what is the molarity of a solution made by dissolving 18.9 g of ammonium nitrate in enough water to make 855…

what is the molarity of a solution made by dissolving 18.9 g of ammonium nitrate in enough water to make 855 ml of solution?\nnh₄no₃: 80.06 g/mol\n? $\frac{mol}{l}$

what is the molarity of a solution made by dissolving 18.9 g of ammonium nitrate in enough water to make 855 ml of solution?\nnh₄no₃: 80.06 g/mol\n? $\frac{mol}{l}$

Answer

Explanation:

Step1: Calculate moles of ammonium nitrate

$n=\frac{m}{M}$, where $m = 18.9\ g$ and $M=80.06\ g/mol$. So $n=\frac{18.9\ g}{80.06\ g/mol}\approx0.236\ mol$.

Step2: Convert volume to liters

$V = 855\ mL=855\times10^{- 3}\ L = 0.855\ L$.

Step3: Calculate molarity

$Molarity=\frac{n}{V}$, substituting $n = 0.236\ mol$ and $V = 0.855\ L$, we get $M=\frac{0.236\ mol}{0.855\ L}\approx0.276\ mol/L$.

Answer:

$0.276$