Posted by **Missy** on Tuesday, February 28, 2012 at 6:18pm.

I really need help with this question.

If 2 trials using 10.0 mL of a solution with an unknown concentration were titrated using close to 20mL of a standard solution each trial, what approximate volume of the standard solution would be needed to titrate 20mL of the solution wit the unknown concentration.

- Chemistry -
**DrBob222**, Tuesday, February 28, 2012 at 6:51pm
10 mL*x = 20*y

20*x = ?y. Wouldn't that be 40 mL of the std?

If that's confusing to you (and the whole problem is confusing), just make up a number for the standard solution. Let's call that 0.1M

So 10mLunk x ?M = 20mLstd x 0.1M

Solve for ?M unk = (20x0.1/10) = 0.2M for the unknown. Now we reverse that.

20 mL unk x 0.2 = ?mLstd x 0.1M

?mL std = 20unk x 0.2/0.1 = 40 mL std.

## Answer this Question

## Related Questions

- Chemistry - A solution of acetic acid having a concentration of about 0.2M is to...
- chemistry - why do you need to construct a calibration curve when doing ...
- Please help with Chemistry????? - A standard solution with a FeSCN2+ ...
- Chemistry - Include an explanation, balanced chemical equation, units, ...
- chemistry - The densities of three solutions with known concentrations ( 20% , ...
- Chemistry - A standard solution with a FeSCN2+ concentration of 1.55x10^-4M has ...
- Chemistry - The densities of three solutions with known concentrations ( 20% , ...
- Chemistry - Consider a solution containing 4.35 mM of an analyte, X, and 1.09 mM...
- analytical chemistry - Any help is greatly appreciated 5mL of a solution A (...
- Chemistry - A 5.00-mL sample of a sulfuric acid solution of unknown ...

More Related Questions