Phenolphthalein Essays

to the point where the chemical reaction has reached its conclusion and no additional titrant should be added. The end point of this experiment can be obtained when the indicator used changes colour. For example colourless to light pink when phenolphthalein is used and red to orange and subsequently yellow when methyl orange is used. Equivalence point, also known as stoichiometric point in an acid-base titration refers to the point where the reacting acid and base is in equal proportions. In the

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples. (15 points) Example 1: The baking soda (NaHCO3) mixed with vinegar (CH3COOH) created foam as well as the washing soda (Na2CO3) when mixed with the vinegar. Example 2: The color change when the starch and iodine (I2) mixed. As well as the color change when the red cabbage was combine with the vinegar and ammonia. Example 3: When the Epsom salt (MgSO4) was combined

we can also measure the amount of reactants. The concentration of ethanoic acid in the vinegar can be determined through stoichiometric calculations, Using the values obtained from the titration, and also the chemical equation as a reference. Phenolphthalein indicator is used in this acid-base titration Equipment and materials: Commercial vinegar, Yamaha brand 0.1 mol/dm3, NaOH soloution Phenolpthalein indicator soloution (50.00 ± 0.5 cm3 ) cm3 burrete (250.00 ± 0.5 cm3) volumetric flask a

In the chemical reaction of hydrochloric acid, HCl, and sodium hydroxide, NaOH, the theoretical ratio is one HCL for every one NaOH. By then taking a known measurement of HCl, in this case 10mL, in addition to the phenolphthalein indicator and deionized water, and titrating it with NaOH, the amount of NaOH that causes the reaction to be complete was calculable given that we know when the reaction was complete. After calculating the moles of each substance added to complete the reaction, the experimental

Exercise 1 1. Suppose a household product label says it contains sodium hydrogen carbonate (sodium bicarbonate). Using your results from Data Table 1 as a guide, how would you test this material for the presence of sodium bicarbonate? B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript33 Words If I had a household product labeled sodium bicarbonate, I would add an acidic substance and expect bubble to be created. As we know acid reacts with bubbles when combined with sodium

the concentrations of solutions of acids and bases. Through the titration process, we are able to identify physical changes to the mixture such as the colour change to indicate the end point of the experiment. For example, the colour changes of phenolphthalein from colourless to pink and methyl orange from red to orange and subsequently yellow. Acids produce hydrogen ions and bases produce hydroxide ions. This causes the indicator to change colour due to the colour difference from the undissociate molecules

order the color change would not happen. The titrant used was NaOH. The indicator for both parts of the experiment was phenolphthalein. Phenolphthalein is an indicator that changes color depending on the pH of the solution it is in.3 Specifically, phenolphthalein is colorless when the pH of a solution is acidic or neutral, but when the solution becomes slightly basic, phenolphthalein turns slightly pinkish, and then darker pink as the solution becomes more basic.3 This allows for a clear understanding

salt and water. In order to properly conduct this lab procedure many different properties of acids and bases need to be understood. Acids have a pH lower than seven, turn litmus paper red, and when mixed with phenolphthalein remain colorless. However, when a base is mixed with phenolphthalein it turns a vibrant pink shade. Also bases have pH greater than seven and turn litmus paper blue. Bases do not react with metals, feel slippery like soap, and have a bitter taste, whereas acids do react with metal

rectified spirit neutral to phenolphthalein indicator. • Phenolphthalein indicator solution. • Standard aqueous potassium hydroxide or sodium hydroxide solution 0.1N or 0.5N. The solution should be stored in a brown glass bottle and colorless. Procedure: 1. Mix the mustard oil thoroughly before weighing. 2. Weigh approximately about 5 to 10 g of oil sample in a 250 ml conical

Claim: Through the tests performed in lab, it was concluded that unknown powder E was NaHCO₃, powder K was MgSO₄ and powder V was cornstarch. Evidence: Unknown element E was first tested with phenolphthalein and the solution turned pink, this test left 3 possible compounds; NaHCO₃, Na₂CO₃, and CaCO₃. Next the compound was tested with iodine and the solution turned yellow showing that now there was two compounds that could be the identity of unknown powder E; NaHCO₃ and CaCO₃. After that compound

highly reactive and it is solutions are not considered to be carcinogens, the molar mass for H2SO4 is 98.09 g/mol. However, hydrochloric acid is corrosive and it is colorless, with the molecular formula HCL. The molar mass for HCl is 36.46 g/mol. Phenolphthalein is flammable and harmful; it is absorbed through the skin. To be safe avoid contact with eyes, skin, and clothing. In case of skin contact, eye contact, ingestion or inhalation, lab coats, gloves and safety spectacles were worn at all times throughout

