If it takes 17.8 mL of 0.0126 M Ca(OH)2 to reach the end point of a titration to

Question

If it takes 17.8 mL of 0.0126 M Ca(OH)2 to reach the end point of a titration to neutralize 25.0 mL of hydrochloric acid solution, what was the concentration of the hydrochloric acid solution? The chemical equation is started for you below.
A). 0.0252 M HCl B). 0.00561 M HCl C). 0.0157 M HCl D). 0.0179 M HCl E). 0.00897 M HCl
can you please work this out for me? If it takes 17.8 mL of 0.0126 M Ca(OH)2 to reach the end point of a titration to neutralize 25.0 mL of hydrochloric acid solution, what was the concentration of the hydrochloric acid solution? The chemical equation is started for you below.
A). 0.0252 M HCl B). 0.00561 M HCl C). 0.0157 M HCl D). 0.0179 M HCl E). 0.00897 M HCl
can you please work this out for me?
A). 0.0252 M HCl B). 0.00561 M HCl C). 0.0157 M HCl D). 0.0179 M HCl E). 0.00897 M HCl
can you please work this out for me?

Explanation / Answer

V1 = 17.8 ml

M1 = 0.0126 M of Ca(OH)2

V2 = 25

M2 = ?

find equation

Ca(OH)2 + 2HCl = 2H2O + CaCl2

then, ratio is 1:2

mol of base = MV = 17.8*0.0126 = 0.22428 mmol of base

then we need twice of that

mmol of acid = 2*0.22428 = 0.44856 mmol of acid

then

[Hcl] = mmol/ml = 0.44856/(25) = 0.0179424

D). 0.0179 M HCl

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