Question

Tartaric Acid, H2C4H4O6, is neutralized with NaOH. A sample of 3.0 g of tartaric acid reacts with 45 mL of the bas

Answer 1

The concentration of NaOH is 0.888mol/L.

H2C4H4O6(aq)+NaOH(aq)→Na2C4H4O6(aq)+H2O(l) -------(1)

To balance the equation (1), we need to multiply NaOH and H2O by 2, The balance chemical reaction is:

H2C4H4O6(aq)+2NaOH(aq)→Na2C4H4O6(aq)+2H2O(l)

We know that the atomic mass of tartaric acid is 150.087g/mol.

Then, moles of tartaric acid =3.0g/150.087g/mol=0.0200mol

The concentration of NaOH ([NaOH]) =moles volume

 ⇒[NaOH]=(2×0.02mol)/45mL×10−3L.mL−1

⇒[NaOH]=0.888mol/L.

How does NaOH work to neutralize tartaric acid?

With 0.100 M NaOH, tartaric acid, H2C4H4O6, is neutralized. 45 mL of base and 3.0 g of tartaric acid react in a sample.

What results from the reaction of sodium hydroxide with hydrochloric acid?

For instance, when hydrochloric acid (HCl) and sodium hydroxide mix, the hydroxide ion from NaOH reacts with the hydrogen ion to create water (H 2 O). The residual acid then mixes with the lingering sodium ions to create sodium chloride, an ionic molecule (NaCl).

What is NaOH, or sodium hydroxide?

Sodium hydroxide (NaOH) is a very hygroscopic and strongly basic organic chemical. It reacts with a variety of substances to produce quite varied outcomes and is also known as caustic soda or dye.

Learn more about molal concentration:

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