'Ag aq cl aq' diaporamas de présentation

Equilibrium constants

Equilibrium constants. Equilibrium constants. P C c P D d. K =. P A a P B b. [C] c [D] d. K =. [A] a [B] b. Equilibrium constants. P C c P D d. K =. P A a P B b. [C] c [D] d. K =. [A] a [B] b. [solid] = 1. Equilibrium of solids and solutions.

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Chemistry 232

Chemistry 232. Reaction Equilibria in Nonideal Systems. The Equilibrium Constant. For a nonideal system, the nonstandard Gibbs energy of reaction is written. The Equilibrium Condition. If we apply the equilibrium conditions to the above equation. The Autoionization of Water.

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8.4 Water

8.4 Water. Density of water. The density of liquid water is calculated using the formula: Density = mass/volume where: D = density (g/mL or g/m -3 ) m = mass (g) V = volume (mL). Temperature and density. Generally as the temperature of a substance increases it expands and its

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GRAVIMETRIC ANALYSIS

GRAVIMETRIC ANALYSIS. Budi Hastuti, S. Pd, M.Si. Gravimetric Analysis. A Gravimetric analysis is based upon the measurement of the weight of a substance that has a KNOWN composition AND IS chemically related to the analyte. Gravimetric Analysis. Accurate and precise.

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Ions in solids and solutions.

Ions in solids and solutions. -. -. +. -. +. +. -. -. +. Ions in ionic solids. Cl -. Na +. ? -. ? -. ? -. ? -. ? -. ? -. ? -. ? -. ? +. ? +. ? +. ? +. ? +. ? +. ? +. ? +. ? -. ? +. Ions in solution. Hydrated ions. -. +. Most electronegative. Polar molecules. O.

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15.6 Solubility Equilibria

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Chapter 17 Equilibrium 17.1 How Chemical Reactions Occur Particle collisions

Chapter 17 Equilibrium 17.1 How Chemical Reactions Occur Particle collisions 1. Particles MUST collide for a chemical reaction to occur. 2. Orientation of particle collision is important. 3. Effectiveness of particle collision is important.

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Concentration Cells

Concentration Cells. M | M + (aq, L) || M + (aq, R) | M Cell reaction: M + (aq, R) ? M + (aq, L) since ? r G ? = 0 (why?). The cell emf. The emf of a cell can be calculated by the difference of the potentials of the two electrodes, E cell = E right - E left

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Solubility Equilibria

Solubility Equilibria. End of Chapter 17. Solubility Equilibria. AgCl ( s ) Ag + ( aq ) + Cl - ( aq ). MgF 2 ( s ) Mg 2+ ( aq ) + 2F - ( aq ). Ag 2 CO 3 ( s ) 2Ag + ( aq ) + CO 3 2 - ( aq ). Ca 3 (PO 4 ) 2 ( s ) 3Ca 2+ ( aq ) + 2PO 4 3 - ( aq ).

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Solubility Equilibria

Solubility Equilibria. End of Chapter 16. Solubility Equilibria. AgCl ( s ) Ag + ( aq ) + Cl - ( aq ). MgF 2 ( s ) Mg 2+ ( aq ) + 2F - ( aq ). Ag 2 CO 3 ( s ) 2Ag + ( aq ) + CO 3 2 - ( aq ). Ca 3 (PO 4 ) 2 ( s ) 3Ca 2+ ( aq ) + 2PO 4 3 - ( aq ).

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Solubility Equilibria

Solubility Equilibria. End of Chapter 17. Solubility Equilibria. AgCl ( s ) Ag + ( aq ) + Cl - ( aq ). MgF 2 ( s ) Mg 2+ ( aq ) + 2F - ( aq ). Ag 2 CO 3 ( s ) 2Ag + ( aq ) + CO 3 2 - ( aq ). Ca 3 (PO 4 ) 2 ( s ) 3Ca 2+ ( aq ) + 2PO 4 3 - ( aq ).

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Equilibrium Constant

Equilibrium Constant. Chemistry Mrs. Coyle. Equilibrium Position. http://www.chm.davidson.edu/ronutt/che115/K/Sol_1.gif. Equilibrium Expression Equilibrium Constant, K eq. The concentrations are at the equilibrium position.

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Solubility equilibria

Unit 17. Solubility equilibria. Dissolution: the process in which an ionic solid dissolves in a polar liquid. AgCl (s) ? Ag + ( aq ) + Cl - ( aq ) Precipitation: the process in which ions leave a solution and regenerate an ionic solid.

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Solubility Product Constant

Solubility Product Constant. Chemistry Mrs. Coyle. Solubility Equilibrium. AgCl(s) ? Ag + (aq) + Cl - (aq) The concentration of AgCl (s) is constant and AgCl is a strong electrolyte (dissociates almost completely), so K sp = [Ag + ] [Cl - ] K sp is the solubility product constant.

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