Logarithms. The logarithm of a number is the number of times 10 must be multiplied by itself to equal that number.

Slides:

Advertisements

Similar presentations

Properties of acids Taste Sour (kids, don’t try this at home).

Advertisements

PH (potential of Hydrogen). According to the Bronsted-Lowry theory, both acids and bases are related to the concentration of hydrogen ions. Acids will.

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)

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

Ch.15: Acid-Base and pH Part 1.

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

Acids & Bases How We Measure Acids and Bases pH Blue Base.

What is the concentration of the solution?. What is in the flask?

Neutralization Reactions Reaction that occurs between an acid and a base. Example: HCl + NaOH  NaCl + H 2 O & Water Products always include: A “Salt”

Chapter 10 Acids and Bases

8.2 Strong and Weak Acids and Bases

Strong Acid-Base Calculations

TOPIC: pH Do Now: Identify as acid, base, salt, or covalent Electrolyte or Not 1. NaCl 6. CaI2 2. C2H5OH 7. HF 3. H2SO4 8. Mg(OH)2 4. NaOH 9. NH3 5. C12H22O11.

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

THE MATHEMATICS IN A TITRATION CURVE (WITH A LITTLE BASE 10 AND LOGARITHM ARITHMATIC ADDED)

Examples-pH and pOH. Example Find the pH of a 0.03 M solution of HBr.

Section 6.2 pg pH and pOH Calculations.

Chapter 10 Acids and Bases (10.1) Acid-Base Strength.

Here we’ll go over an example where a strong acid is mixed with a strong base, and we calculate the pH of the final mixture. Strong Acid–Strong Base Mixture.

Properties of acids n Taste Sour (kids, don’t try this at home). n Conduct electricity. n Some are strong, some are weak electrolytes. n React with metals.

Titrations of acids and bases. HA + H 2 O H 3 O + + A -

The pH Scale The Power or Potential of Hydrogen Topic 8.4.

PH – A Measure of Acidity and Basicity Logarithm: In mathematics, the logarithm of a number is the exponent to which another fixed value, the base, must.

Yesterday’s Homework. The concentration of either the H + ion or the OH - ion is given for three aqueous solutions at 298 o K. For each solution, calculate.

Ch. 18: Acids & Bases Sec. 18.3: What is pH?. Objectives n Explain the meaning of pH and pOH. n Relate pH and pOH to the ion product constant for water.

The Equilibrium of Weak Acids and Bases. The dissociation of an acidic or basic compound in aqueous solution produces ions that interact with water (REVIEW!)

Ch. 20 Acids and Bases. Observable Properties of Acids and Bases Sour Taste Electrolytes when in aqueous solution React with metals to produce Hydrogen.

* Name the following acids: * HI * HNO 3 * HCl * Write the formula for the following acids: * Hydrofluoric Acid * Nitrous Acid * Hydrobromic acid.

Acid Base Calculations Calculations involving pH Titration calculations.

Acid-Base Titration & pH Objectives 1.Describe the self-ionization of water 2.Define pH and give the pH of a neutral solution at 25 o C 3.Explain.

O 2 vs CO binding a heme. Understand and identify weak and strong electrolytes OWL – 7.6 o Strong electrolyte Dissolve & 100% Dissociate Strong electrolyte.

Acids and Bases pH and Associated Calculations

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.

ACIDS AND BASES a review. Arrhenius Acids and Bases Acids = H+, Bases = OH- Modified Acids = H3O+, Bases = OH-

Ch. 15 pH. What is pH? ► pH is a logarithmic measurement of how acidic a solution is. ► pH = “pouvoir hydrogen” = hydrogen power ► If the pH = 1 to 6.9,

Unit 3 Acids and Bases. Hydrogen ions and pH Ion product constant of water (K w ) H 2 O  H + + OH - In pure water : [H + ] = [OH - ] * [ ] are used to.

Chapter 16 Acid-Base Titration and pH. Aqueous Solutions and the Concept of pH Self-ionization of water – 2 water molecules produce a hydronium ion and.

1 Acid-Base Titration and pH Chapter Self-Ionization of water Two water molecules produce a hydronium ion and a hydroxide ion by transfer of a proton.

Yesterday’s Homework Page 611 # 19 Page 612 # 20.

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

Ch. 3 - pH.  Rate is low  # of hydronium ions = # of hydroxide ions Dissociation of water.

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.

Aqueous Solutions and the Concept of pH Section 15.1.

Strengths of Acids and Bases

The substances on the left side of the number line (from 0 to 7) are all acids. The substances on the right side of the number line (from 7 to 14) are.

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)

Acids & Bases Lesson 6 Strong Acid-Base Calculations.

Logarithms. The logarithm of a number is the number of times 10 must be multiplied by itself to equal that number.

Power of hydrogen. pH scale logarithmic scale expresses H +1 concentration, [H +1 ] pH = -log[H +1 ]pH = -log[H +1 ] If pH changes by factor of 1, [H.

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.

Objective/Warm-Up SWBAT describe reactions of acids and bases and discuss the pH scale. What is the molarity of sodium hydroxide if 20.0 ml of the solution.

