Lecture 112/14/05 Exam 1 Wednesday:  Come early if you want extra time Review session today 4 – TSC 006.

Slides:

Advertisements

Similar presentations

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

Advertisements

Hydrogen Ions and Acidity The Ionization of Water and pH.

213 PHC. Acid-Base Equilibria (1) By the end of this lecture, you should be able to:  Define the pH of a solution.  Calculate the pH of strong acids.

Lecture 112/9/ Mix 0.2 L of 0.3 M Ca(NO 3 ) 2 and 0.2 L of 0.06 M NaF. Does a precipitate form? K sp (CaF 2 ) = 3.9 x Write the balanced.

Lecture 122/13/06 Seminar cancelled. Bronsted-Lowry Acids Proton donor (H + or H 3 O + ) Acidic vs. non-acidic protons Bronsted-Lowry Bases Proton acceptor.

Lecture 122/12/07. pH What is it? How do you measure it?

Lecture 132/15/06 Seminar: Friday 1:30 Will be around at 5 for questions.

Strong Acid-Base Calculations

Strength of Acids and Bases. What makes a strong acid or base?  The strength of an acid or base is based on how many acid or base particles break down.

Acid/Base Indicators Substance that changes color in the presence of an acid or a base – Red or Blue Litmus – Phenolphthalein (phth) – Bromothymol blue.

Chemistry Notes: pH Calculations Chemistry

  Water acts as both acid and base  Dissociates into H 3 O + and OH - ions  2H 2 O (l)  H 3 O + (aq) + OH - (aq)  Rewritten,  H 2 O (l) + H 2.

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 =

pH Scale Soren Sorensen ( ) pH Scale Acid Base Zumdahl, Zumdahl, DeCoste, World of Chemistry  2002, page 515 [H + ] pH

Section 16.2 Determining the Acidity of a Solution 1.To understand pH and pOH 2.To learn to find pH and pOH for various solutions 3.To use a calculator.

The pH Scale. pH Scale We use this scale to measure the strength of an acid or base. pH is defined as the –log[H+] pH can use the concentration of hydronium.

The pH Scale. [H + ]pHExample Acids 1 X HCl 1 x Stomach acid 1 x Lemon juice 1 x Vinegar 1 x Soda 1 x Rainwater.

In aqueous solution… In aqueous solution… HCl (aq)  H + (aq) + Cl - (aq) Acids Acids increase hydrogen ion concentration [H + ] Courtesy Christy Johannesson.

PH Scale & Indicators.

C. Johannesson Ch. 18- Acids & Bases II. pH. C. Johannesson A. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0 

Let’s take a look at water  2H 2 O  H 3 O + + OH -  [H 3 O + ][OH - ]= 1x M 2  [H 3 O + ]= 1x10 -7 M  [OH - ]= 1x10 -7 M  K w = 1x M.

Acids and Bases.

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.

pH Scale Soren Sorensen ( )

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

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

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.

PH And pOH. Water Water autoionizes H 2 O + H 2 O H 3 O+ + OH- Hydrogen ion concentration determines the acidity of the solution Kc = [H3O+][OH-] ionization.

CHAPTER 16 Acids and Bases The pH Scale The pH Scale Soil at a high pH makes hydrangea flowers pink Soil at a low pH makes hydrangea flowers blue.

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.

Acids & Bases Lesson 6 Strong Acid-Base Calculations.

Acid-Base Titration and pH l Aqueous Solution and the Concept of pH – Hydronium Ions and Hydroxide Ions – The pH Scale – Calculating Involving pH l Determining.

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

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 ]pH.

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

Understanding pH Sources:

Acids and Bases Bundle 4: Water.

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

Acids and Bases Calculating pH.

Ch. 19 Acids & Bases II. pH.

DO NOW... HINT...if log (x) = y, then x = 10y PH, pOH & logs!

Acids and Bases Bundle 4: Water.

Acids and Bases Bundle 4: Water.

Calculations with Acids and Bases

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

Strength of Acids & Bases Strong vs. Weak pH

Strength of Acids & Bases Strong vs. Weak pH

Acids & Bases II. pH.

CHAPTER 13 Acids and Bases 13.2 The pH Scale.

Unit 14 – Acid, Bases, & Salts

Unit 13 – Acid, Bases, & Salts

Acid/Base: pH and pOH.

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

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

Unit 13 – Acid, Bases, & Salts

PH and pOH Chem 332.

pOH and [OH-] Calculations

PH and pOH Chem 332 – O’Dette.

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.

Unit 13 – Acid, Bases, & Salts

DO NOW... HINT...if log (x) = y, then x = 10y

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

Power of hydrogen.

Presentation transcript:

Lecture 112/14/05 Exam 1 Wednesday:  Come early if you want extra time Review session today 4 – TSC 006

pH: Describes the concentration of H 3 O + pX = -log X pH = -log [H 3 O + ] [H 3 O + ] = 10 -pH So if [H 3 O + ] = M, pH = ? If pH = 6, [H 3 O + ] = ?

Autoionization of Water H 2 O + H 2 O ↔ H 3 O + + OH - K w = [H 3 O + ][OH - ] What is the definition of neutral, acidic, and basic solutions? Neutral: [H 3 O + ] = [OH - ] Acid: [H 3 O + ] >[OH - ] Base: [H 3 O + ] < [OH - ]

K w = [H 3 O + ][OH - ] THUS at 25°C, neutral pH = 7

T (°C)KwKw x x x x x x Neutral pH = 7.27 Neutral pH = 6.92

pH and pOH K w = [H 3 O + ][OH - ] At 25 °C =[H 3 O + ][OH - ] -log ( =[H 3 O + ][OH - ]) -log ( ) = -log([H 3 O + ][OH - ]) -log ( ) = -log[H 3 O + ]-log[OH - ] 14 = pH + pOH

How do you measure pH? What is the pH range? pH meter Indicator (color change)

pH of some common substances pH Bleach12.5 Baking soda8.4 Egg White7.7 Milk6.8 Unpolluted rain5.6 Coffee4.9 Coke2.9 Stomach acid1.2

Degree of ionization

pH of strong acid? What is the pH of a M HNO 3 solution?