Determine the pH at the equivalence (stoichiometric) point in the titration of 47.52 mL of 0.165 M C2H5NH2(aq) with 0.121 M HCl(aq). The Kb of ethylamine is 6.5 x 10-4.
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Determine the pH at the equivalence (stoichiometric) point in the titration of 47.52 mL of 0.165 M C2H5NH2(aq) with 0.121 M HCl(aq). The Kb of ethylamine is 6.5 x 10-4.
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- 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.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.Consider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?
- Calculate the pH during the titration of 20.00 mL of 0.1000 M ethylamine, C2H5NH2(aq), with 0.2000 M HNO3(aq) after 7.24 mL of the acid have been added. Kb of ethylamine = 6.5 x 10-4.A 20.00 mL aliquot of lactic acid solution (HCH3H5O3) was titrated with 0.0980 M KOH(aq) using both an indicator and a pH meter. Ka (HCH3H5O3), is 1.38 x10-4. A total of 28.64 mL of 0.0980 M KOH(aq) was required to reach the equivalence point 1. Calculate the molarity of the lactic acid solution. 2. Calculate the pH of the lactic acid solution 3. Calculate the pH and [CH3H5O3-] at the half-equivalence point. 4. Calculate the pH at the equivalence point of the titration. 5. Suggest an appropriate indicator for titration. 6. Calculate the pH of the solution after 10.00 mL of 0.0980 M NaOH(aq) was addedCalculate the pH during the titration of 30 mL of 0.1000 M C2H4COOH(aq) with 0.1000 M NaOH(aq) after 29.47 mL of the base have been added. Ka of acrylic acid = 5.5 * 10^-5.
- A sample of 0.10 M CH3COOH(aq) of volume 25.0 cm3 is titrated with 0.10 M NaOH(aq). The Ka for CH3COOH is 1.8 x 10-5. (a) What is the pH of 0.10 M CH3COOH(aq)? (b) What is the pH after the addition of 10.0 cm3 of 0.10 MNaOH(aq)? (c) What volume of 0.10 M NaOH(aq) is required to reach halfway to the stoichiometric point? (d) Calculate the pH at that halfway point. (e) What volume of 0.10 M NaOH(aq) is required to reach the stoichiometric point? (f) Calculate the pH at the stoichiometric point.Determine the pH at the equivalence (stoichiometric) point in the titration of 48.38 mL of 0.171 M HCN (aq) with 0.135 M NaOH(aq). The Ka of HCN is 4.9 * 10^-10.To a buffer containing 0.150 mol NH3 and 0.250 mol NH4 0.050 mol of HCl (aq) is added. Calculate the pH of the solution given that Ko of NH3 is 1.8 x 10-5.
- 1) Calculate the pH of a solution prepared by dissolving 1.90 g of sodium acetate, CH;COONA, in 85.0 mL of 0.20 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. K, of CH3COOH is 1.75 x 10-5. pH =During the course of the titration of a 20.0 ml of solution containing 0.1 M of NaOH and 0.08 M of hydrazine (NH2-NH2) (Ka = 1.05 x 10) by a 0.2 M standard perchloric acid (HC104) titrant, calculate the pH of the titration mixture after (a) 5.0 ml; (b) 10.0 ml; and (c) 15.0 ml of HC1O4 titrant is added.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?