Concept explainers
(a)
Interpretation: The value of equilibrium constant, relationship between
Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The
To determine: The value of equilibrium constant.
(b)
Interpretation: The value of equilibrium constant, relationship between
Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The
To determine: The relationship between
(c)
Interpretation: The value of equilibrium constant, relationship between
Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The
To determine: The expression for
(d)
Interpretation: The value of equilibrium constant, relationship between
Concept introduction: The equilibrium constant is defined as the numeric number that describes the relationship between amount of product and amount of reactant at equilibrium. The
To determine: The
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Chemistry: An Atoms First Approach
- Calculate the pH of a 0.200-M solution of C5H5NHF. Hint: C5H5NHF is a salt composed of C5H5NH+ and F ions. The principal equilibrium in this solution is the best acid reacting with the best base; the reaction for the principal equilibrium is C5H5NH+(aq)+F(aq)C5H5N(aq)+HF(aq)K=8.2103arrow_forwardMagnesium hydroxide, Mg(OH)2, is the active ingredient in die antacid TUMS and has a Ksp value of 8.9 1012. If a 10.0-g sample of Mg(OH)2 is placed in 500.0 mL of solution, calculate the moles of OH ions present. Because the Ksp value for Mg(OH)2 is much less than 1, not a lot of solid dissolves in solution. Explain how Mg(OH)2 works to neutralize large amounts of stomach acid.arrow_forwardCalculate the CO2+ equilibrium concentration when 0.100 mole of [CO(NH3)6](NO3)2 is added to a solution with 0.025 M NH3. Assume the volume is 1.00 L.arrow_forward
- What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?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_forwardFor each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly. (a) NH4+(aq) + Br(aq) NH3(aq) + HBr(aq) (b) HPO42(aq) + CH3CO2(aq) PO43(aq) + CH3CO2H(aq) (c)[Fe(H2O)6]3+(aq) + HCO3(aq) [Fe(H2O)5(OH)]2+(aq) + H2CO3(aq)arrow_forward
- What is the effect on the concentrations of NO2-, HNO2, and OH- when the following are added to a solution of KNO2 in water: (a) HCl. (b) HNO2. (c) NaOH. (d) NaCl. (e) KNO The equation for the equilibrium is: NO2(aq)+H2O(l)HNO2+OH(aq)arrow_forwardSulphurous acid, H2SO3, is a weak acid capable of providing two H+ ions. (a) What is the pH of a 0.45M solution of H2SO3? (b) What is the equilibrium concentration of the sulphate ion SO32, in the 0.45M solution of H2SO3?arrow_forwardThe pigment cyanidin aglycone is one of the anthocyanin molecules that gives red cabbage (Brassica oleracea var. capitata f. rubra) its characteristic red coloration. Many chemistry students have used this red cabbage indicator to study acid-base chemistry. Estimate tire pH range at which cyanidin agly-cone shows a color change. Anth-H(aq) Anth(aq) + H+ (aq) Ka = 1.3 107arrow_forward
- What are the major species in solution after NaHSO4 is dissolved in water? What happens to the pH of the solution as more NaHSO4 is added? Why? Would the results vary if baking soda (NaHCO3) were used instead?arrow_forwarda. What is the equilibrium constant, K, for the reaction between HCN (Ka = 6.2 x 10⁻¹⁰) and OH⁻ at 25 °C? b. What is the equilibrium constant, K, for the reaction between NH₄⁺ (Ka = 5.6 x 10⁻¹⁰) and OH⁻ at 25 °C?arrow_forwardEquilibrium: Co(H2O)6 2+ (aq) + 4 Cl-(aq) ⇌ CoCl4 2- (aq) + 6 H2O (l) pink blue a. You put 5 mL of stock solution into each of five test tubes. (25 mLs divided evenly into 5 test tubes). Test tube 1 was your control. To test tube 2, you added some water. Which direction did the equilibrium shift? How do you know? b. To test tube 3 you added some silver nitrate. Did this shift the equilibrium? If so, how is that possible as silver ion and nitrate ion are not in the equation? c. To test tube 5, you put the stock solution into hot water and it turned blue; then you put it into ice water and it turned pink. Explain what happened.arrow_forward
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