The value of Ka for phenol (a weak acid) , C,H5OH , is 1.00×10-10 . Write the equation for the reaction that goes with this equilibrium constant. (Use H3O* instead of H*.) +

Sodium chloride is added to water (at 25C) until it is saturated. Calculate the Cl concentration in such a solution. Species G(kJ/mol) NaCl(s) 384 Na+(aq) 262 Cl(aq) 131

Analyze both reactions and indicate whether the equilibrium tends to favor the reactants or the products. Reaction A: H30* + NH,* NH2 HO, Reaction B: + "OH + ОН Select the true statement(s). Reactions A and B tend to favor the products. Reactions A and B tend to favor the reactants. Reaction A tends to favor the reactants, Reaction B favors the products. Reaction A tends to favor the products, Reaction B favors the reactants.

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For the reaction:    2HBr    →     H2     +    Br2                 ΔH = -17.4 kcal/mol.   And Keq =  32 X 10 20 Is the reaction exothermic or endothermic?       Are products or reactants favored?     Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of Br2  is increased?     Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of H2  is decreased?

Vinegar (chemical name : acetic acid, CH3COOH) is a weak acid. Consider the ionization of acetic acid in water. CH3COOH(aq) = H*(aq) + CH3COO (aq) Kc=6.80 ×10-4 If the initial concentration of acetic acid is 0.150 M. What is the concentration of hydrogen ions (H*) at equilibrium? O 0.0100 M O 0.0500 M O 0.100 M O 0.500 M

Consider the following equilibrium: BaSO4(s)<===> Ba2+(aq) + SO4 2-(aq) ; change in heat is >0 Which direction will equilibrium shift if H2SO4 is added? Why? BaCl2 is added? Why? NaCl is added? Why? Heat is added? Why?

Consider the following chemical reaction at equilibrium: NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + HO⁻(aq) If one drop of aqueous sodium hydroxide (NaOH) is added, in which direction will the equilibrium shift? A) reactants B) products C) neither the reactants nor the products

The dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋  CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.

In the reaction:        2A       ⇆                B       +      3C            For the reaction,   ΔH = -23 kcal/mol   and Keq =  26 X 10 -26   Is the reaction exothermic or endothermic?     Are products or reactants favored?     Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of C is increased?     Using Le Chatelier’s Principle, what happens to the equilibrium if the concentration of A is increased?