a) Sodium acetate, CH3COONa was hydrolysed in water, H2O. Show the reaction equations involved. What is the effect of the salt on the pH of this solution?
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Q: Sodium acetate, CH3COONA was hydrolysed in water, HzO. Show the reaction equations involved. What is…
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Q: Sodium acetate, CH3COONa was hydrolysed in water, H2O. Show the reaction equations involved. What is…
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- (a) Sodium acetate, CH3COONA was hydrolysed in water, H2O. Show the reaction equations involved. What is the effect of the salt on the pH of this solution? (b) (i) Define buffer solution. (ii) 2.50 g of sodium acetate, CH3COONA was dissolved in 150.0 mL of water, H2O. A solution of 0.025 M ethanoic acid, CH3COOH was added into the above salt solution. Calculate the pH of the mixed solution. [pKa of CH3COOH = 4.75, Molar mass of CH3COONA = 82.0 g mol-1] (c) Explain how the above buffer solution maintain its pH when a small amount of sodium hydroxide, NaOH is added.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 addedSodium acetate, CH3COONa was hydrolysed in water, H2O. Show thereaction equations involved. What is the effect of the salt on the pH of thissolution?
- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid, CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. a. Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. b. Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)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?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 0.100 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?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.The precipitation of Al(OH)3 (Ksp = 1.3 x 10-33) is sometimesused to purify water. (a) Estimate the pH at whichprecipitation of Al(OH)3 will begin if 5.0 lb of Al2(SO4)3is added to 2000 gal of water. (b) Approximately howmany pounds of CaO must be added to the water toachieve this pH?
- 6. (a) Aspirin is a weak acid with a pKa of 3.6 and MW 180 g/mol. The saturation solubility (S) of aspirin in water is 3.3 g /L and a saturated solution has pH equal to your answer to question 4(b) above. What is the solubility of the unionised form (So) of aspirin at this pH using units of mol/L and g/L. (b) Use the So value (just obtained) to calculate the saturation solubility (S) of aspirin in water at pH 6.6 using units of mol/L and g/L. (c) If you modified the aspirin suspension APF12 formula by replacing the purified water with pH 6.6 buffer, would the product be a suspension or solution?Sodium acetate, NaCH3CO2, of mass 7.4 g is used to prepare 250 cm3 of aqueous solution. What is the pH of the solution?Five solutions A, B, C, D and E when tested with universal indicators showed pH as 4, 1, 11, 7 and 9 respectively. Which solution is:(a) neutral?(b) strongly alkaline?(c) strongly acidic(d) weakly acidic?(e) weakly alkaline
