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

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

1 ml of starch, 5 ml of 0.0200 M Na2S2O3 and 5 ml of a 0.5 M C2H3NaO2 buffer were put into a 100 ml graduated cylinder. Using a pipet, 2 ml of 0.250 M KI was added, and distilled water was poured into the graduated cylinder up to the 80 ml graduation. This solution was then transferred into a flask. Using a 50 ml burette, 20 ml of 0.100 M H2O2was added into this flask, and the mixture was briefly mixed. A chronometer was started and time until the solution turned blue was calculated and noted.

The content of these tubes was then later transferred to separate small labeled beakers. The initial pH of the water in test tube A was then measured and recorded using a pH meter. Next. One drop and 1 mL of 0.1 M HCl was added to the water in test tube A, and the pH was measured and recorded. The pH meter was rinsed off each time it was used with distilled water and blotted dry. The initial pH of test tube B was then measured and recorded. Using a graduated cylinder and a pipette, 1 mL of 0.1 M HCl was added to the buffer in test tube B, and the pH was measured and recorded. Then, an additional 2 mL of 0.1 M HCl was added to test tube B, and the pH was measured and recorded again. After adding those 2 mL, three more millimeters of 0.1 M HCl

The objective of the lab was to measure the % of NaCO3 in an Alka-Seltzer tablet in different measures of an acidic solution (Vinegar). Through understanding of stoichiometric relationships and limiting reactants, quantities of substances yielded or consumed in a reaction

1.007x 10-4 M HCl Conclusion: In conclusion, we have conducted this experiment in which we have gathered tons of data on HCl-NaOH titration. In the end we gathered the data to discover the unknown concentration of our solution. It took some practice and some stoichiometry, but that was what it took to disclose the unknown

Experiment 5 titled “Acids, Bases, Salt, and pH”. The purpose of this lab is to become familiar with some properties of salt, bases, and acids, measure acidity (pH), and correlate abnormal acidity of blood or urine. The activities for this lab is to measure the pH of some acid solutions and base solutions using pH paper/meter, and neutralize an acid solution by reacting with base solutions. To begin this experiment (Acid), there will be bottles of different acids (hydrochloric, nitric acid, sulfuric, and acetic acids) on top of the bench. Place one drop of each acid on a blue and red litmus paper and then place a drop of each liquid on (pH) paper. Record the observations. For the Base, place one drop of each liquid (sodium hydroxide, ammonium

Conclusion: The purpose of this lab was to find the missing molarity of HCl with the use of titration formula. The molarity of HCl was concluded to be 0.468M. Through the lab experiment it is seemingly shows a neutralization of acid and base creating water and salt in the solution from double replacement reaction. It also presented the relationship of neutralization between an acid and base molarity is equal in terms of volume/ratio of 1:1 in a titration equation.

In this lab, sodium hydroxide, NaOH (0.0973M), will be the titrate and will be added to the flask containing the unknown acid until it turns into a pinkish solution. This pinkish solution means that it is neutralized. The agent that makes it pink is the phenolphthalein that would be added to the acid solution and what the phenolphthalein does is it turns pink when in normal conditions, but colorless when in acidic conditions. The whole point of the lab is to titrate the sodium hydroxide into the flask with the unknown acid in order to get that pinkish color. Neutralizing the solution helps identify the concentration of the unknown acid because the sodium hydroxide’s concentration is known. With the data being found, the moles and concentration

After being rinsed with water and sodium carbonate, the buret was filled with 60 mL of nitric acid. The beaker was placed 2 cm under the buret. Then the sodium carbonate was titrated until the methyl red changed from red to yellow. The final buret reading was recorded to determine the final volume of the base. The titration data was used to graph a titration

Purpose: The motive of this experiment is to determine the pH with potentiometric measurement using a pH meter and electrode.

The initial volume of HCl was recorded at 13.01 ml. The final volume was recorded at 20.62 ml and the initial volume was subtracted from the final volume to determine the exact volume of HCl at 7.61 ml. Exactly two drops of phenolphthalein indicator solution was added to the HCl. The initial volume of NaOH was recorded at 24.11 ml and titrated. As the solution neared the end point, the titration of NaOH was slowed to one drop at a time. The flask was shaken vigorously for as long as two minutes or until the solution became colorless. When the solution remained light pink for two minutes, the final volume NaOH was recorded at 32.61 ml. The initial volume NaOH was subtracted from the final volume NaOH to determine the exact volume NaOH at 8.50 ml. The exact volume HCl (7.61 ml) was divided by the exact volume NaOH (8.50 ml) and the quotient was multiplied by 100 to get the HCl/NaOH ratio of 0.8953.

The purpose of this lab was to determine how to use an indicator in a titration process, in addition to using indicators to determine pH.

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.

The volumes of NaOH titrated at the endpoint and equivalence point related to one another throughout the experiment. The volume was always greater at the endpoint than at the equivalence point. For the titration of HCl and NaOH, the amount of NaOH added at the endpoint was 9.00 mL and the 2nd derivative curve amount was 9.033 mL. Throughout Trial 2 and titrations of KHP and NaOH, this same trend was seen. The most accurate volume amount of NaOH was determined by looking at the equivalence point. This is the point where all of the H+ was neutralized by OH-. The endpoint is where the indicator, phenolphthalein, changed color based on pH. The color

There are numerous types of spectrometers that can be utilized for the purpose of this lab; the one utilized for this lab is the Spec20D. An acid-base indicator is a substance that is added to s solution and indicates pH change by means of changing colors. For example, bromocresol green is an acid-base indicator, which is a monoprotic organic acid with a molecular weight of 698.02 g/mol. The absorbance of the indicator solution will be tested over a range of wavelengths utilizing the protonated form to determine the wavelength of highest absorbance; then the same tests will be conducted, but when the indicator is in the deprotonated form. Lastly, the tests will be conducted with both species present, utilizing the wavelengths derived from the first two tests. The data will then be plotted and the pKa can then be derived. For the