Question

Question #550c5

Answer 1

The concentration is 0.200 mol/L.

Explanation:

Step 1. Calculate the moles of hydrogen chloride

We can use the Ideal Gas Law to do this:

`color(blue)(bar(ul(|color(white)(a/a)pV = nRTcolor(white)(a/a)|)))" "`

We can rearrange this equation to get

`n = (pV)/(RT)`

In this problem,

`p color(white)(l)= "100 kPa"`
`V = "0.500 L"`
`R = "8.314 kPa·L·K"^"-1""mol"^"-1"`
`T = "300 K"`

∴ `n = (100 color(red)(cancel(color(black)("kPa"))) × 0.500 color(red)(cancel(color(black)("L"))))/(8.314 color(red)(cancel(color(black)("kPa·L·K"^"-1")))"mol"^"-1" × 300 color(red)(cancel(color(black)("K")))) = "0.020 05 mol"`

Step 2. Calculate the concentration of the solution

`c = "0.020 05 mol"/"0.100 L" = "0.200 mol/L"`