Titration Lab

My results yielded a high Average Molarity .270M . The ideal would be around 1.000M . Deviation was ± 1.20

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

The purpose of this experiment is to determine an unknown concentration of acid (hydrochloric acid) with a standard solution of a base (sodium carbonate) using titration method.

The results showed the molarity of the NaOH solution. This experiment was completed twice and a new average molarity

One of these errors could have possibly been that the solutions were left uncovered during the testing phase. An uncovered solution can be contaminated with certain particles of elements found in the air that settle in the solutions, creating colors that are not are not linked with that specific element. This can be compensated for by covering the solutions with a lid prior to testing, in order to limit exposure to any outside factors.

3. If a student did not remove all of the bubbles from inside the buret before reading the initial volume and beginning the titration, will this cause the calculated concentration of the hydrochloric acid determined from that trial to be higher or lower than the actual concentration? Explain your answer in complete

In order for the media to show the change in acidity the solutions are modified and include an indicator chemical. This indicator will change color depending on the ph level of the media it is in. For all the media used in this experiment, the indicator changes to a yellow color when in the presence of an acid and turns magenta/pink when in the presence of a base or alkali.

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

To determine the concentrations in both parts, the change in pH is monitored for every added amount of 0.1035 M NaOH. The pH of the solution is taken using the Orion Model 420A pH reader. The data for Figures 1-4 can be found in Appendix. B.

After the solution had reached the desired temperature of 80°C, a stir bar was placed inside the flask and the titration using the KMnO4 solution began. The titration process was considered completed when the solution had changed color from clear to a light pink. Once the color change was apparent, the final volume of the KMnO4 solution used was recorded. The process was then completed once more to ensure accurate results.

The first titration (with use of the PASCO program) is the most accurate titration that the lab group can perform. The titration curve gives many different variables, with accuracy that passes what humans can do without a machine. But the problem with this titration is that the curve or change to neutrality can often be sudden and out of nowhere. This means that it is very hard to just titrate a solution to become neutral, and often will change into the opposite property, essentially an acid to base and vice versa. The titration with use of an indicator is less accurate, but shows a more visual representation about how a titration takes place. The change in color is a less accurate indication of the volume it takes a solution to change to be neutral, but the visual change is helpful in a classroom laboratory setting. The preference is the first titration method, because it is more accurate and can give more reliable data, since the PASCO machine and drips added are not affected by human

During a titration the pH of the solution will be monitored using a pH meter from that we get a titration curve. The titration curve is then used to determine the equivalent molecular weight and Ka value of the unknown weak acid, from that we are

In Part 1, ~0.30g of KHP is dissolved in 25.00 mL of water, and titrated with NaOH. The volume of NaOH added to reach the endpoint is recorded and corrected (Table 1). The number of moles of NaOH reacted in trial 1 and trial 2 are 0.001534 mol and 0.001433 mol (Equation 1). The concentration of NaOH in trial 1 and trial 2 are 0.07331 M and 0.06628 M (Equation2). The average concentration of NaOH is 0.06979 M (Equation 3). The average deviation is 0.003515 M (Equation 4). In Part 2, ~0.13g of Na2CO3 is dissolved in 25.00 mL of water, and titrated with HCl. The volume of HCl added to reach the endpoint is recorded and corrected (Table 2). The number of moles of HCl reacted in trial 1 and trial 2 are 0.001225mol and 0.001253mol (Equation 5). The concentration of HCl in trial 1 and trial 2 are 0.03298M and 0. 0.03477M (Equation 6). The average concentration of HCl is

Before beginning our investigation, we gathered our materials, which were: a pipette, pipette bulb, burette. To neutralize the reaction of the unknown concentration, called the analyte, we had to determine the the volume of one reactant of known concentration, known as the titrant. The titrant,which was the base, (hydrochloric acid), was added little by little into the burette until color of the analyte, (purple), was reached. The change in color was determined using a

The best titration for this lab would be Trial 3. This trial had the smallest interval in adding NaOH and most accurately shows the pH before the evolution, how it slowly increases, spikes up and then levels off again. The first trial only shows the strong base part of the graph, and the second trial was better than the first, but the smaller interval on the third trial most accurately represents a titration curve for a strong acid and strong base.