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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
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.
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.
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.
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