Exercise: Determine AHP and AS for the auto-ionization of water.2 H₂OTemperature (°C)025354050H₂O (aq) + OH(aq)Ln(K₂)Ku1.14 101.00×102.09 x 1042.92 x 1045.47x10-¹4Ln(K) = -Hints:1. The linear equation that correlates the temperature and equilibrium constant iscalled vant's Hoff equationAH1T(K)3. Take the reciprocal of T(K)-4. Covert Kw to Ln(K)5. Obtain the best-fit straight line, slope8.314 J/mol.k→ AH = -slope x 8.3146. ASY-intercept x 8.314R2. Convert T in °C to T in K, T(K)= T(C) +273T(K)+45°ΔΗRsince R (ideal gas constant) ==

The van't Hoff equation relates the temperature and equilibrium constant as- Ln (K)=-∆H°R1T+∆S°R

Answered: Determine AHF and AS" for the…

Determine AHF and AS" for the auto-ionization 2 H₂O Temperature (°C) K₂ H₂O() 25 35 40 50 of water. + OH) 1.14 10 1.00×10 2.09 - 10 2.92 × 10 5.47 104 T(K) Ln(K₂)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Exercise Consider the following data to determine the effect of concentration on the ionization of acetic acid (CH3COOH, ka = 1.8 × 105). [CH3COOH]_[H*]eg.__ Calculate the [H*]eq. Hints: 1) Build ICE table for the equilibrium I C 2) K- E CH3COOH(aq) [CH3COOH]; -X 0.001 0.004 0.010 0.015 0.050 [CH3COOH]; -X % ionization of CH,COOH CH3COO 0 +X +X [CH₂COO"] [H]g. [CH₂COOH) 3) X=[H]q[CH₂COO], then X²-k₁ x [CH₂COOH], this is true if [H]q [CH,COOH] (aq) -x100 ≤ 5% +H* (aq) 0 +X +X 4) If % ionization of CH3COOH > 5% then you have to solve for the quadratic equations
The equilibrium concentration of hydroxide ion in a saturated magnesium hydroxide solution is that Ksp (Mg(OH)₂) = 1.5 × 10-¹¹.) Submit Answer Retry Entire Group 2 more group attempts remaining M. (Assume
The pH at 25 °C of an aqueous solution of the sodium salt of o-cresol (NaC,H,O) is 11.60. Calculate the concentration of CH,O° in this solution, in moles per liter. K, for HC,H,0 is equal to 6.3x1011. M Submit Answer
Chemistry Question 1 Consider a flask containing 50.00 mL of 0.0426 M trimethylamine ((CH3);NH3). This is titrated with a 0.0957 M hydrochloric acid solution from a burette. Given: K, of (CH,),NH3 is 6.5 × 10~s. 1 1.1 Determine the pH of the solution in the flask after 28.00 mL of the acid has been added? You must show any reaction equation(s) that you may think are necessary. 1.2 Determine the pH of the solution in the flask at the half-way point of the titration.
Calculation Propanoic acid, a weak acid found in human sweat, has the following aqueous ionization reaction equation." CH3 CH2CO2H(aq)=H+(aq) + CH3CH2CO, (aq) Ka = 1.3 x 10–5 The measured pH for an aqueous propanoic acid solution is 1.78. What is the molar concentration of this solution?
Exercise: Consider the following data to determine the effect of concentration on the ionization of acetic acid (CH3COOH, k, = 1.8 × 105). [H*]cq. % ionization of CH3COOH [CH₂COOH]; 0.01 (a) Calculate the [H*]eq. (b) Plot the % ionization of CH3COOH vs. [CH3COOH]; (c) State whether the following statement is TRUE or FALSE, Circle your answer The % ionization of CH3COOH increases as [CH3COOH]; increases. True, False 2) K- 0.04 0.10 0.15 0.50 Hints: 1) Build ICE table for the equilibrium I C CH₂COOH(aq) [CH₂COOH]; -X E [CH₂COOH]; -X [CH,COO] [H*]eq. [CH₂COOH]q 3) X=[H]eq=[CH3COO™]q 4) X²=k₂x [CH₂COOH]; CH3COO(aq) + Ha (aq) 0 5) % ionization of CH₂COOH: 0 +X +X X=√√K x[CH,COOH], [H*]q [CH₂COOH]; -x100 +X +X
Exercise 1 Calculate the pH of each of the following solutions: (a) 0.63 M NaCH3CO2(aq), K, = 5.62 × 10-10, %3D (b) 0.19 M NH4CI(aq), K, = 5.6 × 10-10; %3D (c) 0.65 M KCN(aq), K½ = 2 × 10-5.
The solubility of CUCO, in water at 25 °C is measured to be 0.0019 Use this information to calculate K for CUCO2. L sp Round your answer to 2 significant digits. Explanation Check 2021 McGraw-Hill Education. All Rights Reserved. Term cer の

The percentage deprotonation of a weak, monoprotic acid HA in a 0.110 M solution is 2.4%. What is the pH and Ka of the acid? Please provide only typed answer solution no handwritten solution needed allowed
What is the pressure of CO, in equilibrium with carbonated water at 25 °C and pH = 4.60? Poo, = 4.9 x10-11 Incorrect atm
This question has multiple parts. a Which of the following reactions show how HCO3- acts as a Bronsted-Lowry acid? (Select all that apply.) HCO3-(aq) + H2O → H2CO3(aq) + OH-(aq) HCO3-(aq) + Na+(aq) → NaHCO3(s) HCO3-(aq) + H3O+(aq) → H2CO3(aq) + H2O HCO3-(aq) + OH-(aq) → CO32-(aq) + H2O HCO3-(aq) + H2O → CO32-(aq) + H3O+(aq) b Which of the following reactions show how HCO3- acts as a Bronsted-Lowry base? (Select all that apply.) HCO3-(aq) + H2O → H2CO3(aq) + OH-(aq) HCO3-(aq) + Na+(aq) → NaHCO3(s) HCO3-(aq) + H3O+(aq) → H2CO3(aq) + H2O HCO3-(aq) + OH-(aq) → CO32-(aq) + H2O HCO3-(aq) + H2O → CO32-(aq) + H3O+(aq)
Which of the following statements is/are false for the pH of a 0.01 M Na PO, solution versus the pH of a 0.01 M in FeSO4 solution? (Select all that apply) O The activity coefficient for H is smaller in 0.01 M Na PO, than in 0.01 M FESO4.- The OH activity in 0.01 M Na PO4 is not equal to the OH activity in 0.01 M FESO4. The H+ activity in 0.01 M Na3PO4 is not equal to the H' activity in 0.01 M FeSO4. O The activity coefficient for OH is larger in 0.01 M Na PO, than in 0.01 M FESO4. The H concentration in 0.01 M Na PO4 is equal to the H concentration in 0.01 M FeSO4.