Periodic Table Sol part 1 and 2, Concentration and Molarity

What properties can help predict the solubility of a substance

Atomic size and ionic charge

What happens to solubility as you move down a group on the periodic table?

Solubility decreases due to increasing atomic size, which reduces the solvation by water molecules

Solubility increases for what substances?

Salts and compounds containing alkali metals and nitrate ions

What happens to solubility when moving across a period?

The solubility predictions are more complex as it is based on the ions and anions involved

What compounds are generally soluable?

Most chlorides, bromides, and iodides are soluble

What compounds are the excecptions?

Lead, mercury, and silver

Why are lead, mercury, and silver generally insoluble

The attraction between these metals is too strong to break apart, which makes the bonds difficult to break apart

What is the process of water molecules surrounding and interacting with dissolved ions

Solvation

How does the ionic size affect solubility

As you move down a group the ionic size increases which makes it harder for water molecules to surround and solvate them

What happens to metal cation solubility as you move a group?

It decreases

Why does metal cation decrease as you move down a group?

The ionic radius of metal cations increases, which weaken hydration interactions with water molecules

How are solubility trends across a period?

They’re more complex and variable

What are solubility charts used for?

Tools for predicting whether double replacement reactions will occur

What happens if products are insoluble

They form precipitates

What happens if all products are soluable

No reaction takes place

Why do ionic compounds dissolve in water?

Water is a polar molecule so it has a partial negative charge on the oxygen atom, and a partial positive charges on the hydrogen atom. These charges attract the ions in salt which allows dissolution to occur

What is an unsaturated solution?

A solution that can still dissolve more solute

What is a saturated solution?

A solution that has dissolved the maximum amount of solute possible at that temperature. Any additional solute will remain solid

What is a dilute solution?

A solution with a low concentration of solute

What is a concentrated solution?

A solution with a high concentration of solution

What is a supersaturated solution?

A solution that contains more solute than it can normally hold at that temperature (unstable)

What is Calcium Carbonate found in

Found in antacid used for stomach aches which may produce unwanted gams

How does temperature affect solubility

Increasing temp increases solubility for most solids, while decreasing solubility of gases

How does pressure affect solubility

Increasing the pressure of a gas above a liquid increases the amount of gas that can be dissolved in the liquid (Doesn’t really affect solids)

How does molecular size affect solubility?

Larger molecules are less soluble

How does Surface Area affect solubility

It does not affect solubility, but it affects the rate of dissolving

How does the size of surface area affect the rate

A larger surface area exposes more solute particles to the solvent, leading to more frequent collisions and a faster rate of dissolution

What dissolves faster, powdered or granulated sugar?

Powdered dissolves faster because it has a much larger surface area

How does type of solvent/solute particles affect solubility

“Like dissolves Like”

What factor does not affect the rate of dissolving

Solubility

What affects the total amount of sugar that can be dissolved?

The solvent and temp

Why does increasing temp increase solubility

The higher temp means the particles are moving faster, so there is more contact, making it easier for the sugar to dissolve

What is Concentration?

A broader term for the amount of substance (solute) in a given amount of another substance (solvent)

What is Molarity

The number of moles of solute per liter solution (mol/L)

What does 1.25 M of solution mean?

There are 1.25 Moles of solute per 1 L of solution

What is Mass Concentration

Mass of solute divided by volume of solution

What is weight percent

Mass of solute divided by the total mass of the solution multiplied by 100