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How many moles of sodium hydroxide are required to prepare a #447.1mL# volume of a solution that is #1.20mol*L^-1# in the solute?

Answer 1

Caleb Adams

We need a bit over #0.5*mol#..............

#"Molarity"="Moles of solute"/"Volume of solution"#

And thus #"moles of solute"="volume of solution"xx"molarity"#

I'm solving this problem dimensionally so that I can determine when to divide and when to multiply. Is this clear?

And so we take the product..........(given that #1*mL-=10^-3L#)...

#447.1xx10^-3*cancelLxx1.20*mol*cancel(L^-1)=0.537*mol#.

We can even be more explicit than this and quote the mass of #NaOH# required for this solution........

"Mass of NaOH" is equal to 0.537molxx40.0gmol^-1, or 21.5g.

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Answer 2

Naomi Aronson

The number of moles of sodium hydroxide required is 0.53652 moles.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

How many moles of sodium hydroxide are required to prepare a #447.1*mL# volume of a solution that is #1.20*mol*L^-1# in the solute?

How many moles of sodium hydroxide are required to prepare a #447.1mL# volume of a solution that is #1.20mol*L^-1# in the solute?