If 20.0mL of 0.122M NaOH are required to reach the first equivalent point of a solution of citric acid(tripotic acid H3C6H5O7).How many mL of NaOH in total are required to reach the second equivalence point?

Really this is analytical chemistry. It will take twice as much to reach the second as it did to reach the first.

it will double

To determine the number of mL of NaOH required to reach the second equivalence point, we need to understand the reaction between citric acid (H3C6H5O7) and NaOH.

Citric acid is a triprotic acid, meaning it can donate three protons (H+ ions) per molecule. NaOH, on the other hand, is a strong base that can accept one proton (OH- ion) per molecule.

The balanced chemical equation for the reaction between citric acid and NaOH is as follows:

H3C6H5O7 + 3NaOH → 3H2O + Na3C6H5O7

From the equation, we see that for every molecule of citric acid, three molecules of NaOH are required to reach the second equivalence point. This implies that the ratio of moles of NaOH to citric acid is 3:1.

So, to find out the number of moles of NaOH required to reach the second equivalence point, we can use the following equation:

moles of NaOH = moles of citric acid x 3

To determine the moles of citric acid initially reacted in the first equivalent point, we use the formula:

moles of citric acid = volume of citric acid (in L) x concentration of citric acid (in mol/L)

Given that 20.0 mL (0.020 L) of 0.122 M NaOH is required to reach the first equivalence point, we assume that the volume of citric acid is also 0.020 L.

Now we can calculate the moles of citric acid initially reacted:

moles of citric acid = 0.020 L x 0.122 mol/L
= 0.00244 mol

Next, we can calculate the moles of NaOH required to reach the second equivalence point:

moles of NaOH = 0.00244 mol x 3
= 0.00732 mol

Finally, we can determine the volume of NaOH required:

volume of NaOH = moles of NaOH / concentration of NaOH

Let's assume the concentration of NaOH is also 0.122 M (not provided in the question). Then:

volume of NaOH = 0.00732 mol / 0.122 mol/L
= 0.0599 L

Converting this to mL:

volume of NaOH = 0.0599 L x 1000 mL/L
= 59.9 mL

Therefore, approximately 59.9 mL of NaOH are required to reach the second equivalence point in this solution.