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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Asked Oct 9, 2019
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Please help with 4c, 4d, and 4e. We havent learned kaw of equivalents so please do 4c a different way. thank you 

4. You are given an unknown hydrated metal salt containing the bromide ion with the
general formula of MBr n H2O. From previous experimentation, the mass % of Br
was determined to be 51.83 % by mass Br.
a. A 1.000 g sample of the hydrated metal salt is dehydrated to remove water of
hydration. After drying, the sample is found to weigh 0.650 g. What is the
mass percent water in the metal salt?
1,0005
O.350 9 4 Mass
water
O.6509
3503100= 351
sat is 357
The masS percert
water in the mQta
b. What is the mass percent of water in the metal salt?
os letter a
Same answer
2 Moles
c. Based on the formula of the hydrate, MBr2 n H2O, and the mass percent
values determined in parts a and b, determine the molar mass and identity of
the metal. Wa ss of Br in
of Br ins Present in mol
MBr2
19 0f the
51.32
sample
Mass of metol in 1S=Mass of thesa le -Mass Of Br
Mass of water
O-3505
O-51889-
ImolBr
.0005
F0.51839
0.1314-9
O o.51839 Brx
=0.0 50-0.S183
d. 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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4. You are given an unknown hydrated metal salt containing the bromide ion with the general formula of MBr n H2O. From previous experimentation, the mass % of Br was determined to be 51.83 % by mass Br. a. A 1.000 g sample of the hydrated metal salt is dehydrated to remove water of hydration. After drying, the sample is found to weigh 0.650 g. What is the mass percent water in the metal salt? 1,0005 O.350 9 4 Mass water O.6509 3503100= 351 sat is 357 The masS percert water in the mQta b. What is the mass percent of water in the metal salt? os letter a Same answer 2 Moles c. Based on the formula of the hydrate, MBr2 n H2O, and the mass percent values determined in parts a and b, determine the molar mass and identity of the metal. Wa ss of Br in of Br ins Present in mol MBr2 19 0f the 51.32 sample Mass of metol in 1S=Mass of thesa le -Mass Of Br Mass of water O-3505 O-51889- ImolBr .0005 F0.51839 0.1314-9 O o.51839 Brx =0.0 50-0.S183 d. 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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Expert Answer

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:

Mass of metal in the compound 100-51.83-35
=13.17 g
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Mass of metal in the compound 100-51.83-35 =13.17 g

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Step 3

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

51.83 g
B79.904 g.mol*
= 0.6486 mol of Br
As, 2 mol of Br -»0.6486 mol of M
1mol of Br, 0.6480 mol of M
2
0.3243 mol of M
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51.83 g B79.904 g.mol* = 0.6486 mol of Br As, 2 mol of Br -»0.6486 mol of M 1mol of Br, 0.6480 mol of M 2 0.3243 mol of M

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