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- 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.)Weak base B has a pKb of 6.78 and weak acid HA has a pKa of 5.12. a Which is the stronger base, B or A? b Which is the stronger acid, HA or BH+? c Consider the following reaction: B(aq)+HA(aq)BH+(aq)+A(aq) Based on the information about the acid/base strengths for the species in this reaction, is this reaction favored to proceed more to the right or more to the left? Why? d An aqueous solution is made in which the concentration of weak base B is one half the concentration of its acidic salt, BHCl, where BH+ is the conjugate weak add of B. Calculate the pH of the solution. e An aqueous solution is made in which the concentration of weak acid HA twice the concentration of the sodium salt of the weak acid, NaA. Calculate the pH of the solution. f Assume the conjugate pairs B/BH+ and HA/A are capable of being used as color-based end point indicators in acidbase titrations, where B is the base form indicator and BH is the acid form indicator, and HA is the acid form indicator and A is the base form indicator. Select the indicator pair that would be best to use in each of the following titrations: (1) Titration of a strong acid with a strong base. (i) B/BH+ (ii) HA/A (2) Titration of a weak base with a strong acid. (i) B/BH+ (ii) HA/AAmino acids are an important group of compounds. At low pH, both the carboxylic acid group (CO2H) and the amine group (NHR) are protonated. However, as the pH of the solution increases (say, by adding base), the carboxylic acid proton is removed, usually at a pH between 2 and 3. In a middle range of pHs, therefore, the amine group is protonated, but the carboxylic acid group has lost the proton. (This is called a zwitterion.) At more basic pH values, the amine proton is dissociated. What is the pH of a 0.20 M solution of alanine hydrochloride, [NH3CHCH3CO2H]Cl?
- (a) Calculate the pH in the solution formed by adding10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoicacid (C6H5COOH, Ka = 6.3 x 10-5). (b) Calculate the pHin the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.(a) Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoic acid (C6H5COOH, Ka = 6.3 * 10-5). (b) Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.4 a) Calculate the pH of the solution formed when 100 cm³ of 0.100 mol dm³ H₂SO4 is added to 50 cm³ of 0.500 mol dm NaOH. b) Calculate the pH of the solution formed when 25 cm³ of 0.250 mol dm³ HCI is added to 15 cm³ of 0.100 mol dm KOH. 5 Calculate the pH of the solution formed when 3.5 g of impure sodium hydroxide (98.7 % purity) is dissolved in water and made up to 100 cm³, and then 25 cm³ of 0.35 mol dm³ diprotic acid is added.
- What is the percent ionization of nitrous acid in a solution that is 0.230 M in nitrous acid (HNO2) and 0.270 M in potassium nitrite (KNO2)? The acid dissociation constant of nitrous acid is 4.50 x 10-4.11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting the resulting solution to a volume of 1.0 L. What is the effect of adding 0.020 mol CH3COO (aq) to this solution? How will pH change (calculate pH before and after the addition. Ka of CH3COOH is 1.76 x10-5)? How will concentrations of CH3COOH and CH3COO at equilibrium change?9) What will be the pH (aq., 25 oC) of 100.0 mL of a solution of 1.50 M C2H5NH3Br and 1.25 M C2H5NH2, after 2.00 mL of 10.00 M HCl has been added to it? Kb C2H5NH2 = 5.6 x 10–4
- Determine the pH during the titration of 36.4 mL of 0.299 M ethylamine (C,H;NH, K, = 4.3×104) by 0.299 M HBr at the following points. (Assume the titration is done at 25 °C.) Note that state symbols are not shown for species in this problem. (a) Before the addition of any HBr| (b) After the addition of 14.0 mL of HBr (c) At the titration midpoint (d) At the equivalence point (e) After adding 55.0 mL of HBrA milkman adds a very small amount of baking soda to fresh milk.(a) Why does he shift the pH of the milk from 6 to slightly alkaline?(b) Why does this milk take a long time to set a curd?An aqueous solution of benzoic acid and sodium benzoate has a pH of 5.1. The dissociation constant of benzoic acid is 6.5 x 10^-5. What is pKa of benzoic acid, concentration of sodium benzoate and benzoic acid?
