Lab Report Determining The Molarity Of Acid

Does the amount of active ingredient in different types of tablets decrease or increase per milligram after its expiration date? Overtime, the concentration of acid in a low dose aspirin tablet increases, as the concentration of acid in a high dose aspirin tablet decreases. However, due to various experimental errors, the claim is not a strong and compelling one. What is assumed to have happened is that both low dose aspirin tablets and high dose aspirin tablets increase in concentration of acid as the expiration is surpassed.

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

For lab eight, the molarity of the NaOH solution is 0.07823 M. For lab nine, the molarity of the NaOH solution is 0.4224 M. The molarity of the NaOH solution for both lab eight and nine was not accurate because the solution did not turn the color to pink. Some source of error in this lab is oxalic acid is not completely moved from the plastic lab tray to the beaker. There is a small amount of substance left in the plastic lab tray that cause the mass of the beaker with NaOH solution to have less mass than I measured previously. Another source of error is not all the base was delivered from the burette to the beaker with oxalic acid. Some base remained on the side of burette instead of fully going into the beaker. This leftover base would change

1.007x 10-4 M HCl Conclusion: In conclusion, we have conducted this experiment in which we have gathered tons of data on HCl-NaOH titration. In the end we gathered the data to discover the unknown concentration of our solution. It took some practice and some stoichiometry, but that was what it took to disclose the unknown

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

In this experiment, the concentration of acetic acid in a sample of vinegar was calculated. The sample used for the experiment was sample 4, created on 2/22/2017. The concentration was calculated by titrating the vinegar with NaOH. Unfortunately, NaOH does not form a pure solution so its concentration also had to be calculated. This was done by using it to titrate a solution of KHP, which does form a pure solution. Once the concentration of NaOH was known, it could be used to calculate the mols of acetic acid in a known volume of vinegar, giving us the concentration.

Experiment 5 titled “Acids, Bases, Salt, and pH”. The purpose of this lab is to become familiar with some properties of salt, bases, and acids, measure acidity (pH), and correlate abnormal acidity of blood or urine. The activities for this lab is to measure the pH of some acid solutions and base solutions using pH paper/meter, and neutralize an acid solution by reacting with base solutions. To begin this experiment (Acid), there will be bottles of different acids (hydrochloric, nitric acid, sulfuric, and acetic acids) on top of the bench. Place one drop of each acid on a blue and red litmus paper and then place a drop of each liquid on (pH) paper. Record the observations. For the Base, place one drop of each liquid (sodium hydroxide, ammonium

The lab is about trying to find a neutral potential hydrogen balance (PH) and molarity with following a certain number of steps. In the lab they received material such as, filter paper, vinegar, baking soda, glass rod, water, beaker, graduated cylinder, PH balance meter, and PH strips. After, collecting the material they had to do the first trial with information the teacher had given them to create their own procedure. The first trial was similar to the others except for the amounts would change for each substances. In the first lab the students were told to put fifty milliliters of water in the beaker and mix it in with one gram of sodium bicarbonate. After, mixing the two ingredients the group had to pour the mx into the ring stand. When

The experiment conducted by scientists, Mona Howell and Emily Yau, portrayed a variety of unexpected results. The hypothesis was made that our seeds that were microwaved for 5, 10, and some of the 15 second seeds will grow, the seeds that were microwaved for 20, 30, and 60 seconds will not sprout because the radiation will kill the seed, and the radish seeds in the 1 and 2 teaspoons will sprout. However, some of our hypothesis was proved wrong because during our radiation experiment during trial 2, some of the seeds that were microwaved for a minute even grew. On the other hand, during our acidity experiments, our hypothesis was correct proving that too much acidity damages the dominant seed. A total of three trials were held for each experiment,

Before the commencement of the practical, all necessary glassware and measurement tools were rinsed appropriately. The pipette was rinsed three times with vinegar solution, whereas the volumetric flask was rinsed three times with distilled water. 20mL of the vinegar solution was measured and transferred to the volumetric flask, where it was diluted with distilled water by filling the flask to the 200mL graduation line. A 20ml aliquot of the aforementioned solution was extracted from the volumetric flask via the volumetric pipette and subsequently transferred to the conical flask. Three drops of phenolphthalein indicator were then added. The burette was filled with the provided NaOH solution of 0.1M, with volume measurements taken from the bottom of the meniscus. The conical flask was placed under the burette, from which a rough titration of the vinegar solution began. Titrations halted once a permanent color change was visible in the conical flask. This process was repeated until three concordant titre values were obtained.

The objective of the lab was to prepare standardize solution (titrant: NaOH) of sodium hydroxide, and to determine the concentration of a hydrochloric acid and KHP solution using acid‐base titration. Standardization is the process of determining the exact concentration (molarity) of a solution. The molarity (M) of a solution is used to represent the amount of moles of solute per liter of the solution. Titration is one type of procedure often used in standardization process. A titration is a technique where a solution of known concentration is used to determine the concentration of an unknown solution.

Titration is the process of adding measured volumes of a base or acid with a known concentration to an acid or base with an unknown concentration in order to determine the unknown concentration. Volume measurements play an important role in titration. It involves measuring the exact volume of a solution with a known concentration that will react with a measured volume of a solution that has an unknown concentration. The solution that has a known concentration is called a standard solution. Acid- base titration is based on neutralization that occurs in the reaction. If a base is added to an acid until the acid is neutralized, then the moles of base and the moles of acid will be equal. In other words, the moles of H+ ions must equal the number of moles of OH- ions. The following equation can be used to calculate the unknown molarity of an acidic or basic solution: (Molarity of the acid) * (Volume of the acid) = (Molarity of the Base) * (Volume of the Base) or MaVa = MbVb. Equivalence point is when there is enough of the standard solution to neutralize the unknown solution.

For this experiment, a weak acid-buffer titration will be performed. While acids produce hydronium ions in water, bases produce hydroxide ions. To determine how strong an acid or base is, levels of dissociation are observed. While a strong acid or base entirely dissociates in solution, a weak acid or base only partially dissociates in solution. The extent to which a weak acid dissociates in an aqueous solution can be denoted by the constant, Ka, which stands for the ratio in products to reactant. The following equation is used to describe the mentioned ratio in an acid-dissociation:

To employ the Henderson-Hasselbalch equation for calculations of amounts of a weak acid and its conjugate base required to prepare the buffer solutions of specific pH. Examine pH behavior of buffer solutions using previously studied methods of measuring pH. Reinforce the proper use of volumetric glassware in preparation of solutions of a required concentration. Practice with titration technique in the determination of a buffer capacity.

The aim of this investigation was to determine the precise molarity of two (NaOH(aq)) sodium hydroxide solutions produced at the beginning of the experiment through the acid-base titration technique.