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:

Given Data:

                       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:

c is the answer because when something is left after something evaporates that shows the chemical change.

the correct answer would be d. hope this !