Balance the chemical equation given below,and determine the number of milliliters of 0.00300 M phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide. _____ Ca(OH)₂(aq)+ _____ H₃PO₄(aq)→ _____ Ca₃(PO₄)₂(aq)+ _____ H₂O(l)

Question

Quizplus · Accepted Answer

The balanced chemical equation is:

3 Ca(OH)2(aq) + 2 H3PO4(aq) → Ca3(PO4)2(s) + 6 H2O(l)

According to the equation, 3 moles of calcium hydroxide react with 2 moles of phosphoric acid. Therefore, the number of moles of phosphoric acid required to neutralize 35.00 mL of 0.00150 M calcium hydroxide is:

(35.00 mL) x (0.00150 mol/L) = 0.0525 mmol Ca(OH)2

(0.0525 mmol Ca(OH)2) x (2 mmol H3PO4/3 mmol Ca(OH)2) = 0.0350 mmol H3PO4

To calculate the volume of 0.00300 M phosphoric acid required to provide 0.0350 mmol H3PO4, we can use the equation:

Molarity = moles of solute / volume of solution (in L)

Volume of solution (in L) = moles of solute / molarity

Volume of solution (in L) = 0.0350 mmol / (0.00300 mol/L) = 11.7 mL

Therefore, the answer is B, 11.7 mL.

Balance the Chemical Equation Given Below,and Determine the Number of Milliliters