Acids, Bases, and Solutions

Calculating pH SCH3U/4C Ms. richardson.

Unit 5: Acid-Base Calculations Lesson 4: Mixing Strong Acids + Bases

Calculating Concentration

Review Practice What is the molality of a solution created by adding 58 grams of magnesium hydroxide to 4 liters of water? Answer: 0.25 m Mg(OH)2 What.

Acids and Bases.

pH Scale Definition of Acids and Bases

Calculating Concentration

Acids and Bases.

Acids and Bases.

AP Chem Take out HW to be checked Today: Acid-Base Titrations.

PH and pOH Acid Neutral Base.

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

Ch. 15 & 16 - Acids & Bases III. Titration (p )

Power of hydrogen.

Presentation transcript:

Logarithms

The logarithm of a number is the number of times 10 must be multiplied by itself to equal that number.

Logarithms 1000 = 10 x 10 x 10 log 1000 = 3

Logarithms To find the logarithm of a number, count the zeroes. If the number is in scientific notation, look at the exponent.

Logarithms 1 = 1 x = 1 x = 1 x = 1 x = 1 x log 1 = 0 log 10 = 1 log 100 = 2 log 0.1 = -1 log 0.01 = -2

Logarithms You can multiply two numbers by adding their logarithms.

Logarithms You can multiply two numbers by adding their logarithms. 100 x 1000 = 100,000

Logarithms You can multiply two numbers by adding their logarithms. 100 x 1000 = 100, = 5

Logarithms You can multiply two numbers by adding their logarithms. 1 x 10 8 = 100,000,000

Logarithms You can multiply two numbers by adding their logarithms. 1 x 10 8 = 100,000, = 8

Logarithms You can multiply two numbers by adding their logarithms. 2 x 10 8 = 200,000,000 ? + 8 = ?

Logarithms So what’s the logarithm of 2? You have to look it up. 2 x 10 8 = 200,000,000 ? + 8 = ?

Logarithms So what’s the logarithm of 2? You have to look it up. 2 x 10 8 = 200,000, = 8.301

Logarithms What if the number is small instead of big?

Logarithms What if the number is small instead of big? = 3 x 10 -4

Logarithms What if the number is small instead of big? = 3 x log = log 3 + log 10 -4

Logarithms What if the number is small instead of big? = 3 x log = log 3 + log = – 4

Logarithms What if the number is small instead of big? = 3 x log = log 3 + log = – 4 =

Logarithms Try a few!

Logarithms log 10 3 =

Logarithms log 10 3 = 3

Logarithms log 10 8 =

Logarithms log 10 8 = 8

Logarithms log =

Logarithms log = -10

Logarithms log 2 =

Logarithms log 2 = 0.301

Logarithms log 5.8 =

Logarithms log 5.8 = 0.763

Logarithms log 9.2 =

Logarithms log 9.2 = 0.963

Logarithms log 4 x =

Logarithms log 4 x =

Logarithms log 4 x = =

Logarithms log 8.3 x 10 5 =

Logarithms log 8.3 x 10 5 =

Logarithms log 8.3 x 10 5 = = 5.919

Logarithms log 7.1 x =

Logarithms log 7.1 x =

Logarithms log 7.1 x = =

Logarithms log 4.8 x =

Logarithms log 4.8 x =

Logarithms log 4.8 x = =

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

[H + ] = What is the pH?

[H + ] = = 3.5 x 10 -3

[H + ] = = 3.5 x log = log log 10 -3

[H + ] = = 3.5 x log = log log = – 3

[H + ] = = 3.5 x log = log log = – 3 = –2.456

[H + ] = = 3.5 x log = log log = – 3 = –2.456 pH = 2.456

pH = 6.13 What is the [H + ]?

pH = 6.13 –pH = –6.13

pH = 6.13 –pH = –6.13 = 0.87 – 7

pH = 6.13 –pH = –6.13 = 0.87 – 7 [H + ] = 7.4 x 10 -7

pH = 8.7 What is the pOH?

pH = 8.7 pOH = 14 - pH

pH = 8.7 pOH = 14 - pH = 14 – 8.7

pH = 8.7 pOH = 14 - pH = 14 – 8.7 = 5.3

pH = 8.7 pOH = 14 - pH = 14 – 8.7 = 5.3 The solution is acidic.

Always Remember:

The molarity of a solution refers to how many moles per liter it has.

Always Remember: The molarity of a solution refers to how many moles per liter it has. 1.0 M = 1.0 mol/L

Always Remember: A strong acid or base dissociates completely in water.

Always Remember: A strong acid or base dissociates completely in water. 1.0 M HCl = 1.0 M H +

Always Remember: A strong acid or base dissociates completely in water. 1.0 M HCl = 1.0 M H M NaOH = 1.0 M OH -

Always Remember: Polyprotic acids have more than one hydrogen.

Always Remember: Polyprotic acids have more than one hydrogen. 1.0 M H 2 SO 4 = 2.0 M H +

Always Remember: Polyprotic acids have more than one hydrogen. 1.0 M H 2 SO 4 = 2.0 M H +.

Suggested Homework Page 609 # 18 Page 611 # 19 Page 612 # 20