Practice Problem: Solubility Product Constant Calculations

Practice Problem: Solubility Product Constant Calculations

Assessment

Interactive Video

Chemistry, Science

11th Grade - University

Practice Problem

Hard

Created by

Wayground Content

FREE Resource

The video tutorial explains how to use solubility product constants with fluorite as an example. It covers the dissolution of fluorite into calcium and fluoride ions, and how to calculate their concentrations in a saturated solution. The tutorial then guides viewers through writing the KSP expression and calculating the solubility product value for fluorite using stoichiometry and equilibrium principles.

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5 questions

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1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the chemical formula for fluorite?

CaSO4

CaF2

CaCO3

CaCl2

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

If the calcium ion concentration in a saturated solution is 2.1 * 10^-4 M, what is the fluoride ion concentration?

8.4 * 10^-4 M

1.05 * 10^-4 M

4.2 * 10^-4 M

2.1 * 10^-4 M

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How many fluoride ions are produced for each calcium ion when fluorite dissolves?

Two

Three

One

Four

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the KSP expression for fluorite?

[Ca^2+][F^-]

[Ca^2+]^2[F^-]

[Ca^2+]^2[F^-]^2

[Ca^2+][F^-]^2

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the calculated KSP value for fluorite?

3.7 * 10^-10

3.7 * 10^-11

3.7 * 10^-12

3.7 * 10^-13

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