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

Solution Stoichiometry

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Solution Stoichiometry

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Multiple Choice

You mix a 125.0-mL sample of a solution that is 0.0117 M in NiCl₂ with a 175.0-mL sample of a solution that is 0.250 M in NH₃. After the solution reaches equilibrium, what concentration of Ni²⁺(aq) remains?

0.0058 M

0.0000 M

0.0029 M

0.0117 M

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Verified step by step guidance

First, calculate the initial moles of NiCl₂ in the 125.0 mL solution. Use the formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert 125.0 mL to liters by dividing by 1000.

Next, calculate the initial moles of NH₃ in the 175.0 mL solution using the same formula: \( \text{moles} = \text{volume (L)} \times \text{molarity (M)} \). Convert 175.0 mL to liters by dividing by 1000.

Write the balanced chemical equation for the reaction between Ni²⁺ and NH₃ to form the complex ion \([\text{Ni(NH}_3)_6]^{2+}\). This will help you understand the stoichiometry of the reaction.

Determine the limiting reactant by comparing the mole ratio of Ni²⁺ to NH₃ based on the balanced equation. The limiting reactant will be completely consumed, and the excess reactant will determine the equilibrium concentration.

Calculate the concentration of Ni²⁺ remaining at equilibrium. Subtract the moles of Ni²⁺ that reacted from the initial moles, then divide by the total volume of the mixed solution (125.0 mL + 175.0 mL converted to liters) to find the concentration.