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A {millnice} mL solution is made by mixing {gramsnice} g of {chem[2]} and water. The percentage weight per volume of the solution is [[0]] % w/v of {chem[2]}.

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Percentage weight per volume is the weight of the solute in grams divided by the amount of solution in millilitres expressed as a percentage. That is, we do the division and multiply by 100.

In particular, if a {millnice} mL solution is made by mixing {gramsnice} g of {chem[2]} and water. The percentage weight per volume of the solution is:

\n\n\n\n\n\n\n\n\n\n\n\n\n\n

$\\dfrac{\\text{grams}}{\\text{millilitres}}\\times 100$	$=$	$\\dfrac{\\var{gramsnice}}{\\var{millnice}}\\times 100$ % w/v
	$=$	$\\var{ansnice}$ % w/v

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A {millb} mL solution is made by mixing {gramsb} g of {chem[3]} and water. The percentage weight per volume of the solution is [[0]] % w/v of {chem[3]}.

Percentage weight per volume is the weight of the solute in grams divided by the amount of solution in millilitres expressed as a percentage. That is, we do the division and multiply by 100.

In particular, if a {millb} mL solution is made by mixing {gramsb} g of {chem[3]} and water. The percentage weight per volume of the solution is:

\n\n\n\n\n\n\n\n\n\n\n\n\n\n

$\\dfrac{\\text{grams}}{\\text{millilitres}}\\times 100$	$=$	$\\dfrac{\\var{gramsb}}{\\var{millb}}\\times 100$ % w/v
	$=$	$\\var{ansb}$ % w/v

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A {mill} mL solution is made by mixing {grams} g of {chem[0]} and water. The percentage weight per volume of the solution is [[0]] % w/v of {chem[0]} (to 2 decimal places).

Percentage weight per volume is the weight of the solute in grams divided by the amount of solution in millilitres expressed as a percentage. That is, we do the division and multiply by 100.

In particular, if a {mill} mL solution is made by mixing {grams} g of {chem[0]} and water. The percentage weight per volume of the solution is:

\n\n\n\n\n\n\n\n\n\n\n\n\n\n

$\\dfrac{\\text{grams}}{\\text{millilitres}}\\times 100$	$=$	$\\dfrac{\\var{grams}}{\\var{mill}}\\times 100$ % w/v
	$=$	$\\var{ans}$ % w/v (to 2 dec. pl)

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A {per} % {chem[1]} solution contains {amount} g of {chem[1]} in every...

It is important to know {per} % {chem[1]} solution contains {per} g of {chem[1]} in every 100 mL of solution.

Given this, since we have {amount} g of {chem[1]} we have two times the standard amount and so we must have two times the solution, that is 200 mL.

Given this, since we have {amount} g of {chem[1]} we have ten times the standard amount and so we must have ten times the solution, that is 1000 mL.

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100 mL.

", "

200 mL.

", "

500 mL.

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1000 mL.

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{number} moles of a solute are dissolved to create {litres} L of solution. The molar concentration is [[0]] mol/L (to one decimal place).

Molar concentration is the number of moles divided by the volume of solution in litres.

In particular, if a {litres} L solution is made by mixing {number} moles of a solute then the molar concentration is calculated as follows:

\n\n\n\n\n\n\n\n\n\n\n\n\n\n

$\\dfrac{\\text{number of moles}}{\\text{litres}}$	$=$	$\\dfrac{\\var{number}}{\\var{litres}}$ mol/L
	$=$	$\\var{onedec}$ mol/L (1 dec. pl)

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The molecular weight of {chem[0]} is [[0]] g/mol (round each atomic weight to the nearest whole number for this exercise).

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{chem[1]}

How many moles of {chem[0]} are present in {grams} g of {chem[0]}?

[[0]] moles

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The number of moles is the weight of the compound in grams/mol divided by the molecular mass of the compound in grams.

In particular, the number of moles in {grams} g of {chem[0]} is calculated as follows:

\n\n\n\n\n\n\n\n\n\n\n\n\n\n

$\\dfrac{\\text{mass of compound (g)}}{\\text{molecular mass (g/mol)}}$	$=$	$\\dfrac{\\var{grams} \\text{g}}{\\var{chem[2]} \\text{g/mol}}$
	$=$	$\\var{mult}$ mol

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chem formula, sentence for molecular mass

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