Consider the dissociation of the following salt in an aqueous solution, AgCl (s) = Ag* (aq) + Cl¯(aq) What is the expression for the equilibrium constant for a saturated solution, Ksp? [AgCl] [Ag*][Cl ] Ksp O Ksp = [Ag*][Cl¯] Ksp = [A£C1] [Cl¯] [Ag*][Cl¯] [A£CI] Ksp

Consider the dissociation of the following salt in an aqueous solution, AgCl (s) = Ag* (aq) + Cl¯(aq) What is the expression for the equilibrium constant for a saturated solution, Ksp? [AgCl] [Ag][Cl ] Ksp O Ksp = [Ag][Cl¯] Ksp = [A£C1] [Cl¯] [Ag*][Cl¯] [A£CI] Ksp

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: Consider the insoluble compound aluminum phosphate , AlPO4 . The aluminum ion also forms a complex…

A: Given , Insoluble compound Aluminium phosphate (AIPO4)

Q: Mercury (I) chloride, Hg2Cl2, was formerly administer orally as a purgative. Although we usually…

A: Answer : Hg2Cl2 can be dissolved based on the below reaction Hg2Cl2(aq) -> 2Hg+(aq) + 2Cl-(aq)…

Q: Consider the insoluble compound zinc sulfide , ZnS. The zinc ion also forms a complex with hydroxide…

A: Given: Kf = 2.9 x 1015

Q: The concentration of Cl- in a saturated solution of CuCl is 1.11*10^(-3) mol/L at a certain…

Q: Silver chromate is sparingly soluble in aqueous solutions. The Kp of Ag, CrO, is 1.12 × 10¬12, What…

A: Silver Chromate is a sparingly soluble salt. It's dissociation in an aqueous medium is written…

Q: A solution of acetic acid is allowed to come to equilibrium: CH3COOH(aq) + H20() = H30*() +…

A: Answer: D Here the concept of lee Chatelier principle will be applied

Q: Think about this reaction and its equilibrium constant: Ag3PO4(s) = 3 Ag*(aq) + PO43-(aq) K=2.95×…

A: Welcome to bartleby!

Q: Assuming the above reaction is exothermic in the forward direction (toward the product side),…

Q: 03)3 and U. along with some distilled water, into three separate containers. Then, to each…

A: Chemical equilibrium is the state in where both the reactants and products are have no net change…

Q: At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0058 M. You have found Ksp…

A: The solubility of In2(SO4)3 in water is 0.0058 (M)and the solubility product (Ksp) is 7.1 ×…

Q: Consider the reaction: Fe* (ag) + SCN (aq) = FESCN?* (ag) A solution is made containing an initial…

A: Given: Concentration of Fe3+= 1.0×10-3MConcentration of SCN-= 8.0×10-4MConcentration of FeSCN2+=…

Q: At equilibrium, a 1.0 L reaction vessel contains 2.3 mol of Mg(OH), and 0.170 mol of OH. What is the…

Q: Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb²* (aq) + 2 Cl¯ (aq) Suppose…

A: Here, we shall answer only the first question which allows us to determine the Equilibrium Constant…

Q: Given the equation Ag*(aq) + 2 NH3 (aq) → [Ag(NH3),]*(aq) K = 2.00 × 107 determine the concentration…

A: Ksp of AgCl = 1.77 × 10-10 Kf = 2.00 × 107 Mass of AgCl = 767 mg = 0.767 g Volume = 100.0 mL =…

Q: The solubility product of silver chromate (VI) at room temperature is 2.4 x 10^-12. Calculate the…

A: Given : Ksp of silver chromate (Ag2CrO4) = 2.4 x 10-12

Q: Express the equilibrium constant for the following reaction. CH4(g) +2 O2(g) = CO2(g) + 2 H2O(g)…

Q: Calculate the silver ion concentration, [Ag'], of a solution prepared by dissolving 1.00 g of AgNO3…

A: The objective of the question is to calculate the equilibrium concentration of .

Q: Copper(I) ions in aqueous solution react with NH3 (aq) according to Cu+ (aq) + 2 NH3 (aq). →…

A: Two equations can be represented as; CuBr ⇌ Cu+ + Br- ...KspCu+ + 2NH3 ----> [Cu(NH3)2]+…

Q: Consider the reaction Fe (s) + 2 Ag+ (aq) ⇋ Fe2+(aq+) + 2 Ag(s) . If Ag+ is added to the…

A: •Here we have to use LE CHATLIER'S principle:- •According to this principle if we increase the…

Q: 3. If you have a solution that is 0.001 M carbonate (CO), to what concent concentration of Ag" be…

Q: Consider the given reaction. A(aq) + B(s) = C(aq) K = 9.40 Suppose 18.0 mol A reacts with excess B…

A: Answer :- [C] = 2.21 M…

Q: The Solubility Product Constant for cobalt(II) sulfide is 5.9 × 10-²¹. The molar solubility of…

Q: A monoprotic weak acid, HA, dissociates in water according to the reaction HA(aq) + H₂O(1) H₂O+ (aq)…

A: Equilibrium constant K, for a reaction is defined as the product of the molar concentrations of the…

Q: A student determines that an aqueous solution that contains 0.459 M potassium acetate and 0.455 M…

A: Equilibrium constant is defined as the ratio of concentration of products to the concentration of…

Q: Calculate the value of Kp of barium bromate, Ba(BrO3)2 given that the concentration of the barium…

A: We have Concentration of Ba+2 as 0.0393 M, we have to calculate the value of Ksp.

