A Comparison Between Sodium Thisulfate And Carbonic Acid

Identify oxides of non-metals that act as acids and describe the conditions under which they act as

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).

Aspirin, Alka-seltzer, and Tylenol showed up acidic from the Universal indicator, whereas sodium bicarbonate and the unknown were blue and basic. This is because sodium is a non-reactive ion, as it is part of NaOH, a strong base, where as bicarbonate attaches to H+ ions to form carbonic acid, thus increasing OH- concentration and pH. On the other hand, Aspirin, or acetylsalicylic acid, forms salicylic acid and acetic acid, lowering pH. Alka-seltzer also showed up as acidic because it contains aspirin.

In this experiment different pH levels ranging from 3 to 11 were used to test the effects on daphnia heart rate. The pH scale ranges from 0 to 14. A pH ranging from 0 to 6 is acidic, a pH of 7 is neutral, and a pH higher than 7 ranging from 8 to 14 is basic. PH revolves around hydrogen ions (H+). The reason pH levels can be acidic, basic, or neutral is because acids give hydrogen ions away while bases accept hydrogen ions. (Decelles, 2002).

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

Higher amounts of alkalinity help to stabilize the pH (Waterfilters.net 2017). Only one of our samples had any carbonate alkalinity, and that was Sample 4 with 10 ppm. The other three samples had no carbonate. Sample 1 had the highest amount of bicarbonate with 62.2 ppm. Sample 2 had 23.6 ppm and Sample 3 had 38.0 ppm of bicarbonate. Sample 4 had the lowest amount of bicarbonate with 30.0 ppm. None of the samples had any hydroxide alkalinity. The sample with the highest total alkalinity was Sample 1 and Sample 2 had the lowest total

will have a pH between 1 and 6 and the weak bases between 8 and 14. The exact order of weak acids and weak bases is determined by comparing the ionization constants (Ka for the weak acids and Kb for the

They ended up being strong and weak bases and this was determined through a pH paper test as well as a flame test. The pH test determined what the pH was and if they were acids or bases and the flame test determined the cation of the substance. The strong base was Potassium Hydroxide (KOH) with a pH of 14. The weak base was Sodium Acetate (NaCH3OO) with a pH of 9. The equivalence point of a chemical reaction is when the chemical equivalent amount of acids and bases have been mixed. For this reaction this point was 19.35 mL of titrant for the strong base and 23.5 mL of titrant for the weak base. While the end point is the point at which a titration is complete, indicated by a color change. This occurred around 19.65 mL of titrant for the strong base and around 25.70 for the weak base. Possible errors in this experiment could include misreading the buret, if one is not accurate it can change the results. Also if the pH meter was not calibrated correctly then the readings for the pH would be incorrect because the wrong pH would be given. If this experiment could be redone then making sure the directions are read carefully would be a number one priority because at times it became confusing, as well as going slow on the titrations so that the readings are

Most enzymes have an optimum pH of around 7, which is fairly neutral. To ensure the experiment is a fair test, I will use the same pH of hydrogen peroxide in every test.

5. Was the pH level always within the “normal” range for the human body? Yes

must be above 8.5 and below 6.5. If the pH is too acidic, then the

To keep this a fair test I have made sure that the acid used is the

1. During my experiment, as my lab partner and I added more sodium hydroxide, the pH level began to rise. As the pH level climbed, the solution began to have more precipitate. In the stomach the pH level is 2.

The acid-balance must be regulated with a range of 7.35 and 7.45 in order for the body to function normally. A pH of below 7.35 is considered acidic and a pH of above 7.45 is considered alkaline or basic. Body acids exist in two forms; volatile and nonvolatile acids. Volatile acids can be eliminated as CO2, usually known as carbonic acid, which is a weak acid. Nonvolatile acids can be eliminated by the kidneys, example are sulfuric and phosphoric. These acids are strong compared to volatile acids.

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;