19.2 Hydrogen Ions and Acidity > Chapter 19 Acids, Bases, and Salts Hydrogen Ions and Acidity Acid-Base Theories
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1 Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base Theories 19.2 Hydrogen Ions and Acidity 19.3 Strengths of Acids and Bases 19.4 Neutralization Reactions 19.5 Salts in Solution 1 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
2 CHEMISTRY & YOU What factors do you need to control so a fish has healthy water to live in? Goldfish can live for 20 years or more in an aquarium if the conditions are right. 2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
3 Hydrogen Ions from Water Hydrogen Ions from Water How are [H + ] and [OH ] related in an aqueous solution? 3 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
4 Hydrogen Ions from Water Water molecules are highly polar and are in constant motion, even at room temperature. On occasion, the collisions between water molecules are energetic enough for a reaction to occur. A water molecule that loses a hydrogen ion becomes a hydronium ion (H 3 O + ). A water molecule that loses a hydrogen ion becomes a hydroxide ion (OH ). 4 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
5 Hydrogen Ions from Water Self-Ionization of Water The reaction in which water molecules produce ions is called the self-ionization of water. In an aqueous solution, hydrogen ions are always joined to water molecules as hydronium ions. 5 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
6 Hydrogen Ions from Water Self-Ionization of Water In pure water at 25 C, the concentration of hydrogen ions is only M. The concentration of OH is also M because the numbers of H + and OH ions are equal in pure water. Any aqueous solution in which [H + ] and [OH ] are equal is a neutral solution. 6 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
7 Hydrogen Ions from Water Ion-Product Constant for Water The ionization of water is a reversible reaction, so Le Châtelier s principle applies. Adding either hydrogen ions or hydroxide ions to an aqueous solution is a stress on the system. In response, the equilibrium will shift toward the formation of water. The concentration of the other ion will decrease. 7 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
8 Hydrogen Ions from Water Ion-Product Constant for Water The ionization of water is a reversible reaction, so Le Châtelier s principle applies. In any aqueous solution, when [H + ] increases, [OH ] decreases. Likewise, when [H + ] decreases, [OH ] increases. 8 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
9 Hydrogen Ions from Water Ion-Product Constant for Water For aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals [H + ] + [OH ] = Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
10 Hydrogen Ions from Water Ion-Product Constant for Water The product of the concentrations of the hydrogen ions and the hydroxide ions in water is called the ion-product constant for water (K w ). K w = [H + ] [OH ] = Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
11 Hydrogen Ions from Water Ion-Product Constant for Water Acidic Solutions When some substances dissolve in water, they release hydrogen ions. HCl(aq) H + (aq) + Cl (aq) The hydrogen-ion concentration is greater than the hydroxide-ion concentration. A solution in which [H + ] is greater than [OH ] is an acidic solution. The [H + ] is greater than M. 11 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
12 Hydrogen Ions from Water Ion-Product Constant for Water Basic Solutions When sodium hydroxide dissolves in water, it forms hydroxide ions in solution. NaOH(aq) Na + (aq) + OH (aq) The hydrogen-ion concentration is less than the hydroxide-ion concentration. A basic solution is one in which [H+] is less than [OH ]. Basic solutions are also known as alkaline solutions. 12 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
![Sample Problem 19.2 Using the Ion-Product Constant for Water If the [H + ] in a solution is 1.](/docs-images/89/99400172/images/13-5.jpg "0 10 5 M, is the solution acidic, basic, or neutral? What is the [OH ] of this solution? 13 Copyright Pearson Education, Inc.")
