Acids and Bases. Acids and Bases in. our Lives. Acids and Bases in our Lives. Acids and Bases in our Lives. Chapter 11
|
|
- Allan Clement Brooks
- 5 years ago
- Views:
Transcription
1 Acids and Bases Chapter 11 Acids and Bases in our Lives We produce lactic acid in our muscles when we exercise. Acid from bacteria turns milks sour in the products of yogurt and cottage cheese. We have hydrochloric acid in our stomachs to help digest food and we take antacids, which are bases such as sodium bicarbonate, to neutralize the effects of too much stomach acid. Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste. Lemons and grapefruits taste sour because they contain acids such as citric and ascorbic acid (vitamin C). Vinegar tastes sour because it contains acetic acid. Acids and Bases in our Lives In the environment, the acidity or ph of rain, water, and soil can have significant effects. When rain becomes too acidic, it can dissolve marble statues and accelerate the corrosion of metals. In lakes and ponds, the acidity of water can affect the ability of plants and fish to survive. The acidity of soil around plants affect their growth. It can stop the plant from taking up nutrients through the roots
2 Acids and Bases in our Lives The lungs and kidneys are the primary organs that regulate the ph of body fluids, including blood and urine. Major changes in the ph of the body fluids can severely affect biological activities within the cells. Buffers are present to prevent large fluctuations Acids and Bases Describe and name acids and bases. Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 AcidBase Titration 11.9 Buffers Acids The term acid comes from the Latin word acidus which means sour. In 1887, the Swedish chemistry Svante Arrhenius was the first to describe acids as substances that produce hydrogen ions (H + ) when they dissolve in water.
3 Acids are Electrolytes Because acids produce ions in water, they are also electrolytes (can conduct electricity). Hydrogen chloride dissociates in water to give hydrogen ions, H +, and chloride ions, Cl : It is the hydrogen ions that give acids a sour taste. Naming Acids Binary acids: H n X hydro[nonmetal ic] acid Change the ending of the nonmetal to ic and insert into the brackets. hydro and acid do not change. HCl HBr H 2 S Naming Acids Acids have two common formats: Binary acids: H n X H n = some number of H s x=nonmetals Examples: HCl, HBr, H, H 2 S Polyatomic acids: H n XO m XO m = polyatomic ion Examples: H 2 SO 4, H 3 PO 4, HClO 4 Polyatomic Ion Review More O s = ate SO 4 2 Less O s = ite SO 3 2 Chlorine can form 4 polyatomic ions with oxygen: ClO 4 ClO 3 ClO 2 ClO
4 Naming Acids Polyatomic Acids: H n XO m [Polyatomic ion] acid ate to ic ite to ous H 2 SO 4 H 3 PO 4 HClO 3 Bases You may be familiar with some household bases such as antacids, drain cleaners, and oven cleaners. According to the Arrhenius theory, bases are ionic compounds that dissociate into cations and hydrogen ions (OH) when they dissolve in water. They are electrolytes. Bases Most Arrhenius bases are formed from a metal from Groups 1 or 2 and one or more hydroxides (OH ) M(OH) n M=metal (OH) n = 1 or more hydroxide group Examples: LiOH, Ca(OH) 2 The hydroxide ions give bases common characteristics such as a bitter taste or slippery feel.
5 Naming Bases Bases have the same names that we used for ionic compounds. LiOH NaOH Ca(OH) 2 Al(OH) BrønstedLowry Acids and Bases Identify the conjugate acidbase pairs for Brønsted Lowry acids and bases. Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 AcidBase Titration 11.9 Buffers Arrhenius Acids and Bases The definitions we gave in section 11.1 for acids and bases were first described by Arrhenius. So we call acids and bases described by H + and OH as Arrhenius acids and bases. Arrhenius acid: substances that produce H + in water. Arrhenius base: substances that produce OH in water.
6 BrønstedLowry Acids and Bases In 1923, a pair of scientists, J.N. Brønsted and T.M. Lowry expanded the definitions of acids and bases. The shortcoming of the Arrhenius definitions was that there were many molecules that didn t have OH groups that acted like bases. A new set of definitions describing BrønstedLowry acids and bases included a greater number of molecules. H + = H 3 O + A free hydrogen, H+, does not actually exist in water. Its attraction to polar water molecules is so strong that the H+ bonds to a water molecules and forms a hydronium ion, H 3 O + BrønstedLowry Acids and Bases BrønstedLowry acid: a substance that donates a hydrogen ion, H + BrønstedLowry base: a substance that accepts a hydrogen ion, H + Arrhenius acid: produces H + Arrhenius base: produces OH BrønstedLowry acid: donates H + BrønstedLowry base: accepts H + BrønstedLowry Acids HCl donates its H + to water producing H 3 O + and Cl By donating the H +, HCl is acting as the acid in this reaction. By accepting the H +, water is acting as a base in this reaction.
