Help please with this chemistry molar calculation

[TheePhysicsStudent]

Homework Statement

I was practising questions from a book printed in the 1980s, and I'm unsure where I went wrong with this Q, the answer is 68.2%

Relevant Equations

I dont use equations for chemistry mole calculations, i just think my way through it so I don't know

The question

My Working:

 

[Steve4Physics]

In your initial hand-written equation, you have “$NaHCO_3 \cdot Na_2CO_3$. This means you have implicitly assumed that you are starting with equal (molar) amounts of $NaHCO_3$ and $Na_2CO_3$. It goes wrong from there.

Suppose the 0.500g of reactant contains x grams of $NaHCO_3$ and y grams, of $Na_2CO_3$.

Can you set up 2 simultaneous equations for x and y and solve them?

Edit: ask for hints if you can't!

 

[Chestermiller]

1 dm^3 = 1000 cc, so 15 cc of the acid solution contains ?? moles of HCl?

 

[symbolipoint]

Maybe this could reassure you or maybe not:
1 decimeter is 10 centimeters.
(careful! these two lines have a mistake.)
0.100 mole/(dm^3) * (10/1)^3(dm/cm)^3

100 mole/(cm)^3

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THAT above is obviously wrong. This is the kind of trouble I have when I do things strictly through keyboard and computer screen. My work later using pen and paper was bettter.

Should have that been like so:
0.100 (moles/dm^3)*(1/10)(dm/cm)(1/10)(dm/cm)(1/10)(dm/cm)
0.100(1/1000)(moles/cm^3)
0.000100 moles per cubic centimeter

 

[Chestermiller]

Maybe this could reassure you or maybe not:
1 decimeter is 10 centimeters.

0.100 mole/(dm^3) * (10/1)^3(dm/cm)^3

100 mole/(cm)^3

0.1 mole/1000cc=$0.0001\ moles/cc$