I need help calcuating the normailty of acetic acid(vinegar) for the two tritati

Question

I need help calcuating the normailty of acetic acid(vinegar) for the two tritations columns of 17.00ml and 34.80ml. Then, average the values. Also calculate the mass percent of acetic acid present using my average normality assuming the density of acetic acid solution is 1.01g/ml. The base of this titration is the NaOH the acid is the H2SO4. During the expiriment we are not given the concentration so im having a hard time figuring out the normality on acetic acid. Please show steps on how to solve.

Explanation / Answer

Let us be first clear about Normality which is an equivalent term of Molarity.

Normality Normality (equivalents per liter of solution, eq./L) is convenient for measuring volumes of different solutions containing amounts of solute necessary to react completely with each other. One equivalent of acid is the amount of acid that can supply 1 mol of H+ . One mole of HCl equals one equivalent of HCl, 1mol H3PO4 = 3 equivalents because there are 3 moles H+ ions in each mole of H3PO4. For example, if we mix 1 liter of 1.0 N NaOH with 1 liter of 1.0 N H2SO4, we shall have added the proper amounts of acid and base to neutralize each other completely even though sulfuric acid has two hydrogen atoms per molecule. This follows from the fact that in the neutralization reaction, H+ ions react with OH- ions in a 1:1 ratio to form water. H+ + OH- ? H2O

Calculations for Titration of Vinegar NA = normality of the acid (for acetic acid N = M) VA = volume of the acid (usually mL, in this lab, it

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