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We will calculate the pH of the solutions using the following 3 steps for each problem. Step 1: What is left in solution? Step 2: What are the equilibrium concentrations of the species in solution?
pH of Weak Acids W 332 Everett Community College Tutoring Center Student Support Services Program 1) The acid dissociation constant (K a) for benzoic -acid is 6.3 x 105. Find the pH of a 0.35 M solution of benzoic acid. 2) Find the pH of a 0.275 M hypochlorous acid solution. K a = 3.0 x 10-8.
The pH of the solution of the conjugate base of a weak acid can be calculated by considering the equilibrium it is involved in. The calculation is very similar to that in Model 2.
Determine the NaOH concentration & the pH. 7. List 3 strong acids and explain why these acids are considered strong acids. 8. List 3 weak acids and explain why these acids are considered weak acids. 9. -What is the pH and pOH of a 1.2 x 10 3 HBr solution? 10. What is the pH and pOH of a 2.34 x 10-5 NaOH solution?
Acids & Bases – Weak Acids/Bases Practice 4) Calculate (a) the pH and (b) the percent ionization of a 0.250 M HC 2 H 3 O 2 solution. Ka (HC2H3O2) = 1.8 x 10-5. (The formula for acetic acid may also be written as CH 3 COOH.) HINT: Begin by filling out the equilibrium table below. Balanced Equation HC 2 H 3 O 2 + ↔ H + C 2 H O –
2-‐23-‐12 Follow-‐up Wkst – Acid and Base pH Calculations. For each of the following solutions: Write a chemical equation, identify the limiting reactant (if there is one), and calculate the pH. We will calculate the pH of the solutions using the following 3 steps for each problem.
In Worksheet 8, you used an “ICE” approach to work out the pH of a solution containing a weak acid. For example, you worked out that a 0.500 M solution of CH 3 COOH(aq) has a pH of 2.531.
