Consider the following hypothetical dissociation:
(a) addition of A(NO3)3
(b) increase in temperature
(c) adding Na+, forming NaB
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Chemistry: Principles and Reactions
- Consider citric acid, H3C6H5O7, added to many soft drinks. The equilibrium constants for its step-wise ionization areKa1=7.5104 ,Ka2=1.7105, andKa3=4.0107. Write the overall net ionic equation and calculate K for the complete ionization of citric acid.arrow_forwardFor conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)arrow_forwardKafor acetic acid (HC2H3O2) at 25°C is 1.754105 . At 50°C, Kais 1.633105 . Assuming that H° and S° are not affected by a change in temperature, calculate S° for the ionization of acetic acid.arrow_forward
- The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10–5. If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present?arrow_forwardThe ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?arrow_forwardSaccharin, a sugar substitute, is a weak acid with the formula, HC7H4NSO3. The pKa of saccharin is 2.320. d. What are the equilibrium concentrations of the reactants and products in a 0.100M solution of saccharin? e. What is the pH, pOH, and %ionization of this weak acid?arrow_forward
- Write the equilibrium for the autoionization of sulfuric acids (H 2 SO 4 ) and write the expression for the equilibrium constant for this process.arrow_forwardSuppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the calculations would then have to be made to determine the molar concentrations of the base?arrow_forwardProve that Ka3 Kb1 = Kw for phosphoric acid, H3PO4, by adding the chemical equilibrium expressions that corresponds to the third ionization step of the acid in water with the first of the three successive steps of the reaction of phosphate ion, PO43, with water.arrow_forward
- Consider a 0.60-M solution of HC3H5O3, lactic acid (Ka = 1.4 104). a. Which of the following are major species in the solution? i. HC3H5O3 ii. C3H5O3 iii. H+ iv. H2O v. OH b. Complete the following ICE table in terms of x, the amount (mol/L) of lactic acid that dissociates to reach equilibrium. c. What is the equilibrium concentration for C3H3O3? d. Calculate the pH of the solution.arrow_forwardAcrylic acid is used in the polymer industry in the production of acrylates. Its K, is 5.6 X 10“’. What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?arrow_forwardWhat is the freezing point of vinegar, which is an aqueous solution of 5.00% acetic acid, HC2H3O2, by mass (d=1.006g/cm3)?arrow_forward
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