Empirical Formula Of Hydrated Compound Lab Report
Experiment 5
Determination of Empirical Formulas of Hydrate and Oxide Compounds
Room #216
Locker# 1137
Date of Experiment: May 11, 2014
Date of Submission: May 16, 2014
Purpose:
To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide.
Results:
Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound.
Hydrated Compound code: C-14
Mass (g)
Crucible + Lid
30.581g
Crucible + Lid + Hydrated compound
31.590g
Hydrated Compound
1.004g
Crucible + Lid + contents (after 1st heating)
31.122g
Crucible + Lid + contents (after 2nd heating)
31.131g
Dehydrated compound
0.5455g
Mass=Mass of Hydrated compound – Mass of dehydrated compound
= 1.004 – …show more content…
Discussion:
From Filling out the table on page 104 of the lab manual I could already narrow by unknown hydrate down to only two options. My unknown compound I was given was green so I knew it had to be either copper (ll) chloride dehydrate or nickel (ll) chloride hexahydrate.
After completing the dehydration part of the experiment I found my substance to have a water loss of 45.369%. The value I calculated for the percent water loss of my unknown compound was very close to what the percent water mass of nickel (ll) chloride hexahydrate is.
My unknown compound started off as a bright green solid. During the dehydration process with the addition of heat it turned a yellowish orange colour. It had all clumped into a large piece and had some cracks on the surface. After the addition of the second round out heat my unknown compound became an orange colour and had some bubbles form on the top.
After rehydrating the compound became a darker orange with some green colouring around the edges of the
Determination of Empirical Formulas of Hydrate and Oxide Compounds
Room #216
Locker# 1137
Date of Experiment: May 11, 2014
Date of Submission: May 16, 2014
Purpose:
To determine the identity of an unknown hydrated salt calculating the percent water loss after heating and also to determine the empirical formula of magnesium oxide.
Results:
Table 1: Determination of the mass of waters of hydration of an unknown hydrated compound.
Hydrated Compound code: C-14
Mass (g)
Crucible + Lid
30.581g
Crucible + Lid + Hydrated compound
31.590g
Hydrated Compound
1.004g
Crucible + Lid + contents (after 1st heating)
31.122g
Crucible + Lid + contents (after 2nd heating)
31.131g
Dehydrated compound
0.5455g
Mass=Mass of Hydrated compound – Mass of dehydrated compound
= 1.004 – …show more content…
Discussion:
From Filling out the table on page 104 of the lab manual I could already narrow by unknown hydrate down to only two options. My unknown compound I was given was green so I knew it had to be either copper (ll) chloride dehydrate or nickel (ll) chloride hexahydrate.
After completing the dehydration part of the experiment I found my substance to have a water loss of 45.369%. The value I calculated for the percent water loss of my unknown compound was very close to what the percent water mass of nickel (ll) chloride hexahydrate is.
My unknown compound started off as a bright green solid. During the dehydration process with the addition of heat it turned a yellowish orange colour. It had all clumped into a large piece and had some cracks on the surface. After the addition of the second round out heat my unknown compound became an orange colour and had some bubbles form on the top.
After rehydrating the compound became a darker orange with some green colouring around the edges of the