Determine the concentration of H,O* in a 0.064 M solution of oxalic acid, H₂C₂O4. H_C,O,(@q) +HO(0) = HO* (aq) +HC.O, (@q) K =0.054 HC,O, (aq) +H_O(0) = H\O*@q)+C_O (aq) K = 54×10-3
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- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCN (aq) + OH" (aq) CN" (aq) + H,0 (1) K =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H,0(1) =NH,* (aq)+ OH°(aq) K =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. (CH3)3N (aq) + H20(1)=H(CH3)3N* (aq) + OH(aq) )
- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HCIO(aq) + H,O(1)=H;0*(aq) + CIO"(aq) K =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2 (aq) + OH" (aq)NO, (aq) + H2O (1) K =Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO,(aq) + H2O(1)=H;0*(aq) + NO,"(aq) K =
- Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-Consider the reaction at 25 degrees celsius 2NO3-(aq)+8H^+(aq)+3Cu(s)=3Cu2+(aq)+2NO(g)+4H2O(l) At what pH is the reaction at equilibrium with all other ionic species at 0.01M and gases at 1 atm?Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant is K= 1.8 x 10-4. HCOOH(aq) + H,O(1) = HCOO (aq) +H,O*(aq) Calculate the equilibrium concentration of H3O* in a 0.985 Msolution. M
- Using the following equations, determine (a) Equilibrium expressions, K, and K2; (b) The equation for the reactions that the sum of the two equations; (c) The equilibrium expression, K3, for the sum of the two equations 1. CO33 (aq) + H*(aq) 2HCO;"(aq) 2. HCO, (aq) + H*(aq) H,CO;(aq) K¡ = ? K3 = ?Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NO, (aq) + H20 ()=HNO, (aq) + OH¯ (aq) K =