Solution Chemistry

Question 1

what terms describes the solubility of a solid or gas in a liquid

Answer 1

soluble and insoluble

Question 2

what terms describes the solubility of a liquid in a liquid

Answer 2

miscible and immiscible

Question 3

in what conditions are gases most soluble?

Answer 3

low temp high pressure

Question 4

when are solid solutions most soluble?

Answer 4

in warm temperatures

Question 5

alloys

Answer 5

a mixture of two or more metals. ex: sterling silver, brass

Question 6

amalgam

Answer 6

a solid solution of metals that contains mercury

Question 7

list things that solubility is dependent upon

Answer 7

temperature, pressure if a gas, chem. nature of the solute/solvent (polarity)

Question 8

formula for molarity?

Answer 8

moles of solute/liters of solution

Question 9

percent by mass formula?

Answer 9

mass of solute/mass of solution * 100

Question 10

percent by volume formula?

Answer 10

volume of solute/volume of solution * 100

Question 11

parts per million formula

Answer 11

grams of solute/grams of solution * (1x10^8)

Question 12

colligative properties

Answer 12

• only applied to solutions
• depends only on the ratio between solute and solvent, not the kind of solute
• the more particles in the solution the greater the temperature change

Question 13

why does the difference between FP and BP increase with the amount of solute added?

Answer 13

because the solute particles decrease vapor pressure and get in the way of the solute’s particles during freezing

Question 14

formula for change in boiling/freezing point temperature

Answer 14

change in T = ikm, where k is altered for boiling or freezing

Question 15

what does k (b) mean in the change in BP/FP formulas?

Answer 15

constant for the solute

Question 16

what is water’s k value for BP?

Answer 16

0.52

Question 17

what is water’s k value for FP?

Answer 17

1.86

Question 18

what is i in the change in temperature formulas?

Answer 18

the van’t hoff factor, the number of ions per formula unit if the solute is an ionic substance. Polyatomic ions are counted as one ion.

Question 19

the actual value for change in temperature is usually ______ than the expected value because _______________

Answer 19

lower, because at any point in time, some of the ions in the solution will be paired

Question 20

molality formula

Answer 20

moles of solute/kg of SOLVENT

Question 21

electrolytes

Answer 21

a substance, which when dissolved in water is able to conduct electricity

Question 22

what do strong electrolytes do?

Answer 22

they dissociate completely

Question 23

what are the parameters for conducting electricity

Answer 23

you must have something that moves and carries a charge

Question 24

what do weak electrolytes do?

Answer 24

they only dissociate slightly, therefore mostly staying together

Question 25

complete ionic equation

Answer 25

separation of aqueous solutions into positive and negative ions, putting coefficients in front

Question 26

net ionic equation

Answer 26

only keep the ions that make the solid, liquid, or gaseous product on the reactant side and only keep that product on the other side (none of the aqueous components)

Question 27

formula for dilutions

Answer 27

M of initial * Volume of initial = M of final * V of final

Question 28

in dilutions, should the final molarity be smaller or greater than the original

Answer 28

smaller, because you are DILUTING IT

Question 29

explain how to do a dilution in the lab

Answer 29

- do the math - add like 20 ml of water into a volumetric flash - add in the calculated amount of stock solution - stir then cool (most of these are exothermic) - add deionized water to graduated marking

Question 30

calculations for making a solution from a solid reactant?

Answer 30

still us MV = MV but convert to grams where needed

Question 31

procedure for making a solution from solid reactant

Answer 31

- calculations - add deionized water in flask, a small amount - measure out solute and add to flask - heat/stir to dissolve - cool to room temperature and add deionized water to the mark