13 Sample Problem 19.2 Using the Ion-Product Constant for Water If the [H + ] in a solution is M, is the solution acidic, basic, or neutral? What is the [OH ] of this solution? 13 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
14 Sample Problem Analyze List the knowns and the unknowns. Use the expression for the ion-product constant for water and the known concentration of hydrogen ions to find the concentration of hydroxide ions. KNOWNS UNKNOWNS [H + ] = M K w = Is the solution acidic, basic, or neutral? [OH ] =?M 14 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
15 Sample Problem Calculate Solve for the unknowns. Use [H + ] to determine whether the solution is acidic, basic, or neutral. [H + ] is M, which is greater than M. Thus, the solution is acidic. 15 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
16 Sample Problem Calculate Solve for the unknowns. Rearrange the expression for the ionproduct constant to solve for [OH ]. K w = [H + ] [OH ] [OH ] = K w [H + ] 16 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
17 Sample Problem Calculate Solve for the unknowns. Substitute the known values of [H + ] and K w. Then solve for [OH ]. [OH ] = = M When you divide numbers written in scientific notation, subtract the exponent in the denominator from the exponent in the numerator. 17 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
18 Sample Problem Evaluate Does the result make sense? If [H + ] is greater than M, then [OH ] must be less than M M is less than M. To check your calculation, multiply the values for [H + ] and [OH ] to make sure that the result equals Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
19 A solution does not have an equal number of H + and OH ions. What do you know about this solution? 19 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
20 A solution does not have an equal number of H + and OH ions. What do you know about this solution? You know that the solution is not neutral. Without knowing more information, you cannot say if it is acidic or basic (alkaline). 20 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
21 The ph Concept The ph Concept How is ph used to classify a solution as neutral, acidic, or basic? 21 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
22 The ph Concept Expressing hydrogen-ion concentration in molarity is not practical. A more widely used system for expressing [H + ] is the ph scale. The ph scale ranges from 0 to Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
23 The ph Concept Hydrogen Ions and ph The ph of a solution is the negative logarithm of the hydrogen-ion concentration. ph = log[h + ] 23 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
24 The ph Concept Hydrogen Ions and ph In pure water or a neutral solution, the [H + ] = M, and the ph is 7. ph = log( ) = (log 1 + log 10 7 ) = (0.0 + ( 7.0)) = 7.0 If the [H + ] of a solution is greater than M, the ph is less than 7.0. If the [H + ] is less than M, the ph is greater than Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
25 The ph Concept Hydrogen Ions and ph A solution with a ph less than 7.0 is acidic. A solution with a ph of 7.0 is neutral. A solution with a ph greater than 7.0 is basic. 25 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
26 Interpret Data Hydrogen Ions and ph When [H + ] is given in the format 1 10 n, it s easy to find the ph. It s just the absolute value of the exponent n. Also, note that [H + ] [OH ] always equals Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
27 CHEMISTRY & YOU In an aquarium, the ph of water is another factor that affects the ability of fish to survive. Most freshwater fish need a slightly acidic or neutral ph. For a saltwater tank, the ideal ph is slightly basic. What might explain this difference in the ideal ph range? 27 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
28 CHEMISTRY & YOU In an aquarium, the ph of water is another factor that affects the ability of fish to survive. Most freshwater fish need a slightly acidic or neutral ph. For a saltwater tank, the ideal ph is slightly basic. What might explain this difference in the ideal ph range? Natural freshwater is slightly acidic, while natural saltwater typically contains compounds that make it slightly basic. Fish have adapted to these conditions in the wild and need them replicated in their tanks. 28 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
