Analysis of Soda Ash and Volumetric Analysis of a Carbonate-Bicarbonate Mixture

We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30

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

Phenolphthalein is a weak acid and does not fully dissociate ergo it creates an equilibrium. When the HCl is added, the equilibrium is to the left, The concentration of the anions is too low for the pink color to be observed. However, the NaOH is a strong base and makes the solution’s equilibrium shift to the right. The concentration of the anion becomes sufficient for the pink color to be observed.

In this experiment, you have been asked by your teacher, to investigate the design of a small-scale airbag system they want to produce as a child safety device to put into baby strollers. Because of sodium azide’s toxicity (which is used in many vehicular airbags), it is suggested you use the reaction of NaHCO₃ (sodium bicarbonate or baking soda) with an aqueous solution of HCL (stomach acid) to produce CO₂ gas to test your engineering design. The reaction of hydrochloric acid and sodium bicarbonate is: HCL + NaHCO₃, one mole of CO₂ gas is produced. Regarding the other products, NaCl dissolves in the water to create a salt solution which occupies only a small portion of the volume inside the bag.

4. Temperature will be kept consistent at room temperature - All tested will be done in the Biology laboratory with the windows shut to make sure the temperature will not change during the tests. The higher the temperature, the shorter the time will be needed for the chemical reactions to happen and phenolphthalein to turn from pink to colourless.

My hypothesis is that if I lose the weight of CO2 in Alka Seltzer then I will be able to determine the percent of sodium bicarbonate in the Alka Seltzer. This is because

The reaction turned dark blue. When Bromothymol Blue reacts with an acid, it turned orange, and when it reacts with a base, the end result is blue.

Acids were varying shades of red or pink and the bases were varying shades of green. The only unexpected result was the variability of color change in the pH 12 buffer solution, though this was attributed to the text, Table 2, stating the pigments are not stable at pH 12 (Pearson, 37).

After about an hour of reaction time, the mixture was isolated via vacuum filtration and was then acidified with 6 M HCl during the work up step. The reaction mixture was initially basic because of the sodium bicarbonate added during the beginning of the reaction. This was confirmed by a litmus paper test, with the reaction mixture spot showing up green which correlates to a pH of 8. However, the incorporation of HCl into the reaction mixture greatly acidified the solution. The litmus paper was spotted with the resulting reaction mixture and appeared red, which suggests a pH of about 2.

The first type is the color indicator method. It uses an indicator (such as phenolphthalein) that changes color after an amount of acid has been added to the solution. The point where the color change occurs is called the endpoint. The second method is the potentiometric titration curve. It utilizes a pH meter in order to record pH values after a certain amount of acid to the solution.

However much reagent needed to change the colour of the solution (thereby having a chemical reaction) is recorded ("Acid-Base Titrations - Chemwiki", 2013). Phenolphthalein is an example of an acid-base indicator, which are used to test the pH of a substance by changing the colour. This indicator weak and colourless, but when mixed with water it forms pink anions. The pH range of phenolphthalein is 8.2-10.0. Indicators are an important part of acid-base titrations as they are the main signal of a chemical reaction and completion of the test ("ACID_BASE INDICATORS", 2016).

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

A few drops of hydrochloric acid, HCL were added to both of the solutions and the observations were recorded. It is observed that bubbles were formed in the sodium carbonate solution. It can be said that effervescence occurred during the reaction. Effervescence can be defined as the escape of gas from a solution and the foaming and fizzing that results from the release of a gas. As there is a gas that is released from the solution, the composition of the solution and its molecular formula must have undergone a change during the reaction and this change can be classified as a chemical change.

deduce it’s pH number, this is done by analyzing its color, and determine if the solution is acidic

The purpose of this lab was to standardize the NaOH and then use the standardized NaOH to find the molarity of acetic acid or vinegar. We standardized the NaOH so that the molarity would be as accurate as possible to then find the molarity of vinegar in the next lab. The results for the lab resulted in the NaOH being .193M. In the second lab, we used the .193M of NaOH to find the molarity of the vinegar. The balanced equation is NaOH(aq)+HC2H3O2(aq)= H2O(l)+NaC2H3O2(aq)which is why the phenolphthalein turned pink. From our lab results, we found that the molarity of the vinegar was .856M. The class average was........ One source of error was that the solution was dark pink in color. This would cause the amount of sodium hydroxide used to go