Please helpNumber the answer the each question clearly Part A: CALCIUM - determine how many pieces of calcium you needA.Fill a large test tube with water and invert it into a beaker full of water.Drop a piece of dean calcium into the beaker and hold the inverted test tube immediately above it.When the reaction is over (or when the tube is full of gas), remove it from the beaker but keep it inverted and bring a flaming splint to itsmouth.Save the liquid in the beaker and test it with a strip of red litmus paper.i.ii.iii.iv.OBSERVATIONS: gas produced; pop with flaming splint; water turned red litmus paper blueВ.Hold a flake of calcium with the crucible tongs and put it into a bunsen flame for 2-3 minutes.Allow the residue to cool.iii.i.i.Wet a piece of red litmus paper and touch the residue.Then drop the residue into a test tube and half fill it with water.Does the residue dissolve?iv.V.OBSERVATIONS: residue did not dissolve very well and turned litmus paper blueC.Very carefully drop a small piece of clean calcium into 5 mL of hydrochloric acid in a small test tube and collect the gas by placing yourthumb over the test tube.i.ii.Test the gas with a flaming splint.OBSERVATIONS: vigorous reaction and white solid formed; gas popped in a flaming splintPart B: MAGNESIUM - determine how many pieces of magnesium you needD.Clean two pieces of magnesium ribbon.Drop one piece into a test tube of cold water and the second into a test tube of very hot water.Observe each test tube carefully for signs of a reaction.Drop a piece of red litmus paper into each test tube.Remove the magnesium strips and re-use them for the next experiments.i.ii.ii.iv.V.OBSERVATIONS: cold water showed no reaction; hot water showed vigorous reaction; red litmus did not turn blueDrop a piece of clean magnesium from the cold tube into a test tube containing some dilute hydrochloric acid.Test the gas with a flaming splint.ví.vii.OBSERVATIONS: magnesium reacts producing bubbles: gas popped in a flaming splintE.Burn a strip of magnesium in the air using the crucible tongs and transfer the residue to a test tube of water.Note the solubility of the solid.Drop a piece of red litmus paper into the test tube.Heat the liquid and note all changes.i.i.ii.iv.OBSERVATIONS: bright light produced, solid only slightly soluble: turned litmus paper blue 1. Compare the chemical reactivity of caldium and magnesium. Justify your answer.2. Explain the red litmus paper observation.3. Can you suggest a reason for the difference in chemical reactivity of these two elements even though they are in the same group?4. Are alkali metals or alkali earth metals more reactive? Support your answer with your observations.5. How are group I and group II metals similar and how are they different in terms of their chemical properties?SimilaritiesDifferences

1. Calcium is more reactive then magnesion . As 'Ca' reacts with both cold water and hot water .…

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Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter6: Properties Of Hydrates

Section: Chapter Questions

Problem 1ASA: A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a...

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A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 26.742g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool and finds it has a lower mass; the crucible, cover and contents then weigh 25.598g. In the process the sample was converted to off-white anhydrous MnCl2. a. What was the mass of the hydrate sample? _ghydrate b. What is the mass of the anhydrous MnCl2? _gMnCl2 c. How much water was driven off? _gH2O d. What is the percent by mass of water in the hydrate? water=massofwaterinsamplemassofhydrateinsample100 _massH2O e. How many grams of water would there be in 100.0g hydrate? How many moles? _gH2O; _molesH2O f. How many grams of MnCl2 are there in 100.0g hydrate? How many moles? What percentage of the hydrate is MnCl2? Convert the mass of MnCl2 to moles. The molar mass of MnCl2 is 125.85g/mol. _gMnCl2; _molesMnCl2 g. How many moles of water are present per mole MnCl2? _ h. What is the formula of the hydrate? _
The following information was recorded by a student team working to prepare nickel sulfate. Plan: Prepare NiSO4 by reacting NiO with 6 M H2SO4 The expected product is NiSO4·6H2O. We will filter the crystals from the reaction solution to get the product. NiO + H2SO4 --> NiSO4 + H2O molar mass of NiO: 74.69 g/molmolar mass of NiSO4: 154.75 g/mol molar mass of NiSO4·6H2O: 262.85 g/mol mass of NiO used: 7.5 gvolume of 6M H2SO4 used: 50 mL heated the solution for 30 minutes, cool and filtered the crystals mass of product: 17.4 g Two students calculated percent yield using this data. One student got 66.2% and another got 112%. Based on this information, which of the following statements are true. One or more statements are correct. Group of answer choices The percent yield of 112% was calculated using the molar mass for the hydrated product. The percent yield of 66.2% was calculated using the molar mass for the anhydrous product. Both percent yields are incorrect because…
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