What is the pH of a buffer solution that contains 0.180 M of a fictitious base and 0.135 M of its conjugate acid? The pK b of the base is 5.720.
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- What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when [HA]=0.540 and [A-]=0.580.What molar ratio of salt to acid would be required to prepare a buffer solution with a pH of 5.9? The pK a of the acid is 5.7.The pKa of a particular weak acid is 4.85. What is the pH of the weak acid solution when exactly half of the acid is neutralized?
- The ionization constant of lactic acid, CH,CH(OH)CO,H, an acid found in the blood after strenuous exercise, is 1.36 x 10-4. What is the concentration of hydronium ion in the solution of 0.102 M lactic acid? CH;CH(OH)CO,H (aq) + H,O (1) → H;O• (aq) + CH;CH(OH)CO, (aq) O 0.00372 M O 0.0165 M O 0.00549 M O 0.227 MThe pKb of the organic base nicotine (denoted Nic) is 5.98. Write the corresponding protonation reaction, the deprotonation reaction of the conjugate acid, and the value of pKa for nicotine.When the reversible reaction HC2H;O2 (aq) E> H(aq) + C2H3O2 (aq) is at equilibrium at room temperature, pH of the reaction mixture is 5. What will be the change in pH when you add a large amount of NaOH (aq) to the reaction mixture? a) pH will not change because NaOH is not a part of the reaction equation. b) pH will not change because acetic acid and NaOH form a buffer. c) pH will increase because NaOH will completely neutralize acetic acid. d) pH will decrease because NaOH will completely neutralize acetic acid. In the reversible reaction A (aq) + B(aq) E > C(aq), reactant A is very expensive. What are two ways to get it to react as fully as possible to form as much C as possible? a) remove C as it forms, and use an excess of A b) add another reactant that will form a precipitate with B c) remove C as it forms, and use an excess of B d) add another reactant that will form a precipitate with A
- Calculate the pH for a mixture of one mole of benzoic acid and one mole of sodium benzoate. The pKa of benzoic acid is 4.2. 0 2 8 8 2 8 2 5 6Calculate the pH of the solution in which 0.2M NH4Cl and 0.1M NH3 are present. The pKb of ammonia solution is 4.75.Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86.
- 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.A chemical system is set up by placing some solid ammonium chloride in an ammonia solution. The equilibrium established can be represented as follows: NH4*(aq) + H2O(e) 2 H30*(aq) + NH3(aq) The pH of the solution is taken, then a small amount of NaOH(aq) is added and the pH is taken again. What can be said about the change in pH for the solution? The pH significantly increases because a strong base has been added to the solution. The pH significantly decreases because a strong base has been added to the solution. There is very little change to the pH of the solution. If anything the pH of the solution decreases slightly. There is very little change to the pH of the solution. If anything the pH of the solution increases slightly.The balanced molecular equation for complete neutralization of H2SO4 by KOH in aqueous solution is: Group of answer choices 2H+ (aq) + 2OH- (aq) → 2H2O (l) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq)