The fully hydrated form of sodium sulfate is the decahydrate, na2so4 • 10h2o. when heated the hydrated salt loses water. how many water molecules are found per formula unit in a partially dehydrated sample of sodium sulfate with a formula mass of 197 amu (i. e. find n for na2so4 • nh2o)?

There are found 3 water molecules per formula unit in a partially dehydrated sample of sodium sulfate with a formula mass of 197 amu.

Explanation:

The fully hydrated form of sodium sulfate is the decahydrate has structural formula of Na2SO4*10H2O

The molar mass of the decahydrate is 323 amu

When heated the hydrated salt loses water.

The molecular mass is now 197 amu

Na2SO4 has a molecular mass of 142.04 amu

1 molecule of water has a molecular mass of 18 amu

Before heating, the mass of Na2SO4*10H2O = 323 amu

After heating, the mass of Na2SO4*nH20 = 197 amu

The mass of nH2O  lost = 323-197 = 126 amu

1* H2O has a molecular mass of 18 amu

n = 126/18 = 7

The mass after heating - the mass of Na2SO4 = The mass of nH2O

197 - 142 = 55

The mass of nH2O / the mass of 1*H2O = n

55/ 18 = 3

This partially dehydrated sample of sodium sulfate is Na2SO4*3H2O

There are found 3 water molecules per formula unit in a partially dehydrated sample of sodium sulfate with a formula mass of 197 amu.

answer : third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

explanation :

let us write down the given equations

equation 1 :

equation 2 :

equation 3 :

let us use hess's law to find out which 2 equations can be added to get the third equation.

let us reverse equation 2 and multiply it by 2. the new equation that we get is,

equation 4 :

let us add equation 1 & 4

the above equation is similar to equation 3 but has different value for dhrxn.

therefore third trial had the contaminated sample and the correct value for dhrxn should be 1000 kj/mol

wanswer:

explanation: