1. Acids, Bases, & Molarity
Chemistry 10
Mrs. Page

2. Learning Objectives
Define acid and base according to Bronsted-Lowry theory
List the general characteristics of acids and bases.
Name common binary acids and oxyacids given their chemical formulas
Define the terms solute, solvent, solution, solubility and molarity
Calculate molarity

3. ACIDS Have you ever had a muscle cramp after working out?
This is a result of lactic acid building up in your muscles when oxygen is limited.

4. Define acid and base according to Bronsted-Lowry theory
What is an acid?
An acid is a substance that produceds H+ ions in water.
According to the Bronsted-Lowry theory an acid is a proton donor
It comes from the Latin word acidus that means "sharp" or "sour".
The more H+ ions, the more acidic the solution.

5. Properties of Acids Tastes Sour Conduct Electricity
List the general characteristics of acids and bases.
Properties of Acids
Tastes Sour
Conduct Electricity
Corrosive, which means they break down certain substances. Many acids can corrode fabric, skin, and paper
Some acids react strongly with metals
Turns blue litmus paper red
pH below 7
Picture from BBC Revision Bites

6. Some Common Uses of Acids
Acetic Acid = Vinegar
Citric Acid = lemons, limes, & oranges. It is in many sour candies such as lemonhead & sour patch.
Ascorbic acid = Vitamin C which your body needs to function.
Sulfuric acid is used in the production of fertilizers, steel, paints, and plastics.
Lactic acid is also produced by bacteria in milk – this is why milk turns sour.
Insects such as millipedes, scorpions, and ants use acids to deter predators.

7. Naming Acids HCl HF H2S HBr H3P HI Binary Acids Named by anion
Name common binary acids and oxyacids given their chemical formulas
Naming Acids
Chemical Formula
Chemical Name
Binary Acids
Named by anion
Starts with hydro-
Anion name ending in –ic
Add the word acid
HCl
Hydrochloric Acid HF
Hydrofluoric Acid
H2S
Hydrosulfuric Acid
HBr
Hydrobromic Acid
H3P
Hydrophosphoric Acid HI
Hydroiodic Acid

8. Name common binary acids and oxyacids given their chemical formulas
Naming Acids
Oxyacids
These acids contain polyatomic ions (and therefore usually contain O atoms)
Based on the polyatomic anion bonded to hydrogen
If polyatomic ion is –ite then acid is –ous
If polyatomic ion is –ate then acid is -ic

9. Naming Acids HNO2 HNO3 H2SO4 H3PO4 H2SO3 H2CO3 Nitrite Nitrous Acid
Name common binary acids and oxyacids given their chemical formulas
Naming Acids
Chemical Formula
Polyatomic Ion
Name of Acid
HNO2
Nitrite
Nitrous Acid
HNO3
Nitrate
Nitric Acid
H2SO4
Sufate
Sulfuric Acid
H3PO4
Phosphate
Phosphoric Acid
H2SO3
Sulfite
Sulfurous Acid
H2CO3
Carbonate
Carbonic Acid

10. What is a base? A base is a solution that has an excess of OH- ions.
Define acid and base according to Bronsted-Lowry theory
What is a base?
A base is a solution that has an excess of OH- ions.
Chemists sometimes use the term “alkali” for a base that is soluble in water.
Alkali is of Arabic origin meaning “ashes of a plant.”
Bases are substances that can accept hydrogen ions, H+ (proton acceptors)

11. Properties of Bases Feel Slippery Taste Bitter Corrosive
List the general characteristics of acids and bases.
Properties of Bases
Feel Slippery
Taste Bitter
Corrosive
Can conduct electricity. (Think alkaline batteries.)
Do not react with metals.
Turns red litmus paper blue.
pH above 7

12. Some Common Uses of Bases
Bases give soaps, ammonia, and many other cleaning products some of their useful properties.
The OH- ions interact strongly with certain substances, such as dirt and grease.
Chalk and oven cleaner are examples of familiar products that contain bases.
Your blood is a basic solution.
Quinine is base used as a drug to treat malaria.
Lidocaine, a local anesthetic used by dentists, is a base.
Like acids, some bases are harmless while others are very dangerous.

13. Solutions Most acids and bases dissolve in water.
Define the terms solute, solvent, solution, solubility and molarity
Solutions
Most acids and bases dissolve in water.
A solution is a homogenous mixture of 2 or more substances
The solute is the substance(s) present in the smaller amount(s)
The solvent is the substance present in the larger amount

14. Define the terms solute, solvent, solution, solubility and molarity
How well a solute dissolves in a solvent is called solubility.
We used the solubility table to determine if a precipitate formed in a chemical reaction.
Acids and bases are soluble in water
The properties of acids and bases are only exhibited when they are in solution
Many factors affect solubility such as pressure, amount of solute, amount of solvent, and temperature. (think about making Kool-Aid)

