Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Complete Ionic Equations

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Complete Ionic Equations

Previous problemNext problem

Struggling with General Chemistry?

Join thousands of students who trust us to help them ace their exams!Watch the first video

Multiple Choice

When 100.0 mL of a solution that is 0.00100 M in Cu(NO₃)₂ is mixed with 100 mL of a 0.20 M solution of NH₃, what concentration of When 100.0 mL of a solution that is 0.00100 M in Cu(NO₃)₂ is mixed with 100 mL of a 0.20 M solution of NH₃, what concentration of Cu²⁺ remains in solution? remains in solution?

5.0 × 10⁻⁴M

2.9 × 10⁻¹³M

3.7 × 10⁻¹⁴M

2.9 × 10⁻¹⁶M

Previous problemNext problem

Verified step by step guidance

Determine the initial moles of Cu(NO3)2 and NH3. Use the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). For Cu(NO3)2, \( \text{moles} = 0.00100 \text{ M} \times 0.100 \text{ L} \). For NH3, \( \text{moles} = 0.20 \text{ M} \times 0.100 \text{ L} \).

Write the balanced chemical equation for the reaction between Cu(NO3)2 and NH3. The complex ion formed is \([\text{Cu(NH}_3)_4]^{2+}\). The balanced equation is: \( \text{Cu}^{2+} + 4\text{NH}_3 \rightarrow [\text{Cu(NH}_3)_4]^{2+} \).

Calculate the limiting reactant. Compare the mole ratio from the balanced equation with the initial moles calculated. Since 4 moles of NH3 are required for every mole of Cu2+, determine which reactant is in excess.

Determine the moles of Cu2+ that react completely with NH3. Subtract the moles of Cu2+ that react from the initial moles to find the moles of Cu2+ remaining.

Calculate the concentration of Cu2+ remaining in the solution. Use the formula: \( \text{concentration} = \frac{\text{moles of Cu}^{2+} \text{ remaining}}{\text{total volume of solution}} \). The total volume is the sum of the volumes of the two solutions mixed.