Question

Write the chemical reaction for the autoionization of water (equilibrium constant Kw). Look up the numerical...

  1. Write the chemical reaction for the autoionization of water (equilibrium constant Kw).

  2. Look up the numerical value for Kw at Tinitial (Use the average of Tinitial from both trials) -Its 6.81x10^-15

  3. How is the equation in Question 1 related to the net ionic equation for the strong acid-strong base neutralization shown below?

    H3O+(aq) + OH-(aq) → H2O(l) + H2O(l)

  4. Use the value of Kw and the relationship between the equations in Questions 1 and 3 to find the numerical value

    of K for the neutralization reaction in question 3.

  5. Use the value of K calculated for the neutralization reaction in Question 4 to calculate ΔG for the neutralization reaction. (Use average Tinitial from the two trials as the value of T.)

  6. Use the values of ΔG and ΔHn that you have already calculated to calculate ΔS° for the reaction. (Use average Tinitial from the two trials as the value of T.)

0 0
Add a comment Improve this question Transcribed image text
Answer #1

Chemical reaction for autoionization of water, H₂O(l) + H₂O(l) H₂O + (aq) + OH (94) Kw = 6.81810-15 = [H₂0 tags] [ot cons] Ne

Add a comment
Know the answer?
Add Answer to:
Write the chemical reaction for the autoionization of water (equilibrium constant Kw). Look up the numerical...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions
  • Part A Which is a net ionic equation for the neutralization reaction of a strong acid...

    Part A Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base? Which is a net ionic equation for the neutralization reaction of a strong acid with a weak base? HCl(aq) + NH3(aq) ↔ NH4Cl(aq) H3O+(aq) + NH3(aq) ↔ NH4+(aq) + H2O(l) HCl(aq) + NaOH(aq) ↔ H2O(l) + NaCl(aq) H3O+(aq) + OH-(aq) ↔ 2 H2O(l)

  • The answer 1.225 x 10^-7 is coming up as incorrect. INTERACTIVE EXAMPLE Autoionization of Water The...

    The answer 1.225 x 10^-7 is coming up as incorrect. INTERACTIVE EXAMPLE Autoionization of Water The value of Ky at 25 °C is 1.0 x 10-14 At 30 °C, the value of Ky is 1.5*10-14. a.) Using LeChatelier's principle, predict whether the autoionization of water is exothermic or endothermic. 2 H2O(1) = H30+ (aq) + OH- (aq) b.) Calculate [H30*] and [OH-] in a neutral solution at 30°C. HOW DO WE GET THERE? What are the concentrations of [H3O+] and...

  • pH operates off of a ___________ scale.                 The autoionization constant of water is abbreviated ________....

    pH operates off of a ___________ scale.                 The autoionization constant of water is abbreviated ________.                 The molar concentration of hydronium in pure water at 25ºC has been measured to be ________.                 The relationship between hydronium and hydroxide in any dilute aqueous solution is represented by _________.                 The p in pH stands for _________.                 The relationship between pH and pOH is ___________.                 The pH value of a 1 M solution of strong acid would be...

  • The value for the equilibrium constant for the following chemical reaction, the auto-ionization of water, is...

    The value for the equilibrium constant for the following chemical reaction, the auto-ionization of water, is 1.0x10-14 at 298 K 2H2O(l) ßà OH-(aq) + H3O+(aq) K = 1.0x10-14 Using this information and your equilibrium identities, select the correct value for the equilibrium expression for the reaction shown below (at 298 K as well) : OH-(aq) + H3O+(aq)  ßà 2H2O(l) K = ? Question 4 options: 1x10-14 0.5x10-14 2x10-14 -1x10-14 1x1014 1x10-15

  • please calculate the value of the equilibrium constant 2. The beaker contains 0.1894 M CHCOOH and...

    please calculate the value of the equilibrium constant 2. The beaker contains 0.1894 M CHCOOH and the buret contains 0.2006 M NaOH. Write a complete balanced equation for the neutralization reaction between CH,COOH and NaOH and then write a balanced net ionic equation for this chemical reaction. Neutralzatu: CH3COOH (44) + NaOH(a) - CH3COONS (0) + H2O(l) Net equation : CH3COOH (44) + OH (41) - CH3COO(0) MLO (A) 6. Calculate the value of the equilibrium constant for the balanced...

  • The value of the equilibrium constant for the following chemical reaction (the auto-ionization of water) is...

    The value of the equilibrium constant for the following chemical reaction (the auto-ionization of water) is 1.0x10-14 at 298 K. 2H2O(l) ßà OH-(aq) + H3O+(aq) K = 1.0x10-14 Using this information and your equilibrium identities, select the correct value for the equilibrium expression for the following chemical reaction (at 298 K as well): 6H2O(l) ßà 3OH-(aq) + 3H3O+(aq) K = ? Question 5 options: 1x1014 1x10-28 1x10-14 1x10-42 3x10-14 1x10-15

  • A process at constant T and P can be described as spontaneous if ΔG < 0...

    A process at constant T and P can be described as spontaneous if ΔG < 0 and nonspontaneous if ΔG > 0. Over what range of temperatures is the following process spontaneous? Assume that gases are at a pressure of 1 atm. (Hint: Use the data below to calculate ΔH and ΔS [assumed independent of temperature and equal to ΔH° and ΔS°, respectively] and then use the definition of ΔG.) PCl3(g) + Cl2(g) → PCl5(g) ΔHf° (kJ mol-1) -287.0 -374.9...

  • 1)Write the balanced NET IONIC equation for the reaction that occurs when hydrocyanic acid and potassium...

    1)Write the balanced NET IONIC equation for the reaction that occurs when hydrocyanic acid and potassium hydroxide are combined. (aq)(s)(l)(g) + (aq)(s)(l)(g) (aq)(s)(l)(g) + (aq)(s)(l)(g) + (aq)(s)(l)(g) This reaction is classified as . A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid + Weak Base 2)Write the balanced NET IONIC equation for the reaction that occurs when nitric acid and ammonia are combined. Use H3O+ instead of H+....

  • What is the net ionic equation for the neutralization reaction between a HI with NH3? HI...

    What is the net ionic equation for the neutralization reaction between a HI with NH3? HI (aq) + NH3 (aq) ⇌ NH4I (aq), HI (aq) + OH- (aq) ⇌ H2O (l) + I- (aq), H3O+ (aq) + OH- (aq) ⇌ 2 H2O (l) H3O+ (aq) = NH3 (aq) = NH4+ (aq) + H2O (l) Which statement about buffers is NOT true? A buffer can be made by neutralizing some of the weak base in solution by adding a strong acid,...

  • The equilibrium constant for the reaction,                                   &nb

    The equilibrium constant for the reaction,                                                               2Fe3+ (aq) + Hg22+(aq)   2Fe2+ (aq) + 2Hg2+ is Kc = 9.1 x 10-6 @298K a. What is ΔGo at this temperature? b. If reactants and products in their standard state concentrations (1M) are mixed, in which direction does the reaction proceed? Provide a numerical justification for your response. c. Calculate ΔG when [Fe3+] = 0.20 M, [Hg22+] = 0.010 M, [Fe2+] = 0.010 M, and [Hg2+] = 0.025 M. In which direction will the...

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT