Concept explainers
For each of the following reactions, predict whether the equilibrium lies predominantly to the left or to the right. Explain your predictions briefly.
- (a) H2S(aq) + CO32−(aq) ⇄ HS−(aq) + HCO3−(aq)
- (b) HCN(aq) + SO42−(aq) ⇄ CN(aq) + HSO4(aq)
- (c) SO42−(aq) + CH3CO2H(aq) ⇄ HSO4−(aq) + CH3CO2−(aq)
(a)
Interpretation: The direction of the equilibrium for the given reaction is to be determined.
Concept introduction: An acid-base reaction reaction is represented as written below.
The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants
Answer to Problem 38PS
The equilibrium for the given reaction will lie in right direction predominantly.
Explanation of Solution
The equilibrium for the given reaction will move in left side is explained below.
Here, the acid
(b)
Interpretation: The direction of the equilibrium for the given reaction is to be determined.
Concept introduction: An acid-base reaction reaction is represented as written below.
The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants
Answer to Problem 38PS
The equilibrium for the given reaction will lie in left direction predominantly.
Explanation of Solution
The equilibrium for the given reaction will move in left side is explained below.
Here, the conjugate acid
(c)
Interpretation: The direction of the equilibrium for the given reaction is to be determined.
Concept introduction: An acid-base reaction reaction is represented as written below.
The base will take up the proton from acid and form its conjugate acid and simultaneously acid will form its conjugate base. The equilibrium will be forward or backward can be determined by using the dissociation constants
Answer to Problem 38PS
The equilibrium for the given reaction will lie in left side predominantly.
Explanation of Solution
The equilibrium for the given reaction will move in left side is explained below.
Here, the conjugate acid
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Chapter 16 Solutions
Chemistry & Chemical Reactivity
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- HA is a weak acid. Which equilibrium corresponds to the equilibrium constant Kb for A−? Group of answer choices HA(aq) + H2O(l) ⇌ H2A+(aq) + OH− A−(aq) + H3O+(aq) ⇌ HA (aq) + H2O(l) HA(aq) + OH−(aq) ⇌ H2O(l) + H+(aq) A−(aq) + H2O(l) ⇌ HA(aq) + OH−(aq) A−(aq) + OH−(aq) ⇌ HOA2−arrow_forwardIdentify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base in each reaction: (a) (CH3)3N(aq) +H2O(1) = (CH3)3NH+(aq)+ OH (aq) (b) HNO3 (aq) + H2O(1) = H3O+(aq) + NO3-(aq) Drag the appropriate items to their respective bins. Reset Help (CH3)3N H2O (a) (CH3)3NH+ OH HNO3 H2O (b) H30+ NO3 Brønsted- Lowry acid Brønsted- Lowry base Conjugate acid Conjugate basearrow_forwardSelect the reaction that depicts the ionization of a weak acid in water. Group of answer choices HNO3(aq) + H2O(l) ⇌ NO3‒(aq) + H3O+(aq) NH3(aq) + H2O(l) ⇌ NH2‒(aq) + H3O+(aq) NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH‒(aq) HF(aq) + H2O(l) ⇌ F‒(aq) + H3O+(aq)arrow_forward
- For each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base. C4H5N(aq)+H2O(l)⇌C4H5NH+aq)+OH(aq)C4H5N(aq)+H2O(l)⇌C4H5NH+(aq)+OH−(aq) Express your answers as chemical formulas. Enter your answers in the order given in the question separated by commas.arrow_forwardDrinking water is often disinfected with Cl₂, which hy-drolyzes to form HClO, a weak acid but powerful disinfectant Cl₂(aq)+2H₂O(l) ⇌HClO(aq)+H₃O(aq)+Cl(aq)The fraction of HClO in solution is defined (a) What is the fraction of HClO at pH 7.00 (Kaof HClO = 2.9X10⁻⁸)? (b) What is the fraction at pH 10.00?arrow_forwardThe following reaction shows the first deprotonation of carbonic acid. Identify the conjugate acid. H₂CO3 (1) H₂O (1) HCO3- (aq) H3O+ (aq) H₂CO3 (1) + H₂0 (1)→ HCO3 (aq) + H3O+ (aq)arrow_forward
- Calculate the ionization constant for each of the following acids or bases from the ionization constant of its conjugate base or conjugate acid:(a) F−(b) NH4+(c) AsO43−(d) (CH3)2 NH2+(e) NO2−(f) HC2 O4− (as a base)arrow_forwardConsider the following acidic equilibrium: H₂CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + H₃O⁺(aq). If you add NaHCO₃ to this solution, which of the following will occur? A) The reaction quotient will decrease. B) The reaction will shift in the reverse direction. C) The equilibrium constant will increase. D) No changes to the equilibrium positions will take place.arrow_forwardIndicate whether each of the following statements is corrector incorrect.(a) Every Brønsted–Lowry acid is also a Lewis acid.(b) Every Lewis acid is also a Brønsted–Lowry acid.(c) Conjugate acids of weak bases produce more acidic solutionsthan conjugate acids of strong bases. (d) K+ ion is acidic in water because it causes hydrating watermolecules to become more acidic.(e) The percent ionization of a weak acid in water increasesas the concentration of acid decreases.arrow_forward
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