Titration Lab

pH was recorded every time 1.00 mL of NaOH was added to beaker. When the amount of NaOH added to the beaker was about 5.00 mL away from the expected end point, NaOH was added very slowly. Approximately 0.20 mL of NaOH was added until the pH made a jump. The pH was recorded until it reached ~12. This was repeated two more times. The pKa of each trial are determined using the graphs made on excel.

2. Calculate the molarity of the Hydrochloric acid in the flask. You may refer to the Titration demo at the beginning of the honors lesson, just above the Virtual Lab to see sample calculations.

Question: The equivalence points of the two titration curves were not in the same pH range. Explain. (Why was the pH at the equivalence point different for the two different acids?)

To improve the results from the experiment buffer solutions that were not whole pHs could have been used e.g. pH 4.5, 5.5 etc. This would have provided more reliable results as a wider range of results would have been produced. Using pHs with decimals would also help to more accurately determine the optimum pH as the optimum may have been above or below the pH stated in the hypothesis; 8. In this experiment however the optimum is taken at 8 because the graph does not rise again.

2. In Part I of this experiment, acetic acid is titrated with NaOH. The net ionic equation for acetic acid reacting with NaOH is CH3COOH+ NaOH =NaC2H3O2+H2O. The equivalence point is when the moles of the titrant and other solution are equal.. You detect the equivalence point by obtaining the point on the graph where the steep pH occurs. In titrating acetic acid with NaOH, the pH is greater than 7 at the equivalence point because NaOH is a strong base so it results in a higher pH, due to the OH- ions in the solution.

a) Tap and drag over the area of the graph where the resting heart rate is displayed to select the data.

In experiment 3.11, we found out whether or not a larger amount of a liquid would get hotter when it boils. To answer this, we heated a specific amount of unknown liquid and recorded the temperature every fifteen seconds. In our scatter plot, we were able to find the boiling point of our liquid. We know that the slope of our graphs is when the liquid molecules were moving around and heating up. The plateau of our graph points is where the liquid started to evaporate and boil. This is were we found our boiling point at. Shantel and I decided that our boiling point was about 98º Celsius. If you had another slope in your graph, that was when you were simply heating the leftover gas. The histogram showed us that there were about equal amounts of data in the higher temperature (about 95º Celsius) bins for both 20mL of liquid and 10mL of liquid. Also, in the lower temperature bins (75º to 80º Celsius) there was about equal amount of data for 20mL of liquid and 10mL of liquid. There was 7 pieces of data for 10mL of liquid in the lower bins, and 6 pieces of data for 20mL of liquid. If a larger amount of liquid did have a higher boiling point, the clusters would be organized by volumes or amount. For example, all of the 20mL pieces of data would be in the higher temperature bins, and all of the 10mL pieces of data would be in the lower temperature bins or flipped. Rather, the bins were clustered by identity. The boiling point is a characteristic property.

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

Within an acid-base titration the titration curve resembles the strengths of the corresponding acids and bases. A strong acid will correspond with a weak conjugate base, and a weak conjugate acid will correspond with a strong base. This is based on the Bronsted-Lowry model. The weak acid will donate protons to the hydroxide ion. Weak acids will have a low Ka value, the Ka value is the tendency of the acid to dissociate:

Using Graph 1: The Volume of Titrant Added in order to reach the Endpoint and the Corresponding pH Values, observe the vertical line of each titration and see the points in which the horizontal lines intersect it. These points give the

My hypothesis was that the shells will slowly erode the shells. My hypothesis is correct because the cup with the biggest change in acid also had the biggest weight change. I know my hypothesis is correct because the shells all changed at least a little in weight. One thing I did not state that should have been stated was that the more amount of acid the more it affects the erosion of the shell. I think that i can prove my hypothesis true if I continued this research until it finally completely erodes. Something is true from what I learned and

A titration is a common method used in the scientific labs for quantitative analysis of chemicals, we use titrations to determine the unknown concentration of an identified analyte using a solution of known concentration. Normally, the known solution (titrant) is put into a burette to a known quantity of the unknown solution (analyte) until the reaction is complete. We can tell that the reaction is complete by using an indicator which usually signals the end of the reaction by a colour change, also known as the endpoint. Alternatively, pH meters can be used to record something known as the pH difference; pH is a measure of hydrogen ion concentration of a solution. Solutions with a high concentration of hydrogen ions have a low pH, while solutions

First, three titration curves and three second derivative curves were created to determine the average pH at the half-equivalence point from the acetic acid titrations. Titration curves were used as visuals to portray buffer capacity. The graphs and a table, Table 1, that showcased the values collected were created and included below. The flat region, the middle part, of Figures 1, 2 and 3, showed the zone at which the addition of a base or acid did not cause changes in pH. Once surpassed, the pH increased rapidly when a small amount of base, NaOH, was added to the buffer solution. Using the figures below and

corresponds to the point in which the concentration of weak acid is equal to the

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.