2, 5.00 mL of 5 .00 x 10\'1 M Fe(NO)); are mixed with 5.00 mL of 0.5 Mi HNO. Cal

Question

2, 5.00 mL of 5 .00 x 10'1 M Fe(NO)); are mixed with 5.00 mL of 0.5 Mi HNO. Calculate the molarity of Fe in the diluted solution. 3. 5.00 mL of s.00x101 M Fe(NO,) are mixed with 2.00 mL of 1.00 x10*M NaSCN and 3.00 mL of0.5M HNO A. Calculate the molarity of the Fe in the diluted solution. B. Calculate the molarity of the SCN in the diluted solution. C. Assume that the following reaction goes to completion: Fe3+ (aq) + SCN(aq) FeSCN2-(aq) Excess Reagent Limiting Reagent Calculate the molarity of the FeSCN2 in the diluted solution.

Explanation / Answer

Solved the first problem in the posted image as per Chegg guidelines, post multiple question to get the remaining problem answer

Q2)

Number of moles of Fe(+3) = Volume of solution (in L) * Molarity

=> 5.00/1000 * 0.5

=> 2.5 * 10^(-3) moles

Volume of solution = Volume of Fe(NO3)3 + Volume of HNO3 = 5mL + 5 mL = 10 mL

Molarity of Fe(+3) in solution = number of moles of Fe(+3)/volume of solution (in L)

=> 2.5 * 10^(-3)/10 * 10^(-3)

=> 0.25 M

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