'Weak acid strong base' presentation slideshows

Chemistry 100 - Chapter 17

Chemistry 100 - Chapter 17 . Applications of Aqueous Equilbria. The Common Ion Effect. Add sodium format e (HCOONa) to a solution of formic acid (HCOOH) that has already established equilibrium? HCOOH (aq) ? H + (aq) + HCOO - (aq) weak acid

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Chapter 15

Chapter 15. Applications of Equilibrium. Common Ions. An ion that is present in both An acid and its conjugate base HNO 2 and NaNO 2 A base and its conjugate acid NH 3 and NH 4 Cl This common ion effects the position of the equilibrium and the pH.

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Chapter 17

Chapter 17. Additional Aspects of Equilibria. Salt Solutions in Water Salt solutions completely ionize in H 2 O. If their ions can react with H 2 O to form H + of OH - , the pH of the solution will change.

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Chemistry, The Central Science , 10th edition AP edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

Chemistry, The Central Science , 10th edition AP edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten.

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Chapter 16: Applications of Aqueous Equilibria

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Chapter 18

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Topic 18- Acids and bases

Topic 18- Acids and bases. 18.1 Calculations involving acids and bases 18.2 Buffer solutions 18.3 Salt hydrolysis 18.4 Acid-base titrations 18.5 Indicators. 18.1 Calculations involving acids and bases. pH = -log[H + ] pOH = -log[OH - ] [H + ] = 10 -pH [ OH - ] = 10 -pOH

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Titrations. . .

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VOLUMETRIC ANALYSIS

VOLUMETRIC ANALYSIS Volumetric analysis is an analysis in which the amount of the unknown is calculated from a known volume of added solution. TITRATIONS In a titration, the titrant (solution with a known concentration of a reagent) area added to analyte until their reaction is complete.

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Acid Base Titrations

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Neutralization and Titration

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Ionization of water

Ionization of water. HOH( l) H + (aq) + OH - (aq) The reverse reaction is highly favored. Water at 25 ? C : [H + ] = 10 -7 moles/L [OH - ] = 10 -7 moles/L Since [H + ] = [OH - ], water is neutral [H + ] ? [OH - ] = equilibrium constant

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Acid-Base Reactions

Acid-Base Reactions. Strong and Weak Acids Titration Common Acid Names. Textbook section 4.3. What is an ACID?. Defined: ACID Produces H + ions in water solution BASE Produces OH - ions in water solution. Acid Characteristics: Sour Taste (lemon)

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Unit #3: Acids and Bases

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Titration Lab

Titration Lab. Weak Acid/Strong Base Example: 50.0 mL of 0.1000 M Acetic acid titrated against 0.1000 M NaOH. Initial pH (no OH -1 added). Here we will calculate pH using the K a and an I, ?, E table. We should expect an acidic pH, as no OH -1 has been added yet.

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Indicators

Indicators. Indicators. Weak acids, HIn, that have different colours in the undissociated form, HIn and the disscociated form In - . HIn (aq) H + (aq) + In - (aq). Methyl Orange. HIn (aq) H + (aq) + In - (aq). Add H + (aq) equilibrium to left red.

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CHAPTER 15

CHAPTER 15. AP CHEMISTRY. COMMON ION EFFECT. If you have HC 2 H 3 O 2 (aq) <=> H + (aq) + C 2 H 3 O 2 - (aq) What would happen if you added the salt NaC 2 H 3 O 2 ? Addition of C 2 H 3 O 2 - would cause the system to shift to the left This is called the COMMON-ION EFFECT

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Quiz on Ch. 14 and 15

Quiz on Ch. 14 and 15. What does pH measure? What are the terms for a liquid with a pH of 3, a pH of 7, and a pH 10 ? pH measures [H+] concentration in a solution 3= acid 10=base 7= neutral 2) An acid produces _ hydronium ___ ___ ions ___ when added to a solution

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Chapter 21 Section 2

Chapter 21 Section 2. Equivalence point - midpoint on vertical portion of a titration curve *when # of equiv of acid = # of equiv of base -page 617 and page 626. -neutralization reaction of strong acid and strong base gives equiv point of pH = 7

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