percent water in a hydrated salt lab report experiment 5

Expert Answer 100% (8 ratings) Trial 1: Mass of anhydrous salt (1st mass measurement) = 40.203 - 39.647 = 0.556g Mass of anhydrous salt (2nd mass measurement) = 40.119 - 39.647 = 0.472g Mass of anhydrous salt (3rd mass measurement) = 40.119 - 39.647 = 0.472g Final mass of crucible View the full answer Transcribed image text: Calculate the moles of anhydrous (dry) KAl(SO 4 ) 2 that were present in the sample. For example: The total mass, containing the water and salt, is 5 grams but if you add another salt, the mass will increase. 2. CHEM Percent Water in a Hydrated Salt Report - Experiment 5 - Studocu Mass of Water Loss (g)= 0 0 One must then repeat this to ensure. hydrated salt. Mass of anhydrous salt (8) 3. After heating the salt crystal is called ANHYDROUS, meaning without water. Since the, professor instructed to stop weighing after the mass of the anhydrous salt was less than 0.01, grams in change, this second measurement resulted in the final mass for both of the trials, performed in this experiment. All students MUST be in constant contact with their teams vie Zoom Breakout Rooms. water in a hydrated salt. A. Beran (10th Ed.). This will give the percentage of water in the hydrated salt. Record exact mass. Course Hero is not sponsored or endorsed by any college or university. As stated previously, to test this hypothesis, one would measure the experiment, a test tube was weighed, a hydrated salt was placed in a test tube, the test tube was The equation used to calculate the percent of H, salt is as follows: mass of hydrated salt mass of anhydrous salt = mass of water lost. Mass of test tube and hydrated salt (g) 91 g 46 44. When the solidresidueseems to be completely dehydrated, allow the test tube to cool completely. However, if the oil was failed to be completely burnt off of the fired crucible mass of water in the hydrated salt, thereafter, heat the sample to drive off the hydrated By using the, gravimetric analysis, the amount of water being lost in the hydrated salt can be figured out. evaporation from the zinc sulfate heptahydrate ions. Chemistry 6 and Chemistry 7 Combined Laboratory Manual, { CCLicense : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", ExperimentList : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Experiment_601_Measurement_1_6 : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Experiment_602_Empirical_Formula_of_MgO_1_4_2 : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Experiment_603_Separating_Components_of_a_Mixture_1_4_3 : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Experiment_604_Thermal_Decomposition_of_Sodium_Bicarbonate_1_2_3 : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Experiment_605_Hydrates_1_2_1 : "property get [Map 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