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

Answer:

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

Explanation:

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

$M=\frac{n}{V}$

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.

$M=\frac{n}{V}\\ n=M\times V\\n=11.0\frac{mol}{L} \times 200.0mL \times \frac{1L}{10^{3}mL } =2.20\times10^{3} mol\\2.20\times10^{3} mol\times \frac{10^{3}mmol}{1mol} =2.2010^{6}mmol$

Answer 2

Answer:

$n=2.20x10^{3} mmol$

Explanation:

Hello,

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

$M=\frac{n}{V}$

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

$n=M*V=11.0mol/L*200.0*\frac{1L}{1000mL}\\n=2.2mol$

Finally, this value in millimoles turns out into:

$n=2.2mol*\frac{1000mmol}{1mol}\\n=2.20x10^{3} mmol$

Best regards.