# What volume of #0.5*mol*L^-1# #"sulfuric acid"# is required for equivalence with a #20*mL# volume of #0.5*mol*L^-1# #NaOH(aq)#?

We need a

I. A stoichiometric equation is required.

Additionally, (ii) we require equal amounts of every reagent.

The formula for "Moles of NaOH" is 20*mLx10^-3*L*mL^-1x0.1*mol*L^-1 = 2x10^-3*mol.

It is obvious that we need to titrate the base using an acid that is LESS concentrated.

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To find the volume of sulfuric acid required for equivalence, you use the equation:

[ n_{acid} \times V_{acid} = n_{base} \times V_{base} ]

Where ( n ) represents the number of moles and ( V ) represents volume. Since sulfuric acid (( H_2SO_4 )) is a diprotic acid, it requires twice as many moles as NaOH for neutralization.

[ n_{acid} = 2 \times n_{base} ]

[ V_{acid} = \frac{{2 \times n_{base} \times V_{base}}}{{n_{acid}}} ]

[ V_{acid} = \frac{{2 \times 0.5 \times 20}}{{0.5}} = 40 , mL ]

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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.

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.

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.

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