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

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

General Chemistry

18. Aqueous Equilibrium

Solubility Product Constant: Ksp

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Multiple Choice

A 120.0 mL sample of a solution that is 2.8 × 10^-3 M AgNO3 is mixed with 225.0 mL of a solution that is 0.10 M in NaCN. After the solution reaches equilibrium, what concentration of Ag+ remains?

2.8 × 10^-3 M

1.2 × 10^-4 M

0 M

5.6 × 10^-3 M

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Verified step by step guidance

First, calculate the initial moles of AgNO3 in the 120.0 mL solution. Use the formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Convert the volume from mL to L by dividing by 1000.

Next, calculate the initial moles of NaCN in the 225.0 mL solution using the same formula: \( \text{moles} = \text{concentration} \times \text{volume} \). Again, convert the volume from mL to L.

Write the balanced chemical equation for the reaction between AgNO3 and NaCN. The reaction is: \( \text{Ag}^+ + \text{CN}^- \rightarrow \text{Ag(CN)}_2^- \). This shows that Ag+ ions react with CN- ions to form a complex ion.

Determine the limiting reactant by comparing the initial moles of Ag+ and CN-. Since the reaction consumes Ag+ and CN- in a 1:1 ratio, the reactant with fewer moles will be the limiting reactant.

Calculate the concentration of Ag+ remaining after the reaction reaches equilibrium. Since Ag+ is the limiting reactant and reacts completely, the concentration of Ag+ will be zero.