Ferrous sulphate heptahydrate is used to fort | vedclass

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(A) The molar mass of ferrous sulphate heptahydrate $(FeSO_4 \cdot 7H_2O)$ is calculated as: $55.85 + 32.0 + 4 	imes 16.0 + 7 	imes 18.0 = 277.85 \;

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$4.97$

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(A) The molar mass of ferrous sulphate heptahydrate $(FeSO_4 \cdot 7H_2O)$ is calculated as: $55.85 + 32.0 + 4 	imes 16.0 + 7 	imes 18.0 = 277.85 \; g/mol$.Given,$10 \; ppm$ of iron in $100 \; kg$ of wheat means:$10 = \frac{	ext{mass of Fe (in mg)}}{	ext{mass of wheat (in kg)}}$Mass of $Fe$ required $= 10 	imes 100 = 1000 \; mg = 1 \; g$.In $FeSO_4 \cdot 7H_2O$,the mass fraction of $Fe$ is $\frac{55.85}{277.85}$.Let $w$ be the mass of the salt in grams:$w 	imes \frac{55.85}{277.85} = 1 \; g$$w = \frac{277.85}{55.85} \approx 4.97 \; g$.

Ferrous sulphate heptahydrate is used to fortify foods with iron. The amount (in $grams$) of the salt required to achieve $10 \; ppm$ of iron in $100 \; kg$ of wheat is
Atomic weight : $Fe = 55.85$,$S = 32.0$,$O = 16.00$

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Ferrous sulphate heptahydrate is used to fortify foods with iron. The amount (in $grams$) of the salt required to achieve $10 \; ppm$ of iron in $100 \; kg$ of wheat isAtomic weight : $Fe = 55.85$,$S = 32.0$,$O = 16.00$