7 BrønstedLowry acid: donates H + BrønstedLowry base: accepts H + BrønstedLowry Bases Water: a BL acid and base Water gives an H + to NH 3 forming NH 4 + and OH Water can act as both a BronstedLowry acid or base depending on what it reacts with. NH 3 acts as the base by accepting the H + Water acts as the acid by donating the H+ BrønstedLowry acid: donates H + BrønstedLowry acid: donates H + BrønstedLowry base: accepts H + BrønstedLowry base: accepts H + Practice Practice Identify the reactant that is a BronstedLowry acid and the reactant that is a BronstedLowry base: Identify the reactant that is a BronstedLowry acid and the reactant that is a BronstedLowry base: HBr(aq) + H 2 O(l ) H 3 O + (aq) + Br (aq) CN (aq) + H 2 O(l ) HCN(aq) + OH (aq)
8 Conjugate AcidBase Pairs According to BronstedLowry theory, a conjugate acidbase pair consists of molecules or ions related by the loss of one H + by an acid, and the gain of one H + by a base. Every acidbase reaction contains two conjugate acidbase pairs because an H + is transferred in both the forward and reverse directions. Conjugate AcidBase Pairs When the base H 2 O gains an H +, its conjugate acid, H 3 O + is formed. Conjugate AcidBase Pairs When an acid such as HF loses one H +, it becomes F. HF is the acid, and F is its conjugate base. * The conjugate is always what is formed by donating or accepting H +. So it is always on the products side. Conjugate AcidBase Pairs Now if we combine the two previous examples:
9 Conjugate AcidBase Pairs Amphoteric Substances Water can act like an acid when it donates H + or as a base when it receives H + Substances that can act as both acids and bases are amphoteric. Water is the most common amphoteric substance and its behavior depends on the other reactant. Water will donate H + when mixed with a base and will accept H + when mixed with an acid. Amphoteric Substances Practice Another example of an amphoteric substance is bicarbonate, HCO 3. With a base, HCO 3 acts as an acid and donates H + to give CO 3. With an acid, HCO 3 acts as a base and accepts H + to give H 2 CO 3 Identify the conjugate acidbase pairs in the following reaction: HBr(aq) + NH 3 (aq) Br (aq) + NH + 4 (aq)
10 Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 AcidBase Titration 11.9 Buffers Strong vs Weak In the process called dissociation, an acid or base separates into ions in water. The strength of an acid is determined by the moles of H 3 O + that are produced for each mole of acid that dissolves. The strength of a base is determined by the moles of OH that are produced for each mole of base that dissolves. Strong acids and bases dissociate completely in water. Weak acids and bases dissociate only slightly, leaving most of the initial acid or base undissociated Strengths of Acids and Bases Write equations for the dissociation of strong and weak acids; identify the direction of reaction. Strong Acids Strong acids are examples of strong electrolytes because they donate H + so easily that their dissociate in water is essentially complete. When HCl (a strong acid) dissociates in water, H + is transferred to H 2 O. The resulting solution contains essentially only H 3 O + and Cl. Thus one mole of a strong acid dissociates in water to yield one mole of H3O+ and one mole of its conjugate base. We write the equation for a strong acid, such as HCl, with a single arrow.
11 Weak Acids Weak acids are weak electrolytes because they dissociate slightly in water, forming only a small amount of H 3 O + ions. When acetic acid dissociates in water, it donates the H+ to water. However, only part of the acetic acid molecules dissociate into ions. Most remain as molecules. Thus one mole of a weak acid partially dissociates in water to give less than a mole of H 3 O + and C 2 H 3 O2 We write the equation for a weak acid in aqueous solutions with a double arrow to indicate that the forward and reverse reactions are at equilibrium. Strong and Weak Acids The rest are weak acids. Strong and Weak Acids There are only 6 common strong acids: Hydroiodic acid HI Heavily regulated Hydrobromic acid HBr Used to make other molecules and extracting ore Perchloric acid HClO 4 Rocket fuel ingredient Hydrochloric acid HCl Stomach acid Sulfuric acid H 2 SO 4 Drain cleaner, leadacid batteries Nitric acid HNO 3 Explosives ingredient
12 Diprotic Acids Some weak acids, such as carbonic acid, are diprotic acids that have two H +, that dissociate one at a time. For example, carbonated soft drinks are prepared by dissolving CO 2 in water to form carbonic acid, H 2 CO 3. H 2 CO 3 dissociates partially into HCO 3 and H + in water: H 2 CO 3 (aq) + H 2 O(l) H 3 O + (aq) + HCO 3 (aq) HCO 3 is also a weak acid and will partially dissociate into CO 2 3 and H + HCO 3 (aq) + H2 O(l) H 3 O + (aq) + CO 2 3 (aq) Acid Summary A strong acid in water dissociates completely into ions. A weak acid in water dissociates only slightly into a few ions but remains mostly as molecules. Strong acid: HI(aq) + H 2 O(l) H 3O+(aq) + I (aq) Weak acid: HF(aq) + H 2 O(l) H 3 O+(aq) + F (aq) Diprotic Acids Sulfuric acid, H 2 SO 4, (a strong acid) is also a diprotic acid. H 2 OS 4 will dissociate completely into H + and HSO 4 : H 2 SO 4 (aq) + H 2 O(l) H 3 O + (aq) + HSO 4 (aq) HSO 4 is a weak acid and dissociates only partially: HSO 4 (aq) + H2 O(l) H 3 O + (aq) + SO 4 2 (aq) Bases As strong electrolytes, strong bases dissociate completely in water. KOH(s) K+(aq) + OH(aq) Weak bases are weak electrolytes that are poor H+ acceptors and produce very few ions in solution. NH 3 (g) + H 2 O(l) NH 4 + (aq) + OH (aq)