15. 𝑀= 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝐿𝑖𝑡𝑒𝑟𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
Define the terms solute, solvent, solution, solubility and molarity
Molarity
Molarity (M) is a measure of the concentration of a solution.
Concentration – how much solute in comparison to how much solvent
𝑀= 𝑚𝑜𝑙𝑒𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑒 𝐿𝑖𝑡𝑒𝑟𝑠 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛

16. CALCULATING MOLARITY Calculate moles of solute
Calculate molarity
CALCULATING MOLARITY
Calculate moles of solute
Convert units of solution to liters
Use molarity formula 𝑴= 𝒎𝒐𝒍𝒔 𝒔𝒐𝒍𝒖𝒕𝒆 𝑳𝒊𝒕𝒆𝒓𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏

17. =𝟎.𝟔𝟐𝟖 𝑴 CALCULATING MOLARITY 𝑴= 𝒎𝒐𝒍 𝑳 = 𝟎.𝟐𝟏𝟔 𝒎𝒐𝒍 𝟎.𝟑𝟒𝟒 𝑳
Calculate molarity
CALCULATING MOLARITY
Calculate moles of solute
Convert units of solution to liters
Use molarity formula 𝑴= 𝒎𝒐𝒍𝒔 𝒔𝒐𝒍𝒖𝒕𝒆 𝑳𝒊𝒕𝒆𝒓𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏
12.6 g of NaCl are dissolved in water making 344mL of solution. Calculate the molar concentration.
12.6 g NaCl
1 mol NaCl
= mol NaCl
g NaCl
344 mL sol’n
1 L
= L sol’n
1000 mL
𝑴= 𝒎𝒐𝒍 𝑳
= 𝟎.𝟐𝟏𝟔 𝒎𝒐𝒍 𝟎.𝟑𝟒𝟒 𝑳
=𝟎.𝟔𝟐𝟖 𝑴

18. =𝟏.𝟔 𝑴 CALCULATING MOLARITY 𝑴= 𝒎𝒐𝒍 𝑳 = 𝟎.𝟓𝟓𝟕 𝒎𝒐𝒍 𝟎.𝟑𝟓 𝑳
Calculate molarity
CALCULATING MOLARITY
Calculate moles of solute
Convert units of solution to liters
Use molarity formula 𝑴= 𝒎𝒐𝒍𝒔 𝒔𝒐𝒍𝒖𝒕𝒆 𝑳𝒊𝒕𝒆𝒓𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏
What is the molarity of 350 mL of a solution containing g of NaHCO3?
46.8 g NaHCO3
1 mol NaHCO3
= mol NaHCO3
g NaHCO3
350 mL sol’n
1 L
= 0.35 L sol’n
1000 mL
𝑴= 𝒎𝒐𝒍 𝑳
= 𝟎.𝟓𝟓𝟕 𝒎𝒐𝒍 𝟎.𝟑𝟓 𝑳
=𝟏.𝟔 𝑴

19. 𝒙=𝟎.𝟑𝟏𝟑 𝒎𝒐𝒍 = 7.50 g LiOH CALCULATING MOLARITY 𝟏.𝟐𝟓= 𝒙 𝒎𝒐𝒍 𝟎.𝟐𝟓𝟎𝟎 𝑳
Calculate molarity
CALCULATING MOLARITY
Calculate moles of solute
Convert units of solution to liters
Use molarity formula 𝑴= 𝒎𝒐𝒍𝒔 𝒔𝒐𝒍𝒖𝒕𝒆 𝑳𝒊𝒕𝒆𝒓𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏
How many grams of LiOH is needed to prepare mL of a 1.25 M solution?
250.0 mL sol’n
1 L
= L sol’n
1000 mL
𝑴= 𝒎𝒐𝒍 𝑳
𝟏.𝟐𝟓= 𝒙 𝒎𝒐𝒍 𝟎.𝟐𝟓𝟎𝟎 𝑳
𝒙=𝟎.𝟑𝟏𝟑 𝒎𝒐𝒍
0.313 mol LiOH
g LiOH
= 7.50 g LiOH
1 mol LiOH

20. 𝒙=𝟎.𝟑𝟓 𝑳 = 350 mL solution CALCULATING MOLARITY 𝑴= 𝒎𝒐𝒍 𝑳
Calculate molarity
CALCULATING MOLARITY
Calculate moles of solute
Convert units of solution to liters
Use molarity formula 𝑴= 𝒎𝒐𝒍𝒔 𝒔𝒐𝒍𝒖𝒕𝒆 𝑳𝒊𝒕𝒆𝒓𝒔 𝒐𝒇 𝒔𝒐𝒍𝒖𝒕𝒊𝒐𝒏
What volume of solution will contain 25 g of H3PO4 if the solution concentration is 0.75 M?
25 g H3PO4
1 mol H3PO4
= 0.26 mol H3PO4
g H3PO4
𝑴= 𝒎𝒐𝒍 𝑳
𝟎.𝟕𝟓𝐌= 𝟎.𝟐𝟔 𝒎𝒐𝒍 𝒙 𝑳
𝒙=𝟎.𝟑𝟓 𝑳
0.35 L
1000 mL
= 350 mL solution
1 L