Complete the balanced dissociation equation for the compound below in aqueous solution. If the compound does not dissociate, write NR after the reaction arrow. Ba(OH)2 (s) ->

What is the [H3O*] in a 175 mL sample of 0.0629 M KOH(aq)?   6.08 x 10-13 mol L-1   8.17 x 10-14 mol L-1   2.78 x 10-14 mol L-1   1.59 10-13 mol L-1   9.08 x 10-13 mol L-1

Fill in the left side of this equilibrium constant equation for the reaction of hydrofluoric acid (HF) with water. = Ka plo H

1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous solution with an initial NaA concentration of 0.061 M. 2.) We place 0.149 mol of a weak acid, HA, in enough water to produce 1.00 L of solution. The final pH of the solution is 1.11 . Calculate the ionization contant, Ka, of HA. 3.)We place 0.527 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.35 . Calculate the ionization constant, Ka, of HA.