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2.24 m of hydrogen chloride gas is dissolved at STP in a quantity of water until the volume of the solution becomes 500 ml. What volume of hydrochloric acid is required to titrate 20 ml of 0.2 m calcium hydroxide?
Accepted Answer
Here's how to solve the problem:
1. Calculate the moles of calcium hydroxide:
20 mL of 0.2 M Ca(OH)₂ = 0.02 L
0.2 mol/L = 0.004 moles Ca(OH)₂
2. Calculate the moles of HCl needed:
The balanced chemical equation for the reaction is:
2HCl(aq) + Ca(OH)₂(aq) → CaCl₂(aq) + 2H₂O(l)
The stoichiometry shows that 2 moles of HCl are needed for every 1 mole of Ca(OH)₂.
So, 0.004 moles Ca(OH)₂
(2 moles HCl / 1 mole Ca(OH)₂) = 0.008 moles HCl
3. Calculate the volume of HCl solution:
Let 'x' be the volume of HCl solution needed in liters.
The concentration of the HCl solution is given as 2.24 M.
Therefore, x
2.24 mol/L = 0.008 moles HCl
x = 0.008 moles / 2.24 mol/L = 0.00357 L
Convert to milliliters: 0.00357 L
1000 mL/L = 3.57 mL
Therefore, 3.57 mL of the 2.24 M hydrochloric acid solution is required to titrate 20 mL of 0.2 M calcium hydroxide.
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