Tartaric acid, h2c4h4o6, has two acidic hydrogens. the acid is often present in wines and precipitates from solution as the wine ages. a solution containing an unknown concentration of the acid is titrated with naoh. it requires 21.65 ml of 0.3000 m naoh solution to titrate both acidic protons in 50.00 ml of the tartaric acid solution. part a write a balanced net ionic equation for the neutralization reaction.

Balance Chemical equation:

C4H6O6 + 2NaOH ⇒ Na2C4H4O6 + 2H2O

Given dа ta:

Molarity of NaOH = 0.3000

Vol. of NaOH = 21.65

Solution:

moles of NaOH = (0.3000 * 21.65) : 1000 = 0.0064 mol

According to balance chemical equation

NaOH : C4H6O6

2 : 1

0.0064 = (1/2) * 0.0064 = 0.0032 mol

So these 0.0032 mol of tartaric acid are prsent in 50.0 ml of solution.

So in I littre of solutions, its concentration will be as follow

M = 0.0032 * 1000/50 = 0.064 M

Result:

The concentration of acid will be 0.064 M.