We can also (via stochiometric and molar ratios), calculate the ratio of salt to water. * Watch glass
Minutes in set up time. Other hygroscopic substances, such as solid \(\ce{NaOH}\), absorb so much water from the atmosphere that they dissolve in this water, these substances are said to be deliquescent. Write out the balanced chemical equation for the dehydration of copper sulfate hydrate (CuSO4.5H2O). Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. Cross), Forecasting, Time Series, and Regression (Richard T. O'Connell; Anne B. Koehler), Psychology (David G. Myers; C. Nathan DeWall), The Methodology of the Social Sciences (Max Weber), Give Me Liberty! Heating on the other hand would introduce heat change and thus a Lab Report
Also as I was calculating the empirical formula, I wasn't quite sure the figures were correct so I might have miscalculated. Score October 3, 2017 February 29, 2016 What is wrong with reporter Susan Raff's arm on WFSB news? Try to avoid and popping or . Added deionized water to the anhydrous copper sulfate, at which point it became hydrated again, and returned to its original blue coloration. This is a student-centered, active learning lesson without lecture or notetaking! The reaction occurred and 2.4469 grams of solid copper, Cu, precipitated; therefore, showing that the limiting reagent was iron. Measure the mass of the empty crucible using the balance. Percent of Water in Copper Ii Sulfate Pentahydrate This lesson also covers the benefits of daily exercise an, Naming and Formulas: Polyatomic Ion Compounds and Hydrates Lesson Experiment_605_Hydrates_1_2_1 - Chemistry LibreTexts 2021-22, PDF Mark K Nclex Study Guide: Outline format for 2021 NCLEX exam. Copper Sulfate's Water of Hydration Lab: Enrichment Activity. The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8.001 grams of copper (II) sulfate, CuSO4, and 2.0153 grams of iron powder, Fe. Compounds to be tested: \(\ce{Na2SO4*10H2O}\), \(\ce{FeCl3}\), \(\ce{KAl(SO4)2}\), \(\ce{CaCl2}\), \(\ce{CuSO4}\). It is generally possible to remove the water of hydration by heating the hydrate. 7: Gravimetric Analysis (Experiment) - Chemistry LibreTexts