err...how the hell do i do this?

[ManBearPig]

A 0.140 M red food dye solution was diluted as shown in the table below to make a set of standard or calibration solutions. Use this information to calculate the concentrations of solutions 1, 2, 3, and 4.

Standard Solution Dilution Data
Solution
number 1 2 3 4
Volume of 0.140 M
dye solution
(mL) 11.9 8.4 4.9 1.5
Volume of water
(mL) 0 3.5 7.0 10.4

When entering answers, be sure to include a zero before the decimal point when appropriate. And do not round the answers; this is not the final step in calculating the unknown concentration..
Concentration of Solution 1: 0.140 M
Concentration of solution 2:
Concentration of solution 3:
Concentration of solution 4:

i can only get the first one. i have no idea how to get the others. help please?

 

[stars]

put the lime in the coconut

 

[Rastus]

homework forum-------->

 

[tweakmm]

Read your textbook fool.

We don't do homework here.

 

[BigPoppa]

Molarity is expressed in Moles/Liter. They give your the concentration of Red dye: 0.140 Moles/Liter. If you multiply the Molarity (M/L) by the amount of dye in the solution(mL, convert to L), you get Moles of dye in the solution. I think you can go from there.

 

[SociallyChallenged]

Simple dilution problem. MiVi = MfVf. Do your own homework.

 

[ManBearPig]

thanks...i figured it out.

An unknown solution of the same red dye has an absorbance of 0.498 at 500 nm. What is the concentration of this unknown solution?



any takers?

dont be angry

 

[RedArmy]

a=ebc maybe? I have no idea...even though I should since Im taking chem 111 right now

 

[HamburgerBoy]

ATOT is most certainly not your chemistry class.

 

[ManBearPig]

Originally posted by: HamburgerBoy
ATOT is most certainly not your chemistry class.

im just bad at chemistry and you guys are good at it. i honestly do try though.