13 Bases in household products Practice By comparing their relative strengths, we can determine the direction of a reaction. H 2 SO 4 (aq) + H 2 O(l) H 3 O + (aq) + HSO 4 (aq) Direction of Reaction There is a relationship between the components of each conjugate acidbase pair: Strong acids have weak conjugate bases. As the strength of the acid decreases, the strengths of the base increases. In any acidbase reaction, there are two acids and two bases. However one acid is stronger than the other acid. And one base is stronger than the other base. H 3 SO 4 (aq) + H 2 O(l) H 3 O + (aq) + HSO 4 (aq) Practice Which direction will the reaction favor? CO 3 2 (aq) + H2 O(l) HCO 3 (aq) + OH (aq)
14 Practice Which direction will the reaction favor? HF(aq) + H 2 O(l) H 3O + (aq) + F (aq) 11.4 Dissociation Constants for Acids and Bases Write the expression for the dissociation constant of a weak acid or weak base. Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 AcidBase Titration 11.9 Buffers As we have seen, acids have different strengths depending on how much they dissociate in water. Because the dissociation of strong acids in water is essentially complete, the reaction is not considered to be an equilibrium situation. However, because weak acids in water dissociate only slightly, the ion products reach equilibrium with the undissociated weak acid molecules.
15 Formic acid HCHO 2, the acid found in bee and ant stings, is a weak acid. It dissociates in water to form hydronium ion, H 3 O +, and formate ions CHO 2 Practice Write the equilibrium expression. HCHO 2 (aq) + H 2 O(l) H 3 O + (aq) + CHO 2 (aq) * Only (aq) states are included in equilibrium expressions. (s) and (l) are ignored (including water). Writing Dissociation Constant Expressions Because weak acids and bases reach an equilibrium when mixed in water, we can write an equilibrium constant expression (just like in ch. 10). aa + bb cc + dd K a = [ ] = [ ] [ ] [ ] [ ] [ ] K a is called the acid dissociation constant. Writing Dissociation Constants An equilibrium expression can also be written for weak bases: CH 3 N 2 (aq) + H 2 O(l) CH 3 NH 3 + (aq) + OH (aq) Kb = [ ] = [ ] * Only (aq) states are included in equilibrium expressions. (s) and (l) are ignored (including water).
16 Dissociation Constants Just like in chapter 10, K s less than 1 indicate that there is more reactant than product. Which is in agreement of how we defined weak acids and weak bases. (Mostly molecules (reactants) and a small amount of ions (products)). Strong acids and bases have very large K s because its almost 100% dissociated. These K s are not usually bothered with. Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 AcidBase Titration 11.9 Buffers
17 11.5 Dissociation of Water Use the water dissociation constant expressions to calculate the [H 3 O + ] and [OH ] in an aqueous solution. Water In many acidbase reactions, water is amphoteric, which means tat it can act either as an acid or a base. In pure water, there is a forward reaction between two water molecules that transfers H + from one water molecule to the other. One molecule acts as an acid by losing H+ and the other water molecule that gains H + acts as the base. Every time H+ is transferred between 2 water molecules, the products are one H3O+ and one OH, which reacts in the reverse direction to reform two water molecules. In this section, we will use the dissociation constant expression and apply it to a very important equilibrium reaction: water reacting with itself. Water Dissociation Constant, K w H 2 O(l) + H 2 O(l) H 3 O + (aq) + OH (aq) Kw = Experiments show that in pure water and 25 C, *ignore (s) and (l) [H3O+] = [OH] = If we plug the concentrations back into Kw: Kw =
18 Neutral, Acidic, and Basic Solutions The K w applies to any aqueous solution at 25 C because all aqueous solutions contain H 3 O + and OH. When [H 3 O + ] and [OH ] in a solution are equal, the solution is neutral. However most solutions are not neutral; they have different concentrations of [H 3 O + ] and [OH ]. Neutral, Acidic, and Basic Solutions If acid is added to water, there is an increase in [H 3 O + ] and a decrease in [OH ], which makes it an acidic solution. If base is added to water, [OH ] increases and [H 3 O + ] decreases, which gives a basic solution. However for any aqueous solution, whether it is neutral, acidic, or basic, [H 3 O + ][OH ] = 1.0 x 1014 Using K w to calculate [H 3 O + ] and [OH ] If we know [H 3 O + ], we can use K w to calculate [OH ] or if we know [OH ] we can use K w to calculate [H 3 O + ]. Kw = [H 3 O + ][OH ] [OH ] = [ ] [H 3 O + ] = [ ]
19 Practice A vinegar solution has a [OH ] = 5.0 x M at 25 C. What is [H 3 O + ] of the vinegar solution? Is the solution acidic, basic, or neutral? Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 Buffers Practice What is the [H 3 O + ] of an ammonia cleaning solution with [OH ] = 4.0 x 10 4 M? Is the solution acidic, basic, or neutral? 11.6 The ph Scale Calculate ph from [H 3 O + ]; given the ph, calculate the [H 3 O + ] and [OH ] of a solution.
