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Ka-acid-ionization - Ka Kb Ka 1 2 3 4 Comparing the pH of...

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Ka, Kb Ka, Kb
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Comparing the pH of two acids Comparing the pH of two acids 1. Predict the pH of HCl and HF (below) 2. Calibrate a pH meter 3. Measure the pH of HCl(aq) and HF(aq) 4. Complete the chart below HCl (aq) HF (aq) [ ] in mol/L (on label) Net ionic equation Predicted [H + ] Predicted pH pH measured Actual [H + ] Conductivity (demo) Higher / stronger Lower / weaker 0.05 0.05 HCl H + + Cl HF H + + F 0.05 0.05 -log(0.05)=1.3 -log(0.05)=1.3 1.3 2.3 ? 10 –pH = 0.05 10 –pH = 0.005
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Questions Read15.3. (pg. 607+) 1. Based on your results, which acid ionizes (forms ions) to a greater degree? 2. Which two measurements taken in the lab support your answer to 1? 3. What is another name for Ka? 4. Solve PE 5, 6 5. Write the Ka equation for HCl (aq) and HF (aq) from today’s lab 6. Solve for PE 8, 9 (use this equilibrium for butyric acid: HBu H + + Bu ) 7. For HF(aq) set up a RICE chart, then solve for Ka. How does your value for Ka compare to the accepted value (pg. 608)? 8. Try PE 10 (follow example 15.7 on pg. 610)
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Answers Answers 1. HCl ionizes more than HF 2. HCl has a lower pH (indicating more H + ), & a higher conductivity (indicating more ions) 3. Ka: acid ionization constant 4. HNO 2 H + + NO 2 , Ka=[H + ][NO 2 ]/[HNO 2 ] HPO 4 2– H + + PO 4 3– ,Ka=[H + ][PO 4 3– ]/ [HPO 4 2– ] 1. HCl H + + Cl , Ka=[H + ][Cl ]/[HCl] HF H + + F , Ka=[H + ][F ]/[HF]
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PE 8 - pg. 610
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