Question Completion Status: QUESTION 2 2.5 points As described in part B of the

Question

Question Completion Status: QUESTION 2 2.5 points As described in part B of the lab, you are preparing a solution by mixing 3.00 mL of 0.00200 M KSCN in HNO3 with 5.00 mL of 0.00200 M Fe(NO3)3 in HNO3 and 2.00 mL 0.25 M HNO3. Calculate the final concentration of KSCN in HNO3 of this solution (before reaction occurs). O 0.00200 M O0.000600 M 0.000400 M 0.0000315 M 0.000200 M O o QUESTION 3 2.5 points In figure 1, absorbance vs concentration is plotted. What does the slop TTIT Paragraph: Arial 43(12pt) t T. Click Save and Submit to save and submit. Click Sqve All Answers to sau

Explanation / Answer

Ans 2 : 0.000600 M

Number of moles of KSCN = molarity x volume (L)

= 0.00200 x 0.003

= 0.000006 mol

Total volume = 0.003 L + 0.005 L + 0.002 L

=0.01 L

So the concentration of KSCN = no. of mol / total volume

= 0.000006 / 0.01

= 0.000600 M

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