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Many acids are partially dissociated into ions in aqueous solution. Trichloroacetic acid
What is the percentage of molecules dissociated if the freezing point of a 1.00 m solution of trichloroacetic acid in water is
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- Phosphoric acid, H3PO4, is a triprotic acid, for which Ka1 =7.2 x 103, Ka2 = 6.3 × 10-8 and Ka3 = 4.2 x 1013. What is the value of K for the following equation. HPO42 (aq) + H20(1) Z H,PO4 (aq) + OH"(aq) Express your answer in scientific notation rounded to three significant figures.arrow_forwardAt a particular temperature, aluminum hydroxide , Al(OH)3, has a Ksp = 2.52×10-31. What is the hydroxide ion concentration in a saturated aluminum hydroxide solution?arrow_forwardHypochlorous acid (HOCl) has an ionization constant of 3.2 × 10 -8. What is its percent ionization in 1.0 M and 0.10 M solutions, respectively?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!). (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_forward1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439M solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is the identity of thisunknown acid?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!). (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_forward
- An aqueous solution of formic acid, that is 1.00 percent by weight formic acid, has a density of 1.0006 g/mL. A student determines that the freezing point of this solution is -0.418 °C. Based on the observed freezing point, what is the percent ionization of the acid and the value of Ka? Kf for H2O is 1.86 °C/m. % ionized = % Ka =arrow_forwardUse the following neutralization reaction to answer the questions: 2HCl(aq) + Ca(OH)2(aq) → CaCl2(aq) + 2H2O(l) Determine the number of moles of HCl needed to perfectly neutralize 0.037 moles of Ca(OH)2. Starting with 0.037 moles of Ca(OH)2, what would be the concentration of CaCl2(aq) if the total volume of the solution is 500.0mL?arrow_forwardThe pHpH of a solution of Ba(OH)2Ba(OH)2 is 10.66 at 25∘C.25∘C. What is the hydroxide ion concentration in the solution? If the solution volume is 125mL125mL what mass of Ba(OH)2Ba(OH)2 must have been dissolvedarrow_forward
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