Solutions, Acids, and Bases

a homogeneous mixture of two or more substances in one state of matter

the substance that is dissolved

the substance that does the dissolving (most abundant)

solution

any solution where water is the solvent

the number of moles of solute dissolved in every liter of solution

M = moles of solute over liters of solution

the moles of solute dissolved in each kilogram of solvent

m = moles of solute over kg of solvent

n (solute) = MV

When the solvent particles are strongly attracted to the solute particles. Every solute particle is pulled away from the other solute particles and ends up surrounded by solvent particles, resulting in a homogenous mixture

When a solution reaches the point where it can't dissolve any more solute

a measure of the amount of solute that can be dissolved in a solvent under given conditions

a substance that can donate H+ ions in solution

a substance that can accept H+ ions in solution

an acid loses a H+

a base gains a H+

chemicals that change color depending on the pH of the solution

a measure of the strength of an acid or base, a measure of the concentration of hydrogen ions in a solution.

acids that do not completely dissociate in water

less than 100% of the molecules form ions in water

substances that have a strong attraction for H+ in solution

substances that have a weak attraction for H+ in solution

when an acid and a base react in the proper amounts to neutralize each other.

a carefully controlled reaction where an unknown solution is reacted with a known solution

A solution with a known concentration

pH=-log[H+]

MaVa = MbVb

100% dissociation, more H+, lower pH, weak bonds with hydrogen

less than 100% dissociation, fewer H+, higher pH, stronger bond

HCl --> H+ + Cl-

solutions that contain more solute than the solvent would normally dissolve under current conditions

the point when the standard solution completely neutralizes the unknown solution because the moles of acid are equal until the moles of base