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pH meter CCC Kei Heep Secondary School F.6 Chemistry by Wong CS Chemistry CE Homepage Chemistry AL Homepage
pH value pH = log [H + ] For 1 M HCl (aq), pH = 0 For 0.1 M HNO 3 (aq), pH = 1 For 10 M NaOH (aq), pH = 15
Apparatus pH with a glass electrode Thermometer Buffer solution of pH 4 and 7
Calibration Step 1 Insert the electrode and thermometer in distill water. Adjust the temperature knob to the reading of room temperature.
Calibration Step 2 Insert the electrode in the buffer solution with pH = 7. Adjust the AP knob to 7.00.
Calibration Step 3 Wash the electrode with distill water. Insert the electrode in the buffer solution with pH = 4. Adjust the pH knob to pH = 4.00.
Measure pH value Wash the electrode with distill water. Insert the electrode in the solution which you want to test. Record the reading when steady.
Weak Acid HA (aq) + H 2 O (l) H 3 O + (aq) + A (aq) Initial: x At eq.: x-y y y Assume x >> y
Buffer solution HA (aq) + H 2 O (l) H 3 O + (aq) + A (aq) Initial: x x At eq.: x-y y x+y Assume x >> y [H + ] = y = K pH = pK
Test the pH of most common solution - pH panel http://www.miamisci.org/ph/phpanel.html
Indicator CCC Kei Heep Secondary School F.6 Chemistry by Wong CS Chemistry CE Homepage Chemistry AL Homepage.
PH In the Laboratory. Ionization of Water Equllibrium Constant, K eq.
Example 15.6: Find the pH of M HNO 2 (aq) 25 °C 9 Tro, Chemistry: A Molecular Approach, 2/e.
Exp. 21: Acid – Base Equilibria: Ionization Constant of an Acid, K a Acids and bases are classified as “strong” or “weak”. strong - essentially complete.
The pK a Scale. Acid Dissociation Constant, K a K a, is a measure of how readily H + ions are released HA (aq) + H 2 O (aq) H 3 O + (aq) + A - (aq) K.
Lecture 23 10/28/ mL of 0.02 M KOH with 0.1 M HBr Construct curve from 4 points Initial pH X = 0 mL, Y = ? Equivalence point X = V eq, Y = 7 Before.
PH of Weak Acids AP Chemistry Unit 9 Chapter 14. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK.
PART A M C V C = M D _______ V D = (1.0 M)(5.0 mL) ___________________ (50.0 mL) = 0.10 M HC 2 H 3 O 2.
Lecture 152/22/06 Topics due. Neutralization: Acid + Base = Water + Salt pH of neutralized solution? Strong Acid + Strong Base HCl (aq) + NaOH (aq)
Experiments in Analytical Chemistry -Determination of pK 1, pK 2, and pK 3 of phosphoric acid.
Lecture 122/12/07. pH What is it? How do you measure it?
EXPERIMENT (5) Preparation and Properties of Buffer Solution.
Lecture 142/19/06. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? NaOH CaO.
1 Function of the Conjugate Base The function of the acetate ion C 2 H 3 O 2 is to neutralize added H 3 O +. The acetic acid produced by the neutralization.
Titrations Definition: Volumetric determination of the amount of an acid or base by addition of a standard acid or base until neutralization.
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.
Acid – Base Equilibria Buffer Solutions: –Question: Was the ICE Problem set up needed? –Answer: No. The assumption of x << [HA], [A - ] is valid for all.
Ionization of Water CHEM 7784 Biochemistry Professor Bensley.
Equilibrium constant, Ka By Soo Jeon. background Most weak acids dissociate 5% or less, that is, 95% or more of the acid remains as HA. The smaller the.
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.
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.
Buffers solutions that resist pH changes base addition ofacid containacidic componentHAHA+ OH - H 2 O + A - basic component A-A- + H + HA conjugate.
Ch Acids & Bases II. Strength of Acids & Bases (p ) Strong vs. Weak pH.
Acids ph buffers A2 chemistry. Using the post it notes write down the name of the species and whether each species round the room is an acid, base or.
Drill: Calculate the pH of 2.0 x M HI. Calculate the pH of 3.3 x M HI.
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.
Procedure for calculating pH of a titration Volume of titrant needed is based on amount of analyte.
Acids and Bases! Acids and Bases (and calculations involving them) are essential to all areas of analytical chemistry!
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.
Acids and Bases. HA H + + A - HCL H + + CL - CH 3 COOH H + + CH 3 COO -
Acids and Bases © 2009, Prentice-Hall, Inc. Sections Acids and Bases Chemistry, The Central Science, 11th edition Brown & LeMay.
Calculate the pH of 2.0 x M HI. Acid-Base Equilibria.
Drill: Determine the pH of 0.25 M HZ. K aHZ = 2.5 x
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.
Acid/Base Chemistry Part II CHEM 2124 – General Chemistry II Alfred State College Professor Bensley.
ANALYTICAL CHEMISTRY CHEM 3811 CHAPTER 10 DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university.
Acid Dissociation Constant. Dissociation Constants For a generalized acid dissociation, the equilibrium expression would be This equilibrium constant.
12 AP Chemistry Buffers. What is a Buffer? A buffer solution is one, which can absorb additions of acids or bases with only slight changes in pH values.
H+H+ H+H+ H+H+ OH - New Way Chemistry for Hong Kong A-Level Book 2 1 Chapter 17 Acid-base Equilibrium I : The Basic Concepts 17.1Concept of Acid and Base.
Team pHFine Scale By Ethan Kurteff. * In the blue tank, an artificial seawater solution (8.05 pH) is mixed. This and distilled water are added >
Experiment 24 pH ranges and pH of Buffer Solutions CHE1181.
Acids, Bases, and Salts Preparation for College Chemistry Columbia University Department of Chemistry.
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.
The pH scale is a convenient way to represent solution acidity. The pH is a log scale based on 10, where pH = -log[H + ] Thus for a solution where [H +
Aqueous Solutions and the Concept of pH Section 15.1.
Neutralization Of strong acids and bases. Example1 1- How many ml of M H 2 SO 4 are required to neutralize exactly 525 ml of 0.06 M KOH? 2- What.
The Ionic Product of Water KwKw. Ionic Product of water, K w Just because a solution contains [H + ] it doesn’t necessarily mean it’s acidic. All aqueous.
Which is the stronger acid? 1.HNO 2 2.HNO 3 Which is the stronger base? 1.NO NO 3 -
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