For the following reaction between Mohr\\\'s salt (iron as FeSO4(NH4)2SO4·6H2O)

Question

For the following reaction between Mohr's salt (iron as FeSO4(NH4)2SO4·6H2O) and potassium dichromate (dichromate as K2Cr2O7), determine the volume (in milliliters) of a 0.100 M solution of Mohr's salt that is needed to fully react with 0.0800 L of 0.100 M potassium dichromate. (The reaction is shown in its ionic form in the presence of a strong acid.)

Cr2 O7^2- + 6Fe^2+ +14H^+ ------- 2Cr^3+ +6Fe^3+ +7H2O

For the same reaction, what volume (in milliliters) of 0.100 M potassium dichromate is required to fully react with 0.0800 L of a 0.100 M solution of Mohr's salt?

Explanation / Answer

Cr2 O7^2- + 6Fe^2+ +14H^+ ------- 2Cr^3+ +6Fe^3+ +7H2O

1 mol Cr2 O7^2- = 6 mol Fe^2+

M1 = concentration of K2cR2o7 = 0.1 M   , M2 = concentration of mohrs salt = 0.1 M

V1 = vol of K2cR2o7 = 0.08 L     ,         V2 = vol of mohrs salt = ?

n1 = 1 ,                                   n2 = 6

M1V1/n1 = M2V2/n2

(0.1*0.08/1) = (0.1*V2/6)

V2 = vol of mohrs salt = 0.48 L

    = 480 ml

M1V1/n1 = M2V2/n2

(0.1*V1/1) = (0.1*0.08/6)

V1 = vol of K2CrO7 = 0.0133 L

    = 13.3 ml

V1 = vol of K2Cr2O7 = 13.3 ML

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