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Acid Base Calculations

Acid Base Calculations. Calculations involving pH Titration calculations. A 1.0 x 10 -4 M solution of HNO 3 has been prepared for a laboratory experiment. A) Calculate the [H 3 O + ] of this solution B) Calculate the [OH - ].

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Acid Base Calculations

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  1. Acid Base Calculations Calculations involving pH Titration calculations

  2. A 1.0 x 10-4 M solution of HNO3 has been prepared for a laboratory experiment.A) Calculate the [H3O+] of this solution B) Calculate the [OH-] HNO3(l) + H2O(l) H3O+(aq) + NO3-(aq) We can assume 100% ionization (strong acid) so HNO3 concentration equals H3O+ concentration [H3O+][OH-] = 1.0 x 10-14 [H3O+][OH-] = 1.0 x 10-14 [H3O+] [H3O+] [OH-] = 1.0 x 10-14 [H3O+] [OH-] = 1.0 x 10-14 = 1.0 x 10-10 M 1.0 x 10-4

  3. What is the pH of a 1.0 x 10-3 M NaOH solution? [H3O+][OH-] = 1.0 x 10-14 [H3O+] = 1.0 x 10-14 [OH-] [H3O+] = 1.0 x 10-14= 1.0 x 10-11 1.0 x 10-3 pH = -log [H3O+]= - log (1.0 x 10-11) = 11.0

  4. The pH of a solution is measured and determined to be 7.52.A) What is the hydronium ion concentration?B) What is the hydroxide ion concentration? C) Is the solution acidic or basic? log [H3O+] = -pH pH = -log [H3O+] [H3O+] = antilog (-pH) = antilog (-7.52) = 3.02 x 10-8 M [H3O+][OH-] = 1.0 x 10-14 [OH-] = 1.0 x 10-14 = 3.3 x 10-7M 3.02 x 10-8 [OH-] = 1.0 x 10-14 [H3O+]

  5. Titration Calculation In a titration, 27.4 ml of a 0.0154 M NaOH is added to 20.0 mL sample of HCl solution of unknown concentration. What is the molarity of the acid solution? HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq) SA SB Neutralization First we need to figure moles of NaOH used to neutralize HCl in reaction. 0.0274 L x 0.0154 mol/L = 4.22 x 10-4mol of NaOH

  6. Titration Calculation = 4.22 x 10-4mol of NaOH HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq) = 4.22 x 10-4mol of HCl M of HCl = 4.22 x 10-4mol of HCl .0200 L M of HCl= .021 M

  7. Titration Endpoint How can you tell when you have added enough NaOH?

  8. Titration Curve

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