Chapter 2 Chemistry comes alive

1. Chapter 2 Chemistry comes alive For Quiz 2c

2. Biochemistry The study of the chemical composition and reactions of living matter.

3. Biochemistry • Organic compounds • Contain carbon, are covalently bonded, and are often large • Inorganic compounds • All other chemicals in the body • Do not contain carbon • Water, salts, and many acids and bases

4. Today • We will go over • Water • Salts • Acids • Bases • pH • Buffers

7. The Chemistry of Life Water

8. Water is the single most abundant substance on Earth!

9. What are the Properties of Water?

10. Water is different than other substances – it expands as it freezes!

11. Water Most abundant and important inorganic compound in living material. Makes up 60% - 80% of the volume of most living cells.

12. Properties of Water • High heat capacity • absorbs and releases large amounts of heat before changing temperature • This prevents sudden changes in body temperature cased by external factors like sun or wind or internal factors like heat released during vigorous muscle activity • As a part of blood, water redistributes heat among body tissues, ensuring temperature homeostasis

13. Properties of Water • High heat of vaporization • changing from a liquid to a gas requires large amounts of heat • As we sweat, perspiration (mostly water) evaporates from our skin removing large amounts of heat • This is a very efficient cooling mechanism for our bodies!

14. Properties of Water • Polar solvent properties • Water is often called the universal solvent • dissolves ionic substances • forms hydration layers around large charged molecules • serves as the body’s major transport medium

15. Properties of Water • Reactivity • an important part of hydrolysis and dehydration synthesis reactions • Food is digested to their building blocks by adding a water molecule to each bond - Hydrolysis reactions • Carbohydrates and proteins are synthesized from smaller molecules by removing a water molecule for each bond formed – dehydration synthesis

16. Properties of Water • Cushioning • resilient cushion around certain body organs • Helps protect organs from physical trauma • Cerebrospinal fluid surrounding the brain is an example

17. Salts

18. Salts • Inorganic compounds • Contain cations other than H+ and anions other than OH– • Are electrolytes; they conduct electrical currents

19. Salts • Maintaining proper ionic balance in our body fluids is one the most crucial homeostatic roles of the kidneys. • When this balance is severely disturbed, virtually nothing in the body works.

20. Acids and Bases Acids and Bases are also electrolytes, Conduct electrical current

21. Acids • Tastes sour • Dissolves many metals • Acids release H+ and are therefore proton donors HCl  H+ + Cl – Acids are proton donors!

22. Bases • Tastes bitter • Feel slippery • Bases release OH– and are proton acceptors NaOH  Na+ + OH– Bases are proton acceptors!

23. Acid-Base Concentration (pH) • Acidic solutions have higher H+concentration and therefore a lower pH • Alkaline (basic) solutions have lower H+ concentration and therefore a higher pH • Neutral solutions have equal H+ and OH– concentrations

24. Acid-Base Concentration (pH) • Acidic: pH 0–6.99 • Basic: pH 7.01–14 • Neutral: pH 7.00 Figure 2.12

25. Neutralization • When acids and bases are mixed, they react with each other in a displacement reaction to form water and a salt. HCl + NaOH -> NaCl + H2O

26. Buffers • Systems that resist abrupt and large swings in the pH of body fluids are buffering systems • If blood pH varies from the narrow range of 7.35 – 7.45 by more than a few tenths, it can be fatal! • Homeostasis of acid-base balance is regulated by the kidneys and lungs and by chemical systems called Buffers.

27. Buffer systems • Carbonic acid-bicarbonate system is a very important chemical blood buffer • Carbonic acid dissociates reversibly, releasing bicarbonate ions and protons • The chemical equilibrium between carbonic acid and bicarbonate resists pH changes in the blood

28. Quiz 2d Now!