$ 4 The value of K, for hypochlorous acid, HCIO, is 3.50x10-8. Write the equation for the reaction that goes with this equilibrium constant. (Use H30+ instead of H*.) 000 000 F4 R F Submit Answer % + 5 T G FS Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining A Cengage Learning | Cengage Technical Support 6 MacBook Air Y F6 H 87 & + F7 U * 8 F8 9 K >> F9 O 0 F10 P 4) F11 Previous + Next> Save and Ex F12 1

$ 4 The value of K, for hypochlorous acid, HCIO, is 3.50x10-8. Write the equation for the reaction that goes with this equilibrium constant. (Use H30+ instead of H.) 000 000 F4 R F Submit Answer % + 5 T G FS Use the References to access important values if needed for this question. Retry Entire Group 9 more group attempts remaining A Cengage Learning | Cengage Technical Support 6 MacBook Air Y F6 H 87 & + F7 U 8 F8 9 K >> F9 O 0 F10 P 4) F11 Previous + Next> Save and Ex F12 1

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU6: Showtime: Reversible Reactions And Chemical Equilibrium

Section: Chapter Questions

Problem SII3RE

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Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

$
4
The value of K, for hypochlorous acid, HCIO, is 3.50x10-8.
Write the equation for the reaction that goes with this equilibrium constant.
(Use H3O+ instead of H*.)
000
000 F4
R
F
Submit Answer
%
+
5
T
G
FS
Use the References to access important values if needed for this question.
Retry Entire Group 9 more group attempts remaining
A
Cengage Learning Cengage Technical Support
6
MacBook Air
Y
F6
H
87
&
+
F7
U
*
8
F8
9
K
>>
F9
O
0
F10
P
F11
Previous
+
Next>
Save and Ex
F12
11

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Question is attached.
21
Calculate the Ka from the following data. + 2 H₂O 2 H3O+ H₂S 1.000 M 0 start: equil: 0.9923 M 0.0154 M 0.0077 M The amount of H₂S that was converted into product is The stoichiometry tells us that 1 mol H₂S will give us mol of H30+1 M H₂S will give Thus, M H30+1 [ ][ Ka = [ ] x [ Ka the concentration of [H3O+¹] is squared because its coefficient is 2 a. acetic b. hydrochloric c. phosphoric d. Al+3 g. HF (aq) h. CaCO3(s) i. OH-1 k. SO4² -1 n. HPO4² 0. H₂PO4¹ p. CO3-² r. H₂S u. H₂O(liq) aa. 0.9923 hh. 1.84 x 10-6 v. H₂CO3 W. PO4³ bb. 0.0077 CC. 3 y. C₂H30₂-1 ee. 1 kk. 0.05656 ii. 0.01250 = 5 [] j. H30+1 q. HCO3-1 x. HC₂H3O2 dd. 2 jj. 0.22100 + S-² 0 0.0077 M 1² 1² = e. CO₂ M S-² and 1. Mg+2 S. HS-1 M mol of S-² and ff. 0.0154 f. CaF2(aq) m. Cl-1 t. S-² z. 1 x 10-14 gg. 3.95 x 10-3
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