The acetate ion, CH3COO–, reacts with water as a weak base: CH3COO–(aq) + H2O(l) ⇄ CH3COOH(aq) + OH–(aq), with K = 5.7 x 10-10 at 25°C. If sodium acetate were dissolved in water to make a 0.35 M solution, what would be the resulting concentration of OH–? (M) (no scientific notation)

Write the equilibrium constant expression for this reaction: NH(aq) → NH3(aq) + H+ (aq) - x Ś

Consider the following chemical equilibrium for the weak acid HF in water: HF(g) + H_2O(l) \rightleftharpoons  F^-(aq) + H_3O^+(aq). Which of the following statements is correct when water is evaporated from to the system?

Write the equilibrium constant expression for this reaction: C,H1,04(aq)+2 OH (aq) → 2 CH,CO0 (aq)+C,H,O2(aq) olo

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Write the expressions for K, for the following reactions. In each case indicate whether the reaction is homoge- neous or heterogeneous. (a) 203(g) = 302(8) (b) Ti(s) + 2 Cl2(8) = TIC14(I) (c) 2 C,H,(8) + 2H,0(g) = 2 C,H¿(8) + O2(8)| (d) C(s) + 2 H2(8) = CH4(8) (e) 4 HCI(aq) + Oz(8) = 2 H20(1) + 2 Cl2(8) (f) 2 C3H18(1) + 25 O2(g) = 16 CO2(8) + 18 H20(g) (g) 2 C3H18(1) + 25 O2(8) 16 CO2(8) + 18 H20(I)

HOC((ag) = H*(aq) + OC1¯(aq) The ionization of hypochlorous acid represented above has K = 3.0*10-OCI (aq) + HO(1) = HOC1(aq) + OH (aq)', What is K for this reaction? 3.ОЕ8 3.ЗЕ7 3.ЗЕ-7 3.0E-8 3.ОЕ6 OO O O

Write down the equilibrium constant expression for the following equation: HF (aq) + H2O (I) = F- (aq) + H3O+ (aq) 2H2 (g) + O2 (g) = 2H2O (g) 2N2O (g) = 2N2 (g) + O2 (g)

Consider the following equilibrium for nitrous acid, HNO2, a weak acid: HNO2(aq) + H2O (l) <====> H3O+(aq) + NO2-(aq) In which direction will the equilibrium shift if NaOH is added?  NaNO2 is added ? HCl is added? The acid solution is made more dilute ?

Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K = 1.8 x 10-4. HCOOH(ag) - H,0(1) – HCOO (ag) + H,0*(aq) Calculate the equilibrium concentration of H3o* in a 0.985 Msolution. M