Calculate the pH during the titration of 30.00 mL of 0.1000 M ammonia with 0.1000 M HCl(aq) after 12.46 mL of the acid have been added. Kb of ammonia = 1.8 x 10-5.
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Calculate the pH during the titration of 30.00 mL of 0.1000 M ammonia with 0.1000 M HCl(aq) after 12.46 mL of the acid have been added.
Kb of ammonia = 1.8 x 10-5.
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- Consider the titration of a 50.00 mL sample of 0.500 M hydrazoic acid, HN3, with 0.500 M NaOH (aq., 25 oC). The Ka HN3 = 4.50 x 10–4. What is the pH of the solution after 15.00 mL of NaOH has been added?Consider the titration of 100.0 mL of 0.200 mol/L ethanoic acid, HC2H3O2(aq) (Ka = 1.8 x 10-5), by 0.100 mol potassium hydroxide solution. Calculate the pH of the resulting solution when 150.0mL of potassium hydroxide solution has been added?Sketch reasonably accurately the pH curve for the titration of 25.0 cm3 of 0.15 M Ba(OH)2(aq) with 0.22 M HCI(aq). Mark on the curve (a) the initial pH, (b) the pH at the stoichiometric point.
- Determine the pH at the equivalence (stoichiometric) point in the titration of 44.27 mL of 0.138 M morphine(aq) with 0.271 M HCl(aq). The Kb of morphine is 1.6 x 10-6.In a titration of acetic acid by sodium hydroxide, what is the pH of a 100.0 mL of a 0.1000 M CH3CHO2H(aq) solution after 25.00 mL of 0.2000 M NaOH(aq) has been added? The Ka of acetic acid is 1.75 x 10-5,What is the pH of the solution when 20.0 mL of 0.155 M of NH3(aq) is titrated with 15.0 mL of 0.225 M of HCl(aq)? The Kb of NH3 is 1.8 x 10-5.
- Determine the pH at the equivalence (stoichiometric) point in the titration of 38.83 mL of 0.262 M (CH3)2NH(aq) with 0.111 M HCl(aq). The Kb of (CH3)2NH is 5.4 x 10-4.For the titration curve of 20 mL of 0.275 M (CH3)3N (aq) with 0.325 M HCl (aq), determine the initial pH and the pH before the equivalence point.Write the expression for the solubility product constant for Pb(OH)2.
- What is the pH of a solution prepared by mixing 19 mL of 0.073 M Ba(OH)2 and 55 mL of 0.48 M KOH? (See the Selected Solubility Product Constants.)A solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of 0.0240M calcium acetate, Ca(C₂H₃O₂)₂. Calculate the pH of the resulting solution. You may assume that the potassium acetate dissolve completely and that the change in volume is negligible with the addition of the solid.What is the pH of the solution which results from mixing 75 mL of 0.50 M NH3(aq) and 75 mL of 0.50 HCl(aq) at 25 ºC? (Kb for NH3 = 1.8 x 10-5)
