In the lab, through calculation, the value of X is determined to equal to 5.361211229, which is close to 5. Therefore, the hydrate is probably CuSO4•5H2O. However, the percentage of error, 7.224%, is not small enough, and the crystals turn out to have a yellowish green color instead of to be white. This can be eliminated by decreasing the amount of hydrate, avoid touching the hydrate with other substances during the reaction, and increasing the intensity of the flame and the time of
This can also speed up the reaction between calcium carbonate and hydrochloric acid with a higher temperature as a higher temperature can let the particles to have a higher kinetic energy for more effective collisions to have a higher rate of reaction. From the calculation, the percentage if calcium carbonate in the toothpaste is found to be at about 20.14% which has a small difference from the literature value of 20%. This maybe cause by the errors when carried out the experiment such as parallax errors. For example, the position of eye level when taking reading or measuring which are not perpendicular to the scale of the instrument will result in the inaccuracy of the data. Next, the other error that might happen is the filter funnel is not inserted properly into the mouth of the conical flask causing some of the hydrochloric acid to be evaporated in the form of vapours.
The compound’s empirical formula was determined to be FeK3(C2O4)3•3H2O. With the molecular formula and the balanced equation for the synthesis of potassium trioxalatoferrate (III) trihydrate, stoichiometry revealed potassium oxalate monohydrate was the limiting reactant. The theoretical yield of 6 grams of potassium oxalate monohydrate was
After we got the different masses, we added them up until we got a final total and we put that mass into a table. Next, we poured the Hydrochloric acid into the flask and we will quickly put the rubber stopper on the flask. After the reaction settled down, we placed the flask with the new substance, the rubber stopper, and the graduated cylinder onto a scale and we got the total mass and we wrote that down on the data table. Finally, we subtracted the beginning weight with the final weight to see the comparison of the mass of the products verses the
Which totaled 93.00 grams then decreased 1.673 grams them the reaction took place. 2. The color of the copper carbonate hydrate as it was heated can help identify the product? The final color ended up being black which was CuO 3. Given that mass was lost from the copper carbonate hydrate during heating, in this decomposition reaction, how many moles of solid product were produced?
During precipitation, NH4Cl cannot be used in place of NH3 because the Cl- can react with Mg2+ thus forming MgCl2. And this is not a desired product in the reaction. Table 1. Data Obtained Constant Weight of Crucible38.3666 ± 0.0002 gConstant Weight of Crucible with Sample41.2928 ± 0.0002 g% Moisture2.45 ± 0.008%%P(as received)5.8 ± 0.008%%P(dry)5.95 ± 0.008%%P2O5 (as received)6.63 ±0.008%% P2O5 (dry)6.80 ±0.008%Using the values obtained, the mass of water, phosphorus, and P2O5 were determined. Calculations can be found in the Appendices.
We concluded that the rate of hydrolysis of (CH3)3CCl is directly proportional to water content in the solvent mixture. Aims of experiment • Determine the rate constants for hydrolysis of (CH3)3CCl in solvent mixtures of different composition (50/50 V/V isopropanol/water and 40/60 V/V isopropanol/water) • Examine the effect of solvent mixture composition on the rate of hydrolysis of (CH3)3CCl Introduction With t-butyl chloride, (CH3)3CCl, being a tertiary halogenoalkane, it is predicted that (CH3)3CCl reacts with water in a nucleophilic substitution reaction (SN1 mechanism), where Step 1 is the rate-determining step. The reaction proceeds in a manner as shown
Even if chemical reactions occur the total mass should stay the same. When doing this experiment there will be times when the mass of a sample cannot be found directly and the formula below will need to be used to find the sample’s mass. Formula 1 : Mass of sample= mass of evaporating dish with sample – mass of evaporating dish For completing this experiment the use of percentages will be used in order to determine the percent of each component in the total mixture. Below is the formula used in order to determine the percentages of each component of a mixture. Formula 2: % Component= 100% component mass (g) sample mass (g) Procedure First, we measured out the evaporating dish to find the mass.
Then calculate Percent Recovered on crystals formed, and preform melting point procedure. 2. You find that a solid substance you are trying to purify is very soluble in ethanol, but not very soluble in water. You decide that you are going to try to recrystallize it from a solvent pair, consisting of ethanol and water. is this decision based on sound rationale?
The formula for sodium acetate is NaC2H3O2, it is quite soluble in water, soluble in ether and slightly soluble in ethyl alcohol. While the chemical compound melts at 622.8℉, it does not have a boiling point for it will decompose. A hydrate is a chemical compound that forms when one or more water molecules are added to the molecules of another substance. Since sodium acetate is a trihydrate (NaC2H3O2·3H2O), it has three molecules of water for every molecule of sodium acetate and because of this, anhydrous sodium acetate quickly transitions into a trihydrate. This is due to sodium acetate being quite hygroscopic, meaning it readily absorbs moisture from the air.