solution chemistry

Question 1

what is a solution?

Answer 1

homogenous mixture of 2+ soluble pure substances, physically combined to form a mixture

Question 2

define solute, solvent. which is in greater amount in a solution?

Answer 2

solute= compound of lesser amount being DISSOLVED in another compound
solvent = compound of greater amount that DISSOLVES the solute

Question 3

what is an aqueous solution? what do we mean by “aqueous”?

Answer 3

solution where the solvent is liquid water
aqueous= something dissolved in water

Question 4

T/F: solutions can only be in a liquid phase

Answer 4

false: solutions can be in any phase of matter!

Question 5

T/F: solvent doesn’t always have to be water.

Answer 5

true

Question 6

T/F: particles are not uniformly distributed in a solution

Answer 6

false! uniform distribution of particles in a solution

Question 7

can components of a solution separate spontaneously?

Answer 7

no

Question 8

can you visually differentiate between a solute and solvent in a solution?

Answer 8

no– solutions are homogenous mixtures

Question 9

what 3 kinds of solutes can we have in an aqueous solution/solute dissolved in H2O?

Answer 9

1. ionic compounds
2. covalent compounds
3. acid/base

Question 10

what makes water polar?

Answer 10

a difference in its electron distribution between its atoms

Question 11

which components of water have positive partial charge? negative partial charge?

Answer 11

positive partial charge = H
negative partial charge= O

Question 12

what do we mean by “dipole”?

Answer 12

has partial positive/negative charged ends

Question 13

what is electronegativity?

Answer 13

tendency of an atom to “hog” electrons

Question 14

why is water special as a solvent?

Answer 14

not many liquids are polar in nature

Question 15

explain how water “sticks to itself”

Answer 15

partial positive H atoms attracted to partial negative charges of O atoms

Question 16

what are hydration shells/spheres? why does this result in ionic compounds?

Answer 16

water molecules surrounding an ion that belonged to an ionic compound.
ex. Na surrounded by O and H atoms
ions are more attracted water than they are to their respective ion they bonded with!

Question 17

what type of compound is a strong electrolyte in H2O? what does this mean?

Answer 17

ionic compounds are strong electrolytes in water
good conductors of electricity

Question 18

what do we mean by aqueous ionic compounds?

Answer 18

individual ions floating around separately in water!

Question 19

T/F: polyatomic ions do not stay as 1 unit when dissolved in water

Answer 19

false!! polyatomic ions DO stay as 1 unit when dissolved in water

Question 20

do covalent compounds break down into different particles when dissolved or do molecules stay intact?

Answer 20

molecules stay intact!
ex. NaCl (ionic) = Na+ + Cl- (went from 1 mol of an ionic compound to 2 mol of ions)
vs.
C12 H22 O11 in H2O = C12 H22 O11 (aq)
(went from 1 mol to 1 mol of compound)

Question 21

are covalent compounds dissolved in water electrolytes? what does this mean about their electricity conductance?

Answer 21

no, covalent compounds in water form NON ELECTROLYTES. cannot conduct electricity!

Question 22

do partial charges/ions form in covalent compounds?

Answer 22

n o o o

Question 23

define a strong electrolyte. what types of substances does this include?

Answer 23

solute that COMPLETELY DISSOCIATES in solution and is a good conductor of electricity.
includes
- soluble ionic compounds
- strong acids
- strong bases

Question 24

define a weak electrolyte. what types of substances does this involve?

Answer 24

solute that PARTIALLY dissociates in solution. somewhat good electricity conductors.
involves
- weak acids
- weak bases

Question 25

what are non-electrolytes? what substances are non electrolytes?

Answer 25

solute that DOES NOT dissociate in solution, and is a poor electricity conductor (or doesn’t conduct electricity at all)
includes covalent compounds