Question

The following is the reaction showing the complete neutralization of calcium hydroxide (a base) with phosphoric acid:

3Ca(OH)2​(aq) + 2H3​PO4​(aq) → Ca3​(PO4​)2​(s) + 6H2​O(ℓ)

A stock solution of calcium hydroxide (base) is made by dissolving 3.51 grams of it into some water and the volume is brought to 750 mL. A 50.0 mL portion of that stock solution is then titrated with a solution of 0.229 M phosphoric acid. How many milliliters (mL) of the acid are needed to completely neutralize the base in this reaction? (tolerance is ±0.1 mL)

Answer 1

9.17 milliliters (mL) of the acid are needed to completely neutralize the base in this reaction.

What is a neutralization reaction

A neutralization reaction is a reaction between an acid and a base to produce a salt and water only.

The process of reacting given volume of acids or bases to determine the concentration or volume of either the acid or base required for neutralization is known as titration in volumetric analysis.

The formula to determine the volume of the acid required is given below:

$\frac{C_{a}V_{a}}{C_{b}V_{b}} = \frac {N_{a}}{N_{b}}$

where $V_{a$ is the volume of acid required

$V_{a} = \frac {C_{b}V_{b}N_{a}}{C_{a}N_{b}}$

Concentration of base, Cb = (3.51/74)/0.75 = 0.063 M

Vb = 50. 0 mL

Ca = 0.229 M

Na = 2

Nb = 3

Va = (0.063 * 50 * 2)/(0.229 * 3)

Va = 9.17 mL

In conclusion, the volume of the acid is determined from the concentration, volume and mole ratio of the reaction.

Learn more about titration at: https://brainly.com/question/186765

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