# 4. You are given an unknown hydrated metal salt containing the bromide ion with thegeneral formula of MBr n H2O. From previous experimentation, the mass % of Brwas determined to be 51.83 % by mass Br.a. A 1.000 g sample of the hydrated metal salt is dehydrated to remove water ofhydration. After drying, the sample is found to weigh 0.650 g. What is themass percent water in the metal salt?1,0005O.350 9 4 MasswaterO.65093503100= 351sat is 357The masS percertwater in the mQtab. What is the mass percent of water in the metal salt?os letter aSame answer2 Molesc. Based on the formula of the hydrate, MBr2 n H2O, and the mass percentvalues determined in parts a and b, determine the molar mass and identity ofthe metal. Wa ss of Br inof Br ins Present in molMBr219 0f the51.32sampleMass of metol in 1S=Mass of thesa le -Mass Of BrMass of waterO-3505O-51889-ImolBr.0005F0.518390.1314-9O o.51839 Brx=0.0 50-0.S183d. Determine the number of waters of hydration, n, in the hydrated metal salt,MBr2 n H2O.Write out the full empirical formula of the hydrated metal salt.10

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Step 1

Given information:

Mass percent of bromine in the compound = 51.83 %

Step 2

As the mass percent of water was calculated 35 % in the question sample thus, the mass of metal will be calculated as follows:

Step 3

c. To calculate the molar mass of metal the follow...

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