Lab Report On Titration

We only added a small amount of HCl to the water and sodium chloride. We did not continue to add more HCl after a significant drop in pH was recorded. We added a total of 2 mL of HCl to both H20 and NaCl before the pH changed. The 1 gram solution of sodium acetate and acetic acid changed after a 8 mL, and the other two never dropped before we reached our total of 10 mL HCl.

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

Methods: First, a burette, ring stand, clamp, and an empty flask were obtained. The burette, with the valve closed, was attached to the ring stand with a clamp, and the empty flask was placed below the burette. Next, 50mL of the NaOH solution were poured into the burette, and a small bit was drained into the empty flask to ensure that the tip of the burette was also full of NaOH solution. The volume of the NaOH in the burette was recorded. Next, approximately 0.6 grams of KHP were massed poured into an empty 125mL flask. Two drops of an indicator solution were added to the KHP

2. (5 pts) List and explain the names and affiliations of the various characters/stakeholders in this story – I’m looking for us to use the story to map out the complexities that are generally associated with solving public health puzzles – the stakeholders you list and explain here should apply to many of the cases we consider going forward.

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.

Its concentration was found through a quantitative and qualitative titration testing. Because HCl is acidic, a 1.07M NaOH solution was used to titrate an aqueous solution of HCl (the unknown solution). The PASCO program gave the final results shown in Figure 1. A typical titration curve can be described as starting at the initial pH of the solution, then some acid/base is added, until a sharp curve either up or down takes the pH past a neutral of 7, and towards the pH level of whatever the added acid’s/base’s pH is (Clark6). The stronger the acid or base being titrated, the faster the change occurs, which means a sharper slope of the titration graph. Also, it is important to note the equivalence point on this titration graph. At the equivalence point “the correct amount of standard solution must be added to fully react with the unknown concentration” (Xavier3). In Figure 1, this equivalence point is shown by where the sharpest slope occurs in the curve, which is seen at about a pH of 5.0

Tools used in this experiment include an electronic scale, a Mohr pipette, a micropipette, test tubes, a bowl of ice, a mortar and pestle, and a ruler. Materials needed include liver extract from bovine liver, water (distilled and regular), hydrogen peroxide, apple cider vinegar, baking soda, and pH paper. In order to achieve and determine our results, we prepared 6 test tubes, each with 2.0 mL of hydrogen peroxide (3% H2O2). We then added 2.0 mL of distilled water into 2 test tubes making that our controlled substance, 0.22g of baking soda into another test tube, 0.24g baking soda into a 4th test tube, and 8.0 mL of apple cider vinegar into the last test tube. The 2 test tubes with the baking soda were used as our basic solution and the 2 test tubes with the apple cider vinegar were used as our acidic solution.

Four square bottles were used during the titration, and a burette filled with NaOH was used to titrate into these bottles. Use a funnel to put in NaOH at the top until the solution is equal to 0.0 mL. In each bottle, 5.0 mL of the bromothymol blue was pipetted, as well as 5.0 mL of 0.10 M KH2PO4 buffer. After that, 15.0 mL of DI water was added into each bottle, following 10.0 mL of the diluted HCl. When all is done, each bottle was mixed thoroughly, until a light orange color appears for all. The pH level of bottle NO. 1 (the initial sample) was recorded and the contents were transferred into a volumetric flask.

At least three more titrations should be performed, this time more accurately, taking into account roughly where the end point will occur. The initial and final readings on the burette (prior to starting the titration and at the end point, respectively) should be recorded. Subtracting the initial volume from the final volume will yield the amount of titrant used to reach the

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 new solution in the Erlenmeyer flask was then titrated exactly like the first solution, and the initial and final buret measurements were recorded once again so that the concentration of acid in the sample could be

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

An acid-base titration is the determination of the concentration of an acid or base by exactly neutralizing the acid/base with an acid or base of known concentration. This allows for quantitative analysis of the concentration of an unknown acid

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.