Question

How many mL of a 1.48 M calcium hydroxide solution are needed to neutralize 36.0 mL of a 1.63 M hydrochloric acid solution

Answer 1

The volume (in mL) of calcium hydroxide, Ca(OH)₂ needed for the reaction is 19.8 mL

Balanced equation

2HCl + Ca(OH)₂ —> CaCl₂ + 2H₂O

From the balanced equation above,

• The mole ratio of the acid, HCl (nA) = 2
• The mole ratio of the base, Ca(OH)₂ (nB) = 1

How to determine the volume of Ca(OH)₂

• Molarity of base, Ca(OH)₂ (Mb) = 1.48 M
• Volume of acid, HCl (Va) = 36 mL
• Molarity of acid, HCl (Ma) = 1.63 M
• Volume of base, Ca(OH)₂ (Vb) =?

MaVa / MbVb = nA / nB

(1.63 × 36) / (1.48 × Vb) = 2

58.68 / (1.48 × Vb) = 2

Cross multiply

2 × 1.48 × Vb = 58.68

2.96 × Vb = 58.68

Divide both side by 2.96

Vb = 58.68 / 2.96

Vb = 19.8 mL

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