20 ph Scale Although we have expressed H 3 O + and OH as molar concentrations, it is more convenient to describe the acidity of solutions using the ph scale. On this scale, a number between 0to14represents the [H 3 O + ] concentration for common solutions Acidic solution ph less than 7.0 Neutral solution ph = 7.0 Basic solution ph greater than 7.0 ph Scale When an acid is added to water, the [H 3 O + ] (acidity) of the solution increases, but the ph decreases. When a base is added to pure water, it becomes more basic. Which means the acidity decreases and the ph increases. Calculating the ph of Solutions The ph scale is a logarithmic scale that corresponds to the [H 3 O + ] of aqueous solutions. ph = log[h 3 O + ]
21 Calculating the ph of Solutions ph = log[h 3 O + ] Because ph is a logarithmic scale, a change of 1.0 ph unit corresponds to a 10x in [H 3 O + ]. Practice What is the ph of bleach with [H 3 O + ] = 4.2 x M? ph = log[h 3 O + ] Practice If a solution of aspirin (acetylsalicylic acid) has a [H 3 O + ] = 1.7 x 10 3 M, what is the ph of the solution? ph = log[h 3 O + ] Practice ph can still be calculated if we are given [OH ] instead of [H 3 O + ]. What is the ph of an ammonia solution with [OH ] = 3.7 x 10 3 M ph = log[h 3 O + ] K w = [H 3 O + ][OH ] = 1.0 x 10 14
22 Practice Calculate the ph of a sample of bile that has [OH ] = 1.3 x 10 6 M K w = [H 3 O + ][OH ] = 1.0 x ph = log[h 3 O + ] Practice If the ph of a solution is 3.0, what is [H 3 O + ]? [H 3 O + ] = 10 ph Calculating [H 3 O + ] from ph If we have ph, we can calculate [H 3 O + ]: ph = log[h 3 O + ] [H 3 O + ] = 10 ph Practice Calculate [H 3 O + ] for a urine sample, which has a ph of 7.5. [H 3 O + ] = 10 ph
23 Practice What are the [H 3 O + ] and [OH ] of Diet Coke that has a ph of 3.17? [H 3 O + ] = 10 ph K w = [H 3 O + ][OH ] = 1.0 x Reactions of Acids and Bases Write balanced equations for reactions of acids with metals, carbonate or bicarbonates, and bases. Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 Buffers Salt Salt: an ionic compound that does not have H + as the cation or OH as the anion. Salts Not Salts KCl NaOH NaCl HCl CaCl 2 H 2 S FeS Ca(OH) 2
24 Acids react with Metals Acids react with certain metals to produce hydrogen gas (H 2 ) and a salt. Active metals include: K, Na, Ca, Mg, Al, Zn, Fe, and Sn. In these single replacement reactions, the metal ion replaces the hydrogen in the acid. Mg(s)+2HCl(aq) H 2 (g) + MgCl 2 (aq) Zn(s) + 2HNO 3 (aq) H 2 (g) + Zn(NO 3 ) 2 (aq) Acids react with Carbonates and Bicarbonates 2HCl(aq)+Na 2 CO 3 (aq) CO 2 (g) +H 2 O(l) + 2NaCl(aq) The acid reacts with CO 2 3 or HCO 3 to produce carbonic acid, H 2 CO 3,which breaks down into CO 2 and H 2 O. Acids react with Carbonates and Bicarbonates When an acid is added to a carbonate (CO 2 3 ) or bicarbonate (HCO 3 ), the products are carbon dioxide gas, water, and a salt. 2HCl(aq)+Na 2 CO 3 (aq) CO 2 (g) +H 2 O(l) + 2NaCl(aq) HBr(aq) + NaHCO 3 (aq) CO 2 (g) + H 2 O(l) + NaBr(aq) Acids and Hydroxides: Neutralization Neutralization: is a reaction between a strong or weak acid with a strong base combine to form water. HCl(aq) + NaOH(aq) H 2 O(l) + NaCl(aq) The H + from the acid and OH from the base form H 2 O. The salt is the base s cation and acid s anion.
