Do you think the indicated pH consistently conforms with the indicated [H,0°]and [OH] concentrations ? Cite a proof using pH 5.

We know that, pH + pOH = Pkw = 14 And pH = -log[H3O+] pOH = -log[OH-] Given, pH = 5…

Answered: Do you think the indicated pH…

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...

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Just need help with 3-7
Determine the predominant form of this molecule at a pH=7 1 ОН 2 н OH 3
[H+] [OH-] pH Acid, Base, Neutral [OH] = (1 x 10 -14):1 x 10- %3D pH = (-)log(10^-5) 1 x 10-5 10^-14:(10^-5) [H+] = (1 x 10 -14): (4.5 x 10-3 ) 4.5 x 10-3 [H+] = 2nd log (-)8.7 %3D 8.7 neutral
The [OH1-] with a pH of 5 is Group of answer choices 1 x 10-5 M 1 x 10-7 M 1 x 10-9 M 1 x 10-10 M
please help! Formic acid (Ka = 1.8 x 10-4) is used as a preservative on hay and animal feed. Hypobromous acid (Ka = 2.0 x 10-9) is used as a germicidal agent for pools and spas. An agricultural chemist wishes to test whether a mixture of the two would be more effective in preventing hay decay over the winter months. Calculate the pH of a solution that is 0.050 M in hypobromous acid and 0.025 M in formic acid.
C To add an H atom in basic solution, add an H20 to the side that needs the H atom, and also add an OH" to the other side. (HOH has one more H than OH"). How many H20 molecules should be added to the right side? How many OH ions should be added to the left? OH" + HS S+ H20 Number of OH ions = Number of H20 molecules =
15.Calculate [OH-] of NaClO, 0.110M; KaHClO = 3.0 x 10-8. Group of answer choices 3.0 x 10-6 1.9 x 10-5 1.9 x 10-4 3.3x 10-6 3.0 x 10-4 16. Calculate pH of KBrO, 0.51M; KHBrO = 2.0 x 10-9. Group of answer choices 10.20 11.20 11.51 12.90 5.10
Imagine that 500 mL of a 0.100 M solution of HOAc(aq) is prepared. What will be the [OAc–] at equilibrium in this solution if the acid dissociation constant Ka(HOAc) = 1.79 x 10–5? a. 1.33 x 10–3 M b. 4.23 x 10–3 M c. 9.46 x 10–4 M d. 0.100 M e. not enough information to tell
h To add an 0 atom in basic solution, add 2 OH" to the side that needs the O atom, and also add an H20 to the other side. (OH has one more O than HOH). How many H20 molecules should be added to the left side? How many OH ions should be added to the right? H20 + CIO3 - CI" + OH Number of H50 molecules = 1 Number of OH ions =2
Construct the expression for Ka for the weak acid, HCSH-O4. HC-H-O:(aq) + H2O(I) = H:O*(aq) + C»H;Os (aq) 1 Based on the definition of Ka, drag the tiles to construct the expression for the given acid. Ка RESET [H:O] [H.O*] [OH] [HC-H.O:] [H:C»H÷O.] [CH:O.] 2[H:O] 2[HO*] 2[OH] 2[HCH.O:] 2[H:C»H-O.*] 2[CH-O.] [H:O]? [H.O*j? [OH-P [HC»H-O.JP [H:CH.O.*]? [CH:O.?
Select the solution below that is the most acidic. [H3O+] = 1.0 × 10–14 M [H3O+] = 1.0 × 10–6 M [OH–] = 1.0 × 10–5 M [OH–] = 1.0 × 10–12 M [H3O+] = 1.0 × 10–10 M
Construct the expression for Ka for the weak acid, HCsH-Oa. HC-H:O-(aq) + H:O(I) = H:O-(aq) + CsH:O-(aq) 1 Based on the definition of Ka, drag the tiles into the numerator or denominator to construct the expression for the given acid. Ka 5 RESET [OH] [HCH.O.] [H.CH-O.] [C-H-O.] 2[H:O] 2[H:O*] [H:O] [H.O*] [OH] [HC>H:O.]* 2[OH] 2[HCSH.O] 2[H.C»H-O.] 2[CH.O.] [CHO.P

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Do you think the indicated pH consistently conforms with the indicated [H,O*] and [OH] concentrations ? Cite a proof using pH 5.