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<div class="moz-cite-prefix">On 6/18/21 1:01 PM, wrote:<br>
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<div>Good Afternoon Dr. Pounds,</div>
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<div dir="auto">My name is and I have several questions about the
lab report. <span></span></div>
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<div dir="auto">1.) After we receive the concentration of the
unknown from the graph, how do we calculate the grams of NiSO4?
I know we use the concentration of the unknown (M) and multiply
it by the 50.00 mL of solution, but what do we use after? Would
we use the molar weight of NiSO4?</div>
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Yes. If you know the molarity of the nickel sulfate solution and
you multiply that by the volume (in liters) then you will have the
moles of nickel sulfate in your unknown. Use the molar mass of the
nickel sulfate (don't forget that its a hydrate) to find the mass.<br>
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<div dir="auto"><span style="font-size: 12pt;">2) Once we get the
grams of NiSO4, how would we compute the gramps of the Nickel
ion? <br>
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<p>The relationship between nickel sulfate hexahydrate and nickel is
1:1 -- so multiply the moles of nickel sulfate hexahydrate in your
solution by the molar mass of just nickel.<br>
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<div dir="auto">3) For the Atomic Spectra Lab, when we make the
graph in order to find the wavelengths, do we need to make 4
separate graphs for each, or only one graph and use that one
graph in order to find the wavelengths for the Helium lamp,
Hydrogen lamp, the salt, and the candle?</div>
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<p>You are only making ONE GRAPH because the only actual wavelengths
you have are for the mercury lamp. Then you can use your
calibration plot to find the actual wavelengths for the other
lamps and the salt. Since the candle was continuous, you do not
need to determine those wavelengths.</p>
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<p>Let me know if you have other questions.<br>
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<div class="moz-signature">-- <br>
<b><em>Andrew J. Pounds, Ph.D.</em></b><br>
<em>Professor of Chemistry and Computer Science</em><br>
<em>Director of the Computational Science Program</em><br>
<em>Mercer University</em><br>
<em>1501 Mercer University Drive, Macon, GA 31207 </em><br>
<em>(478) 301-5627</em><br>
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