HomeworkLib
Question

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

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

DATE 0.10M of Hel Со с 0:1ом Hel is a soprong Acid d if dissociate complete into cons o no d cao Hol BeFone : G > Ho & Co o o0.1002 0.1002 , 18*** Urd 1.8 xsort +02 1881005 to 10 ofto 18 x 10-5 22 = (1-0) (18 r1ors) x 2 + (184105 - 1881os no x2 + 18key (4) ekt (os) + су в 19) — miya, 414e. : c. o o o o o — Гу-2 : Со я о. )ом. Ооо. - HEN ² HO + NO ko {sf] = [cneja ollon pМCorrect option-(B)

0 0
Add a comment
Know the answer?
Add Answer to:
Which of the following solutions would require the quadratic equation to calculate the pH without a...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

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

  • Find the pH of these compounds. use 5% approximation where nescessary. say each compund has m...

    find the pH of these compounds. use 5% approximation where nescessary. say each compund has molarity of 0.10M HCl H2S04 strong acicd! the first proton comes off completely and [HSO4] NaOH NH3 NH4CI CH3COOH Ka 1.8 x 10-5 CH3COONa Kb(CH3COO) 5.6 x 1010 . .solve the quadratic equation. strong base Kb 1.8 x 10-5 Ka(NH4) 5.6 x 1010 HCl H2S04 strong acicd! the first proton comes off completely and [HSO4] NaOH NH3 NH4CI CH3COOH Ka 1.8 x 10-5 CH3COONa Kb(CH3COO)...

  • Which of the following 1.0 M solutions would have the lowest pH? Weak Base Weak Weink...

    Which of the following 1.0 M solutions would have the lowest pH? Weak Base Weak Weink Ka Kb Acid HCN 4.9 x 10-10 HONH2 1.1 x 10-8 A) LINO3 HNO2 4.5 x 10-4 NH3 1.8 x 10-5 B) HONH3Br HIO 2.3 x 10-11 C6H5NH2 4.3 x 10-10 C) H2NNH3CIO4 HBrO 2.5 x 10-9 H2NNH2 1.3 x 10-6 D) Ca(Bro)2 CoH5COOH 6.3 x 10-5 C5H5N 1.7 x 10-9

  • Which of the following solutions would have the lowest pH? Assume that they are all 0.10...

    Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A. A) HF, 3.5 × 10-6 B. B) HCN, 4.9 × 10-10 C. C) HNO2, 4.6 × 10-5 D. D) HCHO2, 1.8 × 10-4 E. E) HClO2, 1.1 × 10-2 F. F) none of these

  • 1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M...

    1. Calculate the pH of the following solutions. Show all of your work. a. 0.0050 M nitric acid, HNO3 b. 0.50 M hydrocyanic acid, HCN Ka = 4.0 x 10-10 2. A student was given the following problem: Calculate the pH of a 0.50 Mama bromide (NHaBr) solution if the Kb of NH3 is 1.8 x 10. The student provided the fo work. Identify the error(s) and calculate the correct pH. NH; (aq) + H20 (1) = NH3 (aq) +...

  • Part A. Calculate the pH of a buffer solution that is 0.247 M in HCN and...

    Part A. Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.171 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). Part B. Calculate the pH of a buffer solution that is 0.230 M in HC2H3O2 and 0.170 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) Part C. Calculate the pH of 1.0 L of the original buffer, upon addition of 0.110 mol of solid NaOH.

  • pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b)...

    pH LI Calculate the pH of the following solutions: Solution (a) 0.10 M CH3COOH 12.9 (b) 0.10 M NH3 Mixture of 25.00 mL of 0.10 M HCl + 25.00 mL of 0.10 NaOH Mixture of 20.00 mL of 0.10 M NaOH + 20.00 mL of 0.10 M CHCOOH (e) Mixture of 20,00 mL of 0.10 M HCI + 20.00 mL of 0.10 M NH; Saturated Mg(OH)2 (s) aqueous solution if water's dissociation is negligible K[CH3COOH) = 1.8x10-Kb [NH:] = 1.8*10-9;...

  • Ka values: HCI HNO3 H2SO4 strong strong strong 1.3 x 10-2 7.5 x 103 7.1 x...

    Ka values: HCI HNO3 H2SO4 strong strong strong 1.3 x 10-2 7.5 x 103 7.1 x 10-4 4.5 x 10-4 1.7 x 10-4 CH3COOH CsH5NH+ H2CO3 H2PO4 HSO4- H3PO4 HF HNO2 HCOOH 1.8 x 100 5.9 x 10-6 4.2 x 10-7 6.2 x 10-8 5.6 x 10-10 4.9 x 10-10 4.8 x 10-11 4.8 x 10-13 NH1+ HCN HCO3- HPO4 6) (20 points) What is the pH of 0.065 M H2CO3 (carbonic acid)? 7) (20 points) What is the pH...

  • Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.168 M...

    Calculate the pH of a buffer solution that is 0.247 M in HCN and 0.168 M in KCN. For HCN, Ka = 4.9 times 10^-10 (pKa = 9.31). PH =

  • Which of the following solutions would have the highest pH? Assume that they are all 0.10...

    Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25 C. The acid is followed by its Ka value. HC102, 1.1 x 10-2 OHCHO2, 1.8 x 10-4 HC6H50, 1.3 * 10-10 O HNO2, 4.6 x 10-4 O HOCI, 2.9 x 10-8

  • Questions 1: A) Calculate the pH of a buffer solution that is 0.246 M in HCN...

    Questions 1: A) Calculate the pH of a buffer solution that is 0.246 M in HCN and 0.166 M in KCN. For HCN, Ka = 4.9×10−10 (pKa = 9.31). B) Calculate the pH of a buffer solution that is 0.200 M in HC2H3O2 and 0.160 M in NaC2H3O2. (Ka for HC2H3O2 is 1.8×10−5.) C) Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.   Calculate the pH of 1.0 L of 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