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Aqueous solutions & concepts of pH Chapter 19-3

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I. Ion Product constant - water A. Acids→ hydronium ions (H 3 O+) Bases → hydroxide ions (OH-) B.Self ionization of water H 2 O + H 2 O OH - + H 3 O + Since every ionized water produces one hydronium ion and one hydroxide, the concentration of hydronium and hydroxide in, otherwise, pure water is the same. [H 3 O + ] = 1.0 x M [OH - ] = 1.0 x M Kw = [H 3 O + ] [OH - ] = 1.0 x M 2

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C. Neutral, Acidic, Basic [H 3 O + ] = [OH - ] neutral 2. [H 3 O + ] >[OH - ] acidic 3. [H 3 O + ] <[OH - ] basic Solve practice problem 18, pg. 609

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D. Calculating D. Calculating [H 3 O + ] &[OH - ] Kw = [H 3 O + ] [OH - ] = 1.0 x M Calculate [OH - ] when have a 1.0 x M NaOH solution NaOH → 2. Calculate [H 3 O + ] of a 1.0 x M H 2 SO 4 solution H 2 SO 4 → 3. 3.Determine hydronium and hydroxide ion concentrations in solution that is 1.0 x M HCl

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Calculate hydronium and hydroxide ion concentrations 1.In a solution that is 1 x M HCl 2.In a solutuion that is 1.0 x M HNO 3 3.In a solution that is 1.0 x M Ca(OH) 2

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II. pH Scale pH = -log pH = -log [H + ] pOH = -log [OH - ] pH + pOH = 14

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A. Calculations with pH Determine the pH of: x M HCl x M KOH x M Sr(OH) 2 solution

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B. Calculating B. Calculating [H 3 O + ] & [OH-] from pH [H 3 O + ] = 10 -pH [OH-] = 10 -pOH 4. 4.pH = 5.0 What is [H 3 O + ] ? 5. 5.pH = 1.50 Calculate [H 3 O + ] &[OH-] Practice problems pg

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