How To Standardize Naoh

You find a sample of a solution that has a faint odor resembling vinegar. You are verifying that it is indeed vinegar and you add a few drops of phenolphthalein. The sample turns pink. What assumptions can you make about this sample?

However, stoichiometry provides a more accurate way of measuring acid concentration, giving specific values in grams and milligrams of acid. The balanced equation ensures that there is a 1:1 ratio between acetylsalicylic acid and sodium hydroxide (Figure 1). By using a 1:1 mole ratio, mL of NaOH can be converted to grams of acetylsalicylic acid per tablet. Therefore, a low dose new tablet using 5mL of NaOH contains 0.09 grams or 90 milligrams of acid (Figure 2). This process is then applied to the other tablets; below lists the results of C9H8O4 per tablet in grams and milligrams (Table

3.0g of salicylic acid was weighed then 3.0mL of acetic anhydride and 6 drops of 85% H3PO4 were added to it. The mixture was warmed over a water bath for 5 minutes while stirring. After warming, 20 drops of distilled water was slowly added. 15mL of water was added then the solution was heated until it became clear. It was allowed to cool and was placed in an ice bath until the solution becomes cloudy. Using pre-weighed filter paper, the mixture was filtered and was allowed to dry in the filter paper.

The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity

was to determine the percentage by mass of acetic acid in vinegar using acid/base titration. The

Upon the addition of water, it was noted that a layer separation occurred and the water layer remained on top, with the 2-methylphenol layer on the bottom layer. Then, conversion calculations were performed to determine the appropriate amount of 3M NaOH to be added to the 2-methylphenol solution. From the calculations, it was determined that 1.08 mL were to be added. 3M NaOH itself was a cloudy solution in appearance and upon the addition of 3M NaOH to the 2-methylphenol solution, it was noted a color change occurred and it became a yellow-green solution. Following this, the same calculations used previously, were used to determine the appropriate amount of sodium chloroacetate, which was found to be 0.38 g (3.26 mmol). Sodium choloroacetate was a white, crushed solid that was then combined with 1 mL of water and was swirled until the sodium chloroacetate completely dissolved. This sodium choloracetate solution was then transferred to the 2-methylphenol solution by the use of a medicine

pointer and will be dreary in an acidic arrangement and will hand pink over a fundamental arrangement. pH is the measure of the acidity or basicity of a fluid arrangement. On the off chance that we perform our tests effectively we expect the NaOH-HCl answer for turn blue, the Ascorbic Acid-NaOH answer for turn a shady blue since fillers in the tablet won't be totally solvent in water, and the Baking Soda-HCl answer for turn clear. A solution is a fluid blend of a solute consistently dispersed in a dissolvable. A fluid arrangement is a solute consistently disseminated in water. A solute is a substance that breaks down in a dissolvable. A dissolvable is a fluid that can break up a particular measure of solute. A large portion of our estimations will be in molarity (M) which is signified by the  number of moles of the solute isolated by what number of Liters of the solution. When blending chemicals with water dependably include water the chemicals not the other path around as this could be perilous. We will institutionalize NaOH since it ingests water and CO2 from the air and KHP serves to precisely measure the fixation. Institutionalize intends to convey an answer for a known

For lab eight, the molarity of the NaOH solution is 0.07823 M. For lab nine, the molarity of the NaOH solution is 0.4224 M. The molarity of the NaOH solution for both lab eight and nine was not accurate because the solution did not turn the color to pink. Some source of error in this lab is oxalic acid is not completely moved from the plastic lab tray to the beaker. There is a small amount of substance left in the plastic lab tray that cause the mass of the beaker with NaOH solution to have less mass than I measured previously. Another source of error is not all the base was delivered from the burette to the beaker with oxalic acid. Some base remained on the side of burette instead of fully going into the beaker. This leftover base would change

After reacting with H2O and becoming NaOH, Phenolphthalein is added and creates a pink colour indicating a base is

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

The purpose of Experiment 3 was to determine the pKa of a common acid-base indicator and color dye, bromothymol blue. Acid-base indicators are usually weak acid or base that change color with various pH levels in a solution, giving one specific color for acidic solutions (HIn) and another color for basic solutions (In^-). In the case of bromothymol blue, a weak acid, the reagent turns yellow in the presence of an acidic solution and turns blue in the presence of a basic solution. As the pH of the solution containing bromothymol blue changes, the equilibrium can either shift towards the reactants (Hln) or the products (In^-). Since bromothymol blue is a weak acid, it’s equilibrium equation can be written as: Hln=H^++In^-. The solution color will change depending whether there is more reactant or product present and additionally, whether it is more acidic or basic. Based

Phenolphthalein is an indicator that is pink in alkaline solutions around pH10. When the pH drops below pH 8.3 phenolphthalein goes colorless. Here, an alkaline solution of milk, lipase and phenolphthalein will change from pink to colorless as the fat in milk is broken down to form fatty acids (and glycerol) thus reducing the pH to below 8.3. The time taken for this reaction to occur is affected by temperature.

There were couple of mistakes that occurred over the span of experiment. These mistakes could have irrelevantly influenced the outcomes obtained through the procedure. One common error that occurred was an extremely basic blunder within the lab and that was over-titration, which regularly happens. This is the point in which an excess of titrate is added to the analyte amid the trial. Therefore, the reaction passed the endpoint as too much of the essential sodium hydroxide was added to the Hydroxide arrangement. Fortunately, this occurred only in one trial. Case in point, phenolphthalein reaches its endpoint when it changes from being clear and straightforward to turning into a light shade of pink. In spite of the fact that this might be, for one of our trials when using this indicator the shading turned into a hot pink shade demonstrating that over-titration had occurred. An improvement for this component of the lab is simple. An improvement to control this error would be to use a burette with a smaller opening. This is because the endpoint can be overshot 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.

In this lab a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.

Vinegar is a diluted acetic acid (CH3COOH) and the concentration of the vinegar can be determined by using titration method.