A 0.00100 mol sample of Ca(OH)2 requires 25.00 mL of aqueous HCl
for neutralization according to the reaction below. What is the
concentration of the HCl?
Equation: Ca(OH)2(s)
+ 2HCl(aq) → CaCl2(aq) + H2O(l)
As per the equation 1 mole of Ca(OH)2 requires 2 moles of HCl
It is given that there are 0.001 moles of Ca(OH)2 in the sample. Therefore, this will require 2* 0.001 = 0.002 moles of HCl
Concentration is given as Molarity = moles of HCl/volume of HCl = 0.002 moles/0.025 L = 0.08M
A 0.00100 mol sample of Ca(OH)2 requires 25.00 mL of aqueous HCl for neutralization according to...
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An aqueous solution of Ca(OH)2with a concentration of 0.161 M was used to titrate 25.00 mL of aqueous HCl. 18.63 mL of the Ca(OH)2was required to reach the endpoint of the titration. Part 1 (1 point) How many moles of base were required to react completely with the acid in this reaction? x 10 mol Ca(OH)2 -- Part 2 (1 point) How many moles of HCl were present in the original 25.00 mL of acid? x 10 mol HCl +...
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