1. Write the reaction for H₂S dissolving into water+2. Write the expression for the Ka[Ka[a. aceticb. hydrochloricg. sulfurous-2n. HPO3-²u. H2Oaa. 2.6990gg. 5.000 x 10-12mm. conjugate acid=h. hydrosulfuric0. H₂PO3-1v. 0.1000][[]c. phosphoricP. CO3-2W. 0.02500bb. 1.000 x 10-11hh. 11.3010oo. base<->d. perchlorici. OH-1 j. H30+1q. HCO3-1 r. H₂Sx. 1.000 x 10-3-2k. SO4²cc. 11.0000ii. 0.01250pp. conjugate basedd. 2jj. 0.22100y. 3.0000e. hydrofluoricI. Mg+2s. HS-1+ee. 1f. sulfuricm. Cl-1t. S-2Z. 1x 10-14ff. 2.000 x 10-3kk. 0.05656 II. acid

Both the questions have been solved in the following step.

1. Write the reaction for H₂S dissolving into water + 2. Write the expression for the Ka Ka = [ b. hydrochloric a. acetic g. sulfurous h. hydrosulfuric n. HPO3-² 0. H₂PO3-1 p. CO3-² u. H2O v. 0.1000 w. 0.02500 aa. 2.6990 gg. 5.000 x 10-12 mm. conjugate acid bb. 1.000 x 10-11 hh. 11.3010 oo. base |][ c. phosphoric i. OH-1 <-> d. perchloric j. H30+1 9. HCO3-1 x. 1.000 x 10-3 r. H₂S CC. 11.0000 ii. 0.01250 pp. conjugate base k. SO4² dd. 2 jj. 0.22100 y. 3.0000 e. hydrofluoric I. Mg+2 s. HS-1 + ee. 1 f. sulfuric t. S-2 z. 1 x 10-14 ff. 2.000 x 10-³ kk. 0.05656 II. acid m. Cl-1

1. Write the reaction for H₂S dissolving into water + 2. Write the expression for the Ka Ka = [ b. hydrochloric a. acetic g. sulfurous h. hydrosulfuric n. HPO3-² 0. H₂PO3-1 p. CO3-² u. H2O v. 0.1000 w. 0.02500 aa. 2.6990 gg. 5.000 x 10-12 mm. conjugate acid bb. 1.000 x 10-11 hh. 11.3010 oo. base |][ c. phosphoric i. OH-1 <-> d. perchloric j. H30+1 9. HCO3-1 x. 1.000 x 10-3 r. H₂S CC. 11.0000 ii. 0.01250 pp. conjugate base k. SO4² dd. 2 jj. 0.22100 y. 3.0000 e. hydrofluoric I. Mg+2 s. HS-1 + ee. 1 f. sulfuric t. S-2 z. 1 x 10-14 ff. 2.000 x 10-³ kk. 0.05656 II. acid m. Cl-1

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

Related questions

Q: Write balanced equations and expressions for Kap for the disso- lution of each ionic compound. a.…

A: a) BaSO4 BaSO4 ------> Ba2+ + SO42- s s KSP = Xx Yy Sx+y…

Q: 7. What is the pH of a solution that is 0.223 M HOCN (cyanic acid, weak acid) and 0.146 M KOCN…

A: To find the pH of the solution, we need to determine the concentration of H+ ions in the solution.…

Q: 6. Solution of 0.02 M Ca(OH)2 a Dissociation reaction: b. Calculated pH.

Q: Q= R= 1. Q 2. R 1. S 2. T S= T= 1. U 2. V U= V = HO Ph

A: We will use general reagents for the step-wise conversion as given. We must keep in mind that more…

Q: The solubility product for A3B is 2.8 x 10-18, What is the solubility of AgB in water, in moles per…

Q: 1. Which of the following reactions best illustrates the reaction of an acid in aqueous solution? +…

A: An acid are compound which will furnish hydrogen ion when dissolved in water similarly a base are…

Q: A formic acid solution has a pH of 3.25. Which of these substancesraises the pH of the solution upon…

A: Given: pH= 3.25 To find: Which of the given substances raises the pH of the solution upon addition

Q: Write dissociation equations and K., expressions for the following salts: a. BaF₂ b. Ag,SO, c. Ca,…

A: Dissociation equations represent dissociation of salt in aqueous solution. Ksp expression is…

Q: a. Calculate the degree of ionization of 0.25 M HCHO2 (formic acid) solution. K. (formic acid) = 1.7…

A: a) The degree of ionization of 0.25 M HCHO2 is to be calculated. b) The degree of ionization of 0.25…

Q: 4. Assume the [NaOH] = 0.150 M: a. If 12.0 mL NaOH is used in the titration, how many moles OH would…

Q: An aqueous solution contains 1x 10^-5 M hydrogen ions. How much hydronium ions does it contain?*

A: Hydrogen ions or hydronium ions are considered to be same.

Q: 3. For this problem, you may ignore the baricity of phosphate ion, PO/, Strontium phosphate (molar…

A: To answer the questions related to the solubility of strontium phosphate and strontium acetate.

