Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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Write the Lewis structures of the reactants and product of each of the following equations, and identify the Lewis acid and the Lewis base in each:(a) CO2 + OH− ⟶ HCO3 −(b) B(OH)3 + OH− ⟶ B(OH)4 −(c) I− + I2 ⟶ I3 −(d) AlCl3 + Cl− ⟶ AlCl4 − (use Al-Cl single bonds)(e) O2− + SO3 ⟶ SO4 2−
Consider the following equilibrium for nitrous acid, HNO2, a weak acid:
HNO2(aq) + H2O (l) <====> H3O+(aq) + NO2-(aq)
In which direction will the equilibrium shift if
NaOH is added?
NaNO2 is added ?
HCl is added?
The acid solution is made more dilute ?
Draw Lewis structures that show how electron pairs moveand bonds form and break in the following reaction, andidentify the Lewis acid and Lewis base.B(OH)3(aq) + 2 H2O(/) + B(OH)4^- (aq) +H3O^+(aq)
Chapter 16 Solutions
Chemistry: An Atoms-Focused Approach
Ch. 16 - Prob. 16.2VPCh. 16 - Prob. 16.3VPCh. 16 - Prob. 16.4VPCh. 16 - Prob. 16.5VPCh. 16 - Prob. 16.6VPCh. 16 - Prob. 16.7VPCh. 16 - Prob. 16.8VPCh. 16 - Prob. 16.9VPCh. 16 - Prob. 16.10VPCh. 16 - Prob. 16.11QA
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- Table 13-4 lists the stepwise Ka values for some polyprotic acids. What is the difference between a monoprotic acid, a diprotic acid, and a triprotic acid? Most polyprotic acids are weak acids; the major exception is H2SO4. To solve for the pH of a solution of H2SO4, you must generally solve a strong acid problem as well as a weak acid problem. Explain. Write out the reactions that refer to Ka1 and Ka2 for H2SO4. For H3PO4, Ka1 = 7.5 103, Ka2 = 6.2 108, and Ka3= 4.8 1013. Write out the reactions that refer to the Ka1, Ka2and Ka3equilibrium constants. What are the three acids in a solution of H3PO4? Which acid is strongest? What are the three conjugate bases in a solution of H3PO4? Which conjugate base is strongest? Summarize the strategy for calculating the pH of a polyprotic acid in water.arrow_forward25. Which of the following acids have relatively strong conjugate bases? a. HCN b. H2S c. HBrO4 d. HNO3arrow_forwardWhat is the ionization constant at 25 C for the weak acid CH3 NH3+, the conjugate acid of the weak base CH3NH2, Kb=4.4104.arrow_forward
- Ionization of the first proton from H2SeO4 is complete (H2SeO4 is a strong acid); the acid-ionization constant for the second proton is 1.2 102. a What would be the approximate hydronium-ion concentration in 0.150 M H2SeO4 if ionization of the second proton were ignored? b The ionization of the second proton must be considered for a more exact answer, however. Calculate the hydronium-ion concentration in 0.150 M H2SeO4, accounting for the ionization of both protons.arrow_forwardFor the following reactions, predict which direction the reaction will shift with the addition of hydrochloric acid. Cu2+ (aq) + 4Cl- (aq) [CuCl4]2- (aq) CaCO3(s)+H+(aq)Ca2+(aq)+HCO3-(aq) AgCl(s) → Ag+(aq) + Cl–(aq)arrow_forwardCalculate the pH of a 0.16 M carbonic acid solution, H 2CO 3(aq), that has the stepwise dissociation constants K a1 = 4.3 × 10 -7 and K a2 = 5.6 × 10 -11arrow_forward
- What is the equilibrium constant expression for the following reaction?0, (aq) + Fe2+(aq) + 8H*(aq) -Mn?+(aq) + Fe3+(aq) + 4H20(l)arrow_forward2. Boric acid, BOH is used as a mild antiseptic. What is the pH of a 0.025 aqueous solution of boric acid? What is the degree of ionisation of boric acid in this solution? The hydrogen ion arises principally from the reaction:B(OH)3(aq) + H2O(l) B(OH)4(aq)_+ H+(aq)The equilibrium constant for this reaction is 5.9 .arrow_forwardA student is required to determine the pH of a water sample that was believed to be contaminated with some Mg(OH)2 solution. Write a protocol to describe the steps and the procedure that the student must perform in order to determine the pH of the water sample.arrow_forward
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