOH‚ standard 3M NaOH solution was obtained. Next‚ calculations were performed to determine the amount 3M NaOH necessary to create 0.5L of the 0.2M solution and‚ as a result‚ 33.333ml of the
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unknown solution used‚ the unknown concentration can be calculated. For example‚ standard base solution (NaOH) is added from a burette to an accurately known volume of the acid solution (HCl). HCl(aq) + NaOH(aq) ------------> H 2 O(l) + NaCl(aq) This reaction (neutralization) can be written as a NET IONIC equation as follows: H+(aq) + OH-(aq) ----------> H 2 O(l) (2) (1) When sufficient NaOH has been added to react with all of the acid‚ the titration is complete -- the equivalence point has been
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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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electronic scale Procedure: Step 1: Standardization of the NaOH solution using Standard 0.1M PHP 1. Take 10ml of the given NaOH solution and dilute with 90ml of water. Fill up the burette with this solution. Take 10ml of 0.1M potassium hydrogen phthalate (PHP) in the conical flask‚ add 1-2 drops of phenolphthalein and titrate with the diluted solution of the NaOH till the solution turns light pink. 2. Calculate the strength of the original NaOH solution. Step 2: Poultry eggshell
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The first part of this lab involved the standardization of the base NaOH with potassium hydrogen phthalate‚ or KHP. First‚ about 400 mL of NaOH (10 M) were poured into the 600-mL beaker. This was used to fill the burette. The 50-mL burette was rinsed through twice with 5 mL of NaOH. Then‚ the burette was mounted on the ring stand using a burette clamp and filled to 0 mL. Some of the NaOH was drained to fill the tip of the burette. The initial volume of NaOH‚ rounded to two decimal places‚ was recorded
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undergoing a reaction with sodium hydroxide. Monoprotic: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Diprotic: H2SO4(aq) + 2 NaOH(aq) → 2 H2O(l) + Na2SO4(aq) Triprotic: H3PO4(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3PO4(aq) Any acid that has more than one proton that undergoes a reaction with a base is called a polyprotic acid. Citric acid is a weak‚ polyprotic acid that undergoes the following reaction with sodium hydroxide. H3C6H5O7(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3C6H5O7(aq) In this experiment you will be
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