Q: The pH of 1.50 mol/L acid is measured to be 5.75. For this acid, the Kais -5.75 = [H₂₂0] A. 2.1 x…

Q: 3. Which equilibrium constant would be most relevant to the following system in equilibrium? NaCl(s)…

A: Given reactionNaCl (s) ⇌Na2+ (aq) + Cl- (aq)We have to identify the relevant equilibrium constant…

Q: A chemistry student weighs out 0.193 g of sulfurous acid (H₂SO3), a diprotic acid, into a 250. mL…

A: mass of sulfurous acid (H2SO3) = 0.193 gConcentration of NaOH solution = 0.1000 M = 0.1000…

Q: The pH at the equivalence point for the titration of a weak acid with a strong base will always be O…

A: Answer: pH defines the acidity of the solution. Mathematically, it is the negative logarithm of H+…

Q: Lactic acid solution is formed. a. b. Write the reaction where Lactic acid is reacted with water.…

Q: A student was titrating a solution of hydrazine, H₂NNH₂, with a strong acid solution. Determine the…

A: In the given question we have to fill the BCA table of titration reaction between hydrazine and…

Q: 3. In a saturated solution of silver bromide, the concentration of bromide ions is 0.50 M. Which of…

A: We have to calculate the value of Ksp

Q: The dissociation constant of HNO3 at 0 ∘C0 ∘C is ?a=46.8. Find the percent dissociated in 0.100 M…

Q: Solution of 0.1 M NaHPO4 a Equilibrium reaction

A: Given compound is 0.1 M NaH2PO4

Q: 1. Complete the table with suitable calculation. 2. Construct a suitable reaction for the above…

Q: A 1.00 liter solution contains 0.60 M ammonia and 0.46 M ammonium iodide. If 0.23 moles of nitric…

A: A buffer solution is formed by the mixing of weak acid with its conjugate base or weak base with its…

Q: The dissociation constant of HNO, at 0 °C is Ka = 46.8. Find the percent dissociated in 0.100 M HNO,…

A: The dissociation constant is a direct result about the law of mass action that represents equilibria…

Q: 8. K/U Write the acid-dissociation constant expressions for each of the following weak acids: a.…

Q: rite the expression for the Ka when HC₂H3O2 is dissolved in water 2H3O2 + H₂O C₂H3021 + H30+1 ][ Ka…

Q: 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium,…

A: Given: Initial moles of HA = 0.030 moles Volume of container = 2.0 L Equilibrium concentration of HA…

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

100%

1. Write the reaction for H₂S dissolving into water
+
2. Write the expression for the Ka
[
Ka
[
a. acetic
b. hydrochloric
g. sulfurous
-2
n. HPO3-²
u. H2O
aa. 2.6990
gg. 5.000 x 10-12
mm. conjugate acid
=
h. hydrosulfuric
0. H₂PO3-1
v. 0.1000
][
[]
c. phosphoric
P. CO3-2
W. 0.02500
bb. 1.000 x 10-11
hh. 11.3010
oo. base
<->
d. perchloric
i. OH-1 j. H30+1
q. HCO3-1 r. H₂S
x. 1.000 x 10-3
-2
k. SO4²
cc. 11.0000
ii. 0.01250
pp. conjugate base
dd. 2
jj. 0.22100
y. 3.0000
e. hydrofluoric
I. Mg+2
s. HS-1
+
ee. 1
f. sulfuric
m. Cl-1
t. S-2
Z. 1x 10-14
ff. 2.000 x 10-3
kk. 0.05656 II. acid

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 1 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Complete the reaction
For the reaction below: which base(s) (I – V) will have an equilibrium constant greater than 1 Base + H-Base + Base = H H O. Na H. II IV V O Iv O I, III, IV O 1,II II O II, V 00
ritration of 100.0mL 0.1ONH 3 with 1on- 0.10M HN0 3. what is the pH afteR 50.0mL oL O.10M HNO
The initial in the unknown analysis is the addition of 6. M HCl. This results in the formation of a precipitate. The solid precipitate is separate from the liquid solution. The solution could potentially contain K+, Ca2+, and Al3+. Next, 3M NH3 is added to the solution to separate the Al3+. This is a result of the fact that the Al3+ forms the hydroxide, Al(OH)3. But Ca2+ also forms the hydroxide, Ca(OH)2. Why does the Ca(OH)2 not separate out with the Al(OH)3?
12. Carbonated water has a [H+Jeg = 3.2 × 10-4 M; this is the result of the dissociation of carbonic acid: H₂CO3 (ag) H+ (aq) + HCO3- (ag) Kc = 4.4 x 10-7 a. Set up the equilibrium constant expression for this acid dissociation. b. Calculate [H₂CO₂]ea. Hint: An ICE table may be handy. c. Carbonic acid is created by dissolving carbon dioxide in water. Given that the Henry's Law constant of carbon dioxide is 29.76 atm/M, what partial pressure of carbon dioxide is needed to make carbonated water?
2023 JSY BEE B Ve 2. It took 9.20 mL of a 0.120 M solution of NaOH to reach the equivalence point of vinegar. How many moles of acetic acid are present?
19. A student prepared a 250.0 mL solution by dissolving 4.559 g of (NH4)2SO4 in enough water. The temperature is 298 K. The base dissociation constant for NH3 is 1.796x10-5. Please answer the following questions. A. B. What is the equilibrium concentration of H3O+ in the solution? Please provider your answer below. 00 + → What is the equilibrium concentration of OH in the solution? Please provider your answer below. OO → $ → $ C. What is the pH of the solution? pH = Please provider your answer below. S M M
Predict the direction in which the equilibrium will lie for the reaction: HF + ClO2− ⇆ HClO2 + F− Ka (HF) = 7.2 x 10−4; Ka (HClO2) = 1.1 x 10−2 a. to the left b. none of thses c. in the middle d. to the right
What is the appropriate expression for the given reaction? a. Ka b. Kb c. Ksp d. Kf e. Kw f. Kp 1. NiCO3(s) ↔ Ni+2(aq) + CO3-2(aq) 2. Hg+2 + Excess I- ↔ HgI4-2 3. H2O(l)↔ H+(aq) + OH-(aq)
The pH of a 0.50 M solution of the weak base ethyl amine, C2H5NH2, is 12.20. a. Write the dissociation reactionb. Calculate Kb for the reactionc. Calculate Ka from Kb