Chemistry question (Normality) please ASAP xD?

first of all... "normality" is an obsolete term today. yes we all use it but it's been dropped by IUPAC, ACS and NIST.

second normality is similar to molarity.

.. molarity = moles solute / L solution

.. normality = moles of "equivalents" / L solution

where an "equivalent" is an H+, an OH- or something that acts like and H+ or an OH-

example...

..1M HCl has 1 mole HCl / L solution

..because it dissociates completely into H+ and Cl-

..1M HCl = 1N HCl

..because we end up with 1 mole H+ per L of solution

.. 2M H2SO4 has 2 moles H2SO4 / L of solution

.. but H2SO4 dissociates into 2 H+'s

.. so that..

...2M H2SO4 = 4N H2SO4

you probably do understand this but I wanted to make sure.

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now for this problem...

the reactions are..

1 CaCO3 + 2 HCl ---> 1 CaCl2 + 1 H2O + 1 CO2

and..

1 NaOH + 1 HCl ---> 1 NaOH + 1 H2O

the idea is..

(1).. all of the CaCO3 is reacted with the HCl

(2).. SOME of the HCl is left over

(3).. the NaOH reacts with the remaining HCl to neutralize it.

Normally (no pun intended) this experiment goes like this..

(1).. we know the normality (or molarity) of the NaOH solution

(2).. we measure the volume of the NaOH solution

(3).. moles NaOH = M x V.... or NxV

(4).. moles unreacted HCl = moles NaOH

(5).. 2 x moles CaCO3 = moles HCl reacted

(6).. total moles HCl = moles HCl reacted + moles HCl unreacted

(7).. molarity (or normality) HCl = moles HCl / L HCl

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but this problem is strange because of the wording

" 6.20 mL of NaOH solution of which 1.000 mL can titrate"

and...

"What is the normality of each of the two solutions?"

plus the comment about the symbol.

I can't tell tell if that means

(a).. you're titrating 1.000mL of the HCl/CaCO3 solution with 6.20mL NaOH

(b).. the normality of the NaOH solution is 1.000N

(c).. if that symbol means "standardized"

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can you copy and paste the exact problem here?