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andrew-mc [135]

3 years ago

11

A sample of 25.0 mL of 0.120 M Ca(OH)2(aq) is titrated with 0.150 M HCl(aq). What volume of HCl(aq) is needed to completely neut

ralize the Ca(OH)2(aq)

1 answer:

stiv31 [10]3 years ago

3 0

Answer:

$V_{HCl}=48.0 mL$

Explanation:

Hello!

In this case, since the reaction between calcium hydroxide and hydrochloric acid shows a 2:1 mole ratio between them:

$2HCl+Ca(OH)_2\rightarrow CaCl_2+2H_2O$

We need to use the following mole ratio:

$2n_{Ca(OH)_2}=n_{HCl}$

That can be written in volumes and concentrations:

$2M_{Ca(OH)_2}V_{Ca(OH)_2}=M_{HCl}V_{HCl}$

Thus, we solve for the volume of HCl as it is the unknown:

$V_{HCl}=\frac{2M_{Ca(OH)_2}V_{Ca(OH)_2}}{M_{HCl}}$

Therefore, we plug in to obtain:

$V_{HCl}=\frac{2*0.120M*25.0mL}{0.150M} \\\\V_{HCl}=48.0 mL$

Best regards!

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Explanation:

An ionic compound is a compound that is formed by ions, so one of the elements must donate electrons (which is the cation, the positive ion), and the other will receive these electrons (which is the anion, the negative ion).

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%IC = 0.995 %

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$x_{Cl}$ = 3.0

$%IC = (1 - e^{-0.25*(3.0 - 1.2)^2})$ *100%

%IC = 55.5%

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