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ad-work [718]
2 years ago
14

A 50.0 mL sample of 0.10 M potassium nitrate is mixed with 100 mL of 0.25 M magnesium nitrate. What is the final concentration o

f nitrate in the solution
Chemistry
1 answer:
ser-zykov [4K]2 years ago
7 0

The final concentration of nitrate is 0.367 M

<h3>Concentration of a substance</h3>

The concentration of a substance is the amount of substance present in a given volume of a solution of that substance.

Concentration = number of moles/ volume

<h3>Equation for the dissociation of potassium nitrate</h3>

KNO3 ---> K+ + NO3-

1 mole of KNO3 produces 1 mole of nitrate

moles of nitrate in a 0.1 M KNO3 solution

  • moles = concentration × volume

volume of KNO3 = 50.0 mL= 0.05 L

moles of nitrate = 0.1 × 0.05

moles of nitrate in KNO3 = 0.005

<h3>Equation for the dissociation magnesium nitrate</h3>
  • Mg(NO3)2 ---> Mg^2+ + 2 NO3-

1 mole of Mg(NO3)2 produces 2 moles of nitrate ion

moles of Mg(NO3)2 = concentration × volume

volume of solution = 100 mL= 0.1 L

moles of Mg(NO3)2 = 0.1 × 0.25 = 0.025

Moles of nitrate = 0.025 × = 0.05

Total moles of nitrate = 0.05 + 0.005 = 0.055 moles

Total volume of solution = 0.1 + 0.05 = 0.15 L

Concentration of nitrate = 0.055/0.15

Concentration of nitrate = 0.367 M

Therefore, the final concentration of nitrate is 0.367 M

Learn more about concentration and solutions at: brainly.com/question/17206790

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