Acid and Base

1. To prepare a standard solution of oxalic acid and use it to standardize an unknown  sodium hydroxide solution.

An example would be pure water. Most of the time the pH is determined by pH paper but there are also other ways to determine the pH. For example, in this lab, cabbage juice was used. Cabbage juice is a great pH indicator because it can be homemade and easy to access.

For part B, 50 mL of an assigned 50 mL pH solution of either 1 M HCl, 1 M NaOH, lemon juice, and 50 mL of household bleach all in separate 250 mL beakers are to be used. For part C, a hot plate or ice are to be used to make the 1.0 mL assigned temperature specific water. This experiment will also use the 1.0 mL of 0.1 Phosphate buffer.

The problem that was trying to be solved in this study deals with analyzing unknown solutions. In this particular case, a chemical company has several unknown solutions and to correctly dispose of them they need to know their properties. To figure out the properties several qualitative tests were performed throughout the study (Cooper 2012).

3.6.3. 2, 4 – D (2, 4–Dichloro phenoxy acetic acid) stock solution (1mg/ml): 10.0mg of 2.4-D being weighed and dissolved completely in 1N NaOH to a final total volume

11. It is then repeated for the solution of unknown concentration (A, B or C).

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

There are different ways that metabolic alkalosis can occur. Generally, the imbalance occurs from a loss of hydrogen ions, a shift of hydrogen ions into the intracellular space, and administration of antacids (Medscape, 2015). Hydrogen ions are lost from the kidneys and the gastrointestinal tract, which occurs from vomiting and diarrhea. When hydrogen ions are excreted from the body, bicarbonate ions are added to the intracellular space (Medscape, 2015).

One milliliter of 6.00-M phosphoric acid was placed into a 125-mL Erlenmeyer flask using a volumetric pipette. Using a slightly larger pipette, six milliliters of 3.00-M sodium hydroxide was transferred into a 50-mL beaker. Then a disposable pipette was used to slowly mix the sodium hydroxide into the phosphoric acid while the solution was swirled around. Then both the beaker and flask were rinsed with 2-mL of deionized water and set aside. A clean and dry evaporating dish was weighed with watch glass on a scale. Then the solution was poured into the dish and the watch glass was placed on top. The solution was then heated with a Bunsen burner to allow for the water to boil off to reveal a dry white solid. After the dish cooled to room temperature it was once again weighed and the new mass was recorded.

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

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

Preserving life is to maintain a good homeostasis. In this case study, there was a problem of metabolic acidosis that caused by a microorganism in the gastrointestinal track after the patient had some fruit juice from a street vendor. That cause the patient to have diarrhea and develop certain signs and symptoms such as abdominal cramping and weakness. To prevent any complication from occurring a good acid and base balance is very important for the body to function properly. Even a slight variation in the acid-base balance should be maintaining. The blood level in the human bodies need the right level of acid and the right level of alkaline to keep its acid-base balance.

of being able to analyze multiple samples in a short amount of time. The most efficient way of determining concentration is to prepare a set of standard solutions of known

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

In the other experiment three pieces of universal pH indicator were placed on a white spotting tile and drop of chlorine water, bromine water and iodine water were transferred on each one of them. The colour of the pH indicators were observed and recorded as shown in the table 1.The halogen solution were filled into the dimples of the spotting tile. They were put in columns and rows which had numbers (1, 2,3 and 4) and letters (A,B and C) in order to differentiate each solutions. After