29 The ph Concept Calculating ph from [H + ] Expressing [H + ] in scientific notation can make it easier to calculate ph. You would rewrite M as M. The coefficient 1.0 has two significant figures. The ph for this solution is The two numbers to the right of the decimal point represent the two significant figures in the concentration. 29 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
30 The ph Concept Calculating ph from [H + ] It is easy to find the ph for solutions when the coefficient is 1.0. The ph of the solution equals the exponent, with the sign changed from minus to plus. A solution with [H + ] = M has a ph of 2.0. When the coefficient is a number other than 1, you will need to use a calculator with a log function key to calculate ph. 30 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
31 Sample Problem 19.3 Calculating ph from [H + ] What is the ph of a solution with a hydrogen-ion concentration of M? 31 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
32 Sample Problem Analyze List the known and the unknown. To find the ph from the hydrogen-ion concentration, you use the equation ph = log[h + ]. KNOWN [H + ] = M UNKNOWN ph =? 32 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
33 Sample Problem Calculate Solve for the unknown. Start with the equation for finding ph from [H + ]. ph = log[h + ] 33 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
34 Sample Problem Calculate Solve for the unknown. Substitute the known [H + ] and use the log function on your calculator to calculate the ph. ph = log( ) = ( ) = Round the ph to two decimal places because the hydrogen-ion concentration has two significant figures. = Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
35 Sample Problem Evaluate Does the result make sense? The value of the hydrogen-ion concentration is between M and M. So, the calculated ph should be between 9 and 10, which it is. 35 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
36 The ph Concept Calculating [H + ] from ph You can calculate the hydrogen-ion concentration of a solution if you know the ph. If the ph is an integer, it is easy to find [H + ]. For a ph of 9.0, [H + ] = M. Most ph values are not whole numbers. When the ph value is not a whole number, you will need a calculator with an antilog (10 x ) function to get an accurate value for the hydrogen-ion concentration. 36 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
![Sample Problem 19.4 Calculating [H + ] from ph The ph of an unknown solution is 6.35.](/docs-images/89/99400172/images/37-4.jpg "What is the hydrogen-ion concentration of the solution? 37 Copyright Pearson Education, Inc.")
37 Sample Problem 19.4 Calculating [H + ] from ph The ph of an unknown solution is What is the hydrogen-ion concentration of the solution? 37 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
38 Sample Problem Analyze List the known and the unknown. You will use the antilog function of your calculator to find the concentration. KNOWN ph = 6.35 UNKNOWN [H + ] =?M 38 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
39 Sample Problem Calculate Solve for the unknown. First, simply swap the sides of the equation for finding ph and substitute the known value. ph = log[h + ] log[h + ] = ph log[h + ] = Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
40 Sample Problem Calculate Solve for the unknown. Change the signs on both sides of the equation and then solve for the unknown. log[h + ] = 6.35 [H + ] = antilog( 6.35) 40 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
41 Sample Problem Calculate Solve for the unknown. Use the antilog (10 x ) function on your calculator to find [H + ]. Report the answer in scientific notation. [H + ] = On most calculators, use the 2 nd or INV key followed by log to get the antilog. 41 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
42 Sample Problem Evaluate Does the result make sense? The ph is between 6 and 7. So, the hydrogen-ion concentration must be between M and M. The answer is rounded to two significant figures because the ph was measured to two decimal places. 42 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
43 The ph Concept Calculating ph from [OH ] If you know the [OH ] of a solution, you can find its ph. You can use the ion-product constant to determine [H + ] for a known [OH ]. Then you use [H + ] to calculate the ph. 43 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
![Sample Problem 19.5 Calculating ph from [OH ] What is the ph of a solution if [OH ] = 4.](/docs-images/89/99400172/images/44-3.jpg "0 10 11 M? 44 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.")
