10.3 Strengths of Acids and Bases

10.3 Strengths of Acids and Bases

• The conjugate acid-base pairs are HSO4 and HCN.

• Weak acids and weak bases don't leave much of the initial acid or base in the water.

• H+ is transferred to H2O, and the resulting solution contains only H3O+ and Cl-.
• The reaction of HCl in H2O is considered 100% to products.
• One mole of a strong acid in water will yield one mole of H3O+ and one mole of its conjugate base.
• We write the equation for a strong acid with a single arrow.

• The other acids are weak.

• The reverse reaction is more prevalent because a weak acid has a strong conjugate base.

• Weak acids can be found in many of the products you use at home.

• Fruits and fruit juices have bicyle acid in them.
• A 5% acetic acid solution is used in salad dressings.

• 2H3O2molecules give H+ to H2O to form H3O+ ion and acetate ion.
• Weak acids are found in foods and back to reactants.
• The reason we notice household products is due to the formation of hydronium ion.

• We use a double arrow to indicate that the forward and reverse reactions are at equilibrium in the equation for a weak acid.

• Carbonic acid is formed by dissolving CO2 in water.
• A weak acid such as H2CO3 can reach equilibrium between the H 2CO3 molecule and the H3O+ and HCO3 molecule.

• The solution of the H3O+ and I- is formed by a strong acid such as HI in water.

• The strong bases give a solution of metal and hydroxide ion in water.
• The Group 1A (1) hydroxides can give high concentrations of OH- ion in water.
• When a KOH solution is formed, it contains only K+ and OH-.
• A few strong bases are less sible in water.

• To open the drain.

• They are low in solubility, but they are completely separated.

• If high concentrations of hydroxide ion cause Window cleaner, ammonia, NH3 severe damage to the skin and eyes, directions must be followed carefully.
• If you spill an acid or a base on your skin or get some in your eyes, be sure to seek medical attention immediately and flood the area with Laundry detergent, Na2CO3, Na3PO4 for at least 10 minutes.

• A weak base, ammonia, NH3 is found in window cleaners.

• CaCO3 is a lime for lawns and agriculture.

• Weak acids and bases are included in the equation for the dissociation of strong and following pairs.

• The acid-base equilibrium can be explained by the concept of reversible reactions.

• When reaction conditions change, use Le Chatelier's principle to determine the effect on equilibrium concentrations.

• A reverse reaction in which products form reactants is the reason why reactants in acid-base reactions are not always converted to products.

• There are two reactions taking place, one in the forward direction and the other in the reverse direction.
• The forward reaction occurs at a faster rate than the reverse reaction.
• As reactants are consumed and products accumulate, the rate of the forward reaction decreases and the rate of the reverse reaction increases.

• The products form reactants at the same rate.

• Let's look at the reaction of the weak acid as it moves to equilibrium.

• Initially, only the reactants are present.

• equilibrium has been reached when the rates of the forward and reverse reactions become equal.
• Even though the forward and reverse reactions continue, the concentrations of the reactants and products remain constant.

• The concentrations of the reactants and products are before equilibrium is reached.

• The rate of reaction of reactants is different from the rate of reaction of products.

• The rate of the reverse reaction is equal to the rate of the forward reaction.

• When we change the concentration of a reactant or product of a system at equilibrium, the rates will no longer be equal.

• There are two water tanks connected to a pipe.
• Water flows in the reverse direction from Tank B to Tank A when the water levels are equal, but in the forward direction from Tank A to Tank B when the water levels are equal.
• There is an increase in the rate at which water flows from Tank A into Tank B if we add more water.
• When the water levels in both tanks are equal, equilibrium is restored.

• The water flows between Tank A and Tank B even though the water levels are higher.

• When levels are equal, equilibrium is reached.

• The rate of flow in the forward direction is increased when water is added to Tank A.

• We will use the reaction of H2O and HF to show how a change in concentration can affect equilibrium and how the system responds to that stress.

• The system increases the forward reaction to relieve stress.

• The rate of the forward reaction is slowed by the decrease in HF concentration.

• If more F- is added to the equilibrium mixture, the rate of the reverse reaction increases as products are converted to reactants.

• Some F- is removed from the reaction mixture at equi librium.
• The reverse reaction is slowed by the decrease in F concentration.

• The equilibrium system changes when some substance is removed.
• The features of Le Chatelier's principle are summarized in tAbLE.

• Immediate treatment of altitude sickness includes hydration, rest, and, (Hb), oxygen, and oxyhemoglobin.

• It takes about 10 days to adapt to lowered oxygen levels.
• A person living at a high altitude can have 50% more 2 level is high in the alveoli of the lung, the reaction shifts in the direction of the product HbO red blood cells than someone at sea level.
• In tissues where O2 concentration is low, the reverse reaction releases the oxygen from the causes a shift in the equilibrium back in the direction of HbO2 product.

• Oxygen diffuses into the blood to the tissues when atmospheric pressure is normal.

• A decrease in the atmospheric pressure at an altitude above 8000 ft results in a reduction in the partial pressure of oxy, which means that less oxygen is available for the blood and body to acclimatize for several days.
• It may be necessary to use an oxygen tank at higher altitudes because of the fall in atmospheric pressure.

• A person will get 29% less oxygen at an altitude of 18 000 ft.
• There is a problem in people with a history of lung disease who have a reduced number of red blood cells.

• Le Chatelier's principle states that a decrease in oxygen will shift the system in the direction of the reactants to reestablish equilibrium.
• A shift depletes the concentration of HbO2

• When stress is applied to a reaction at equilibrium, the system shifts to relieve that stress.

• The equilibrium shifts in the direction of the reactants when the concentration of the product increases.

• Try Practice Problems 10.23 when H2CO3 is removed.

• The system shifts in the direction of acid-base equilibrium when there are lowing changes.
• Le Chatelier's principle is used to determine the products or reactants.

• The system shifts in the direction of change when the concentrations of the reactants and products are not low.

• There is no change in the rate of the reverse reaction.

• The forward and reverse reactions have the same rates.

• The rate of the forward reaction stays the same.