QuestionVilken är al $\left[\mathrm{Cu}^{2+}\right]$ , b) $\left[\mathrm{NO}_{3}^{-}\right]$ i en lösning med koncentrationen $0,15 \mathrm{~mol} / \mathrm{dm}^{3} \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}$ ?

Studdy Solution

STEP 1

1. The compound $\mathrm{Cu(NO}_3\mathrm{)}_2$ dissociates completely in solution.
2. The concentration of $\mathrm{Cu(NO}_3\mathrm{)}_2$ is $0.15 \, \mathrm{mol/dm}^3$ .
3. We need to find the concentrations of $\mathrm{Cu}^{2+}$ and $\mathrm{NO}_3^{-}$ .

STEP 2

1. Write the dissociation equation for $\mathrm{Cu(NO}_3\mathrm{)}_2$ .
2. Determine the concentration of $\mathrm{Cu}^{2+}$ .
3. Determine the concentration of $\mathrm{NO}_3^{-}$ .

STEP 3

Write the dissociation equation for $\mathrm{Cu(NO}_3\mathrm{)}_2$ :
$\mathrm{Cu(NO}_3\mathrm{)}_2 \rightarrow \mathrm{Cu}^{2+} + 2\mathrm{NO}_3^{-}$

STEP 4

From the dissociation equation, we see that one mole of $\mathrm{Cu(NO}_3\mathrm{)}_2$ produces one mole of $\mathrm{Cu}^{2+}$ .
Therefore, the concentration of $\mathrm{Cu}^{2+}$ is the same as the concentration of $\mathrm{Cu(NO}_3\mathrm{)}_2$ :
$[\mathrm{Cu}^{2+}] = 0.15 \, \mathrm{mol/dm}^3$

STEP 5

From the dissociation equation, we see that one mole of $\mathrm{Cu(NO}_3\mathrm{)}_2$ produces two moles of $\mathrm{NO}_3^{-}$ .
Therefore, the concentration of $\mathrm{NO}_3^{-}$ is twice the concentration of $\mathrm{Cu(NO}_3\mathrm{)}_2$ :
$[\mathrm{NO}_3^{-}] = 2 \times 0.15 \, \mathrm{mol/dm}^3 = 0.30 \, \mathrm{mol/dm}^3$
The concentrations are:
a) $[\mathrm{Cu}^{2+}] = 0.15 \, \mathrm{mol/dm}^3$
b) $[\mathrm{NO}_3^{-}] = 0.30 \, \mathrm{mol/dm}^3$

Was this helpful?

Get Studdy

Scan QR code with your device to get Studdy on iOS or Android

QR code

Studdy solves anything!

Download the app

Start learning now

Download Studdy AI Tutor now. Learn with ease and get all help you need to be successful at school.

Parents Influencer program Contact Policy Terms