Concept explainers
(a)
Interpretation:
The effect of adding
Concept introduction:
Equilibrium constant is a constant at any point of equilibrium; where, the ratio of the concentration of the products, each raised to power of their respective coefficient, to the concentration of the reactants, each raised to a power of their respective coefficient. Increase in concentration of any species, shifts the equilibrium in a direction to counteract the change.
(b)
Interpretation:
The effect of adding
Concept introduction:
Equilibrium constant is a constant at any point of equilibrium; where, the ratio of the concentration of the products, each raised to power of their respective coefficient, to the concentration of the reactants, each raised to a power of their respective coefficient. Increase in concentration of any species, shifts the equilibrium in a direction to counteract the change.
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INTRODUCTORY CHEMISTRY
- Ka for acetic acid at 25.0C is 1754 105. At 55.0C, Ka is 1.625 105. What are H and S for the ionization of acetic acid?arrow_forwardGiven a solution of acetic acid, with equilibrium net ionic equation (so only showing the ions in the reaction and not the spectator ions): CH3COOH (aq) + H20 () CH3COO (aq) + H3O* (aq) Have 4 beakers with acetic acid. Each beaker gets one of the following four things added to it. Match each thing with how the equilibrium responds when the thing is added. Prompts Submitted Answers sodium acetate Choose a match calcium acetate nothing sodium chloride shifts left to make more reactants acetic acid shifts right then left then right then left... shifts right to make more productsarrow_forwardThe dissociation of acetic acid, CH3COOH, has an equilibrium constant at 25 degrees celsius of 1.8 x 10-5. CH3COOH(aq) ⇋ CH3COO-(aq) + H+(aq) If the equilibrium concentration of CH3COOH is 0.46 moles in 0.500 L of water and that of CH3COO is 8.1 x 10-3 moles in the same 0.500 L, calculate the concentration of H + for the reaction.arrow_forward
- You are given the following information. acid Ка HF 7.2X10-4 HC2H302 1.8×10-5 HCIO 3.5X10-8 HCN 4.0X10-10 Determine the equilibrium constant for each of the following reactions and indicate which arrow would be more appropriate. (Hint: Reactions that produce less than 0.1% of products and reactions that retain less than 0.1% of reactants are not considered to be "equilibrium reactions"). (a) HC2H302 + F C2H302 K = 0 0.025 + HF (b) HCN + CIO - CN + HCIO K = 40 0.010 (c) HCIO + F - CIO + HF K = 40 87.5 lo+ (d) HF + CN + HCN K = 00 1.14e-2arrow_forwardWrite the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 CH3 COOH (аq) + H20(1) : H30+(aq) + CH3 COO¯ (aq) K =arrow_forwardConsider the cobalt-chloride ion equilibrium shown. Determine how the equilibrium will be affected by the addition of each reagent. Then, fill in the statements accordingly. Co(H, O), (aq) + 4 CI (aq) = CoCl; (aq) + 6 H, O(1) pink blue Adding HCl will shift the equilibrium Adding water will shift the equilibrium Answer Bank right neither direction leftarrow_forward
- Write the equilibrium constant expression for this reaction: NH,(aq)+H"(aq) → NH (aq) 믐arrow_forwardWrite the equilibrium constant expression for this reaction: 2 H* (aq) + C₂0 (aq) H₂C₂O4(aq) X Sarrow_forwardThe value of K, for ethylamine, C,H¿NH, is 4.30×104. Write the equation for the reaction that goes with this equilibrium constant. + +arrow_forward
- Write the equilibrium constant expression, K, for the following reaction. Please enter the compounds in the order given in the reaction. If either the numerator or denominator is blank, please enter 1 K = (CH3)3N(aq) + H₂O(1) — (CH3)3 NH+ (aq) + OH¯(aq)arrow_forwardFill in the Blanks HCO,H(aq) H(aq) + HCо, (аq) K = 1.8 x 104 K%D Blank 1 Blank 2 Blank 3 C Blank 4 Blank 5 Blank 6 Blank 7 Blank 8 Blank 9 Type your answers in all of the blanks and submit Consider the acid ionization reaction for formic acid that has a Ka = 1.8 x 10-4. HCO2H(aq) Ht (aq) + HCO, (aq) Formic acid is a weak acid first found in ants. It causes the burning sensation when ants bite someone. Based upon a 0.15 M aqueous formic acid solution fill in the ICE table in the accompanying diagram then calculate the pH value for the solution. Only enter numerical values or algebraic quantities such +7x or -7x.arrow_forwardConsider the following reaction: CH₃COOH(aq) + H₂O(l) ⇌ CH₃COO⁻(aq) + H₃O⁺(aq). An increase in the pressure of the chamber where this reaction takes place will result in A) an increase in CH₃COOH. B) an increase in CH₃COO⁻. C) an increase in H₃O⁺. D) both (B) and (C). E) no change.arrow_forward
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