The mass of NiCl₂•6HO₂ needed to prepare a 0.035 M 500 mL solution of NiCl₂•6HO₂ is 4.165 g
This is defined as the mole of solute per unit litre of solution. Mathematically, it can be expressed as:
Molarity = mole / Volume
Mole = Molarity × Volume
Mole of NiCl₂•6HO₂ = 0.035 × 0.5
Mole of NiCl₂•6HO₂ = 0.0175 mole
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
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The grams of NiCl₂.6H₂O will be used to prepare a 0.0350M, 500ml of NiCl₂ solution is 2.268 grams.
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.
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