Acids & Bases pH. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0  10 -14 Kw=ionization constant for H2O.

Slides:

Advertisements

Similar presentations

Aqueous solutions & concepts of pH Chapter I. Ion Product constant - water A.  Acids→ hydronium ions (H 3 O+)  Bases → hydroxide ions (OH-) B.Self.

Advertisements

PH.

Ways to measure Acidity/Basicity What is pH? What is pOH?

Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0 

PH and pOH By: Sam F., Sam D., Rochani, Evan, Will, Sherry, Mariana.

Calculating pH and pOH. pH pH = - log [H + ] [H + ] = the hydrogen ion concentration pH: “potential of hydrogen” - A way of expressing the hydrogen ion.

pH scale Logarithmic scale expressing the H + concentration, [H + ]. If the pH changes by a factor of 1, the [H + ] changes by a factor of 10. pH =

A C I D - B A S E T I T R A T I O N A N D p H

Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.

What is pH?. Ion Product Constant for Water  H 2 O(l)  H + (aq) + OH - (aq)  Keq = Kw = [H + ] x [OH - ]  The ion product constant for water (Kw)

How is pH defined? The pH of a solution is the negative logarithm of the hydrogen-ion concentration. The pH may be represented mathematically, using the.

Acids/Bases. Properties of Acids pp 186 Properties of Bases pp 186.

Ch. 15 Titration And pH. Ionization of Water _____________________: two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.

Pg  Amphoteric substance: can act as an acid or as a base ◦ Water is the most common amphoteric substance  Self-ionization of water: H 2.

PH. The Ion product constant for water H 2 O (l) + H 2 O (l)  H 3 O + (aq) + OH − (aq) Dissociation of water is an equilibrium, and since liquid water.

Ch. 15 & 16 - Acids & Bases II. pH (p ) C. Johannesson.

PH ( power of hydronium ion). The pH scale is a way of expressing the strength of acids and bases. Instead of using very small numbers, we just use the.

NOTES: 19.2 – Hydrogen Ions & Acidity (pH and pOH)

C. Johannesson Ch. 15 & 16 - Acids & Bases II. pH (p )

 pH: The negative of the common logarithm of the hydronium ion concentration [H 3 O + ] ◦ pH stands for the French words pouvoir hydrogene, meaning “hydrogen.

A bit more on the pH scale. (molar concentrations of H + and OH - ions) ACIDS BASES Contain greater number of H+ ions than OH- ions pH of (0-6.9)) Contain.

Section 16.2 Determining the Acidity of a Solution 1.To understand and determine pH and pOH 2.To learn methods for measuring pH of a solution Objectives.

K w, pH, and pOH. IONIZATION OF WATER Water is capable of reacting with itself in an ionization reaction H 2 O (l) + H 2 O (l) ⇌ H 3 O + (aq) + OH - (aq)

[H 3 O + ] Aqueous Solutions Brackets means concentration (Molarity) 1x10 -7 M neutral 1x10 -5 M 1x10 -9 M acidic = > [OH - ] acid base M

PH. Ionization of Water  When compounds dissociate/ionize in an aqueous solution, they produce ions - hydronium (H 3 O + ) and hydroxide (OH - )  These.

Part two of acid/base pH calculations

Warm-Up 12/16/2016 A mixture of gases (NO2,CO2, SO2) is collected in a bottle. The partial pressure of NO2 is 1.25 atm, and the partial pressure of.

The pH Scale Hydronium & Hydroxide Ions (H3O+) (OH–) pH Scale

Aim # 5: How do we determine the acidity (or basicity) of a solution?

pH ACIDS, BASES and SALTS Acids Bases - “Call Me Maybe” pH and pOH:

Self Ionization of Water and the pH Scale

Ionization Constant of Water

Ch. 19 Acids & Bases II. pH.

Hydronium Ions and Hydroxide Ions

Hydronium Ions and Hydroxide Ions

Lesson 2 pH and pOH Acid Neutral Base.

Lesson 2 pH and pOH Acid Neutral Base.

Calculations with Acids and Bases

Chapter 9 Acids and Bases

Can you calculate for acids and bases?

Calculating Concentration

The pH Scale Hydronium & Hydroxide Ions (H3O+) (OH–) pH Scale

Chapter 15 Preview Lesson Starter Objectives

Acids & Bases II. pH.

pH Scale Definition of Acids and Bases

Unit 14 – Acid, Bases, & Salts

Unit 13 – Acid, Bases, & Salts

Calculating Concentration

4.11: pH and pOH Chemistry 12.

Ch. 15 & 16 - Acids & Bases II. pH (p ) C. Johannesson.

Calculating pH from the Water Constant

Ch – Acids & Bases II. pH (p. 644 – 658).

Warmup Put the following descriptors in the correct spaces on the Venn diagram…

Acids and Bases.

pH Calculations pH = -log[H+] 10-pH = [H+] pOH = -log[OH-]

PH and pOH Acid Neutral Base.

Unit 13 – Acid, Bases, & Salts

Powerpoint Jeopardy Category 1 Category 2 Category

Calculating pH and pOH.

Calculating pH (and pOH)

Unit 15 – Acid, Bases, & Salts

Unit 13 – Acid, Bases, & Salts

Unit 14 – Acid, Bases, & Salts

Unit 5- lecture 5 Using the pH scale to characterize acids and bases.

1)What is the pH of a M acid solution? pH = 3

Unit 13 – Acid, Bases, & Salts

Ch. 14 & 15 - Acids & Bases II. pH.

Presentation transcript:

Acids & Bases pH

Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0  Kw=ionization constant for H2O

Acidic or Basic [H 3 O + ][OH - ] = 1.0   ACIDIC [H+] is greater than [OH-] [H+] is greater than 1.0   BASIC [OH-] is greater than [H+] [H+] is less than 1.0  10 -7

Ionization of Water  Find the hydroxide ion concentration of 3.0  M HCl. [H 3 O + ][OH - ] = 1.0  [3.0  ][OH - ] = 1.0  [OH - ] = 3.3  M Acidic or basic? Acidic ([H+] > 1 EE -7)

Problem  Colas are slightly acidic. If the [H+] in a solution is 1.0 x M, is the solution acidic basic or neutral? What is the [OH-] of this solution? Known: [H+] = 1.0 x M Kw = [H+] x [OH-] = 1 x Answer 1: Because 1.0 x M is greater than 1.0 x M, the solution is acidic Answer 2: [OH-] = 1 x x = 1.0 x M

pH = -log [H + ] pH Scale 0 7 INCREASING ACIDITY NEUTRAL INCREASING BASICITY 14

pH Scale pH of Common Substances

pH Scale pH = -log [H + ] pOH = -log [OH - ] pH + pOH = 14 [ ] = concentration

pH Scale  What is the pH of M HNO 3 ? pH = -log[H + ] pH = -log[0.050] pH = 1.3 Acidic or basic? Acidic

pH Scale  What is the molarity (conc) of HBr in a solution that has a pOH of 9.6? pH + pOH = 14 pH = 14 pH = 4.4 Acidic pH = -log[H + ] 4.4 = -log[H + ] = log[H + ] (10 x key)= [H + ] [H + ] = 4.0  M HBr