What is the molarity of Cl^- in each solution? b. 0.150 M SrCl₂

Verified step by step guidance

Identify the chemical formula of the compound: SrCl_2.

Determine the number of chloride ions (Cl^-) produced per formula unit of SrCl_2. Each SrCl_2 dissociates into one Sr^2+ ion and two Cl^- ions.

Use the given molarity of SrCl_2, which is 0.150 M, to find the concentration of Cl^- ions. Since each SrCl_2 produces two Cl^- ions, multiply the molarity of SrCl_2 by 2.

Set up the equation: Molarity of Cl^- = 2 * Molarity of SrCl_2.

Substitute the given molarity of SrCl_2 into the equation to find the molarity of Cl^- ions.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in units of moles per liter (M). Understanding molarity is essential for calculating the concentration of ions in a solution, as it allows for the quantification of how much solute is present in a given volume of solvent.

Dissociation of Ionic Compounds

Ionic compounds, such as SrCl2, dissociate into their constituent ions when dissolved in water. For SrCl2, it dissociates into one strontium ion (Sr²⁺) and two chloride ions (Cl⁻). This dissociation is crucial for determining the concentration of specific ions in solution, as the number of ions produced directly affects their molarity.

Stoichiometry of Dissociation

Stoichiometry involves the quantitative relationship between reactants and products in a chemical reaction. In the case of SrCl2, the stoichiometry indicates that for every mole of SrCl2 that dissolves, two moles of Cl⁻ ions are produced. This relationship is vital for calculating the molarity of Cl⁻ ions based on the initial concentration of SrCl2.

Recommended video:

Guided course