The purpose of this experiment was to analyze the % phosphorous in Miracle Gro. Gravimetric Analysis was used to determine the content of phosphorous in this water soluble fertilizer. The overall goal of Gravimetric Analysis is to form the precipitate MgNH4PO46H2O and isolate it from the aqueous solution by vacuum filtration. In order to obtain the precipitate, a series of dissolution reactions and vacuum filtration were performed. First, Miracle Gro was dissolved with DI water and reacted with activated copper to remove coppers ions in the fertilizer.
Purpose: The purpose of this lab is to titrate an unknown solid acid (KH2PO4) with a standardized sodium hydroxide solution. After recording and plotting the data, the acid’s equivalence point will be recorded once the color changes. Using the equivalence point, the halfway point will be calculated, which is used to determine the acid’s equilibrium constant. The acid’s calculated equilibrium constant will be compared with the acid’s established pKa value.
Question3: Experiment 3 The unknown acid sample was 1 • Monoprotic Acid Trails Initial NaOH solution (mL) final NaOH solution (mL) The volume of NaOH to titrate the acid (mL) Amount of Unknown Acid sample 1 (g) The moles of the Unknown Acid (mol) Molar mass of the Unknown Acid (g/mol) A 3.38 28.31 24.93 0.150 0.0026 57.69 B 0.18 29.32 29.14 0.175 0.0029
Phosphate and nitrates are examples of polyatomic ions. Polyatomic ions, also known as molecular ions, are charged chemical species composed of two or more atoms covalently bonded or of a metal complex that can be considered to be acting to a single unit. Phosphates and nitrates are found in fertilizers and some detergents. When rain dissolves these materials make their way into the creeks and rivers. When the surface waters are rich with these materials, they can cause algae to grow, which completes with other organisms for light and other nutrients.
That is where stoichiometry comes along, which is the quantitative relationships or ratios between two or more substances undergoing a physical or chemical change in a balanced equation. It identifies the mole ratio between reactants and products. To understand stoichiometry you have to understand the products and reactants, which involves how to solve balanced reactions. This allows chemists to determine how many moles of a product will be produced from a specific number of moles of a recant or how many moles of reactant are needed to produce a specific amount of a product.
The data shown that red and blue were reflected, and these are the dyes that would be in to make the final solution. To figure out what concentration was needed, a concentration curve was created for the red and blue dye. From the concentration
Determination of the molar mass of magnesium Aim To determine the molar mass of magnesium with the ideal gas equations and Dalton’s law about partial pressures. Materials and chemicals gas measuring tube 50.0cm3 graduated cylinder 1000.0 cm graduated cylinder 10.0cm3 cork with a hole copper wire thermometer barometer magnesium ribbon HCL 35% (concentrated) Background theory Dalton’s Law of Partial states that the total pressure of a gas is equal to the sum of pressure of each individual gas at a specific temperature. The combination of all the partial pressures of the gases that make up the atmosphere gives the total pressure of the atmosphere. The average pressure of the atmosphere is 101 kilopascal(KPa).
Regulating the osmolarity can be accomplished by balancing the concentration of sodium ions with the correct volume of water. Sodium is the main ion that affects the osmolarity of extracellular fluids. The regulation of osmolarity must be assimilated with the regulation of water volume as any changes to one will affect the other. When you need more body fluids you will lose more water than sodium and the osmolarity of the body fluids will increase. The body must keep a certain amount of water however a large amount of sodium can be allowed to be lost.
I. Title: Mass and Mole Relationships in a Chemical Reaction II. Background: Percent yield is the ratio of actual yield to theoretical yield. Amount in percent of one product formed in chemical reaction. Actual yield is the information found is experiments or is given.
a single phosphate compound can be used in a pharmaceutical, personal care products, cleaners and technical uses such as a fire extinguisher, it depends on application, a higher application requires more ingredient. Phosphate products an important part of everyday living. The government authorities says that is safe for working with and for use at home. in many bodies of water,
(Table 2). In the same medium NBRIP used to isolate phosphate solubilizers, values ranging from 31.5 to 519 μg.mL-1 were obtained [41] and in the present study the observed amounts were even higher (26 to 1.735 μg.mL-1 (table 3). A positive correlation between in vitro phosphate solubilization activities of Pseudomonas sp. (LG) with an increase in P content in bean plants inoculated with this bacterium has been observed [42]. In our work, Pseudomonas spp.
Finding the empirical formula for hydrated copper sulfate using calculations to find the amount of each element present in the copper ion, sulfate ion, and water while also comparing the empirical formula to a literature value. Christian Cooper Alexis Powers CHM1210-18M/Gregory Bowers 11-5-15 Purpose: To begin, there are several different goals, techniques, and claims to note in the experiment involving hydrated copper sulfate. The overall goal of this experiment is to find the empirical formula and compare it with a literature value. Yet, in finding the empirical formula of hydrated copper sulfate, there are several process for it to get through, like finding the percentages of copper, water, and finally sulfate.
This will be the only type of cell used in the experiment. Procedure To create the sodium chloride solution: Measure 15 grams of salt (table salt), using an electronic balance. The percentage of sodium chloride that will be added to water to create a solution is 15%. Pour 100 milliliters of water (distilled) in a glass graduated cylinder with an uncertainty of 100 ml +- 0.1 ml, add the 15 grams of salt into the cylinder.
By adding theoretical dose of alum which was 6.55mg of alum, 4.9% of phosphate was removed. However, by adding pragmatic dose of alum which was 20mg of alum, 86% of phosphate was removed. This was because that the equilibrium the equation, Al³⁺ + HₐPO₄³⁻ ͣ ⇌ AlPO₄ + aH⁺ showed that when excess Al³⁺ was added, then the reaction went forward which would make more products of AlPO₄ + aH⁺. Therefore, by adding pragmatic dose of alum of 200mg/L produced more precipitate of AlPO₄ which was the way of removing phosphorus so this was more effective than by adding theoretical dose of alum.
The second most important use of phosphate compounds is in making detergents. The compound most often used in detergents is called sodium tripolyphosphate, acting as a water-softening agent, thereby greatly improving the ability of soaps and detergents to make suds and clean
