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

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

You have a beaker holding 25.0 mL of 1.5 M HCl. You then add 10.0 mL of 2.0 M NaOH to the beaker. What is the pH of the solution after the addition of the NaOH?

7.00

12.00

2.00

1.00

Previous problemNext problem

Verified step by step guidance

Calculate the moles of HCl initially present using the formula: \( \text{moles of HCl} = Molarity \times Volume \). Convert the volume from mL to L by dividing by 1000.

Calculate the moles of NaOH added using the formula: \( \text{moles of NaOH} = Molarity \times Volume \). Again, convert the volume from mL to L.

Determine the limiting reactant by comparing the moles of HCl and NaOH. Since HCl and NaOH react in a 1:1 ratio, the reactant with fewer moles is the limiting reactant.

Calculate the moles of HCl or NaOH remaining after the reaction. Subtract the moles of the limiting reactant from the moles of the other reactant.

Determine the pH of the solution. If HCl is in excess, calculate the concentration of \( \text{H}^+ \) ions and use \( \text{pH} = -\log[\text{H}^+] \). If NaOH is in excess, calculate the concentration of \( \text{OH}^- \) ions, find the pOH using \( \text{pOH} = -\log[\text{OH}^-] \), and then find the pH using \( \text{pH} = 14 - \text{pOH} \).