How Much Sodium Hydroxide Used To Turn The Diluted Vinegar

4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the

Vinegar is a common household product, when mixed with the indicator, phenolphthalein, it turns pink. This indicates that Vinegar is acidic.

mL cylinder to the beaker on the stir plate and empty it into the beaker. Place the pH probe in the beaker and record the pH in the data table. Drag the beaker to the red disposal bucket. Double-click the bottle of NaHCO3 to move it to the Stockroom counter. Repeat steps 5 and 6 for KNO3.

When you add vinegar to the water the water become a little darker but the only way you can tell anything was added is due to the smell.

The purpose of this experiment was to see how the amount of baking soda dissolved in vinegar would affect the pH of the vinegar. We conducted the experiment by testing different amounts of baking soda in constant amounts of vinegar, and dropping the solutions on pH paper. By comparing the colors on the pH paper to a list of colors in relation to numbers on the pH scale, we were able to find out that as more baking soda is added, the pH of the solution goes up as well.

This was done by titrating the vinegar with a base that had a calculated concentration. The final average concentration after three trials was 0.5285% by mass. All of the measurements used were taken to four significant figures. One potential source of error is the use of an indicator and titration. In order to induce a change in the color of the solution, it must become slightly basic, this means that more NaOH was added than was actually required to neutralize the acetic acid. This error would indicate that the concentration of acetic acid was slightly higher than it really is; unfortunately, it is unavoidable with the current experiment setup. Another problem with the titration process is that the base can only be added in drops, limiting the precision even more. Aside from these limitations it appears that the process yielded fairly accurate results, with only a 5.706% error when compared to the industry

Objective: We will be using various combinations of distilled water, hydrogen peroxide, malonic acid, ascorbic acid (Vitamin C), acetic acid (Vinegar), starch solution, laundry detergent, iodine tincture, manganese sulfate, and sulfamic acid to produce multiple pairs of solutions labeled Solution A and Solution B. The goal is to either observe the process of fluorescence or the absence of fluorescence. Fluorescence is the chemical property of generating light after undergoing the process of absorbing and emitting a certain amount of energy, directly causing a physical change in the substance's color. Mixing Solution A and Solution B, while viewing the results under UV light from time to time, should result in the new solution constantly

2. Three beakers and funnel should be washed by water. Burette was rinsed by sodium hydroxide solution and pipette was cleaned by hydrochloric acid solution. Retort stand was set up and the white sheet of paper should be placed under the burette where the beaker was put on to easily realize the colour changes.

2. Place 1250 ml beaker containing 75 ml HCl underneath the buret (buret already set up with the volume recorded) for titration and apparatus.

6. Rinse the 50 mL buret with the 0.1 M NaOH solution. Use the utility clamp to attach the buret to the ring stand. Allow the NaOH to be at the 0.00 mL level of the burette.

We started with a 10.00 mL of sulfuric acid solution that was pipetted into an Erlenmeyer flask. The volume and concentration of the base must be known so that we know three of the four volumes/concentrations. The base concentration was given and the volume was obtained during the experiment. The titration resulted in the two flasks having the desired pale pink color. The volume of the base was obtained using the buret.

<p> The experiment that will be discussed in this paper is called “Acidity Constants of Mandelic Acid and Acetic Acid and Buffers,” which was used to determine the students’ knowledge of acidity constants, and how to calculate such of mandelic acid and acetic acid from laboratory measured pH levels of each solution. In this paper, background information on K<SUB>a</SUB>, pH, mandelic and acetic acid will be given. Procedures for calculating K<SUB>a</SUB>, acid concentration and percent acidity of vinegar, along with percent error, will be given as well. Explanations for pH changes will be present too. </p> <

The purpose of this lab was to determine how much acetic acid is in vinegar by using titration. Along with determining how much acetic acid is in vinegar, the titration is used to determine the molar concentration of acetic acid in vinegar. This was done by filling a buret with NaOH and then slowly dripping it into a flask (set on top of an electric stirrer) filled with 10.0 mL of vinegar and two drops of phenolphthalein indicator. Once the solution begins to turn pink that is when it is close to equilibrium. Once the solution shows any indication of turning pink, the drops should turn into drips and be very slow. It is when the solution in the flask is a barely visible pink color that it is the end point. Once the initial and final

Before mixing, the physical properties of Sodium Bicarbonate and Vinegar were recorded in Table 1.

In a titration, an exact volume of one substance(NaOH) was reacted with a known amount of another substance (HCl). The point at which the reaction was complete in a titration is referred to as the endpoint. We recognized a solution which reached the endpoint: when we saw a solution completely turned into pink color. A chemical substance known as an indicator was used to indicate the endpoint. An indicator is a substance that undergoes a distinct observable change (pink color) when conditions in its solution change. The indicator we used in this experiment was phenolphthalein because Phenolphthalein is a weak acid. The weak acid is colourless and its ion is bright pink. And the solution turned pink when we added a basic solution (NaOH) into the solution because adding hydroxide ions removes the hydrogen ions from the equilibrium which replace them turning the indicator