Sample 1 2 3 Average DDT (ppt) 0.3 0.8 0.4 0.5 PCB (ppt) 0.9 0.4 0.7 0.7 Dieldrin (ppt) 0.3 0.6 0.1 0.4 We finished part I by testing the dissolved oxygen in the water. Our analysis sample shows an average of 9.5ppm dissolved oxygen in a 17 degree Celsius and the normal levels of dissolved oxygen are between 1-10ppb, which suggests the concentration was not harmful to the fish. The results in part one show that the lead and iron were toxic to the fish but it’s not clear on which was the major
This process can separate water from contaminants. The quality of drinking water was examined by testing for contaminants and comparing the difference between two types of bottled water and tap water. Dasani water has the least amounts of contaminants but bottled water overall proved to have less contaminants than tap water. This combined data suggests that it is easy for our groundwater to be contaminated and we need to be careful when discarding hazardous materials. Each person requires at least 20 to 50 liters of clean, safe water a day for drinking, cooking, and simply keeping themselves clean (Why is safe, 2008).
A pH indicator is a halochromic chemical compound that is added in small amounts to a solution so that the pH (acidity or basicity) of the solution can be determined visually. Hence a pH indicator is a chemical detector for hydronium ions (H3O+) or hydrogen ions (H+) in the Arrhenius model. Normally, the indicator causes the color of the solution to change depending on the pH. At 25° Celsius, considered the standard temperature, the pH value of a neutral solution is 7.0. Solutions with a pH value below 7.0 are considered acidic, whereas solutions with pH value above 7.0 are basic.
Titration is an operation of a common laboratory method of quantitative chemical analysis, which determines the unknown concentration of a substance in a solution by adding to a standard reagent of known concentration, this is also known as volumetric analysis. In this case C1V1= C2V2 equation was used. pH is defined by the following equation; pH= -log10H+. pH is measured by the amount of H+ ions in the solution in comparison to OH- ions; therefore, a solution with the higher pH will contain higher concentration of OH-. A solution with a pH of 7 would be neutral, while an acidic solution would have a pH of lower than 7.
The Solubility of Calcium Hydroxide Introduction: Experiment 16 was done to get an understanding of the solubility of calcium hydroxide, or the slightly soluble salts, gather the knowledge to calculate the Ksp using a primary standard for determining the concentration of an acid, and learning the knowledge to prepare a saturated solution of a slightly soluble salt. This experiment has a few different parts to complete to gather all the information needed to get the experimental values that are seen in the text books used every day. Those values were at some point one by one experimentally calculated as in this experiment. For the first part of this experiment is –saturated solution, for each pair of students should prepare the saturated Ca(OH)2 solution. Of course the saturated solutions take time this experiment is done in a two day lab setting part one should be completed during the first day and ready for use on day two.
Abstract The theory that water is contaminated and cannot be filtered to drinking status is tested. Testing was done by taking water and mixing it with different types of contaminates to see what effects pollutants have on groundwater. Contaminates were mixed with the water in beakers and cheesecloth was used to filter the water. I found that contaminated water is not easy to filter for drinking and most the samples were still contaminated after being filtered. Introduction In this lab, water quality and how contaminated water can be filtered to drinking water is examined.
Bases are solutions that have too many OH- ions. Strong acids are known as having low pH levels on the pH scale, between 0-6 on the pH scale. Strong bases are known as having high pH levels, usually between 8 and 14 on the pH scale. Weak acids and weak bases have pH levels close to the middle of the pH scale; seven is considered neutral. Properties of Acids Taste sour (don't taste them!)...
Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base, NaOH, helps bring the pH of the acid, HCl, closer to seven, which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined.
Aim: | The aim of this experiment is to analyse a sample of vinegar and determine it’s concentration. | | | Hypothesis: | It’s expected that the aceatic acid will have the concentration of 0.1mol as this is the molarity of the NaOH as they have a 1:1 ratio of moles as it states in their chemical equations. | | | Apparatus: | * 1 x retort stand * 1 x retort burette clamp * 1 x burette * 1 x pipette * 1 x glass funnel * 2 x Conical Flasks * Sheet of filter paper * 200mL of 0.1 mol L-1 NaOH * 200mL of acetic acid of unknown concentration | | | Procedure: | 1. WARNING: Wear safety glasses and gloves! 2.
Diprotic Acid Abstract: In this experiment, the total amount of acid neutralized by a solution containing both Na2CO3 and NaHCO3 was determined followed by using the information to calculate the concentrations of carbonate and bicarbonate ions in the solution. This was done by equipping LoggerPro with a pH sensor and a drop counter in order to calculate the pH levels after every single drop. Three titrations were performed for analysis: a titration of a known acid with Bromothymol blue indicator, a titration of an unknown acid with Bromothymol indicator, and a titration of an unknown acid with phenolphthalein. The indicators were added for comparison between color indicators and pH titrations. The results showed that the concentration of Na2CO3 in the unknown acid is between 0.03152M and 0.03924M, and the concentration of NaHCO3 is between 0.02148M and 0.02924M.