The two main purposes of the lab were to determine the percent by mass of acetic acid in vinegar and to determine the molar concentration of a strong acid. In both parts of the experiment a volumetric analysis was used. This is primarily the aid of volumetric glassware in order to determine specific measurements and calculations. Potassium hydrogen phthalate was used as the primary acid standard to determine the molar concentration of the sodium hydroxide solution in part one of the experiment.…
moles of base in a mixture. Titration is used to determine the concentration of an unknown solution by using an already known solution. This process is important because it is commonly in the medical field. For example, pharmacists use titration in the creation of drugs. In addition, doctors also titration when determining the concentration necessary to give their patients of different medicines. Without titration, doctors and pharmacists would not be able to treat patients.
Acids and bases can…
I predicted that liquid A was glycerine due to a calculated density of 1.38 g/mL. However I was wrong the actual density of liquid A was 1.38 g/mL and the substance was actually corn syrup. Therefore the percent of error for the density of liquid is 1%. For liquid B I had predicted that its substance would be Glycerine due to the calculated density of 1.19 g/mL. I was incorrect for the density of liquid B which was actually 1.26 g/mL, but because the calculated and actual densities…
Experiments involving chemical reactions can be performed using simple household ingredients and products such as baking soda and vinegar.
When baking soda (sodium hydrogen carbonate) reacts with ethanoic acid which is found in vinegar in a 1:1 ration, the reaction will produce three different products which are water, carbon dioxide and Sodium acetate.
The reaction is:
NaHCO3 + HC2H3O2 → NaC2H3O2 + H2O + CO2
In the experiment, the quantitative relationship between the two reagents which is the…
// Sodium thiosulfate solution (of concentrations 0.1M, 0.2M, 0.3M, 0.4M).
// Hydrochloric acid (2M).
// 100cm3 conical flask.
// 10cm3 measuring cylinder.
// Dropping pipette.
// Small piece of plain paper with a large X drawn with think black pen.
Independent - The concentration of sodium thiosulfate solution (0.1M, 0.2M, 0.3M, 0.4M).
Dependent - The time taken for the cross to not be seen.
// Concentration and volume hydrochloric…
The objective of the lab was to determine the densities of known and unknown metal solids and liquids. For the liquids, initially, an Electronic Scale was placed onto Work Bench, and it was zeroed. An empty 50 mL Graduated Cylinder was placed onto the scale, weighing 54.00 grams. In increments of 10 mL. Until the volume was 30.00 Ml, 10.00 mL of water was poured into the Graduated Cylinder. In between each increase of 10.00 mL, the total volume and mass were recorded. For the known metals, the…
filter paper to remove impurities. Next, weigh 5g of coconut oil into 250ml Erlenmeyer flask. Then, add 100ml of neutralized ethanol and 2ml of phenolphthalein indicator. After that, shake until the mixture is completely dissolved. Titrate with standard base 0.1N NaOH, shake vigorously until the endpoint is reached. This is indicated by a slight pink color that persists for 30 seconds. Record the volume of the titrant used. Finally, repeat the steps more carefully in triplicate, recording each…
Experiment 1: Standardisation of approximately 0.25 M Hydrochloric Acid
The aim of the study was to standardise a solution of hydrochloric acid with an approximate concentration of 2.5 M against sodium carbonate solution. The main steps of this experiment were preparing the sodium carbonate solution, transferring the solution into a conical flask by using a pipette, adding the bromophenol blue indicator and titrating with hydrochloric acid until the first green colour appeared. The…
“normal” range for the human body? If not, when was the pH value outside of the normal range, and what acid/base imbalance did this pH value indicate?
No, acidosis occurred at 40 seconds when the pH dropped out of “normal” range to 7.29.
6. Did the PCO2 level change during the course of this run? If so, how?
Yes, the Pco2 level elevated.
7. If you observed an acid/base imbalance during this run, how would you expect the renal system to compensate for this condition?