Determine the pH of a solution of HF by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The Ka of HF is 6.8 x 10-4. Complete Parts 1-3 before submitting your answer. NEXT > A 0.30 M aqueous solution of HF is prepared. 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) -2x 6.8 x 10-4-2x 0 1 0.30 + x HF(aq) 0.30 0.30 - x + 2 H₂O(1) 6.8 x 10-4 0.30 + 2x 0.15 0.30 - 2x 3 H3O+(aq) + +X 6.8 x 10-4 + x -X 6.8 x 10-4-x F-(aq) RESET +2x 6.8 x 10-4 + 2x

A 0.050 M solution of the salt NaA has a pH of 9.00. Determine the [OH] and the pH of a 0.010 M solution of the acid HA. Show your work in the question parts below. Construct an ICE table for the ionization equation described below.. Use the given information to determine the concentration at equilibrium for all reactants and products.. Initial () Change () Equilibrium () 0.050 + x 0.050 + 2x A (aq) 0 0.050- x A (aq) + H₂O(1) HA(aq) + OH(aq) 0.050 - 2x + 0.050 0.100 + x 0.100 + 2x 0.100 0.100 - x H₂O(l) 0.100 - 2x -X (0.050 + x)² = +x (0.050- x)² +2x HA(aq) (0.100 + x)² RESET -2x (0.100 - x)² + OH (aq)

Given: 0.300M NaOH            35.0L of 0.450M CH3COOH solution. CH3COOH dissociate constant = 1.8*10^-5 write out the equilibrium equation formed at the equivalence point.

11) A 520 ml solution contains 0.130 M formic acid (K, = 1.80 x 10) and 0.130 M sodium formate. First determine the pH of this initial solution. Next, determine the pH if 1 mL of 5.5 M of HCI was added to this solution. Finally, determine if rather than HCI, 1 mL of 5.5 M NaOH was added to the solution.

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)

Given the reaction:    MgBr2    ⇄    Mg2+  +  2Br- Which of the following conditions will decrease the solubility of the salt? Group of answer choices Increase Br- Increase the amount of water Increase the amount of solid MgBr2 Increase in [H3O+]

This is a 3 part question

Write the K, expression for an aqueous solution of acetic acid, CH3COOH :