Strong Acid-Base Calculations

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Presentation transcript:

Strong Acid-Base Calculations Acids & Bases Lesson 6 Strong Acid-Base Calculations

Strong Acids & Bases Calculations

Strong Acids & Bases Calculations When we consider strong acids and bases, remember this: They ionize 100% In other words, [strong acid] = [H3O+] [strong base] = [OH-] When you mix the acid with the base, consider which concentration of H3O+ or OH- is in excess.

Strong Acids & Bases Calculations Part I: strong acid or strong base only in water Part II: Mixing the strong acid and the strong base together.

Part I: strong acid or strong base only in water

1. Calculate the pH of 0.40 M HI. HI  H+ + I- 0.40 M 0.40 M 0.40 M pH = -Log[H+] pH = -Log[0.40] pH = 0.40

2. Calculate the pH of 0.030 M Ba(OH)2. Ba(OH)2  Ba2+ + 2OH- 0.030 M 0.030 M 0.060 M pOH = -Log[OH-] pOH = -Log[0.060] pOH = 1.22 pH + pOH = 14.00 pH + 1.22 = 14.00 pH = 12.78

Try: Calculate the pH of 0.020 M Mg(OH)2

3. Calculate the pH of 100. 0 mL of 1. 0 M HCl after. 300. 0 mL of 3. Calculate the pH of 100.0 mL of 1.0 M HCl after 300.0 mL of water is added to it. HCl  H+ + Cl- 100 1.0 M 400 0.25 M 0.25 M pH = -Log[H+] pH = -Log[0.25] pH = 0.60

Try: Calculate the pH and pOH of 200. 0 mL of 2. 0 M HCl after 300 Try: Calculate the pH and pOH of 200.0 mL of 2.0 M HCl after 300.0 mL of water is added to it.

Part II: Mixing solutions of the strong acid and the strong base together. Helpful hints: Start as always by getting your [H3O+] And [OH-] Hydronium ion and Hydroxide ion will neutralize each other, however if there is extra of one of the two… Find the excess/extra you have. If you have extra [OH-], your solution will be basic. - If you have extra [H3O+], your solution will be acidic.

Example: 200. 0 mL of 0. 200 M HCl is mixed with 400. 0 mL of Example: 200.0 mL of 0.200 M HCl is mixed with 400.0 mL of 0.250 M NaOH. Calculate the pH of the new solution.

TRY: calculate the final [H3O+], [OH-] and new pH in a solution formed when 150.0 mL of 1.5 M HNO3 is added to 250.0mL of 0.80 M KOH

example How many moles of HCl(g) must be added to 40. 0mL of 0 example How many moles of HCl(g) must be added to 40.0mL of 0.180 M NaOH to produce a solution having pH= 12.500, if it is assumed that there is no change in volume when the HCl is added? p.143 example

TRY: How many moles of HCl(g) must be added to 30. 0mL of 0 TRY: How many moles of HCl(g) must be added to 30.0mL of 0.170 M Ca(OH)2 to produce a solution having pH= 10.500, if it is assumed that there is no change in volume when the HCl is added?

Example: calculate the pH resulting from mixing 25. 0 mL of 0 Example: calculate the pH resulting from mixing 25.0 mL of 0.0420 M Ba(OH)2 with 125.0 mL of 0.0120 M HCl. Q60

TRY: calculate the pOH resulting from mixing 50. 0 mL of 0 TRY: calculate the pOH resulting from mixing 50.0 mL of 0.0185 M Sr(OH)2 with 35.0 mL of a solution containing 0.130 g of HCl.

Ex: A chemist has 2. 000 L of 0. 00120 M KOH soltuion Ex: A chemist has 2.000 L of 0.00120 M KOH soltuion. What mass of HCl(g) would have to be added to the KOH solution to produce a solution having a pH of 10.857? -assume no change in volume occurs.

Homework: p.143 #58, 59, 62, 63, 64, 66,67.