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.Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the pH of the solution?
- Calculate the pH of 0.1 mol dm-3 potassium hydroxide (KOH(aq))You have a solution that contains acetic acid, (CH3COOH or HAc). The concentration of acetic acid in the aqueous solution is 0.35 mol / dm3. Ka = 1.7378 x 10 ^ -5 M a. Calculate the pH of the solution. 15 cm 3 of the acetic acid solution was titrated with sodium hydroxide solution, NaOH (aq), at a concentration of 0.5 mol / dm3 b. Describe how you would proceed to perform a titration of an acid of unknown concentration. What information can be obtained from a titration, describe the different phases. c. How much NaOH will be added when the equivalence point occurs?Calculate the ph of a solution prepared by dissolving 1.00g of sodium acetate,CH^3COONa, in 50.0ml of 0.15 M acetate acid, CH^3COOH(aq)
- If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,050 mol∙dm–3), calculate the pH at the equivalence point of the titrationCalculate the pH at the stoich iometric po int of the titration of 25.00 cm3 of 0.150 M lactic acid with 0.188 M NaOH(aq) .A buffer solution of volume 100 cm3 consists of 0.10 M CH3COOH(aq) and 0.10 MNaCH3CO2(aq). (a) What is its pH? (b) What is the pH after the addition of 3.3 mmol NaOH to the buffer solution? (c) What is the pH after the addition of 6.0 mmol HNO3 to the initial buffer solution?
- Outline the change in composition of a solution of the salt of a triprotic acid as the pH is changed from 1 to 14.In the titration of a solution of acetic acid, CH3COOH(aq), with a solution of KOH(aq), the stoichiometric point occurs at a pH greater than 7. (Enter True or False)Calculate the pH, pOH, and fraction of solute protonated or deprotonated in the following aqueous solutions: (a) 0.150 M CH3CH(OH)COOH(aq) (lactic acid), (b) 2.4 x 10-4 M CH3CH(OH)COOH(aq), (c) 0.25 M C6H5SO3H(aq) (benzenesulfonic acid). The appropriate values for pKa or pKb are given inthe table.