Solutions

Question 1

what is a solution?

Answer 1

a homogeneous mixture of subtance that has uniform composition throughout.

Question 2

what is aqueous solution? what is solute & solvent?

Answer 2

a solution in which the solvent is water.
In a solution the substance present in
lesser amount = solute
larger amount =solvent

aqueous = latin word aqua = water

The solute is the substance that is being dissolved, while the solvent is the dissolving medium.

Question 3

what is unsaturated & saturated solution?

Answer 3

An unsturated solution contains lesser amount of solute & can dissolve more solute at a given temp.
A solution in which no more solute can be dissolved at a given temperature is called as saturated solution.

Question 4

what is supersaturated solution?

Answer 4

a solution that contains more than the maximum amount of solute that is capable of being dissolved at a given temperature.

Question 5

how to know whether a solution is saturated or supersaturated?

Answer 5

Saturated if crystals remain at the bottom of the container.
Supersaturated if no crystals remain at the bottom of the container.

pg 107 for another reason

Question 6

physical state of a solution is same as ______________.

Answer 6

physical state of solvent.

Question 7

examples of solid and gaseous solutions?

Answer 7

FMIGTN or page 109

Question 8

give types of solutions? examples of liquid solution

Answer 8

page 109

Question 9

what is solution called when
solid is dissolved in gas
gas is dissolved in liquid
give example

Answer 9

solid in gas
gas in liquid
smoke - solute= solid (carbon particles)
solvent= air
oxygen in water - solute= oxygen
solvent= water

imp. for survival of fish & other aquatic animals

Question 10

6.1 page 110
example of solid in solid.
give 3 examples

Answer 10

alloy gold (solvent) copper (solute)
brass = alloy= Cu and Zn

Question 11

define concentration of a solution?

Answer 11

the quantity of a solute present in given amount of solvent or solution is concentration of solution .

Question 12

what is percentage of solution?
what is m/m?
give example of each?

Answer 12

percentage: unit of concentration.
mass or volume of solute dissolved in 100g or 100cm3 of solution is % of solution.
4 ways to express % of solutions.
m/m v/v m/v v/m
pg 111

Question 13

name concentration units?
how to express them?
Mathematically molarity =?

Answer 13

percentage (% m/v m/m v/v)
molarity (M)
M= moles of solute/ dm3 of solution

Question 14

what is molarity?

Answer 14

the no. of moles of solute dissolve per dm3 of solution
molarity (M): conc. unit in which solute is expressed in moles and solution in dm3.

1dm3 = 1 liter

Question 15

molar mass of N, O, H, Cl, Cu, B, F, Na, Mg, Ca, K, C

Answer 15

+ 2

Question 16

while calculating M, how to convert g/mass to moles

Answer 16

mass in gm/ molar mass
molar mass = sum of atomic masses

Question 16

what does 12M of NaCl mean?

Answer 16

12 moles of NaCl** per dm3.**

0.1 moles= 0.1M

12M= 12 moles
0.1 moles = 0.1M

Question 17

how to convert M to g/dm3

Answer 17

first find molar mass
then apply this formula:
Mass in gm= No. of moles (given)/ molar mass

Question 18

define solubility?

Answer 18

the amount of solute that dissolves in 100g of a solvent at a particular temperature is its solubility.

Question 19

give example of “like dissolves like”?

Answer 19

NaCl & H2O
oil and water
oil and gasoline
pg 118

Question 20

what is colloid? size of colloidal particles? examples? can it scatter light? can it be filtered by filter paper?

Answer 20

a heterogenous mixture of tiny particles of a substance dispersed through a medium.
1-1000nm
milk, butter, cheese, jam, mayonnaise.
yes
no

Question 21

size of solution particles? can it scatter light? can it be filtered by filter paper?

Answer 21

0.1-1nm
can’t be seen
can’t scatter light
can’t be filtered

Question 22

what is suspension? size of suspension particles? can it scatter light? can it be filtered?

Answer 22

a heterogenous mixture containing particles large enough to be seen with the naked eye & clearly distinct from the surrounding fluid.
greater than 1000 nm
yes
yes

Question 23

give examples of alloys?
examples of gemstones?

Answer 23

brass= copper & zinc
steel= iron carbon silicon
ruby opal = solutions of solid

Question 24

define amalgam? what kind of solution?

Answer 24

a solution of any metal in mercury. They are used to make dental filling.
liquid in solid.

silver or tin amalgams

Mercury = solute silver = solvent.

Question 25

molarity of NaOH dissolved in 200 cm3 of solution is 0.1M. what is mass of solute?

Question 26

0.85 % (m/v) of NaCl.
what do we mean by that?
find out molarity of NaCl.

Answer 26

there are 0.85 grams of NaCl for every 100 cm3 of the solution.

remem: molarity is just another way to describe concentration of solute.

or for every 100 milliliters (mL) of the solution.
as 1cm3 = 1mL