44 Sample Problem 19.5 Calculating ph from [OH ] What is the ph of a solution if [OH ] = M? 44 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
45 Sample Problem Analyze List the knowns and the unknown. To find [H + ], divide K w by the known [OH ]. Then calculate ph as you did in Sample Problem KNOWNS UNKNOWN [OH ] = M K w = ph=? 45 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
46 Sample Problem Calculate Solve for the unknown. Start with the ion-product constant to find [H + ]. Rearrange the equation to solve for [H + ]. K w = [OH ] [H + ] [H + ] = K w [OH ] 46 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
47 Sample Problem Calculate Solve for the unknown. Substitute the values for K w and [OH ] to find [H + ]. [H + ] = = M = M 47 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
48 Sample Problem Calculate Solve for the unknown. Next use the equation for finding ph. Substitute the value for [H + ]. ph = log[h + ] = log( ) Use a calculator to find the log. = ( ) = 3.60 Round the ph to two decimal places because the [OH ] has two significant figures. 48 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
49 Sample Problem Evaluate Does the result make sense? A solution in which [OH ] is less than M is acidic because [H + ] is greater than M. The hydrogen-ion concentration is between M and M. Thus, the ph should be between 3 and Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
50 Why do we use the ph scale to express hydrogen-ion concentration? 50 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
51 Why do we use the ph scale to express hydrogen-ion concentration? It is more convenient and practical to use the ph scale. Expressing hydrogen-ion concentration in molarity takes up a lot of space and is not as easy to work with. 51 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
52 Measuring ph Measuring ph What are two methods that are used to measure ph? 52 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
53 Measuring ph Either acid-base indicators or ph meters can be used to measure ph. 53 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
54 Measuring ph Acid-Base Indicators An indicator (HIn) is an acid or a base that dissociates in a known ph range. Indicators work because their acid form and base form have different colors in solution. The acid form of the indicator (HIn) is dominant at low ph and high [H + ]. The base form (In ) is dominant at high ph and high [OH ]. 54 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
55 Measuring ph Acid-Base Indicators The change from dominating acid form to dominating base form occurs within a narrow range of about two ph units. At all ph values below the range, you would see only the color of the acid form. At all ph values above this range, you would see only the color of the base form. 55 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
56 Interpret Graphs Acid-Base Indicators Many indicators are needed to span the entire ph spectrum. 56 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
57 Measuring ph Acid-Base Indicators An indicator strip is a piece of paper or plastic that has been soaked in an indicator and then dried. The paper is dipped into an unknown solution. The color that results is compared with a color chart to measure the ph. Some indicator paper has absorbed multiple indicators. The colors that result will cover a wide range of ph values. 57 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
58 Measuring ph Acid-Base Indicators Soil ph can affect how plants develop. In acidic soils, hydrangeas produce blue flowers. In basic soils, hydrangeas produce pink flowers. 58 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
59 Measuring ph ph Meters A ph meter is used to make rapid, continuous measurements of ph. The measurements of ph obtained with a ph meter are typically accurate to within 0.01 ph unit of the true ph. If the ph meter is connected to a computer or chart recorder, the user will have a record of the ph changes. 59 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
60 Measuring ph ph Meters A ph meter can be easier to use than liquid indicators or indicator strips. The ph reading is visible in a display window on the meter. The color and cloudiness of the solution do not affect the accuracy of the ph value obtained. 60 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
61 You re planting a garden and want to know the approximate ph of your soil. What method should you use? 61 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
62 You re planting a garden and want to know the approximate ph of your soil. What method should you use? While you could use a ph meter and have a very accurate reading of your soil s ph, it is also OK to approximate the ph using a ph indicator strip. 62 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
63 Key Concepts For aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals A solution with a ph less than 7.0 is acidic. A solution with a ph of 7 is neutral. A solution with a ph greater than 7.0 is basic. Either acid-base indicators or ph meters can be used to measure ph. 63 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
64 Glossary Terms self-ionization: a term describing the reaction in which two water molecules react to produce ions neutral solution: an aqueous solution in which the concentrations of hydrogen and hydroxide ions are equal; it has a ph of 7.0 ion-product constant for water (K w ): the product of the concentrations of hydrogen ions and hydroxide ions in water; it is at 25 C 64 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
65 Glossary Terms acidic solution: any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration basic solution: any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration ph: a number used to denote the hydrogenion concentration, or acidity, of a solution; it is the negative logarithm of the hydrogen-ion concentration of a solution 65 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
66 BIG IDEA Reactions The ph of a solution reflects the hydrogen-ion concentration. 66 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
67 END OF Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
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