25 Balancing Neutralization Equations In a neutralization reaction, one H + always reacts with one OH. Therefore, a neutralization may need coefficients to balance the H + from the acid with the OH from the base. 2HCl(a) + Mg(OH) 2 (aq) 2H 2 O(l) + MgCl 2 (aq) Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 Buffers Practice Write the balanced equation for the neutralization of HCl(aq) and Ba(OH) 2 (s) Buffers Describe the role of buffers in maintaining the ph of a solution; calculate the ph of a buffer.
26 Buffers The ph of water and most solutions changes drastically when a small amount of acid or base is added. However, when an acid or base is added to a buffer solution, there is little change in ph. A buffer solution maintains the ph of a solution by neutralizing small amounts of acids and base. Buffers in the Blood If the ph of the blood plasma goes slightly above or below 7.4, changes in our oxygen levels and our metabolic processes can be drastic enough to cause death. Even though we obtain acids and bases from foods and cellular reactions, the buggers in the body absorb those compounds so effectively that the ph of our blood plasma remains essentially unchanged. Buffers in the Blood In the human body, blood contains plasma, white blood cells and platelets, and red blood cells. The plasma contains buffers that maintain a consistent ph of about 7.4. Buffers In a buffer, an acid is present to react with any OH that is added, and a base is present to react with any H + (H 3 O + ) that is added. However, the acid and base must not neutralize each other. Therefore a combination of an acidbase conjugate pair (HA/A ) is used in a buffer. Most buffer solutions consist of nearly equal concentrations of a weak acid and its conjugate base. Or a weak base and its conjugate acid Common buffers: HC 2 H 3 O 2 /C 2 H 3 O 2 H 2 PO 4 /HPO4 2 HPO 2 4 /PO4 3 HCO 3 /CO3 2 NH + 4 /NH3
27 Preparing a Buffer A typical buffer can be made from a weak acid, such as acetic acid (HC 2 H 3 O 2 ) and its salt, sodium acetate (NaC 2 H 3 O 2, written C 2 H 3 O 2 ) As a weak acid, acetic acid dissociates slightly in water to form H 3 O + and a very small amount of C 2 H 3 O 2. HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) For the buffer to work, more C 2 H 3 O 2 is needed so NaC 2 H 3 O 2 is also added to the solution. NaC 2 H 3 O 2 Na + + C 2 H 3 O 2 Using a Buffer How the buffer maintains the [H 3 O + ] (balances the ph) If a small amount of base (OH ) is added, it is neutralized by the acetic acid: HC 2 H 3 O 2 + OH H 2 O + C 2 H 3 O 2 [H 3 O + ] and thus ph of the solution remains the same. Using a Buffer How the buffer maintains the [H 3 O + ] (to balance the ph) When a small amount of acid is added, the additional H 3 O + combines with the acetate ion, C 2 H 3 O 2 : HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) The new H 3 O + is used up to make more reactant which maintains ph. Calculating the ph of a Buffer HC 2 H 3 O 2 (aq) +H 2 O(l) H 3 O + (aq)+c 2 H 3 O 2 (aq) K a = [ ] [ ] By solving for [H3O+] we can obtain the ratio of acetic acid/acetate buffer: [H 3 O + ] = K a x [ ] [ ]
28 Practice The K a for acetic acid (HC 2 H 3 O 2 ) is 1.8 x What is the ph of a buffer prepared with 1.0M HC 2 H 3 O 2 and 1.0M C 2 H 3 O 2? HC 2 H 3 O 2 (aq) +H 2 O(l) H 3 O + (aq)+c 2 H 3 O 2 (aq) Buffering Capacity [H 3 O + ] = Ka x [ ] [ ] Because Ka is constant at a given temperature, [H 3 O + ] (and therefore ph) is determined by the [weak acid]/[conj. Base] ratio. As long as the addition of small amounts of either acid or base changes the ratio only slightly, the changes in [H 3 O + ] will be small and the ph will be maintained. If a large amount of acid or base is added, the buffering capacity of the system may be exceeded. Practice One of the conjugate acidbase pairs that buffers the blood is H 2 PO 4 /HPO4 2, which has a K a of 6.2 x What is the ph of a buffer that is prepared from 0.10 M H 2 PO 4 and 0.50 M HPO 2 4 Chapter 11 Acids and Bases 11.1 Acids and Bases 11.2 BrønstedLowry Acids and Bases 11.3 Strengths of Acids and Bases 11.4 Dissociation Constants for Acids and Bases 11.5 Dissociation of Water 11.6 The ph Scale 11.7 Reactions of Acids and Bases 11.8 Buffers
29
Acids and Bases. Acids and Bases in. our Lives. Acids and Bases in our Lives. Acids and Bases in our Lives. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives We produce lactic acid in our muscles when we exercise. Acid from bacteria turns milks sour in the products of yogurt and cottage cheese. We have
More informationAcids and Bases. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationAcids and Bases. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationAcids and Bases. Acids and Bases in our Lives. Chapter 11
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
More informationChemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
More informationChapter 11. Acids and Bases. Lecture Presentation. Karen C. Timberlake Pearson Education, Inc.
