12. additive. A. B. C. A solution is formed by mixing 20.00 mL of 0.2227 M NaOH and 30.00 mL of 0.3836 M Ba(OH)2. Assume that the volume is What is the equilibrium concentration of OH of the solution at 298 K? Please provider your answer below. f → S What is the pH of the solution at 298 K? Please provider your answer below. What is the equilibrium concentration of H₂O¹? Please provider your answer below. □ (0) M M M

Fill in the Blanks HCO,H(aq) H(aq) + HCо, (аq) K = 1.8 x 104 K%D Blank 1 Blank 2 Blank 3 C Blank 4 Blank 5 Blank 6 Blank 7 Blank 8 Blank 9 Type your answers in all of the blanks and submit Consider the acid ionization reaction for formic acid that has a Ka = 1.8 x 10-4. HCO2H(aq) Ht (aq) + HCO, (aq) Formic acid is a weak acid first found in ants. It causes the burning sensation when ants bite someone. Based upon a 0.15 M aqueous formic acid solution fill in the ICE table in the accompanying diagram then calculate the pH value for the solution. Only enter numerical values or algebraic quantities such +7x or -7x.

0.030 moles of a weak acid, HA, was dissolved in 2.0L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of Ka for the weak acid. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. HA(aq) H20(1) H3Oʻ(aq) A (aq) + + Initial (M) Change (M) Equilibrium (M)

0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Determine the value of Ka for the weak acid. 1 NEXT > Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. H¿O(I) H.O*(aq) A (aq) + НА(ag) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.060 0.015 0.017 0.030 0.013 2.0 8 2/ pe here to search DELL 1L

Determine the pOH of a weak acid (HA) solution by constructing an ICE table and using this information to determine the pOH of the solution. Complete Parts 1-2 before submitting your answer. 1 A 0.200 M aqueous solution of HA is 3.0% dissociated at equilibrium. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) + H₂O(l) 2 H3O+ (aq) 2 NEXT > + A-(aq)

Consider the below equilibrium for acid HA at 25 °C. Calculate the K, of the acid if a solution is created by adding HA to water to produce an initial [HA] = 0.40 M and, after reaching equilibrium, [H3O*] = 7.21 x 10-6 M. %3D HA (aq) + H2O (1) Z A- (aq) + H30* (aq) 1.15 x 10-6 1.30 x 10-10 2.69 x 10-3 5.20 x 10-11 O 7.21 x 10-6

This is a 3 part question