'Base titrations' diaporamas de présentation

Acids and Bases

Acids and Bases. An Introduction. Introduction. Inorganic and organic acids are important industrial chemicals; in 2002, H 2 SO 4 was the number 1 chemical produced in the U.S.: 36,000,000 metric tons (80,000,000,000 lbs) 1metric ton = 1000Kg = 2204.6lbs. Common Household Acids.

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Chapter 17 Additional Aspects of Aqueous Equilibria

Chemistry, The Central Science , 10th edition Brown, LeMay, and Bursten. Chapter 17 Additional Aspects of Aqueous Equilibria. SHS / AP Chemistry. HC 2 H 3 O 2 ( aq ) + H 2 O ( l ). H 3 O + ( aq ) + C 2 H 3 O 2 ? ( aq). 17.1 The Common-Ion Effect. Consider a solution of acetic acid:

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Chapter 17 Additional Aspects of Aqueous Equilibria

Chapter 17 Additional Aspects of Aqueous Equilibria. 17.1: The Common Ion Effect. The solubility of a partially soluble acid is decreased when a common ion is added HC 2 H 3 O 2(aq) + H 2 O (l) H 3 O + (aq) + C 2 H 3 O 2 - (aq) Consider the addition of C 2 H 3 O 2 -

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Acids and Bases

Acids and Bases. Electrolytes. Substance that conducts electricity when dissolved in water Ionizes in water Examples: aqueous ionic solutions, acids, bases. Properties of Acids. Acids have a pH less than 7.0 Acids will burn your skin Dilute acids have a sour taste

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Volumetric analysis

Volumetric analysis. Chemistry 321, Summer 2014. Volumetric analysis involves titrations. A titration is the use of a known concentration reagent to determine the concentration of the analyte . Typically, a buret is used to dispense the volume of the reagent. Titration is a good technique.

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Titrations MATH!!!!

Titrations MATH!!!!. weak base. indicator. K a. strong acid. K b. [H + ]. equivalence point. To Find the Equivalence Point. (ex) When titrating 50.0mL of 0.48M HCN with 0.75M NaOH , what volume of base must be added to reach the equivalence point?. Strong Acid with Strong Base.

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Balancing Redox Equations in Acidic Conditions

Balancing Redox Equations in Acidic Conditions. Take the reaction between potassium permanganate ? KMnO 4 ) and sodium sulfite (NaSO 3 ) 7 steps are required to balance the full ionic equation from 2 separate half equations ( oxidation & reduction ). Step 1.

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Acid-Base Titrations

Acid-Base Titrations. progressive addition of one reactant to another in measured volumes until an endpoint is reached. equivalence point (mL) is when the mole ratio is exactly satisfied, volume used for stoichiometry is shown by an indicator which changes color at the endpoint (pH).

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pH and Titration

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X- + H 3 O + ?HX + H 2 O

X- + H 3 O + ?HX + H 2 O. Add strong acid. Use Ka, [HX] & to calculate [H + ]. Recalculate [HX] & [X - ]. Buffer HX & X -. pH. Add strong base. HX + OH- ? X- + H 2 O. Equilibrium calculation Use Henderson-Hasselbalch. Stoichiometric calculation.

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Notes 16.3

Notes 16.3. Acid/Base Titration. Acid-Base Titrations. A neutralization reaction is when there is equal amounts of H+ and OH- available for a reaction and a neutral solution (pH=7) will result. To analyze the acid/base content of a solution, titrations are often performed

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