Acid dissociation constant

information to solve the equation. An indicator is going to have a reaction with hydroxide ions or hydrogen ions to determine whether the substance is a base or acid. The role of an indicator in a titration is to determine how many oxygen or hydroxide ions are in a solution. The laboratory method that is used to titrate an unknown strong acid solution is a titration. When you drop NaOH ions the OH ions unite with H ions creating water which leave less H ions in the solution making the solution less

This experiment was conducted to determine the extent to which commercially bought pipettes accurately deliver desired volumes. A range of small and large volumes of DI water were drawn using three different sized pipettes and massed using an analytical balance. The weights of the water aliquots were divided by the appropriate density of water at 26 to calculate the actual volumes delivered. Error percent analysis was then utilized to deduce the deviation from the accurate volumes. The three different

The purpose of the experiment was to determine how a buffer works and how to use an acid-base indicator. The way a buffer works was determined by observing the changes in pH of solutions of different concentrations weak acids and their conjugate bases to determine how a buffer affects the pH change. The solution of 10 mL of 0.20 M CH3COOH and 10 mL of 0.20 M CH3COONa had slighter changes in pH than the solution of 10 mL of 0.0020 M CH3COOH and 10 mL of 0.0020 M CH3COONa. Both of these solutions were

Mannitol Salt Agar (MSA) differentiates halophile bacteria, and bacteria’s ability to ferment mannitol. Fermenting mannitol results with a yellow halo around colony from the acid produced (staphylococcal species). MSA is composed of enzymatic digest of casein and animal tissue (nitrogen, vitamin carbon source), D mannitol (carbohydrate), NaCl (7.5%, halophiles), phenol red (indicator pH 6.8 turns yellow), and agar (coagulate), with a final pH of 7.4. Unknown 6 did not grow since it is gram negative

In this lab, the pH of seven different substances and solutions were tested both before and after the addition of multiple drops of acid (HCl), or base (NaOH). Depending on the variation of the affected pH from the original, the buffer range of the substance could be calculated by finding the average pH fluctuation, both with the added acid and the added base. As shown in the graph above, the buffer is labelled in dark blue, and the average pH fluctuation from the original was only 1.12. This low

but the smaller interval on the third trial most accurately represents a titration curve for a strong acid and strong base. 8. The graph for trial 3 does not match the exact graph sketched in the pre-lab as it does not accurately show the equivalence point. The curve sketched in the pre-lab reached the equivalence point when 2.00 ml of NaOH was added. M1*V1=M2*V2 0.02M NaOH * V1 = 0.02M Citric acid * 10 ml Citric

Table 1 shows the original average measurements of the permeability of the Beta Vulgaris cells, however, the data was altered due the outliers. On the raw data, there were some negative numbers due to some experimental errors. For this experiment, there should not be any negatives because it results can either the concentration effected the permeability or it did not at all. This indicates that it can shows 0.000 as the lowest. Due to this, the raw table was altered and changed the negative data

Kevin Malakov 6/28/15 CHM 3001 Professor Charnick Lab #7: pH, Dissociation, Hydrolysis, and Buffers
Lab Abstract: The purpose of this experiment was to “compare calculated and measured pHs of a series of hydrochloric acid and acetic acid solutions.” “Measure the pH of various salt solutions.” Also to “compare measured and calculated pHs of: a buffer solution.” (Lab Manual Page 15) Concentation pH %error HCl pH %error HC2H3O2 1x10-1M 0% 6.9% 1x10-2M 5.0% 2.94% 1x10-3M 3.33% 2.56% 1x10-4M

include 20 mL distilled water and the pH value was decreased from 6.65 to 5.48. The sixth group put 1 mL 2 mM HCl in the falcon tube which contain 20 mL distilled water and pH value was reduced from 6.65 to 6.22. The pH value is expected to decrease when acid added into the water, and this is also true in the three groups. The decrease in pH values at different ratios depends on the use of different millimolar substances. The first group received 1 mL of 100 mM HCl and the pH value was further reduced compared

How will various fruit homogenates buffer against acid? Background This experiment will be testing the buffering ability of two fruits and a root. Pineapple, watermelon and ginger will be tested to determine their buffering ability. The hypothesis is: If hydrochloric acid is added to watermelon, pineapple, and ginger then the ginger will buffer better. The acid will affect the fruit by lowering the pH making them more acidic. Buffering helps organisms to maintain homeostasis. Homeostasis is