0.30 g of citric acid is dissolved in distilled water to produce 100.0 mL of a 0.016 M solution. How much citric acid is needed in order to...

The balanced chemical reaction for this problem is:

`C_6 H_8 O_7 + 3 NaHCO_3 -> 3 CO_2 + 3 H_2O + Na_3C_6H_5O_7 `

First, we need to get how many moles of sodium bicarbonate to be neutralized. 

Moles of NaHCO3 = 

`30 mL * ((1L)/(1000 mL)) * ((0.5 mol es NaHCO_3)/L) = 0.015 mol es NaHCO_3 `

To get the moles of citric acid (C6H8O7) that will react with 0.15 moles of NaHCO3 = 

`0.015 mol es NaHCO_3 * ((1mol e C_6H_8O_7)/(3 mol es NaHCO_3)) = 0.0050 mol es C_6H_8O_7`

Now we can solve for the amount of citric acid needed to completely react with sodium bicarbonate.

(1) In terms of mass:

`0.005 mol es C_6H_8O_7 * ((192.12 grams)/ (1 mol e C_6H_8O_7)) = 0.96 grams of C_6H_8O_7`

(2) In terms of the citric acid solution:

Molarity = moles/volume of solution

Volume of solution = moles citric acid/molarity of the citric acid solution

`Volume of solution = (0.005/0.016) = 0.31 L`