Chemistry, asked by kalpeshg791, 11 months ago

25 ml of hcl librates 10 ml of CO2 at ntp when reacting with excess of caco3 the normality of hcl be

Answers

Answered by Anonymous
0

Answer:

(ii) Volume strength of H O = 5.6 x Normality of H O ... The molarity of a solution obtained by mixing 750 mL of 0.5 M HCl and 250 ... treating 25 g of this sample with excess of dil HCI.

Answered by Abhijeet1589
0

The Normality Of HCl Is 0.03 N

GIVEN

The volume of HCl = 25 ml

the volume of CO₂ formed = 10 ml

TO FIND

Normality of HCl

SOLUTION

We can solve the above problem as follows -

We know that,

Normality = Molarity × n-factor

Where,

n-factor = number of replaceable hydrogen ions ( in case of an acid)

To find the normality of HCl, let us first write the chemical formula and find the molarity of HCl.

CaCO₃ + 2HCl ------------> CaCl₂ + CO₂ + H₂O

The volume of Carbon dioxide gas formed = 10 ml at Ntp

10 mL = 0.01L

we know,

1 mole of gas occupies 22.4 L at Ntp

so,

0.01L =  \frac{1}{22.4}  \times 0.01 = 4.4 \times  {10}^{ - 4} moles

Now, From the above reaction, we can say that -

Moles of HCl = 2 × moles of CO₂

so,

Moles of HCl = 2× 4.4×10⁻⁴ = 8.8 × 10⁻⁴ moles.

Molarity = Moles of solute /volume of solute in 1 liter

Therefore,

Molarity  \: of  \: HCl =  \frac{8.8 \times  {10}^{ - 4} \times  {10}^{3}  }{25}

= 0.03 M

Now,

We know that the n-factor of HCl is 1

So, Normality = Molarity = 0.03

Hence, the Normality of HCl is 0.03 N

#spj2

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