At 40^∘ C, the density of heavy water is 1.02 g / ml and its ionic product is 5.1 ×10^-15. Whic

step 1 In this question we have D2OA is equal to D by M that is equal to 1 .0 2 into 10 0 to the power

At 40^∘ C, the density of heavy water is 1.02 g / ml and...

At $40^{\circ} \mathrm{C}$, the density of heavy water is $1.02 \mathrm{~g} / \mathrm{ml}$ and its ionic product is $5.1$ $\times 10^{-15}$. Which of the following if the only incorrect information regarding heavy water at $40^{\circ} \mathrm{C}$ ? (a) The molar concentration of heavy water is $51 \mathrm{M}$. (b) The dissociation constant of heavy water is $10^{-16}$. (c) Its degree of dissociation is $10^{-8}$. (d) The molal concentration of heavy water is $50 \mathrm{~m}$.

At $40^{\circ} \mathrm{C}$, the density of heavy water is $1.02 \mathrm{~g} / \mathrm{ml}$ and its ionic product is $5.1$ $\times 10^{-15}$. Which of the following if the only incorrect information regarding heavy water at $40^{\circ} \mathrm{C}$ ?
(a) The molar concentration of heavy water is $51 \mathrm{M}$.
(b) The dissociation constant of heavy water is $10^{-16}$.
(c) Its degree of dissociation is $10^{-8}$.
(d) The molal concentration of heavy water is $50 \mathrm{~m}$.

Key Concepts

Density and its Role in Concentration Calculations

Density is a key property of a substance that is used to convert between mass and volume. In the context of solution chemistry, knowing the density of a solvent such as heavy water allows chemists to relate its mass-based measurements (like molality, which requires the mass of the solvent) to volume-based measurements (like molarity, which requires the volume of the solution).

Molar Concentration vs Molality

Molar concentration (molarity) and molal concentration (molality) are two ways of expressing the amount of a substance in a solution. Molarity is defined as moles of solute per liter of solution, while molality is defined as moles of solute per kilogram of solvent. Their use depends on the physical properties measured, and understanding their differences is crucial for accurate descriptions of solution behavior under varying conditions such as temperature.

Ionic Product (Self-Ionization Constant) of a Solvent

The ionic product, also known as the self-ionization constant, is a measure of the extent to which a solvent dissociates into its ions. For water, this is often represented by Kw. In heavy water, the ionic product may differ significantly from that of regular water, thus affecting properties like the dissociation constant and degree of dissociation. This concept is essential for understanding the equilibrium between the undissociated form of the solvent and its constituent ions.

Dissociation Constant and Degree of Dissociation

The dissociation constant reflects the equilibrium established when a solvent self-ionizes, while the degree of dissociation is the fraction of molecules that actually dissociate into ions. These concepts are closely related, as the dissociation constant depends on the extent of ionization in the solvent. They are critical for analyzing the acidity, basicity, and overall ionic behavior of solvents, influencing calculations involving ion concentrations and pH.

Transcript

Please give Ace some feedback