Lecture Presentation Chapter 11 Acids and Bases Chapter 11 Acids and Bases Clinical laboratory technicians prepare specimens for the detection of cancerous tumors and type blood samples for transfusions.
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
More informationAcids and Bases. Properties, Reactions, ph, and Titration
Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some
More informationAcids and Bases. Feb 28 4:40 PM
Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to
More informationChapter 14 Acids and Bases
Chapter 14 Acids and Bases Acids and bases are important substances in health, industry, and the environment. One of the most common characteristics of acids is their sour taste. In 1887, the Swedish chemist
More informationChapter 16 - Acids and Bases
Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:
More informationChapter 15 - Acids and Bases Fundamental Concepts
Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationAcids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationChapter 14 Acids and Bases
Chapter 14 Acids and Bases General Properties of Acids 1. An acid tastes sour - acidus = Latin, sour; acetum= Latin, vinegar 2. An acid turns indicator dye litmus from blue to red. 3. An acid reacts with
More informationCHAPTER 19. Acids, Bases, and Salts Acid Base Theories
CHAPTER 19 Acids, Bases, and Salts 19.1 Acid Base Theories ACIDS tart or sour taste Electrolytes Strong acids are corrosive Acid Facts... indicators will change color Blue litmus paper turns pink react
More informationElectrolytes, Acids and Bases ) 3
Chapter 15 Acid (Latin acidus - sour): sour taste; turns plant dye litmus red; dissolves metals producing H 2 gas. Substances that are neither acids nor bases were called neutral substances. Electrolytes,
More informationChem 30A. Ch 14. Acids and Bases
Chem 30A Ch 14. Acids and Bases Acids and Bases Acids and Bases Acids Sour taste Dissolve many metals Turn litmus paper red. Egs. Ace9c acid (vinegar), citric acid (lemons) Bases Bi>er taste, slippery
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic sour milk, sore muscles acetic vinegar phosphoric soft drinks citric citrus fruits malic apples PROPERTIES OF ACIDS PROPERTIES OF BASES 1. Taste sour 1. Taste bitter 2. react
More informationWhat are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced
What are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced materials? Historically, classified by their observable
More informationAcids and Bases. Acid. Acid Base 2016 OTHS. Acid Properties. A compound that produces H + ions when dissolved in water. Examples!
Acids and Bases Acid A compound that produces H + ions when dissolved in water. Examples! Vinegar Acetic acid Lemon Juice Citric acid Sour Candy Malic acid (and others) Milk Lactic acid HCl(aq) Acid Properties
More informationO + (aq) In this reaction, the water molecule is a Brønsted-Lowry base. It accepts a proton from HF to form H 3
AcidBase Reactions Key Terms conjugate base conjugate acid amphoteric neutralization salt In the previous sections, you learned about three acidbase theories: Arrhenius, BrønstedLowry, and Lewis. The BrønstedLowry
More informationLesson Five: Acids, Bases, ph, and Buffers
Lesson Five: Acids, Bases, ph, and Buffers Arrhenius Acids and Bases Acids and bases can be defined a number of ways. One of the oldest and most common ways is the definition according to Arrhenius, named
More informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationDefinition of Acid. HCl + H 2 O H 3 O + + Cl
Acids Definition of Acid Acids are substances that contain H + ions that ionize when dissolved in water. Arrhenius acid: a compound that increases the concentration of H + ions that are present when added
More informationPrinciples of Reactivity: The Chemistry of Acids and Bases. Acids, Bases and Arrhenius
Principles of Reactivity: The Chemistry of Acids and Bases **a lot of calculations in this chapter will be done on the chalkboard Do not rely on these notes for all the material** Acids, Bases and Arrhenius
More informationAcids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.
Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others
More informationINTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin
Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Acids and Bases Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water.
More informationAcids. Names of Acids. Naming Some Common Acids. Solution. Learning Check Acids and Bases. Arrhenius acids Produce H + ions in water.
Chapter 10 Acids and Bases Acids 10.1 Acids and Bases Arrhenius acids Produce H + ions in water. H 2 O HCl(g) H + (aq) + Cl (aq) Are electrolytes. Have a sour taste. Turn litmus red. Neutralize bases.
