The molarity of the stock Mn²⁺ ions is 0.0288 M
Based on the dilution formula;
- The molarity of A is 0.00144 M
- The molarity of B is 0.0000576 M
- The molarity of C is 0.000001152 M
<h3>What is the molarity of a solution?</h3>
The molarity of a solution is the number of moles of a solute dissolved in a given volume of solution in liters.
- Molarity = number of moles/volume
The molarity of the stock solution is:
moles of Mn²⁺ ions = mass / molar mass
molar mass of Mn²⁺ ions = 55.0 g/mol
moles of Mn²⁺ ions = 1.584 / 55
moles of Mn²⁺ ions = 0.0288 moles
molarity of Mn²⁺ ions = 0.0288 / 1
molarity of Mn²⁺ ions = 0.0288 M
The dilution formula is used to determine the molarities of A, B, and C.
C₁V₁ = C₂V₂
C₂ = C₁V₁ / V₂
Where;
- C₁ = initial molarity
- V₁ = initial volume
- C₂ = final molarity
- V₂ = final volume
Molarity of A = 50 * 0.0288 / 1000
Molarity of A = 0.00144 M
Molarity of B = 10 * 0.00144 / 250
Molarity of B = 0.0000576 M
Molarity of C = 10 * 0.0000576 / 500
Molarity of C = 0.000001152 M
Learn more about molarity at: brainly.com/question/17138838
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