1. Predict if an aqueous solution of 0.5 M sodium cyanide, NaCN, would be acidic, neutral, or basic at 298 K. 2. Write the correct hydrolysis reaction that would be used to calculate the pH of the solution. 3. Create and fill in an ICE table below your reaction in part 2, using x as the variable. Do NOT make assumptions about the size of x; include all terms. 4. Which equilibrium constant is needed? Substitute your terms into the expression for the appropriate equilibrium constant. Do NOT make assumptions about the size of x; include all terms.

Determine the Ka for an acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT The pH for 0.0715 M solution of CC13CO2H is 1.40. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) -0.032 CCI CO₂H(aq) + H₂O(1) H3O+(aq) + CCI CO₂-(aq) RESET 0 0.0715 1.40 -1.40 0.040 -0.040 0.032

For a solution that is 0.0421 M in NH¼Br, do the following. Identify the major species (other than water) that has no effect on pH. Include charge (if any) and phase. eTextbook and Media Balance the equilibrium reaction for the major species that does have an effect on pH. All species should include charge (if any) and phase. On the product side, list the cation (if any) first, followed by the neutral molecule (if any), and the anion (if any). +H,0(1)= Compute the pH of the solution. Kp of NH3 is 1.8E-5.

Determine the concentration of CH NH¸* in a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and use this information to determine the concentration of CH NH+. The Kb for CH NH₂ is 3.8 × 10-10. Complete Parts 1-3 before submitting your answer. 2 1 2 3 NEXT > 2 A buffer solution contains dissolved CH NH and CH NH Cl. The initial concentration of CH NH2 is 0.50 M. The pH at equilibrium of the buffer is 4.20. Let x represent the original concentration of CH NH+ in the water. 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) CH NH2(aq) + H₂O(I) = OH(aq) + C HẠNH, (aq) RESET 0 0.50 x 4.20 -4.20 6.3 x 10-5 -6.3 x 10-5 1.6 × 10-10 -1.6 × 10-10 3.8 × 10-10 -3.8 × 10-10 x +4.20 x-4.20 x + 6.3 x 10-5 x - 6.3 × 10-5 x + 1.6 × 10-10 x-1.6 × 10-10 x + 3.8 × 10-10 x - 3.8 × 10-10

In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of formic acid, HCOOH to be 1.984. Use the information she obtained to determine the K, for this acid. K(experiment) =

Imagine that 500 mL of a 0.100 M solution of HOAc(aq) is prepared.  What will be the [OAc–] at equilibrium in this solution if the acid dissociation constant Ka(HOAc) = 1.79 x 10–5?   a. 1.33 x 10–3 M   b. 4.23 x 10–3 M   c. 9.46 x 10–4 M   d. 0.100 M   e. not enough information to tell

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.

This is the same question with different parts. Also please find Ka and pH

6. Consider a solution that has 0.00500 M HCl and 0.100 M HF. Ka of HF = 7.2x10-4. a. What is the pH of this solution? b. Suppose the solution was like that in A but also had 0.1 M HOI. (i.e. total solution was a mix of 0.00500 M HCl, 0.100 M HF, and 0.1 M HOI). Ka of HOI = 2.0x10-¹¹. Does this solution have an appreciably different pH than the solution in part a? Support your answer with relevant calculations. HINT: Work from strongest acid to the weakest acid.

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 0.30 + x 1 HF(aq) 0.30 0.30 - x + H₂O(l) 6.8 x 10-4 2 0.30 + 2x 0.15 0.30 - 2x H3O+(aq) + +X 3 6.8 x 104 + x -X 6.8 x 10-4-x F-(aq) ✓ RESET +2x 6.8 x 10-4 + 2x