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How many grams of nicl2∙6h2o will be used to prepare a 0. 0350 m, 500. 0 ml of nicl2 solution?

Sagot :

Eduard22sly

The mass of NiCl₂•6HO₂ needed to prepare a 0.035 M 500 mL solution of NiCl₂•6HO₂ is 4.165 g

What is molarity?

This is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:

Molarity = mole / Volume

How to determine the mole of NiCl₂•6HO₂

  • Molarity = 0.035 M
  • Volume = 500 mL = 500 / 1000 = 0.5 L
  • Mole of NiCl₂•6HO₂ =?

Mole = Molarity × Volume

Mole of NiCl₂•6HO₂ = 0.035 × 0.5

Mole of NiCl₂•6HO₂ = 0.0175 mole

How to determine the mass of NiCl₂•6HO₂

  • Mole of NiCl₂•6HO₂ = 0.0175 mole
  • Molar mass of NiCl₂•6HO₂ = 238 g/mol
  • Mass of NiCl₂•6HO₂ =?

Mass = mole × molar mass

Mass of NiCl₂•6HO₂ = 0.0175 × 238

Mass of NiCl₂•6HO₂ = 4.165 g

Thus, 4.165 g of NiCl₂•6HO₂ is needed to prepare the solution

Learn more about molarity:

https://brainly.com/question/15370276

The grams of NiCl₂.6H₂O will be used to prepare a 0.0350M, 500ml of NiCl₂ solution is 2.268 grams.

How do we calculate grams from moles?

Mass in grams of any substance will be calculated by using moles as:

n = W/M, where

W = given mass

M = molar mass

Moles from molarity will be calculated by using the below formula:

M = n/V, where

M = molarity of NiCl₂ solution = 0.0350M

V = volume of solution = 500mL = 0.5L

On putting values, we get

n = (0.035)(0.5) = 0.0175 mol

Now we convert these moles into grams by using the first formula as:
W = (0.0175mol)(129.6g/mol) = 2.268g

Hence required mass of NiCl₂.6H₂O is 2.268g.

To know more about moles & mass, visit the below link:
https://brainly.com/question/15374113

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