Question

A chemist adds 200.0 mL of a 11.0M silver perchlorate (AgCIO solution to a reaction flask. Calculate the millimoles of silver perchlorate the chemist has added to the flask. Be sure your answer has the correct number of significant digits. mmol OP ?

Answer 1

`n=2.20x10^(3) mmol`

Step-by-step explanation:

Hello,

To compute such moles, one must identify that the concentration unit in this problem is molarity, which is defined by:

`M=(n)/(V)`

Since we are inquired to compute the moles, we solve for them as follows:

`n=M*V=11.0mol/L*200.0*(1L)/(1000mL)\\n=2.2mol`

Finally, this value in millimoles turns out into:

`n=2.2mol*(1000mmol)/(1mol)\\n=2.20x10^(3) mmol`

Best regards.

Answer 2

The chemist has added 2.20 x 10⁶ millimoles of silver perchlorate.

Step-by-step explanation:

Molarity is equal to the moles of solute per litre of solution.

`M=(n)/(V)`

where,

n are the moles of solute

V is the volume of solution (expressed in litres)

From this expression, we can find out the moles of solute.

`M=(n)/(V)\\ n=M* V\\n=11.0(mol)/(L) * 200.0mL * (1L)/(10^(3)mL ) =2.20*10^(3) mol\\2.20*10^(3) mol* (10^(3)mmol)/(1mol) =2.2010^(6)mmol`