U16HW Question 8Homework • UnansweredFill in the BlanksType your answers in all of the blanks and submitWhat is the H3o* of the following aqueous solutions:When pH = 2.50, H* =Type your answer hereWhen pH = 6.89, H =Type your answer hereWhen pH = 12.1, H =Type your answer hereUnansweredA Subm.Fullscreen9:27 PMa5/9/2021"prt scdeletehomepg up40144numbackspace6.8.lock8.home4enterKpause↑ shiftM.end.altctrlins

pH is a scale to measure a substance acidic or alkaline in nature . It's value range 0 to 14 . For…

U16HW Question 8 Homework • Unanswered Fill in the Blanks Type your answers in all of the blanks and submit What is the H3O+ of the following aqueous solutions: When pH = 2.50, [H*] = Type your answer here %3D When pH = 6.89, H*] = Type your answer here When pH = 12.1, (H*] = Type your answer here %3D

U16HW Question 8 Homework • Unanswered Fill in the Blanks Type your answers in all of the blanks and submit What is the H3O+ of the following aqueous solutions: When pH = 2.50, [H] = Type your answer here %3D When pH = 6.89, H] = Type your answer here When pH = 12.1, (H*] = Type your answer here %3D

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

Calculate [H3O+], [OH-], pH, pOH for the following solution: H2SO4 7.2x10-3
Which of these correctly shows the acid behavior of hydrochloric acid? HCI + H2O --> CI + 2 OH HCI + H20 --> CI + H3O* HCI + H3O* --> CI + H2O HCI + H20 --> H2CI + OH 2/ Question 2
Determine the [H*], [OH¯], and pOH of a solution with a pH of 5.95 at 25 °C. [H*] = 1.122 x10–6 M [OH] = 8.9 x10-9 M РОН 5.95 Incorrect
For each of the following strong base solutions, determine OH-| and (H30+] and pH and РОН For 2.2 x 10-4 M KOH, determine [OH ] and (H30+). Express your answers in moles per liter to two significant figures separated by a comma. • View Available Hint(s) [OH-], [H3O*] = 2.2×10-44.5×10-11 M Previous Answers Correct Term 2: Correct answer is shown. Your answer 4.57-10-11 = 4.57x10-11 M was either rounded differently or used a different number of significant figures than required for this part. Important: If you use this answer in later parts, use the full unrounded value in your calculations. KOH is a strong base that completely dissociates into K+ and OH in an aqueous solution: KOH(aq) → K*(aq) + OH- (aq) Therefore, the concentration of OH is the same as the given concentration of KOH and is equal to 2.2 x 10-1 M. Then use the ion product constant, substitute the calculated value for OH, and solve for (H3O*]:
A healthy human blood sample is measured in the lab to have [H3O+] = 2.50 x 10-8 M. What is the pH of this blood sample? Enter your answer below, rounded to three sig figs. No label needed.
Complete the table below. Be sure each of your answer entries has the correct number of significant digits. You may assume the temperature is 25 °C. conjugate acid conjugate base formula K. K, formula HBRO 2.3 × 10 HCO, -8 2.2 x 10, CIO 3.3 x 10 02022 McGraw Hill LLC Al Rights Reserved Terms of Use Pvacy Conter Accessbily Check Explanation IA 99+ e to search
The normal pH of human blood ranges from 7.35-7.45. Calculate the [H*], [OH-], and pOH of human blood with a pH of 7.38. Attach File
Determine the pH of a solution with [OH-] = 5.88 × 10-3 M. Your answer should contain 3 decimal places as this corresponds to 3 significant figures when dealing with logs. pH =
A solution has (H*] = 2.5 x 109. What is the pH of the solution? ( Select] Is the solution acidic or basic? [Select ] pH = -log [H+] pOH = -log[OH-] pH + pOH = 14 %3D > >
Determine the pH of a solution if [OH --] = 0.040 M.Compute the [H ++] of a solution when pOH =10.0
For each strong acid solution, determine [H3O+], [OH-], and pH. Submit ▼ ▾ Part E ✓ Correct -1 Calculate [H3O+] and [OH-] for a solution that is 0.435% HNO3 by mass. (Assume a density of 1.01 g mL-¹ for the solution.) Enter your answers in moles per litre to three significant figures separated by a comma. [H3O+], [OH-] = Submit Previous Answers Part F X Incorrect; Try Again pH = 15] ΑΣΦΑΦ → C Submit Previous Answers Request Answer -1 Calculate pH for a solution that is 0.435% HNO3 by mass. (Assume a density of 1.01 g mL-¹ for the solution.) Express your answer to three decimal places. 197| ΑΣΦ Previous Answers Request Answer COL ? ? mol L-1
Calculate the pH of a solution with an H concentration of 2.46 x 104 M. Report the pH with the correct number of significant figures. pH = -log[H] 3.61 ○ 3.609 3.6 O 3.609 1 O 3.609 06