'Ph poh 14' presentation slideshows

power of hydrogen

power of hydrogen. pH scale. Logarithmic scale expressing H +1 concentration, [H +1 ] If pH changes by factor of 1, [H +1 ] changes by factor of 10 pH = -log[H +1 ]. Molarity to pH. To determine pH: express [H +1 ] in scientific notation

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UNIT IV

UNIT IV. pH. Ionization of Water. Pure distilled water still has a small conductivity. Why? 2H 2 O (l) + 59kJ H 3 O + (aq) + OH - (aq). Ionization of Water.

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Intro to Acids & Bases

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pH- p otential H ydrogen

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Calculating pH

Calculating pH. Students will calculate the pH of strong acid and base solutions. Show How Water Becomes an Acid and an Base at the Same Time. Explain How Water Becomes An Acid and a Base. Using an Equation H 2 O ? H + + OH -. What does it mean if an ion is put in brackets?.

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pH Scale

pH Scale. Determines concentration (strength) of an acid or base. Acids below 7 Bases above 7. [http://wps.prenhall.com/wps/media/objects/602/616516/Media_Assets/Chapter15/Text_Images/FG15_03.JPG]. pH Scale. Indicators show the pH level in the lab.

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Acids and Bases

Acids and Bases. Strong Acids, strong bases and pH. Bronsted -Lowry Model of Acids and Bases Acid is a proton donor, base is a proton acceptor. HB ( aq ) + A - ( aq ) ? HA ( aq ) + B - ( aq ) HA and HB are acids, A - and B - are bases

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Unit: Acids, Bases, and Solutions

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Hydrogen Ions and acidity

Hydrogen Ions and acidity. Unit 13 Chapter 19-2. 1 more definition of acids and bases. Lewis acids and bases Acid: accepts a pair of electrons Base: donates a pair of electrons. Self-ionization. A rxn where water molecules produce ions. Neutral Solutions.

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There is a formula to find pH pH = -log [H + ] or pH = -log [ H 3 O + ]

pH. pH. There is a formula to find pH pH = -log [H + ] or pH = -log [ H 3 O + ] (brackets around a substance means that substances concentration in molarity) To find the pH you need to H + concentration Most of the time you will get an acids concentration. Finding the [H + ].

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There is a formula to find pH pH = -log [H + ] or pH = -log [ H 3 O + ]

pH. pH. There is a formula to find pH pH = -log [H + ] or pH = -log [ H 3 O + ] (brackets around a substance means that substances concentration in molarity) To find the pH you need to H + concentration Most of the time you will get an acids concentration. Finding the [H + ].

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pOH

pOH. What is the [H + ]?. If the [H + ] = 1 x 10 -7 M, the pH = 7. That works well with acids, but what about bases? Consider sodium hydroxide: NaOH(aq) ? Na + + OH - What is the [H + ]?. We need a new formula!!. Since bases release hyroxides, OH - , we will calculate the pOH.

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Water

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Hydronium Ions and Hydroxide Ions, continued Neutral, Acidic, and Basic Solutions

Section 1 Aqueous Solutions and the Concept of pH. Chapter 15. Hydronium Ions and Hydroxide Ions, continued Neutral, Acidic, and Basic Solutions. Solutions in which [H 3 O + ] = [OH ? ] is neutral. Solutions in which the [H 3 O + ] > [OH ? ] are acidic. [H 3 O + ] > 1.0 ? 10 ? 7 M

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Acids and Bases - Calculations

Acids and Bases - Calculations. What if I have pH and want to find [H + ]?. We use the antilog [H + ] = antilog(-pH) In the calculator, 2 nd LOG negative value ) -.

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II. pH (p. 481 - 491)

Ch. 15 & 16 - Acids & Bases. II. pH (p. 481 - 491). H 2 O + H 2 O H 3 O + + OH -. A. Ionization of Water. K w = [H 3 O + ][OH - ] = 1.0 ? 10 -14. A. Ionization of Water. Find the hydroxide ion concentration of 3.0 ? 10 -2 M HCl. [H 3 O + ][OH - ] = 1.0 ? 10 -14

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pH of Solutions

pH of Solutions. Experiment # 44. Introduction. Purpose: To find the pH of several common solutions, noting the range of the ph scale, to study the relationship between conjugate pairs of acids & bases the action of buffers. Introduction.

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Calculating pH and pOH

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Previously in Chem104: the concept of K w the concept of the K w circle

Previously in Chem104: the concept of K w the concept of the K w circle p-functions (pH, pK a , pK w ) pH scale P-functions in calcs. Today in Chem104: How K a relates to K b and pK a to pK b More ways to use the K w circle

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Hydrogen Ions and Acidity

Hydrogen Ions and Acidity. Chapter 19.2. What is K w ?. K w is the equilibrium constant for the self-ionization of water Water molecules are in constant motion and can collide to create a hydronium ion and a hydroxide ion. Where does K w come from?. 2H 2 O (l) ? H 3 O + (aq) + OH - (aq)

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