This can be be done by using an antilog in the calculation: 2.60 = -log [H3O+ ] [H3O+ ] = antilog (-pH) [H3O+ ] = 10-2.60 [H3O+ ] = 0.0025 M From a laboratory perspective, the pH of a substance could be calculated by performing a titration to find the molar concentration of the substance itself. Then, this data can be substituted into the Acid Dissociation constant expression to solve for the unknown concentration of hydronium ions in the solution. As soon as this is computed via mathematical calculations, the hydronium ion concentration can then be inserted into the expression used to calculate the pH of the substance. d.
Based on our data the law of mass conservation was observed through the experiments containing ZnCl2(aq) + Na2S(aq) and Pb(NO3)2(aq) + 2 KI(aq). We gained mass after mixing the chemicals and separating the chemicals for both experiments. In the first experiment the difference in the amount mass from the initial mass was 0.46 g and in the second experiment there was a difference in the amount mass from the initial mass which was 0.75 g. In the demo experiment, the chemical reaction created was the release of nitrogen gas and H2O gas. In the experiment, the chemical reaction created was the formation of a solid ZnS and an aqueous sodium chloride. In the alternative experiment, the chemical reaction created was of
Bioinorganic Coordination Chemistry This experiment uses H2TTP made during the last lab and hydrated copper (II) acetate to convert the H2TTP to Cu(TTP). The reaction proceeds by being refluxed for 30 minutes. The final product is a non-iridescent purple color, unlike the vivid, shimmering purple color of the starting H2TTP. Introduction Thin layer chromatography, or TLC, is used as a prerequisite for column chromatography. When performing types of chromatography, like TLC, the polarity of solvents is extremely important.
Errors and improvements for this experiment would be the following: using and adding too much indicator that results in a greater pH reading. In order to be as accurate as possible, one must be as accurate as can be. Inaccuracy in this measure will enable and reveal inaccurate results. Another error was the presence of other acids in the test tube that was rinsed with water. This was evident when the acid was placed in the test tube before 2 drops of the indicator was dropped.
Sodium ions and chlorine ions reacted to form NaCl, a salt. At the equivalence point, the point where the solution is slightly pink, the pH is 7 and the number of moles of the acid equals that of the base. Thus, c(acid).v(acid)=c(base).v(base) at the equivalence
There are many different compounds that involve sodium that are consider useful, and this paper will cover some of the most useful and common compounds. The most familiar one is sodium chloride, which chemical formula is NaCl. Sodium chloride has a molar mass of 58.44 g/mol, a melting point of 1,474̊ F, and a boiling point of 2,575̊ F. Sodium chloride is created when a sodium atom gives one of its electron to a chlorine atom, thus creating a sodium cation and a chlorine anion. Another compound formed with sodium is sodium bicarbonate, or NaHCO3. Which has a molar mass of 58.44 g/mol, a melting point of 122̊ F, and a boiling point of 1,564̊ F. Sodium bicarbonate is produced by the Solvay process; this process involves the reaction of sodium chloride, ammonia, and carbon dioxide in
The iodine is oxidised to produce I2 wh... ... middle of paper ... ... point was subjective; however it would have been a systematic error because I consistently judged the end point of my experiment. To eliminate this inaccuracy I should have used a colorimeter to judge the end point of my experiment. Also the stop clock had a degree of percentage error measured by: There was also a percentage error with the graduated pipettes calculated by: The percentage error of the burette: The percentage error of the graduated pipettes: Overall percentage error: There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
Shusanta Bhattarai Ms. Kelley Formal lab report The conservation of Mass and how it’s connected to chemical reactions Introduction In this lab, we were looking at the conservation of matter, chemical reactions and using mass to find the number of moles present after a reaction. We had previously studied moles (measurement system) and mass. We copiously took notes on the masses of the objects after reactions and observed how the quantity would “change” after a chemical reaction. The conservation of mass is a law that states a mass will stay consistent over time and will not change until it is not combined or removed. We performed a lot of chemical reactions in this lab.
I first started by performing an experiment that helped determine the mass of my sample. The mass of my sample is one of the key components that will help me determine the moles of my sample. By using the ideal gas law (PV=nRT to n= (PV)/RT) using the mass of my sample in grams, the temperature of my sample after it evaporated during the double-boiling lab, the atmospheric pressure in the room using a barometer, and the volume of the flask I found the moles of the sample (approximately 0.00530 moles). Using the moles I found the molecular weight (mass of sample/ moles of sample). The average molecular weight was 94.9 g/mol.
A common method for determining chloride ions involves isolating the silver chloride precipitate via filtration, determining its mass, and using stoichiometry to calculate the percentage of chloride in an impure sample of unknown chloride. Since the unknown chloride is soluble in water, the percent chloride can be analyzed through the addition of an aqueous solution, silver nitrate, which can form a precipitate with the aqueous chloride. Experimental: In order to accomplish this experiment we’ll need to obtain the materials and chemicals that are required. Material that are required to attain are the sintered glass filtering crucibles (3), desiccator (a drying chamber that keeps materials in the absence of air or in the presence of a drying agent. ), analytical balance, hot plate, aluminum foils, 400ml beakers (3), vacuum filter flask, the waste container and turn on the lab convection oven at 110°C.