g Given that 50.0 mL of 0.100 M magnesium bromide reacts with 13.9 mL of silver nitrate solution according to the unbalanced equation MgBr21aq2 AgNO31aq2 S AgBr1s2 Mg1NO3221aq2 (a) What is the molarity of the AgNO3 solution

0.719M AgNO₃

Explanation:

The balanced chemical equation is:

MgBr₂ + 2AgNO₃ ⇄ 2AgBr + Mg(NO₃)₂

Where 1 mole of magnesium bromide reacts completely with 2 moles of AgNO₃

Molarity is the ratio between moles of solution and its volume in liters (The volume of the solution is 13.9mL = 0.0139L). That means all we need is to determine moles of silver nitrate. It is possible to know by using the chemical equation, thus:

Moles AgNO₃:

Moles of MgBr₂:

50.0mL = 0.050L * (0.100mol / L) = 0.00500 moles of MgBr₂.

As 2 moles of AgNO₃ reacts per mole of  MgBr₂ and the reaction occurs completely, moles of silver nitrate are:

0.00500 moles MgBr₂ * (2 moles AgNO₃ / 1 mole MgBr₂) =

And molarity is:  

0.0100 moles AgNO₃ / 0.0139L =

answer; i believe the correct answer is (solid gold);