The equilibrium constant for the following reaction has been estimated to be
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GENERAL CHEMISTRY-MOD.MASTERINGCHEM.
- Consider the reaction: HSO4-(aq) + H2O(l) ⇌ H3O+(aq) + SO42-(aq) Drops of sodium sulfate solution are added to 10 drops of sodium hydrogen sulfate solution until a reaction occurs. The reaction indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? Crystals of solid sodium hydrogen sulfate are added to 10 drops of sodium hydrogen sulfate solution until a reaction occurs. The reaction indicated a shift in the point of equilibrium. In which direction did the equilibrium shift?arrow_forwardWrite the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HF (aq) + OH- (aq)F- (aq) + H2O (l) K =arrow_forwardYou are on one of Saturn's many moons and discover a substance, Y2O that undergoes autoionization just like water on Earth. Y2O + Y2O ⇌ Y3O+ + OY– Through a series of experiments, you determine the equilibrium constant (Keq) for this autoionization reaction at various temperatures. The value of Keq at 28.7ºC is 7.6 x 10-14. What is the pY of the pure substance at this temperature? Report your answer to the hundreths placearrow_forward
- The binding of oxygen by hemoglobin (Hb), giving oxyhemoglobin (HbO2), is partially regulated by the concentration of H3O+ and dissolved CO2 in the blood. Although the equilibrium is complicated, it can be summarized asHbO2(aq) + H3 O+(aq) + CO2(g) ⇌ CO2 −Hb−H+ + O2(g) + H2 O(i)(a) Write the equilibrium constant expression for this reaction.(b) Explain why the production of lactic acid and CO2 in a muscle during exertion stimulates release of O2 from the oxyhemoglobin in the blood passing through the muscle.arrow_forwardWrite the equilibrium constant expression for the following reaction: N2O (g) + NO2 (g) ⇌ 3NO (g)arrow_forward1. Write equilibrium constant expressions for the following reactions: 1a.) HCOOH(aq) ⇌ H+(aq) + HCOO–(aq) 1b.) 2HgO(s) ⇌ 2Hg(l) + O2(g) 2.) For the reaction I2(g) ⇌ 2I(g), Kc = 3.8 x 10–5 at 727°C. (a) What is Kc for the reverse reaction at this temperature? (b) Calculate Kc for the reaction ½I2(g) ⇌ I(g).arrow_forward
- You are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth. Z2O + Z2O ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 26.8ºC is 6.9 x 10-14. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths placearrow_forwardThe acetate ion, CH3COO–, reacts with water as a weak base: CH3COO–(aq) + H2O(l) ⇄ CH3COOH(aq) + OH–(aq), with K = 5.7 x 10-10 at 25°C. If sodium acetate were dissolved in water to make a 0.35 M solution, what would be the resulting concentration of OH–? (M) (no scientific notation)arrow_forwardAcetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (d) When starting with completely un-dissociated acetic acid, is it accurate to assume that [HOAc]0 = [HOAc]eq? Why or why not? (e) A highly concentrated acetic acid solution contains 15.0M acetic acid at equilibrium. What are the equilibrium concentrations of the hydronium and acetate ions in this solution? (f) Creating the concentrated acetic acid solution by dissolving liquid HOAc in water raises the temperature of the water by about 5°C from room temperature. At 50°C, do you expect the solution to contain more or less acetate ion OAc– than what you calculated in (c)? Why?arrow_forward
- Acetic acid is a weak acid, meaning it does not fully dissociate in water. Instead, there is an equilibrium between the dissolved but undissociated molecule and the component ions: HOAc (aq) + H2O (l) ⇌ H3O+ (aq) + OAc– (aq)OAc– is an abbreviation for the acetate ion, CH3COO–, and H3O+ is the hydronium ion (lone protons, H+ (aq), do not exist!). (a) Write the equilibrium constant expression for the dissociation of acetic acid. (b) Vinegar sold commercially is typically 0.8 − 1.0 M acetic acid. A 1.00 M solution of acetic acid is measured by its pH to have an equilibrium concentration of 4.19×10−3 M for both acetate ions and hydronium ions at room temperature. Assuming [HOAc]0 = 1.00M, what is the equilibrium concentration of undissociated acetic acid [HOAc]eq to the correct number of significant figures? (c) What is the value of the equilibrium constant Keq for the dissociation according to the concentrations from part (b)? (d) When starting with completely un-dissociated…arrow_forwardAt 25 oC, Ammonia is a weak base that reacts with water according to this equation: NH3(aq) + H2O(aq) ⇌ NH4+(aq) + OH−(aq) Briefly explain how the equilibrium will shift (to get back to equilibrium) if the following perturbations are made to the system: (a) Addition of HCl (b) Addition of NaOH (c) Addition of NH4Clarrow_forwardThe Haber process for ammonia synthesis is exothermic:N2(g) + 3H2(g) ⇌ 2NH3(g); ΔH° = -92 kJIf the equilibrium constant Kc for this process at 500.°C is 6.0 × 10-2, what is its value at 300.°C?arrow_forward
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning