Pasco Synthesis

In this Chemistry Lab the main objective is to perform accurate chemical analysis for the quantity of elements and compounds in a sample. There will be a compound made then synthesized. The methods used were acid-base titrations, redox titrations, gravity filtration, and distillation. General conclusions included

The Distilled water pH average of HCl for zero drops was 6.67, and the pH for the final thirtieth drop

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.

Titration is a method used to determine an unknown concentration of a known solution. Through this, we may know the chemical that can be dissolved, but not how much of the chemical could be in a specific solution. The purpose of this lab is to be able to determine the concentration of a hydrochloric acid solution using acid base titration in where hydrochloric acid solution is a strong acid and sodium hydroxide is a strong base. In experiment 1, I perform a coarse titration. A coarse titration is a method not very accurate in identifying the end point in the solution, but it does identify the range of titrant volume in which the endpoint happen. In the coarse titration experiment I took a certain amount of sodium hydroxide and added to the

The purpose of this experiment was to determine the molar solubility, the solubility constant, and the effect of a common ion on the molar solubility of calcium hydroxide. To accomplish this the experiment was split into two parts; part A and Part B. in Part A of the experiment a standardized 0.05 M solution of HCl was titrated into a 25 mL solution of saturated Ca(OH)2 which contained 2 drops of orange methyl identifier. Once the titration began, the HCl was added until the methyl orange endpoint was reached, and as a result the volume of the HCl needed for the endpoint to be reached could be used in

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

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

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

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.

As mentioned previously the purpose was to use the titration method in order to find molarity, to find pH. The hypothesis is that very little amount of of HCI is needed to neutralize NaCl. This would need to be tested through this lab, and will be confirmed through the different series of trials. Throughout this we also checked our results and see our accuracy through the scientific process. First in the procedures of this experiment, is we had to neutralize the unknown substance. We had a beaker filled with 50 mL of sodium-hydroxide (NaOH) and buret full with 20 mL of hydrochloride (HCl), Figures 2.3 and 2.4.

To determine the concentration of acid in the solution, the number of NaOH moles supplemented to equivalence point must be discovered, (French et al. 2014).

4. To utilize the titration results to calculate the molarity of the hydrochloric acid and the

You prepare a standard solution by using the M1V1=M2V2 formula, and putting the 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 acidic. The more NaOH ions you add the solution will eventually change color due to the indicator. The data that should be collected during the titration in order to calculate the concentration of HCl should be the number of moles, the volume of the solution, and the amount dropped to make the solution less acidic. You calculate the molarity/ concentration of the unknown HCl solution by using the formula

The purpose of this lab was to use process titration to find concentration of an aqueous solution of Hcl(aq) , using KOH(aq) as the titrant.

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.