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Acids and Bases
HA H + + A - HCL H + + CL - CH 3 COOH H + + CH 3 COO -
0.003M HCl 9M HNO 3 7M CH 3 COOH ethanoic acid or acetic acid 5% ethanoic acid (vinegar) Use dilute or concentrated and weak or strong to describe the acids above.
2H 2 O H 3 O + + OH - [H + ] [OH - ] [H 2 O] H 2 O H + + OH - K c = K w = [H + ] [OH - ] =
[H + ] for pure water is 1 X K w = [10 -7 ] [10 -7 ] = pH is -log [H + ] So the pH of pure water is 7
HA H + + A - H + + OH - H 2 O during titration Strong/weak acids cannot be differentiated by titration.
Mohr burette Remember to: Remove bubbles from the valve area Record data as you titrate including uncertainties What is the second burette for? Flush your burette with distilled water when finished
Acidic pH Basic pH Phenolphthalein
Acids and Bases! Acids and Bases (and calculations involving them) are essential to all areas of analytical chemistry!
EXPERIMENT (5) Preparation and Properties of Buffer Solution.
Buffers. A buffer is a solution whose pH is resistant to change on the addition of relatively small quantities of an acid or base. Buffers have the ability.
Lecture 142/19/06. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? NaOH CaO.
Strong Acids Strong acids fully dissociate so: They are fully separated into their ions They are good conductors of electricity Are not in a state of equilibrium.
Lecture 122/12/07. pH What is it? How do you measure it?
Titration Curves I. Strong Acid+ Strong Base 0.1 M HCl0.1 M NaOH 25.0 mL 2.5 x mol 1. Initial pH HCl H+H+ + Cl- 0.1 M [H + ] = 0.1 M pH =- log.
Calculate the pH of a solution that is 0.20 M in NaCH 3 COO and 0.10 M in CH 3 COOH
Strengths of Acids and Bases. Acids and bases are classified as strong or weak according to the degree to which they ionize in water. Strong acids.
Weak Acid-Strong Base And Strong Acid Weak Base. Arrhenius Acids and Bases Acids are a source of H + ions HCl (aq) H + (aq) + Cl - (aq) Bases are a.
Titrations of acids and bases. HA + H 2 O H 3 O + + A -
Calculate the pH of weak acids. calculate the pH of weak bases. Calculate the pH of salt of weak acids. Calculate the pH of salt of weak bases.
Acid/base chemistry Buffers Henderson-Hasselbalch equation.
Buffer Capacity Lab. Buffer Solutions A buffer solution is a solution that changes pH only slightly when small amounts of a strong acid or a strong base.
Obj. finish 17.2, ) The pH range is the range of pH values over which a buffer system works effectively. 2.) It is best to choose an acid with.
Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the.
PH. Hydrogen Ions and Acidity Water molecules go through self ionization to form hydrogen ion and hydroxide ions. In aqueous solution, hydrogen ions H.
BUFFERS Mixture of an acid and its conjugate base. Buffer solution resists change in pH when acids or bases are added or when dilution occurs. Mix: A.
Calculating pH of strong acids and bases. Strong acids or bases are those which dissociate completely. HCl(aq) + H 2 O(l) → H 3 O + (aq) + Cl - (aq) So.
Ch.15: Acid-Base and pH Part 1. Self-Ionization of Water Pure water is a VERY weak electrolyte It undergoes self-ionization H 2 O (l) + H 2 O (l) H 3.
Finding the pH of Weak Acids. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK Ionize completely.
ASİT. BAZ [H + ].[OH - ]=1x pH=-log[H + ] pOH=-log[OH - ] pH + pOH=14.
Lecture 122/18/05 There is class on Monday. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? Oxide (O 2- : CaO, Na 2 O) O.
Lecture 1: Introduction and review –Quiz 1 –Website: –Review of acid/base chemistry –Universal features of.
Lecture 152/22/06 Topics due. Neutralization: Acid + Base = Water + Salt pH of neutralized solution? Strong Acid + Strong Base HCl (aq) + NaOH (aq)
What do they have in common?. And finally ….. BUFFERS.
Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0
1 Acetic acid, has a K a of 1.7 x Determine the pH of a 0.10 M solution of acetic acid. Hint: First write out the equilibrium expression of the.
Describe the composition of a buffer solution and explain its action. What is a buffer solution? It is an aqueous solution that resists a change.
18.4 Acid-Base Titrations. Assessment Statement Sketch the general shapes of graphs of pH against volume for titrations involving strong and weak.
Strength of Acids and Alkalis By SK Chan. Why do acids/alkalis show different properties? Acid/AlkalipH value Electrical conductivity 0.1 M Ethanoic acid4Low.
Strengths of Acids and Bases. Strong Acids and Bases The strength of an acid depends on how much it ionizes in water Strong acids completely ionize, releasing.
Ionic equilibrium Lec.9. Introduction Ionization: a process in which unionized molecules are changed into ions. Types of electrolytes: Strong electrolytesWeak.
Checking Ch 15.1 A C I D - B A S E T I T R A T I O N A N D p H.
Buffers: -A buffer solution is that solution that allows solutions to resist large changes in pH upon the addition of limited amounts of acid Or base.
The pH Scale. Arrange the substances in order of increasing pH. Match the pH and [H + ] to each substance Try to work out the relationship between pH.
Chemistry Raymond Chang 10 th edition Chapter 16 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Weak acid and base calculations. What’s so hard? Unlike strong acids and bases, weak examples do not dissociate fully. For example, a 1 molL -1 HCl solution.
Topic 08 – Acids/Bases 8.3 – Strong and Weak Acids and Bases.
Acids and Bases Check 1. Define Bronsted-Lowry base; 2. Identify the acid and base; HSO 4 - (aq) + H 2 O(l) ←→ H 3 O + (aq) + SO 4 2- (aq) 3. What is a.
PH. Definitions and Formulas The pH scale is defined as the negative log of the concentration of H + : pH = -log[H + ] The pOH scale is defined as the.
Acids, Bases, and Salts Chapter 19. Acid-Base Theories Essential Question: What are the properties of acids and bases, and what distinguishes the Arrhenius,
CI 8.1 Acids and Bases. Acids Turn litmus red Neutralised by bases pH < 7 Liberate CO 2 from carbonates.
Conjugate acids and bases. When a substance loses ONE hydrogen ion, the species produced is called a “conjugate base” What’s the conjugate base of H 2.
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)
Lecture 193/12/07. Sample (100 mL – 0.1 M) Titrant (0.2 M) Initial pH pH at equivalence point pH at 2X equivalence point X-axis at equivalence point Strong.
Acidic, basic and neutral salts. Salts Salts are formed when acids react with bases. acid + base → salt + water When strong acids react with strong bases.
Acids and Bases Part 3. Strong and Weak Acids and Bases Consider the acid dissociation reaction: HA H + + A - If this equilibrium lies to the right,
Acids and Bases Acids and and Bases Bases. Acid and Bases There are many ways to classify compounds (ionic and covalent, organic and inorganic) – Acid.
Lecture 9 Acid-Base Equilibria -I. Strong acids: HCl HBr HI HNO 3 H 2 SO 4 HClO 4 (HO) n E=O Weak acid (HO) n EO 2 Strong acid We titrate with strong.
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