Ch. 3 Warm-Up What property of water allows a water strider to “walk” on water? Contrast adhesion and cohesion. Give an example of each. Contrast hydrophobic and hydrophilic substances. Give an example of each.

Water and the Fitness of the Environment Chapter 2.5 Water and the Fitness of the Environment

You Must Know The importance of hydrogen bonding to the properties of water. Four unique properties of water, and how each contributes to life on Earth. How to interpret the pH scale. The importance of buffers in biological systems.

1. Polarity of H2O O- will bond with H+ on a different molecule of H2O = hydrogen bond H2O can form up to 4 bonds

2. Properties of H2O Cohesion = H-bonding between like molecules Surface Tension = measure of how difficult it is to break or stretch surface of liquid

Adhesion = bonding between unlike molecules 2. Properties of H2O Adhesion = bonding between unlike molecules Adhesion of H2O to vessel walls counters ↓ pull of gravity

H2O clings to each other by cohesion; cling to xylem tubes by adhesion 2. Properties of H2O C. Transpiration = movement of H2O up plants H2O clings to each other by cohesion; cling to xylem tubes by adhesion

3. Moderation of temperature Heat = Total amount of KE in system Temperature = measure intensity of heat due to average KE of molecules Which has higher temp? More heat?

3. Moderation of temperature Water’s high specific heat Change temp less when absorbs/loses heat Large bodies of water absorb and store more heat  warmer coastal areas Create stable marine/land environment Humans ~65% H2O  stable temp, resist temp. change

3. Moderation of temperature Evaporative Cooling Water has high heat of vaporization Molecules with greatest KE leave as gas Stable temp in lakes & ponds Cool plants Human sweat

3. Moderation of temperature Insulation by ice – less dense, floating ice insulates liquid H2O below Life exists under frozen surface (ponds, lakes, oceans) Ice = solid habitat (polar bears)

A meniscus is the curve of water inside a test tube A meniscus is the curve of water inside a test tube. Based on what you know about the properties of water, choose the answer that BEST describes how this phenomenon works https://www.polleverywhere.com/multiple_choice_polls/wMeKNJH5c2O6rK0

4. Solvent of life Solution = liquid, homogeneous mixture of 2+ substances Solvent = dissolving agent (liquid) Solute = dissolved substance Water = versatile solvent

Hydrophilic Hydrophobic 4. Solvent of life “like dissolves like” Hydrophilic Hydrophobic Affinity for H2O Repel H2O Polar, ions Nonpolar Cellulose, sugar, salt Oils, lipids Blood Cell membrane

What dissolves in water? Hydrophilic substances have attraction to H2O polar or non-polar? Hydrophilic substances have attraction to H2O

What doesn’t dissolve in water? Hydrophobic substances that don’t have an attraction to H2O polar or non-polar? Oh, look hydrocarbons! Hydrophobic substances that don’t have an attraction to H2O fat (triglycerol)

Figure 3.8 A water-soluble protein

Making solutions Find the mass of the compound (molar mass) Multiply the atomic mass of an element by the number of atoms of that element in a compound Add all of the masses together = total mass of the compound Dilute the molar mass to the required volume with distilled water (Molarity)

Calculating Concentrations CiVi=CfVf C= concentration V= volume i= initial f= final

Practice 53.4 mL of a 1.50 M solution of NaCl is on hand, but you need some 0.800 M solution. How many mL of 0.800 M can you make? (1.50 mol/L) (53.4 mL) = (0.800 mol/L) (x) x = 100. mL

5. Acids and Bases H2O H+ + OH- (gains proton) H+ + H2O  H3O+ (hydronium ion) (loses proton) H2O – H+  OH- (hydroxide ion)

7 14 Basic Acidic pH Scale 5. Acids and Bases Acid = increases H+ concentration (HCl) Base = reduces H+ concentration (NaOH) Most biological fluids are pH 6-8 7 14 Basic Acidic pH Scale

pH Scale H+ Ion Concentration Examples of Solutions pH 10–1 H+ Ion Concentration Examples of Solutions Stomach acid, Lemon juice 1 pH 100 Hydrochloric acid 10–2 2 10–3 Vinegar, cola, beer 3 10–4 Tomatoes 4 10–5 Black coffee, Rainwater 5 10–6 Urine, Saliva 6 10–7 Pure water, Blood 7 10–8 Seawater 8 10–9 Baking soda 9 10–10 Great Salt Lake 10 10–11 Household ammonia 11 10–12 Household bleach 12 10–13 Oven cleaner 13 10–14 Sodium hydroxide 14 tenfold change in H+ ions pH1  pH2 10-1  10-2 10 times less H+ pH8  pH7 10-8  10-7 10 times more H+ pH10  pH8 10-10  10-8 100 times more H+ In pure water only 1 water molecule in every 554 million is dissociated tenfold change in H+ ions pH1  pH2 10-1  10-2 10 times less H+ pH8  pH7 10-8  10-7 10 times more H+ pH10  pH8 10-10  10-8 100 times more H+

Figure 3.10 The pH scale and pH values of some aqueous solutions

Calculating pH -log 10-2 = -(-2) = 2 Therefore, pH = 2 [H+] = 10-4 [H+][OH-] = 10-14 If [H+] = 10-6 M, then [OH-] = 10-8 pH = -log [H+] If [H+] = 10-2 -log 10-2 = -(-2) = 2 Therefore, pH = 2 If [OH-] = 10-10 [H+] = 10-4 -log 10-4 = -(-4) = 4 Therefore, pH = 4

H2CO3 (carbonic acid)  HCO3- (bicarbonate) + H+ 5. Acids and Bases Buffers: minimize changes in concentration of H+ and OH- in a solution (weak acids and bases) Buffers keep blood at pH ~7.4 If blood drops to 7 or up to 7.8, then death Carbonic Acid – Bicarbonate System: important buffers in blood plasma H2CO3 (carbonic acid)  HCO3- (bicarbonate) + H+

Ocean acidification threatens coral reef ecosystems CO2 mixed with seawater  Carbonic acid (lowers ocean pH)

The effects of acid precipitation on a forest

Examples of Benefits to Life H2O Property Chemical Explanation Examples of Benefits to Life Cohesion polar H-bond like-like ↑gravity plants, trees Adhesion unlike-unlike plants xylem bloodveins Surface Tension diff. in stretch break surface bugswater Specific Heat Absorbs & retains E oceanmod temp protect marine life Evaporation liquidgas KE Cooling Homeostasis Universal Substance Polarityionic Good dissolver solvent