Solder is an alloy, or mixture, of the metals tin and lead. A 1.50 g sample of s

Question

Solder is an alloy, or mixture, of the metals tin and lead. A 1.50 g sample of solder is dissolved in acid and all of the Sn oxidized to Sn 2+ . The Sn 2+ is reacted with a 0.0525 M solution of sodium dichromate according to the following net ionic equation (included in the picture) and 26.75 mL of the sodium dichromate solution was needed to completely react with the Sn 2+. What is the perect by mass of Sn in the sample of alloy?

Can you please explain the steps you took to solve this problem? I'm given a lot of values here and I'm just not sure where exactly to start or how to utilize these numbers. Please excuse my handwriting in this picture.

Solder is an alloy, or mixture, of the metals tin and lead. A 1.50 g sample of solder is dissolved in acid and all of the Sn oxidized to Sn?". The Sn?" is reacted with m a 0.0525 M solution of sodium dichromate according to the net ionic equation i Hers 14H+(aq) + 3Sn2+(aq) + CnO72-(aq) 3Sn4+(aq) + 2Cr"(aq) + 7H20() Nathyl and 26.75 mL of the sodium dichromate solution was needed to completely react with the Sn2t. What is the percent by mass of Sn in the sample of alloy?

Explanation / Answer

According to given net ionic equation 3 moles Sn2+ requires 1 mole Cr2O72-.

moles dichromate = 26.75 mL x 10-3 L x 0.0525 M = 0.001404375 moles Cr2O72-

moles Sn2+ required = 0.001404375 x 3 = 0.004213125 moles Sn2+ reacted.

mass of Sn (Sn2+) = moles Sn x atomic mass of Sn = 0.004213125 mol x 118.71 g/mol = 0.5 grams

mass percent of Sn = [mass of Sn / total mass of alloy] x 100% = [0.5 g / 1.50 g] x 100% = 33.33%

The perect by mass of Sn in the sample of alloy = 33.33%

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