# chemistry

The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.550. If a trial's absorbance is measured to be 0.350 and its initial concentration of SCN– was 0.0010 M, the equilibrium concentration of SCN– will be?

Is there a formula? Or do I use beer's law?

1. 👍 0
2. 👎 0
3. 👁 48
1. Use Beer' law with the standard to find a in A=abc, then use the trial data to find c given A, a, and b. Then the equilibrium and ICE will tell you how much SCN^- is at equilibrium.

1. 👍 0
2. 👎 0
posted by DrBob222
2. what is an ICE?

1. 👍 0
2. 👎 0
3. I - initial concentration
C - change in concentration
E - Equilibrium concentration

1. 👍 0
2. 👎 0
4. actually, you don't need ICE at all.
[FeNCS^2+]=A(eq)/A(std)*.0002

Plug in the absorbances and find [FeNCS^2+].

After that subtract [FeNCS^2+] from the initial concentration of SCN-.

you should get 0.000873 M

1. 👍 0
2. 👎 0

## Similar Questions

1. ### Chem

There are three questions in particular that I am having problems with. Here they are 1. A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration

asked by Mark on January 19, 2009
2. ### Chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be ____ M. I tried

asked by Renee on April 13, 2008
3. ### Chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be__?__M

asked by UN on June 28, 2008
4. ### equilibrium concentration

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be ? M. Wouldn't that

asked by Christine on April 4, 2007
5. ### chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be ____ M.

asked by Gloria on April 10, 2008
6. ### chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be ?M.

asked by thuy on February 22, 2008
7. ### Chemistry

A standard solution of FeSCN2+ is prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN. The equilibrium concentration of FeSCN2+ ([FeSCN2+]std) for this standard solution is assumed to be M. What permits

asked by Neil on June 20, 2011
8. ### chemistry

The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.500. If a trial's absorbance is measured to be 0.310 and its initial concentration of SCN–

asked by thuy on February 22, 2008
9. ### chemistry

The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.510. If a trial's absorbance is measured to be 0.250 and its initial concentration of SCN¡V

asked by Gloria on April 10, 2008
10. ### chemistry

The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.520. If a trial's absorbance is measured to be 0.275 and its initial concentration of SCN–

asked by Amy on April 8, 2008
11. ### chem

The standard solution of FeSCN2+ (prepared by combining 9.00 mL of 0.200 M Fe(NO3)3 w/1.00 mL of 0.0020 M KSCN) has an absorbance of 0.520. If a trial's absorbance is measured to be 0.275 and its initial concentration of SCN–

asked by anonymous on April 10, 2008

More Similar Questions