a) Silver iodide(s) is formed by the following reaction:

Ag (aq) + I (aq) --> AgI (s)

The Ksp for AgI = 1.8 x 10^-10

Describe, using the chemical reaction, the mathematical formula for
these ions. Assuming these ion concentrations are equal, what would the molarity be for each ion?


b) Ca3(PO4)2 (s) is a chemical found in bones. If the solution used to preserve these bones contains 10^-5 M Ca^2+ and 10^-6 M PO4(^3-) would the bones soften and dissolve over time? Explain your answer

a) The chemical reaction can be represented by the equation:

Ag(aq) + I(aq) ⟶ AgI(s)

Here, Ag(aq) represents the silver ion in aqueous solution, and I(aq) represents the iodide ion in aqueous solution. AgI(s) represents the silver iodide precipitate that is formed.

The mathematical formula for the ion concentrations can be represented as:

[Ag⁺] = [I⁻]

This equation represents the assumption that the ion concentrations for both silver and iodide ions are equal.

Given that the Ksp for AgI is 1.8 x 10^-10, we can use this information to determine the molarity (concentration) for each ion.

Ksp = [Ag⁺][I⁻]

Since [Ag⁺] = [I⁻], we can represent this as [Ag⁺]² = 1.8 x 10^-10.

Taking the square root of both sides, we get:
[Ag⁺] = √(1.8 x 10^-10)

Using a calculator, we find that [Ag⁺] ≈ 1.34 x 10^-5 M.
Similarly, [I⁻] will also be approximately 1.34 x 10^-5 M.

b) In order to determine if the bones would soften and dissolve over time, we need to consider whether the reaction is at equilibrium or not.

The solubility product constant (Ksp) for Ca3(PO4)2 is not given, but for simplicity, let's assume the reaction can be represented as:

Ca3(PO4)2(s) ⟶ 3Ca^2+(aq) + 2PO4^3-(aq)

The mathematical formula for this reaction would be [Ca^2+]^3[PO4^3-]^2.

Given that the solution contains 10^-5 M Ca^2+ and 10^-6 M PO4^3-, we can substitute these values into the formula:

[Ca^2+]^3[PO4^3-]^2 = (10^-5)^3 * (10^-6)^2

Simplifying, we get: [Ca^2+]^3[PO4^3-]^2 = 10^-15.

Since this value is significantly smaller than the Ksp value (which we assume is much larger), the reaction is not at equilibrium. This means that the solution is not saturated with respect to Ca3(PO4)2.

Therefore, the bones would not soften and dissolve over time as there is no excess of Ca^2+ and PO4^3- ions available for the reaction to occur. The existing ions would likely remain in solution or form a thin layer of precipitate on the bone surface, but the bones themselves would not dissolve significantly.

a) The chemical reaction provided is:

Ag(aq) + I(aq) → AgI(s)

From this reaction, we can determine the mathematical formula for these ions:

Ag(aq) indicates silver ions (Ag+)
I(aq) represents iodide ions (I-)
AgI(s) denotes silver iodide (AgI)

Assuming the ion concentrations are equal, let's denote the molarity as x for each ion:

Ag+ concentration = x M
I- concentration = x M

Using the given Ksp value for AgI, we can write the expression for the solubility product:

Ksp = [Ag+][I-] = 1.8 x 10^-10

Substituting the concentrations, we get:

( x )( x ) = 1.8 x 10^-10
x^2 = 1.8 x 10^-10

To solve for x, we take the square root of both sides:

x = √(1.8 x 10^-10)

This gives the molar concentration for each ion.