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Genrish500 [490]
3 years ago
6

Explain the process of preparation of bleaching powder and mention any

Chemistry
2 answers:
Serhud [2]3 years ago
5 0

Answer:

  • Bleaching powder is produced by the action of chlorine  on dry slaked lime.[Ca(OH)2].
  • Ca(OH)2 + Cl2 gives CaOCl2 + H20

Explanation:

<u>Uses:-</u>

  • It is used an oxidising agent in  many chemical industries.
  • It is used for disinfecting drinking water to make it free of germs.
  • It is also used bleaching cotton and linen in the textile industry.

Hope this helps!

Pls don't forget to rate or give brainliest answer!!

grandymaker [24]3 years ago
4 0

Answer:Bleaching powder is synthesized by the action of chlorine gas (produced from the chlor-alkali process) on dry slaked lime (Ca(OH)2).

Ca(OH)2 + Cl2 → CaOCl2 + H2O

Explanation:

   Bleaching powder is a pale yellowish powder existing with a strong smell of chlorine.

   It is soluble in water but due to the presence of impurities, we never observe a clear solution.

   Its chemical formula is CaOCl2 with its chemical name as Calcium hypochlorite.

Calcium hypochlorite

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Answer:

2.1 moles of water formed.

Explanation:

Given data:

Moles of water formed = ?

Moles of Ni(OH) = 4.20 mol

Solution:

Chemical equation:

2Ni(OH)    →  Ni₂O + H₂O

Now we will compare the moles of Ni(OH)  with water.

             Ni(OH)           :            H₂O

                2                 :              1

              4.20             :            1/2×4.20 = 2.1 mol

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If a volume of gas 177.6mL was collected at a temperature of 25.8C and the pressure is 799.7 torr, what is the original concentr
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Answer:

The original concentration of the acid was 0.605 M

Explanation:

Step 1: Data given

Volume of gas = 177.6 mL = 0.1176 L

Temperature = 25.8 °C = 298.95 K

Pressure = 799.7 torr = 799.7/ 760 = 1.0522368 atm

Volume of acid needed to react = 12.6 mL = 0.0126 L

Step 2: Calculate moles

p*V = n*R*T

n = (p*V)/(R*T)

⇒with n = the number of moles = TO BE DETERMINED

⇒with p = the pressure of the gas = 799.7 torr = 1.0522368 atm

⇒with V = the volume of the gas = 177.6 mL = 0.1776 L

⇒with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 25.8 °C = 298.95 K

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Step 3: Calculate original concentration

We need 0.007618 moles of acid to react with the same amount of moles gas

Concentration acid = moles / volume

Concentration acid = 0.007618 moles / 0.0126 L

Concentration acid = 0.605 M

The original concentration of the acid was 0.605 M

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