Question

The salts X(NO₃)₂ and Y(NO₃)₂ (where X⁺ and Y⁺ are metal ions) are dissolved in water to create a solution that is 0.1 M in each of them. Using the provided Ksp values below, determine which aqueous reagent, if any, will precipitate X⁺ before precipitating Y⁺ from the solution.

Given Ksp values:

XCl₂, 1x10⁻⁵¹
YCl₂, 1x10⁻¹⁰
X(OH)₂, 1x10⁻¹⁰
Y(OH)₂, 1x10⁻⁵

A) 1 M NH₃
B) 1 M HCl
C) 1 M HNO₃
D) 1 M NaCl
E) None of the above reagents will cause precipitation

Answer 1

To determine if X⁺ or Y⁺ will precipitate first upon adding 1 M HNO₃, we need Ksp values of potential precipitates involving X⁺ and Y⁺, which are not provided. Predicting precipitates requires comparing the ion product with Ksp to see if a precipitate will form.

Step-by-step explanation:

To answer the question of whether adding 1 M HNO₃ to a solution of X(NO₃)₂ and Y(NO₃)₂ will precipitate X⁺ before Y⁺, we must consider the common ion effect and the solubility products (Ksp) of the potential precipitates. However, the information given does not specify the Ksp values of the metal nitrates or any other precipitates that could form from X⁺ and Y⁺ ions. Therefore, without additional information such as the specific metal ions involved or the Ksp values for their possible precipitates, a prediction cannot be made. Hence, with the given data, we cannot determine conclusively which metal ion will precipitate first upon adding 1 M HNO₃.

Predicting precipitates involves comparing the ion product (often written as Q) with the Ksp of the potential precipitate. If the ion product for a particular cation-anion pair exceeds the Ksp, a precipitate will form until the concentrations adjust to reestablish equilibrium where Q equals Ksp. For example, if solutions of AgNO₃ and NaCl are mixed and the reaction quotient Q for AgCl exceeds its Ksp value, AgCl will precipitate.