hazards of working with solutions HNO3, Fe (NO3)3 and NaSCN

Expert Solution

queen_honey_blossom answered 2 years ago

When measuring the volumes of Fe(NO3)3 and NaSCN solutions in this experiment, the student mistakenly used...

When measuring the volumes of Fe(NO3)3 and NaSCN solutions in this experiment, the student mistakenly used a graduated cylinder instead of volumtetric pipets, After collecting all of the data, the student realized he'd used the wrong piece of equipment, but he didn't redo the experiment. Also, he later realized that he had consistenly misread the graduated cylinder and had thus transferred volumes that were actually 5% lower that the recorded volumes. Incoportate these measurement errors into the data for one...

Given: Molar Concentration of Fe(NO3)3 is 0.2 Molar concentration of NaSCN is 0.001 Volume of Fe(NO3)3...

Given: Molar Concentration of Fe(NO3)3 is 0.2 Molar concentration of NaSCN is 0.001 Volume of Fe(NO3)3 is 10.00 ml (in 0.1 M HNO3) Volume of NaSCN is 2.00 ml (in 0.1 M HNO3) 10.00 ml Fe(NO3)3 + 2.00ml NaSCN + 13.00 ml HNO3= 25 mL Calculate: a) Moles of SCN- b) [SCN-] (25.0 ml) c) [FeNCS2+]

A solution was prepared by mixing 4.00mL of 2.00х10-3M Fe(NO3)3 and 3.00mL of 5.00х10-3M NaSCN and...

A solution was prepared by mixing 4.00mL of 2.00х10-3M Fe(NO3)3 and 3.00mL of 5.00х10-3M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture. Average value of Kc is 787.3

DATA: Calibration Solution 0.2M Fe(NO3)3 in 0.5M HNO3 0.002M KSCN in 0.5 HNO3 0.5M HNO3 Absorbance...

DATA: Calibration Solution 0.2M Fe(NO3)3 in 0.5M HNO3 0.002M KSCN in 0.5 HNO3 0.5M HNO3 Absorbance #1 5mL .50 4.5 .339 #2 5mL 1 4 .758 #3 5mL 1.5 3.5 1.150 #4 5mL 2 3 1.518 Equilibrium Solution 0.002M in Fe(NO3)3 in 0.5M HNO3 0.002 KSCN in 0.5M HNO3 0.5M in HNO3 Absorbance #1 5mL 1 4 .124 #2 5 2 3 .212 #3 5 3 2 .308 #4 5 4 1 .406 #5 5 5 0 .672 1. Concentration...

Fe(NO3)3. 9H2O in 0.5M HNO3 forms a colorless hexa-aquocomplex with the chemical formula {Fe(H2O)6}3+ (aq). This...

Fe(NO3)3. 9H2O in 0.5M HNO3 forms a colorless hexa-aquocomplex with the chemical formula {Fe(H2O)6}3+ (aq). This complex can then undergo an equilibrium reaction with potassium thiocynate (KSCN) to form a red complex with the chemical formula {Fe(H2O)5SCN}2+ (aq). In order to make this reaction occur, the two chemicals need to be mixed with 0.5M nitric acid. This equilibrium reaction is shown below: {Fe(H2O)6}3+ (aq) + SCN-(aq) <--------> {Fe(H2O)5SCN}2+(aq) + H2O (l) a) When recording the absorbance values, what should be...

Create/draw a clear and organized FLOWCHART for K+, Fe+2 or Fe+3, Ni+2, Cr+3, NO3- and PO4-3....

Create/draw a clear and organized FLOWCHART for K+, Fe+2 or Fe+3, Ni+2, Cr+3, NO3- and PO4-3. Discuss observations for any precipitate/color changes, what you would see if it was or wasn't there, etc.

complete equation and net ionic equation: 1. Zn+CuSO4+ZnSO4+Cu 2. 2Zn+Fe(NO3)2=Fe+2Zn(NO3) 3. Zn+SnCl4=4ZnCl+Sn

20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and...

20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and 12.00 mL of water. The equalibrium molarity of Fe(SCN)2+ is found to be 6.82E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-? Fe3+(aq) + 2 SCN-(aq) Fe(SCN)2+(aq) I have the answers (they are correct according to my online homework), but need to know how to get them. Thank you! The correct answeers are: Fe =...

10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and...

10.00 mL of 3.48E-3 M Fe(NO3)3 is mixed with 4.00 mL of 2.84E-3 M KSCN and 6.00 mL of water. The equalibrium molarity of FeSCN2+ is found to be 8.70E-5 M. If the reaction proceeds as shown below, what is the equilibrium molarity of Fe3+ and SCN-? Fe3+(aq) + SCN-(aq) FeSCN2+(aq) Equilibrium Concentration Fe3+ ____________ Equilibrium Concentration SCN- ____________

49.50 grams of Fe(NO3)3 are dissolved in enough water to prepare 550.0 ml of solution calculate...

49.50 grams of Fe(NO3)3 are dissolved in enough water to prepare 550.0 ml of solution calculate the concentration of iron(III) nitrate in the solution in molarity. how many milliliters of this solution would be required to supply 0.084 moles of nitrate ions

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