More informationUnit 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
More informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
More informationDefinition of Acid. HCl + H 2 O H 3 O + + Cl
Acids Definition of Acid Acids are substances that contain H + ions that ionize when dissolved in water. Arrhenius acid: a compound that increases the concentration of H + ions that are present when added
More informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY
ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationChapter 9 Acid-base reactions
CHEM, 2nd edition Cengage Learning Chapter 9 Acid-base reactions Acids and bases are chemical compounds that occur regularly in 'everyday life'. These two types of substances have opposite properties.
More informationCHAPTER Acid & Base
CHAPTER 19 19.1 Acid & Base Common Reactions with Acids Dilute: small amount of solute 1-M Concentrated: large amount of solute Indicator: changes color to show the presence of acids or bases : eat or
More informationName. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com
Periodic Table Name Academic Chemistry Acids & Bases Notes Unit #14 Test Date: 20 cincochem.pbworks.com Acid Base cincochem.pbworks.com Notes Find ph To go from [H 3 O + ] to ph EXAMPLE: [H 3 O + ] = 3.23
More informationChapter 14: Acids and Bases
Chemistry 12 Ch 1 4 : Acids and Bases Page 1 Chapter 14: Acids and Bases Check MasteringChemistry Deadlines Acids and Bases: The sour taste of lemons and lime, the bite of sourdough bread, and the tang
More informationCHAPTER 14: ACIDS AND BASES
CHAPTER 14: ACIDS AND BASES Arrhenius Acids and Bases There are a few definitions of acids and bases, some are somewhat narrow and others are much broader. Arrhenius Acids dissociate when dissolved in
More informationChapter 6. Acids, Bases, and Acid-Base Reactions
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
More informationUNIT #11: Acids and Bases ph and poh Neutralization Reactions Oxidation and Reduction
NAME: UNIT #11: Acids and Bases ph and poh Neutralization Reactions Oxidation and Reduction 1. SELF-IONIZATION OF WATER a) Water molecules collide, causing a very small number to ionize in a reversible
More informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationDuncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) 1. hydro- - HF 2. root of
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More informationCh 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs.
Ch 18 Acids and Bases Big Idea: Acids and Bases can be defined in terms of hydrogen ions and hydroxide ions or in terms of electron pairs. Ch 18 - Acids and Bases I CAN: 1) Compare properties of acids
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationContents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationAcids and Bases Unit 11
Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
More informationName: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.
Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following
More informationUnit Nine Notes N C U9
Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release
More informationChapter 10. Acids and Bases
Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationProperties of Acids. Base Chemistry. Properties of Bases. Three Acid and Base Theories. 1) Arrhenius Theory. May 09, Naming Acids Review
May 09, 2013 Properties of Acids AcidAcid Base Chemistry Base Chemistry Taste sour Are strong or weak electrolytes React with bases to form water and salts React with active metals to produce H2 Turn litmus
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More information10/16/17 ACIDS AND BASES, DEFINED WATER IS AMPHOTERIC OUTLINE. 9.1 Properties of Acids and Bases. 9.2 ph. 9.3 Buffers
ACIDS AND BASES, DEFINED A hydrogen atom contains a proton and an electron, thus a hydrogen ion (H + ) is a proton: Acids: Proton (H + ) transfer between molecules is the basis of acid/base chemistry Ø
More informationACID-BASE EQUILIBRIA. Chapter 16
P a g e 1 Chapter 16 ACID-BASE EQUILIBRIA Nature of Acids and Bases Before we formally define acids and bases, let s examine their properties. Properties of Acids Sour taste Ability to dissolve many metals
More information*KEY* * KEY * Mr. Dolgos Regents Chemistry. NOTE PACKET Unit 9: Acids, Bases, & Salts
*KEY* * KEY * Mr. Dolgos Regents Chemistry NOTE PACKET Unit 9: Acids, Bases, & Salts 1 *KEY* Unit 9: Acids, Bases, & Salts *KEY* Unit Vocabulary: Amphoteric Arrhenius acid Arrhenius base Bronsted-Lowry
More informationChapter 9: Acids, Bases, and Salts
Chapter 9: Acids, Bases, and Salts 1 ARRHENIUS ACID An Arrhenius acid is any substance that provides hydrogen ions, H +, when dissolved in water. ARRHENIUS BASE An Arrhenius base is any substance that
More information11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
More informationAcids and Bases: Chapter 14 & 15
Acids and Bases: Chapter 14 & 15 HW: Read Ch 14: Fill in as much of the acid base table as you can, as you read Acid base conductivity and reactivity Conduc'vity Reac'vity Hydrochloric acid high high
More informationSection 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 2 Acid and Bases 3 Acid and Bases 4 Acids 5 Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain
More informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationAcids and Bases Unit 13
Acids and Bases Unit 13 Chemistry of Acids and Bases 1. Watch video and complete worksheet Standard Deviants Teaching Systems: Chemistry: Module 05: Acids and Bases http://app.discoveryeducation.com/player/view/asset
More informationAcids and Bases. There are a number of definitions of acids and bases we will use two of the most useful definitions for nursing applications.
