Tartaric acid, H 2 C 4 H 4 O 6 , is a diprotic acid (it has two acidic hydrogens

Question

Tartaric acid, H2C4H4O6, is a diprotic acid (it has two acidic hydrogens) .   A solution containing an unknown concentration of the acid is titrated with NaOH. It requires 21.65mL of 0.1500 M NaOH solution to titrate both acidic protons in 55.00mL of the tartaric acid solution.

Which of the following is a balanced net ionic equation for the neutralization reaction? Since tartaric acid is not one of the strong acids, it must be a weak acid. Refresh your memory regarding how weak acids are shown in net ionic equations before completing this Part. Also, don't forget get to identify and leave out the spectator ions.

H+ (aq) + OH- (aq) H2O (l)

2 H+ (aq) + 2 OH- (aq) 2 H2O (l)

H2C4H4O6 (aq) + 2 OH- (aq) C4H4O62- (aq) + 2 H2O (l)

H2C4H4O6 (aq) + 2 OH- (aq) C4H4O62+ (aq) + 2 H2O (l)

Explanation / Answer

Balanced net ionic equation is H2C4H4O6 (aq) + 2 OH- (aq) C4H4O62- (aq) + 2 H2O (l) because the tartarate will be anion and not cation.

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