The video tutorial by Science Professor Dave explains precipitation reactions, focusing on magnesium hydroxide. It covers the solubility product (KSP) and how to determine the pH at which magnesium ions start precipitating. The tutorial includes writing the chemical reaction, calculating hydroxide ion concentration, and determining the pH for precipitation. It emphasizes understanding the relationship between KSP, ion concentration, and pH in promoting precipitation.

What is the solubility product (KSP) of magnesium hydroxide at 25 degrees Celsius?

• 1.0 * 10^-12

• 1.0 * 10^-10

• 1.0 * 10^-11

• 1.0 * 10^-9

In the solubility product reaction of magnesium hydroxide, how many hydroxide ions are produced per formula unit?

• 1

• 4

• 3

• 2

What is the expression for the solubility product (KSP) of magnesium hydroxide?

• [Mg^2+][OH^-]

• [Mg^2+]^2[OH^-]^2

• [Mg^2+][OH^-]^2

• [Mg^2+]^2[OH^-]

What is the hydroxide ion concentration required to start the precipitation of magnesium hydroxide?

• 1.0 * 10^-3

• 1.0 * 10^-6

• 1.0 * 10^-4

• 1.0 * 10^-5

At what pH will magnesium hydroxide start to precipitate from a solution of 0.001 molar magnesium ions?

• pH 8

• pH 9

• pH 10

• pH 11