1) In solutions 1-5, what are the concentrations of the lron() itrate and Potass
ID: 702332 • Letter: 1
Question
1) In solutions 1-5, what are the concentrations of the lron() itrate and Potassium Thiocyanate after mixing of the 2 solutions occurs and before any reaction takes place? Solution #1 : 5.0 mL 0.002 M Fe(NO)3 in 1 M HNO, 1.0 mL 0.002 M KSCN, 4.0 mL water Solution #2: 5.0 mL 0.002 M Fe(NO3)3 in 1 M HNO, 2.0 mL 0.002 M KSCN, 3.0 mL water Solution #3: 5.0 mL 0.002 M Fe(NO)3 in 1 M HNO, 3.0 mL 0.002 M KSCN, 2.0 mL water Solution #4: 5.0 mL 0.002 M Fe(NO3)3 in 1 M HNO, 4.0 mL 0.002 M KSCN, 1.0 mL water Solution #5: 5.0 mL 0.002 M Fe(NOs)s in 1 M HNO, 5.0 mL 0.002 M KSCNExplanation / Answer
Solution 1
Moles of Fe(NO3)3 = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 5 + 1 + 4 = 10 mL = 0.010 L
Molarity of Fe(NO3)3 after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Moles of HNO3 = Volume x molarity
= 5 mL x 1L/1000 mL x 1 mol/L
= 0.005 mol
Total volume = 5 + 1 + 4 = 10 mL = 0.010 L
Molarity of HNO3 after mixing = 0.005 mol / 0.010 L
= 0.5 M
Moles of KSCN = Volume x molarity
= 1 mL x 1L/1000 mL x 0.002 mol/L
= 0.000002 mol
Total volume = 5 + 1 + 4 = 10 mL = 0.010 L
Molarity of KSCN after mixing = 0.000002 mol / 0.010 L
= 0.0002 M
Solution 2
Moles of Fe(NO3)3 = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 5 + 2 + 3 = 10 mL = 0.010 L
Molarity of Fe(NO3)3 after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Moles of HNO3 = Volume x molarity
= 5 mL x 1L/1000 mL x 1 mol/L
= 0.005 mol
Total volume = 10 mL = 0.010 L
Molarity of HNO3 after mixing = 0.005 mol / 0.010 L
= 0.5 M
Moles of KSCN = Volume x molarity
= 2 mL x 1L/1000 mL x 0.002 mol/L
= 0.000004 mol
Total volume = 10 mL = 0.010 L
Molarity of KSCN after mixing = 0.000004 mol / 0.010 L
= 0.0004 M
Solution 3
Moles of Fe(NO3)3 = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 5 + 3 + 2 = 10 mL = 0.010 L
Molarity of Fe(NO3)3 after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Moles of HNO3 = Volume x molarity
= 5 mL x 1L/1000 mL x 1 mol/L
= 0.005 mol
Total volume = 10 mL = 0.010 L
Molarity of HNO3 after mixing = 0.005 mol / 0.010 L
= 0.5 M
Moles of KSCN = Volume x molarity
= 3 mL x 1L/1000 mL x 0.002 mol/L
= 0.000006 mol
Total volume = 10 mL = 0.010 L
Molarity of KSCN after mixing = 0.000006 mol / 0.010 L
= 0.0006 M
Solution 4
Moles of Fe(NO3)3 = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 5 + 1 + 4 = 10 mL = 0.010 L
Molarity of Fe(NO3)3 after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Moles of HNO3 = Volume x molarity
= 5 mL x 1L/1000 mL x 1 mol/L
= 0.005 mol
Total volume = 5 + 1 + 4 = 10 mL = 0.010 L
Molarity of HNO3 after mixing = 0.005 mol / 0.010 L
= 0.5 M
Moles of KSCN = Volume x molarity
= 4 mL x 1L/1000 mL x 0.002 mol/L
= 0.000008 mol
Total volume = 10 mL = 0.010 L
Molarity of KSCN after mixing = 0.000008 mol / 0.010 L
= 0.0008 M
Solution 5
Moles of Fe(NO3)3 = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 5 + 5 = 10 mL = 0.010 L
Molarity of Fe(NO3)3 after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Moles of HNO3 = Volume x molarity
= 5 mL x 1L/1000 mL x 1 mol/L
= 0.005 mol
Total volume = 10 mL = 0.010 L
Molarity of HNO3 after mixing = 0.005 mol / 0.010 L
= 0.5 M
Moles of KSCN = Volume x molarity
= 5 mL x 1L/1000 mL x 0.002 mol/L
= 0.00001 mol
Total volume = 10 mL = 0.010 L
Molarity of KSCN after mixing = 0.00001 mol / 0.010 L
= 0.001 M
Related Questions
Navigate
Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.