Acids and Bases We all know that acids taste sour and bases taste bitter but is this definition useful when you as a nurse will need to determine if a patient is in acidosis? There are a number of definitions
More informationAcids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY
Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationPart One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow
CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
More informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
More informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
More informationThe Chemistry of Acids and Bases
The Chemistry of Acids and Bases 1 Acid and Bases 4 Acid and Bases 2 Acids Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce
More informationACIDS & BASES PROPERTIES OF ACIDS ACIDS PROPERTIES OF ACIDS PROPERTIES OF ACIDS 11/1/2016
SC STANDARD COVERED ACIDS & BASES Standard PS-3.7 Classify various solutions as acids or bases according to their physical properties, chemical properties (including neutralization and reaction with metals),
More informationSCH4U Chapter 8 review
Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic
More informationChapter Test B. Chapter: Acids and Bases
Assessment Chapter Test B Chapter: Acids and Bases PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the
More informationAqueous solutions of acids have a sour Aqueous solutions of bases taste bitter
Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties
More informationChapter Menu Chapter Menu
Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,
More informationAcids, Bases and ph Chapter 19
Acids, Bases and ph Chapter 19 Compounds That Become Acids When Dissolved in Water General Formula: HX H + X - monatomic or polyatomic anion Naming Acids (p. 250) Binary acids Hydro ic Acid HCl: Hydrochloric
More informationAcids and Bases. Chapters 20 and 21
Acids and Bases Chapters 20 and 21 Acid and Bases Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with
More informationAcids and Bases. Two important classification of compounds - Acids and Bases. Properties of BASES
ACIDS AND BASES Acids and Bases Two important classification of compounds - Acids and Bases Properties of ACIDS Taste Sour/Tart Stings and burns the skin Reacts with bases Turns blue litmus paper red Reacts
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationUnit 6: ACIDS AND BASES
Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric
More informationUnit 9. Acids, Bases, & Salts Acid/Base Equilibrium
Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals
More informationThe ph of aqueous salt solutions
The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2
More informationChemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
More informationACIDS AND BASES CONTINUED
ACIDS AND BASES CONTINUED WHAT HAPPENS WHEN AN ACID DISSOLVED IN WATER? Water acts as a Brønsted Lowry base and abstracts a proton (H+) from the acid. As a result, the conjugate base of the acid and a
More informationCHEMISTRY. Chapter 16 Acid-Base Equilibria
CHEMISTRY The Central Science 8 th Edition Chapter 16 Acid-Base Equilibria Kozet YAPSAKLI Why study acids bases? bases are common in the everyday world as well as in the lab. Some common acidic products
More informationAcid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.
Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators
More informationUnit 4 Toxins, Section IV, L17-22
Unit 4 Toxins, Section IV, L17-22 Lesson 17 Heartburn Lesson 18 Pass the Proton Lesson 19 phooey! Lesson 20 Watered Down Lesson 21 Neutral Territory Lesson 22 Drip Drop Acids and Bases What are the properties
More information15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.
15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More informationResources:
I. A/B General A. Definitions 1. Arrhenius 2. B-L 3. Lewis *H+=H3O+ B. Properties 1. Acid 2. Base II. ACIDS A. Types 1. Binary 2. Ternary 3. Acid Anhydride B. Protic 1. mono 2. di 3. tri C. Strengths 1.
More information8.1 Explaining the Properties of Acids & Bases. SCH4U - Chemistry, Gr. 12, University Prep
8.1 Explaining the Properties of Acids & Bases SCH4U - Chemistry, Gr. 12, University Prep Equilibrium & Acids & Bases 2 So far, we have looked at equilibrium of general chemical systems: We learned about
More informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationAims to increases students understanding of: History, nature and practice of chemistry. Applications and uses of chemistry
Aims to increases students understanding of: History, nature and practice of chemistry Applications and uses of chemistry Implications of chemistry for society and the environment 1. Definitions: Lavoisier
More informationUnit 12: Acids & Bases. Aim: What are the definitions and properties of an acid and a base? Properties of an Acid. Taste Sour.
Unit 12: Acids & Bases Aim: What are the definitions and properties of an acid and a base? Mar 23 12:08 PM Properties of an Acid 3. Are electrolytes. (Dissociate and conduct electricity when aq) 2. Turns
More informationName%% %Period%% % Precipitation+Reaction+Practice+
Name%% %Period%% % Precipitation+Reaction+Practice+ 1.%Write%a%balanced%equation%for%the%following%precipitation%reactions,%circle%the%precipitate%that%is% formed:% a) K 3 PO 4 %+%3%Sr(NO 3 ) 2 %% % %
More information