Question
solve this showing all working for tge quadratic equation
there is a rule concerning whether or not to ignore the “-X“ when using the kb equation to formulate the quadratic equation

Q1_(10pts)_(YOU NEED TO USE ICE TABLE WITH UNITS: WRONG INCORRECT ICE TABLE - 0 POINTS). Ka for HCN is 4.9 x 10-10, What is t
0 0
Add a comment Improve this question Transcribed image text
Request Professional Answer

Request Answer!

We need at least 10 more requests to produce the answer.

0 / 10 have requested this problem solution

The more requests, the faster the answer.

Request! (Login Required)


All students who have requested the answer will be notified once they are available.
Know the answer?
Add Answer to:
solve this showing all working for tge quadratic equation there is a rule concerning whether or...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Similar Homework Help Questions
  • Hey guys, I am having a lot of trouble with my homework. Could you please help?...

    Hey guys, I am having a lot of trouble with my homework. Could you please help? I thumbs up anyone who gives a thorough explanation and shows the work! I really need to understand these concepts! Thank you guys! 1) The Ka for HCN is 4.9 ~ 10-10. What is the value of Kb for CN-? 2) Using the data in the table for 0.10 M aqueous species at 25 °C, which conjugate base below is the weakest base? Explain...

  • Hey guys, I am having a lot of trouble with my homework. Could you please help?...

    Hey guys, I am having a lot of trouble with my homework. Could you please help? I thumbs up anyone who gives a thorough explanation and shows the work! I really need to understand these concepts! Thanks in advance! 1) The Ka for HCN is 4.9 ~ 10-10. What is the value of Kb for CN-? 2) Using the data in the table for 0.10 M aqueous species at 25 °C, which conjugate base below is the weakest base? Explain...

  • Hey guys, I am having a lot of trouble with my homework. Could you please help?...

    Hey guys, I am having a lot of trouble with my homework. Could you please help? I thumbs up anyone who gives a thorough explanation and shows the work! I really need to understand these concepts! Thank you! 1) The Ka for HCN is 4.9 ~ 10-10. What is the value of Kb for CN-? 2) Using the data in the table for 0.10 M aqueous species at 25 °C, which conjugate base below is the weakest base? Explain your...

  • RUVILUULI Q. #1. The equilibrium constant for the auto-ionization of water 2H30 (I) = H3O'(aq) +...

    RUVILUULI Q. #1. The equilibrium constant for the auto-ionization of water 2H30 (I) = H3O'(aq) + OH(aq) is 1.0 x 10-4 at 25°C and 3.8 x 10-14 at 40°C. Is the forward process endothermic or exothermic? Need to show your calculation. Ans: exothermic Q. #2. If you have 0.040 M solution two strong acids like HCI and H2SO, which one do you think would have behaves as stronger acids? Explain your answer with ICE table and relevant calculation. K for...

  • Which of the following solutions would require the quadratic equation to calculate the pH without a...

    Which of the following solutions would require the quadratic equation to calculate the pH without a substantial error? A. 0.10 M HCl(aq) B. 0.10 M CH3COOH (aq), Ka(CH3COOH) = 1.8 x 10−5 C. 0.10 M KCN(aq), Ka(HCN) = 4.9 x 10−9 D. 0.10 M KHSO4(aq), Ka(HSO4–) = 1.3 x 10−2

  • Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l)  NH4+(aq) +...

    Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l)  NH4+(aq) + OH-(aq) Kb = 1.77 x 10-5 and Ka = 5.65 x 10-10 a) Calculate the pH of the 0.030 M NH3 solution (Use a labeled ICE table) b) Calculate the pH of the solution at the equivalent point (when equal amount of acid is added. Assume the volume doubles). (Use a labeled ICE table) c) Over which pH range (actual numbers) do you expect...

  • Quest. 4 (15 pts). Ammonia react with water as shown in the following equation: NH3(aq) +...

    Quest. 4 (15 pts). Ammonia react with water as shown in the following equation: NH3(aq) + H2O(l) NH4+(aq) + OH(aq) Kb = 1.77 x 10-4 and Ka = 5.65 x 10-10 a) Calculate the pH of the 0.030 M NH solution (Use a labeled ICE table) b) Calculate the pH of the solution at the equivalent point (when equal amount on added. Assume the volume doubles). (Use a labeled ICE table) c) Over which pH range (actual numbers) do you...

  • You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, T...

    You work in a chemistry lab, and are asked to prepare 500 mL of a buffer solution with pH-3.20, The weak acid solution concentration in this buffer should be 0.250 M and salt is a solid. The following steps walk you through a step by step process of this preparation. a. Choose the proper weak acids for the buffer solution Table 1. Ionization constant Ka for some weak acids Name Hydrofluoric acid Nitrous acid Fulminic acid Acetic acid Hypochlorous acid...

  • QUESTION 9 Chlorous acid has a Ka of 1.1 x 10-2 What is the pH of...

    QUESTION 9 Chlorous acid has a Ka of 1.1 x 10-2 What is the pH of a 0.90 M solution of chlorous acid? HCIO2 --H* + CO2 You WILL need the quadratic in this problem. For full points, show the following • ICE Table . Ka ratio (show the products over the reactants equal to 1.1 x 10-2 • Show your work solving for x o Use a quadratic calculator to plug in "a", "b", and "e" . Once you...

  • all please. its okah if its just the answers 18. Calculate the pH of a buffer...

    all please. its okah if its just the answers 18. Calculate the pH of a buffer solution that is 0.410 M in HOCI and 0.050M in NaOCI. [Ka(HOCI) 3.2 x 10* a. 0.39 d. 749 b. 3.94 e) 6.58 19. Which one of these equations represents the reaction of a weak acid with a weak base! a. H'(aq) + OH (aq)- H:O(aq) b. H'(aq)+ CHsNH2(aq)- CHSNH3 (aq) c. OH (aq) + HCN(aq)- H:O(aq) + CN (aq) d) HCN(aq) + CH...

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