If Ca(OH)2 completely dissociates in water, the resulting solution will contain Ca2+ and OH- ions. In this case, the concentration of Ca(OH)2 can be represented as 0.02 M, indicating that there are 0.02 moles of Ca(OH)2 dissolved in one liter of water.
The complete dissociation of Ca(OH)2 means that every molecule of Ca(OH)2 breaks apart into one Ca2+ ion and two OH- ions. Therefore, for every mole of Ca(OH)2 that dissolves, two moles of OH- ions are produced. This makes the concentration of OH- ions twice the concentration of Ca(OH)2.
So if we have a 0.02 M solution of Ca(OH)2, the concentration of OH- ions would be 0.04 M because each mole of Ca(OH)2 produces two moles of OH- ions upon dissociation.
Which Description is True of 0.02 M Ca(OH)2 if Ca(OH)2 Completely Dissociates in Water?
When it comes to the dissociation of Ca(OH)2 in water, several factors come into play. Understanding these factors is crucial to comprehending the behavior and properties of this compound when it interacts with water.
One significant factor that affects the dissociation of Ca(OH)2 is temperature. As the temperature increases, the solubility of calcium hydroxide also increases, leading to a higher degree of dissociation. This means that at higher temperatures, more Ca(OH)2 molecules will break apart and release hydroxide ions (OH-) into the solution.
Another important factor is concentration. The concentration of Ca(OH)2 in a water solution determines its ability to dissociate. Higher concentrations result in a greater number of particles available for dissociation, leading to increased dissociation rates. Conversely, lower concentrations may hinder dissociation due to limited availability of particles.
Concentration of Ca(OH)2 in Water Solutions
The concentration of Ca(OH)2 can be expressed using various units such as molarity (M), molality (m), or mass percent (%). These different ways help us understand how much solute is present in a given volume or mass of solvent.
For instance, if we have a 0.02 M (molar) solution of Ca(OH)2, it means there are 0.02 moles of calcium hydroxide dissolved per liter (L) of water. With complete dissociation, all those moles would separate into their respective ions—calcium ions (Ca^2+) and hydroxide ions (OH-).
Extent Of Dissociation Of Ca(OH)2 In Water
The extent or degree to which Ca(OH)2 dissociates in water depends on its solubility and the presence of other ions that may influence the equilibrium. In some cases, Ca(OH)2 may not completely dissociate, leading to a partial dissociation.
Understanding the extent of dissociation is essential for various applications involving Ca(OH)2 solutions, such as in chemistry laboratories or industrial processes. Researchers often conduct experiments and use equilibrium constants to determine the degree of dissociation under specific conditions.
The Solubility of Ca(OH)2 in Water
Let’s delve into the concentration of Ca(OH)2 and explore its solubility in water. When Ca(OH)2 is added to water, it undergoes a dissociation process where it breaks apart into calcium ions (Ca^2+) and hydroxide ions (OH^-). This dissociation is influenced by factors such as temperature, pressure, and the initial concentration of Ca(OH)2.
The solubility of Ca(OH)2 refers to the maximum amount of the compound that can dissolve in a given quantity of water at a specific temperature. It is generally expressed in moles per liter (mol/L), also known as molarity. In this case, we are considering a 0.02 M solution of Ca(OH)2.
To determine if Ca(OH)2 completely dissociates in water, we need to examine its solubility product constant (Ksp). Ksp represents the equilibrium constant for the dissolution reaction and provides insight into how much of the compound will actually dissolve.
In summary, several factors affect the dissociation of Ca(OH)2 in water, including temperature and concentration. Higher temperatures and concentrations generally promote greater dissociation. Additionally, understanding the extent of dissociation plays a crucial role in practical applications where precise control over solution behavior is necessary.
