Question

A solution is formed by adding 35g of ammonium nitrate to 250g of water. What is the percent by mass of ammonium nitrate​

Answer 1

Step-by-step explanation:

The percent by mass of ammonium nitrate : 12.28%

Further explanation

The concentration of a substance can be expressed in several quantities such as moles, percent (%) weight / volume,), molarity, molality, parts per million (ppm) or mole fraction. The concentration shows the amount of solute in a unit of the amount of solvent.

So the concentration of a solution can be expressed as a percent which is the ratio of solute to solution. Can be expressed in percent of mass (m / m) or volume percent (v / v)

\rm Percent\:by\:Mass=\dfrac{mass\:of\:solute}{mass\:of\:solution}\times 100PercentbyMass=

massofsolution

massofsolute

×100

\rm Percent\:by\:Volume=\dfrac{volume\:of\:solute}{volume\:of\:solution}\times 100PercentbyVolume=

volumeofsolution

volumeofsolute

×100

Solution = Solute + Solvent

The solute is the substance that is dissolved usually in smaller amounts when compared to solvents

A solution that has a lot of solutes per solvent is described as concentrated, while a solution with a small amount of solute is called dilute.

Adding 35 g of ammonium nitrate(NH₄NO₃), to 250 g of water (H₂O)

solute = ammonium nitrate = 35 g

solvent = water = 250 g

Solution = Solute + Solvent

Solution = 35 + 250 = 285 grams

Then the mass percentage of ammonium nitrate

\begin{gathered}\rm Percent\:mass=\dfrac{mass\:of\:ammonium\:nitrate}{mass\:of\:solution}\times 100\\\\Percent\:mass=\dfrac{35\:grams}{285\:grams}\times 100\\\\Percent\:mass=12.28\%\end{gathered}

Percentmass=

massofsolution

massofammoniumnitrate

×100

Percentmass=

285grams

35grams

×100

Percentmass=12.28%

Answer 2

Given :  A solution is formed by adding 35g of ammonium nitrate to 250g of water.

To Find : The percent by mass of ammonium nitrate

Solution:

Mass of ammonium nitrate = 35 g

Mass of Water = 250 g

Total Mass = 35 + 250 = 285 g

percent by mass of ammonium nitrate  =  (35/ 285) * 100

= (7/57) * 100

= 700/57

≈ 12.281 %

mass of ammonium nitrate is about 12.281 %

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