There were many things that I learned in Module 7 . Some of them where: what is the difference

1. To titrate a hydrochloric acid solution of “unknown” concentration with standardized 0.5M sodium hydroxide.

In this experiment, we learned about stoichiometry, empirical formula, molecular formula, polyprotic acids and bases, metathesis reactions, and moles.

Neutralization reactions are those that involve the reaction of an acid and a base to form water and salt. A solution with a high hydrogen ion concentration is acidic, and a solution with a high concentration of hydroxide ions is

Were you in school today, what did you learn? Yes, learned about acids and bases in chemistry class and the normal stuff math and English.

To start out this study the difference between acids and bases has to be identified. Acids have very low pHs and have a high concentration of hydronium ions, while bases have a high pH and have a high concentration of hydroxide ions. The difference between strong bases and acids, and weak bases and acids is the amount of dissociation. Strong bases and acids dissociate a large amount and let go of their ions in solution, while weak bases and acids may only let go of some of their ions. This is important because if the unknown solutions aren’t strong acids or bases then using their ions to calculate the pH of the solutions will give false results (Diffen 2012).

Acids are a corrosive substance with a pH less than 7. Acidity is caused by a high concentration of hydrogen ions.

When using different methods to measure pH levels there are some tools that can be useful. Some more than others but by putting into action the different methods it may determine which tools will work best and give the best results when testing the pH within a solution. The pH, which stands for the proportion of hydrogen ions in a solution, could be acidic (acidosis), neutral or basic (alkaline). The pH scale goes from numbers 1 through 14. A pH of 7 is neutral;

2. In Part I of this experiment, acetic acid is titrated with NaOH. The net ionic equation for acetic acid reacting with NaOH is CH3COOH+ NaOH =NaC2H3O2+H2O. The equivalence point is when the moles of the titrant and other solution are equal.. You detect the equivalence point by obtaining the point on the graph where the steep pH occurs. In titrating acetic acid with NaOH, the pH is greater than 7 at the equivalence point because NaOH is a strong base so it results in a higher pH, due to the OH- ions in the solution.

concepts that you may have learned in an earlier course and give you an overview of what you will

I found this video very helpful, and definitely helps students prepare for chemistry lab. There were major 8 major topics that they talked about. They talked about handling chemicals, Bunsen burner, glassware, thermometer, glass tubing, centrifuge safety, proper dressing attire, behavior in lab, and emergency equipment. I learned that students should always use small containers that can be controlled easily. Small containers are a lot easier to use. If not, then it can cause accidents. Another point that they made was that students should only mix chemicals together after a professor has approved of it. An important point that the video made is that students should always add the acid to the water never the other way around otherwise it could

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

A few more important terms to keep in mind when doing a lab with chemical and physical changes are

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

There is no required textbook. Class notes, references, and recommend readings are provided during each meeting period and in the follow-up sessions, covering topics on ethics, self-image, evidence-based pedagogies, case studies and tools, psychology, class and lab safety, and more. While most modules are taught by members of the Department of Chemistry, some external experts are invited to both enhance and provide support for the Chemistry community.

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