5.48 mL of 2.01 mM Fe(NO3)3, 3.10 mL of 2.05 mM KSCN and 1.42 mL of water.find the number of moles of Fe3+ and SCN-
To find the number of moles of Fe3+ and SCN- in the given solution, we first need to calculate the number of moles of Fe(NO3)3 and KSCN using the given concentrations and volumes.
Step 1: Calculate the number of moles of Fe(NO3)3:
Number of moles = concentration * volume
Given:
Concentration of Fe(NO3)3 = 2.01 mM = 2.01 mmol/L
Volume of Fe(NO3)3 = 5.48 mL = 5.48 cm³
Converting mL to L:
Volume of Fe(NO3)3 = 5.48 cm³ * (1 mL / 1 cm³) * (1 L / 1000 mL) = 0.00548 L
Number of moles of Fe(NO3)3 = 2.01 mmol/L * 0.00548 L = 0.011 mmol
Therefore, the number of moles of Fe3+ (from Fe(NO3)3) is 0.011 mmol.
Step 2: Calculate the number of moles of KSCN:
Given:
Concentration of KSCN = 2.05 mM = 2.05 mmol/L
Volume of KSCN = 3.10 mL = 3.10 cm³
Converting mL to L:
Volume of KSCN = 3.10 cm³ * (1 mL / 1 cm³) * (1 L / 1000 mL) = 0.00310 L
Number of moles of KSCN = 2.05 mmol/L * 0.00310 L = 0.00635 mmol
Therefore, the number of moles of SCN- (from KSCN) is 0.00635 mmol.
Since water does not contribute any moles of Fe3+ or SCN-, the moles of Fe3+ and SCN- in the solution are only from Fe(NO3)3 and KSCN, respectively.
Thus, the number of moles of Fe3+ is 0.011 mmol and the number of moles of SCN- is 0.00635 mmol.