The aim of this lab is to determine the concentration of a potassium hydrogen phthalate solution (HKC8O4H4) using acid‐base titration. Introduction: Titration is a technique that chemists use to determine the unknown concentration of a known solution (we know what chemical is dissolved, but not how much in a solution). Because we know what the chemical is, we know how it will react with other chemicals and we can use that reaction to determine the concentration of the solution by measuring the formation

to determine the acidity of the two different brands of soft drinks. But before it, the NaOH solution was standardized first. A 0.15 g of potassium acid phthalate was dissolved in 0.05 L of water in an Erlenmeyer flask. Afterwards, 3 drops of phenolphthalein was added. A 50 mL buret was obtained and was washed with NaOH solution. After filling the buret with NaOH (titrant) and preparing the KHP (analyte) in the Erlenmeyer flask, the solutions were titrated. The volume used from the NaOH solution

standardized solution (titrant) used which is 0.100 L was calculated using the M 1 V 1 = M 2 V 2 relationship. It was then gradually added to the vinegar solution until the acid-base reaction was completely neutralized. To regulate the reaction, phenolphthalein, an acid-base indicator, was added beforehand to the vinegar (analyte). The indicator will change its color, signaling that the end point is obtained and the volume of NaOH used can now be

Vinegar or french for sour wine is formed by aerobic bacteria oxidizing grain alcohol to acetic acid and water more generally, vinegar can be defined as a solution composed of acetic acid ,. Water perhaps other substances the conc. of acetic acid in vinegar may be expressed as a Molarity as a mass percent . a titration involve performing a controlled reaction between a solution of known concentration(the titrant) and a solution of unknown concentration (the analyte) here the titration is an aqueous

The KHP was dissolved in about 25 mL of water, 2 drops of phenolphthalein were added to the solution. A buret was rinsed three times with about 5 mL of NaOH, the buret was securely clamped to a ring stand. The buret was filled with NaOH solution to slightly above the zero mark. A waste beaker was placed under the apparatus

based on the observations from the above reactions. Apparatus : Spatula, Test tube, 150ml beaker Materials : Magnesium ribbon, phenolphthalein indicator, 6M HCl, Gra Procedure : The Group 2A Elements : Alkaline Earth Metals-Magnesium and Calcium 1. A piece of magnesium ribbon was acquired. A test tube is filled up with 5ml of water. A few drops of phenolphthalein indicator is added into the test tube that was filled with 5ml of water. The magnesium ribbon was placed into the test tube. The

would be alkaline. Studies have shown that soda water has a pH varying from 5-6 on the PH Scale. Titration is the point when the indicator changes colour and in the experiment phenolphthalein indicator was used and when it changed to a permanent pink that was classified as the titration point. The indicator known as phenolphthalein indicator is a colourless indicator but when used on an acidic mixture the indicator will stay clear it begins to change to a light pink when is reaches a pH of 7 and finally

The soda water will be stored in 5 different temperatures : 5℃, 15℃, 25℃, 35℃, and 45. The desired temperatures will be achieved by using the water bath and refrigerator. I chose phenolphthalein as the indicator, because it is commonly used for titration and is a weak acid. Phenolphthalein is usually used when the solution is strong base and weak acid. When it is added into an acidic solution, the solution will be colourless; when it is added into an alkaline solution, the solution

agar cubes act as cells and the surface area acts as the cell membrane. Each group conducts the experiment so the class average data is as precise as possible. In the experiment, agar cubes with the indicator phenolphthalein are used to determine the diffusion of the cubes. Phenolphthalein is a base/acid indicator that turns clear when in contact with an acid. In this prac, a Sulphuric acid solution is used. When the surface of the agar cube is put in the sulphuric acid, it will become clear, but