Introduction: Chemical Compounds often exist in the form of a hydrate, which means that it is inorganic and that there is a certain amount of water molecules attached loosely to each atoms. So, an example of a hydrate would be ZnSO4 XH2O (X being the number of water molecules). This equation is written in empirical formula which means it is written in it’s simplest form with the subscripts reduced as much as possible. The X has to equal an exact number in accordance to the law of definite proportions, which states that a chemical compound always contains the same proportion of elements by mass. After you evaporate the water from the salts, the mass of the salts subtracted from the mass of the hydrate equals the mass of the water due to the …show more content…
The crucible was put over the Bunsen flame to dry for 2 minutes Next, the crucible was left to cool. The mass of the crucible was taken with the balance. A 2g sample of the Zinc Sulfate was added to the crucible. The mass of both the Crucible and the sample was taken. The clay triangle was placed on the ring stand and the crucible was placed on top of it. The crucible started to be heated on gentle heat for 1-2 minutes The flame’s intensity was increased The crucible was heated for 6 more minutes The crucible was left to cool Next, The mass of the crucible with the leftover substance was taken Data/Results/Observation: The Original mass of the empty crucible was 32.32g. After adding about two grams of hydrous Zinc sulfate the mass of the crucible with the sample before heating it was 33.89g. The substance started as a powdery white substance, but after heating it became a solid and brittle substance with a mass of 33.23g. Analysis and …show more content…
This lab did not have the correct outcome because during the lab as the substance became excited by the heat it and many particles left the crucible and not all could be retrieved and put back into the crucible. To avoid this it would be best to make sure the lid is firmly on and after removing the crucible from the heat let the substance cool before removing the lid, as the substance is still excited and may escape the crucible. Another reason this lab could have an incorrect outcome is if you heat the crucible for less than six minutes and not all the hydrate has evaporated, to avoid this it is recommended that after heating it once and taking the mass heat for a minute or two longer and then take the mass again if the mass remains the same then all the water has evaporated, if not then repeat this step until it
Empirical Formulae of a Hydrate Purpose This experiment determined the empirical formula of hydrated unknown copper (II) chloride by using aluminium foil as drying agents and also the effects of hydrated copper (II) chloride on heating. Introduction A hydrate is a substance containing water or its constituent elements. The water molecule chemical state changes broadly between various groups of hydrates. The water molecules attach either to the center of the metal or crystallized with the metal
this lab will be to determine the percent water in an unknown hydrate, determine the moles of water present in each mole of the unknown substance, and to use the molecular mass to find the empirical formula of a hydrate. In this lab and unknown hydrate will be heated two separate times over a Bunsen burner to remove as much water from the substance as possible, before and after heating the crucible the masses will be calculated and recorded for future reference. To participate in this lab it is
Purpose Hydrates are inorganic salts that lose water when heated and undergo a color change. The loss of water makes the hydrate anhydrous. Copper chloride hydrate is what will be used in the lab to show what happens when a hydrate is heated which can lead to a better understanding of hydrates as a whole and their reactions that can be observed to discover things about the environment they’re in. After the removal of water from the copper chloride hydrate, the solid ,when reacted with aluminum and
Lab Report 1 Introduction: Proper chemical formulas entitle many challenges such as the Law of Multiple proportions that states that there may be more than one plausible mole ratio for the elements in that compound. However if we determine the mass of each element in the compound we will be able to get the true chemical formula. In this experiment, we used the law of definite proportions to find the chemical formula for a hydrated compound containing copper, chlorine, and water molecules