Chapter 4: Problem 86
What volume of a \(0.500 \mathrm{M} \mathrm{HCl}\) solution is needed to neutralize each of the following: a) \(10.0 \mathrm{~mL}\) of a \(0.300 \mathrm{M} \mathrm{NaOH}\) solution b) \(10.0 \mathrm{~mL}\) of a \(0.200 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) solution
Short Answer
Step by step solution
Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Molarity Calculations
To calculate molarity, use the formula:
- Molarity (M) = moles of solute / liters of solution
For instance, if you have a 0.300 M NaOH solution and need to find the moles of NaOH in a given volume, you convert the volume to liters (10.0 mL to 0.0100 L) and multiply by the molarity:
- Moles of NaOH = 0.300 M × 0.0100 L = 0.00300 moles
Stoichiometry
Stoichiometry relies heavily on the balanced chemical equation, which shows the proportion of reactants to products. For example, in the reaction between HCl and NaOH:
- HCl + NaOH → NaCl + H₂O
Conversely, in the reaction between HCl and Ba(OH)₂:
- 2 HCl + Ba(OH)₂ → BaCl₂ + 2 H₂O
Acid-Base Reactions
During an acid-base reaction:
- An acid donates hydrogen ions (H⁺).
- A base accepts hydrogen ions.
The process of neutralization is complete when the acid and base have reacted in stoichiometric proportions, such that no excess of either reactant remains. Mastering this concept is essential to understanding broader chemical processes and interactions.
Solution Chemistry
A solution is a homogeneous mixture, which means that its composition is uniform throughout. It consists of a solute, the substance that is dissolved, and a solvent, the substance in which the solute is dissolved. In many cases, water is the solvent, making the solution aqueous.
Key points in solution chemistry include:
- Concentration: How much solute is present in a given quantity of solvent.
- Solubility: The maximum amount of solute that can dissolve in a particular solvent at a given temperature.