Consider the hydrate FeSO4 • 7H2O.

2 answers:

7 0

The molar mass of the hydrate is 278.06
The molar mass of the anhydrous salt is 151.92
The molar mass of water in the hydrate is 126.14

mr_godi [17]3 years ago

7 0

Answer: The molar mass of the hydrate $FeSO_4$ . $7H_2O$ is 278g. The molar mass of the anhydrous salt $FeSO_4$ is 152 g. The molar mass of the water in the hydrate is $H_2O$ is 126g.

Explanation: Molar mass of Fe = 56 g

Molar mass of of S = 32 g

Molar mass of O = 16 g

Molar mass of H = 1 g

Molar mass of $FeSO_4$ • $7H_2O$ = $1\times \text{molar mass of Fe}+1\times \text{molar mass of S}+11\times \text{molar mass of O}+14\times \text{molar mass of H}$

Molar mass of $FeSO_4$ • $7H_2O$ = $1\times 56+1\times 32+11\times 16+14\times 1=278g$

Molar mass of $FeSO_4=1\times \text{molar mass of Fe}+1\times \text{molar mass of S}+4\times \text{molar mass of O}$

Molar mass of $FeSO_4=1\times 56+1\times 32+4\times 16=152g$

Molar mass of $7H_2O=14\times \text{molar mass of H}+7\times \text{molar mass of O}$

Molar mass of $7H_2O=14\times 1+7\times 16=126g$

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A chemist dissolves 699. mg of pure hydrobromic acid in enough water to make up 180. mL of solution. Calculate the pH of the sol

Sedaia [141]

Answer: 1.32

Explanation:

First, we must obtain the molar mass of HBr. After that, we try to obtain the concentration of the hydrobromic acid from the formula n=CV since the volume of solution and mass of acid was provided. Recall that n=m/M. If the concentration of acid is thus obtained, we make use of the fact that the concentration of H+ in the acid is equal to the molar concentration of HBr to obtain the pH. The pH is the negative logarithm of the concentration we obtained in the initial step.