Q: The following solubility equilibrium has K = 2.8 x 10–3 at 25oC. AgCl(s) +…

A: According to Le Chatelier’s principle, “When a system experiences any disturbance in the equilibrium…

Q: Consider the following equilibrium: Cu²+ (aq) + 4NH3(aq) → Cu(NH3)4²+ (aq) (Kf = 4.8e+12) A solution…

A: Answer:- This question is answered by using the simple concept of calculation of equilibrium…

Q: The equilibrium constant expression for the reaction CuO(s) + H₂(g) = Cu(s) + H₂O(g) is Kc =…

Q: What is the equilibrium constant expression for the following reaction? (Pay careful attention to…

A: The equilibrium reaction given is, => 2 HCl (g) + Mg(OH)2 (s) ⇔ MgCl2 (aq) + 2 H2O (l)

Q: You studied the following equilibrium to determine the value of K, for the system: Fe³+ (aq) + SCN-…

A: Definition of equilibrium constant - The ratio between the amount of reactant and the amount of…

Q: Consider the reversible dissolution of lead(II) chloride. PbCl2 (s) Pb²+ (aq) + 2 Cl¯ (aq) Suppose…

A: equilibrium constant is defined as products concentration divided by reactent concentration to the…

Q: Consider the following equilibrium using LeChatelier’s Principle – note the colors:…

A: The equilibrium reaction given is

Q: In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoCL, Co²+…

A: Answer:Le-chatalier's principle states that on changing any parameter of the system that is in…

Q: The reaction below reaches equilibrium in a closed reaction vessel. 4 HCl(aq) + MnO2 (s) = Cl₂(g) +…

A: Le Chatelier's principle: This principle is used to predict the effect of a change in conditions on…

Q: Consider the following reaction:  Ag+ (ag) + 2 NH3 (aq) = Ag(NH3)2+ (aq) Keq = 7.99 An…

A: Given reaction is an equilibrium reaction with Keq (equilibrium constant) = 7.99

Q: Determine the molar solubility of AgCl in a 1.0 M solution of NH3. Kp of AgCI - 1.ó x 10 10 K of…

A: Given, Concentration of NH3 = 1M Ksp of AgCl is =1.6× 10^ -10. Kf of Ag(NH3)2 + = 1.5 × 10^7. We…

Q: In an aqueous chloride solution cobalt(II) exists in equilibrium with the complex ion CoC14². Co²+…

A: We would use the given observation at low and high temperature to answer these questions.

Q: Consider the following equilibria: 2SO3(g) 2SO2(g) + O2(g) Kc1 = 2.3 × 10…

Q: A student determines that an aqueous solution that contains 0.220 M sodium hypochlorite and 0.250 M…

A: Answer: Value of equilibrium constant is always equal to the ratio of molar concentration of product…

Q: Write the equilibrium constant expression, Keq, or solubility product constant, Ksp, for each of the…

A: Answer for adove Given question

Q: Fe (s) + 2 Ag+ (aq) ⇋ Fe2+(aq+) + 2 Ag(s) K = 0.98546 Hg2Cl2 (s) + 2 NaBr (aq) ⇋ 2 NaCl (aq) +…

A: Given reactions: Fe (s) + 2 Ag+ (aq) ⇋ Fe2+(aq+) + 2 Ag(s) K = 0.98546 Hg2Cl2 (s) + 2 NaBr (aq) ⇋ 2…

Q: The equilibrium constant for the reaction below is 2.76×10−16. Cu2+(aq)+2Ag(s)↽−−⇀2Ag+(aq)+Cu(s)…

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%

Consider the dissociation of the following salt in an aqueous solution,
AgCl (s) = Ag+ (aq) + Cl¯ (aq)
What is the expression for the equilibrium constant for a saturated solution, Ksp?
[AgCl]
[Ag*][Cl ]
KsP
K sp = [Ag*][Cl¯]
Ksp = [AgCl] [Cl"]
[Ag*][Cl¯]
[A£CI]
KsP

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

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

A mixture of 0.60 mol Cl2(g) and 0.40 mol F2(g) was allowed to come to equilibrium in a 1000-mL flask. If 2x represents the molar concentration of CIF(g) at equilibrium, which expression represents the equilibrium constant? C2(g) +F2(g) 2 2CIF(g) (2x)2 (0.60 – x) · (0.40 – x) x2 (A) (B) (0.60 — х) - (0.40- х) 2x 2r2 (D) (0.60 – x) · (0.40 – x) (0.60 – x) · (0.40 – x) O A В O c
When 1.55 g of solid silver bromide is added to 1.00 L of water, the salt dissolves to a small extent. AgBr(s) = Ag* (aq) + Br (aq) The silver and bromide ions in equilibrium with AgBr each have a concentration of 5.7 x 10 M. What is the value of K, for AgBr?
Express the equilibrium constant for the following reaction. N2(g) + 3H2(g) ⇒ 2NH3(g) K = K = K = K = K= [N₂][H₂]1/3 [NH 3]1/2 [NH 3]6 [N₂]³[H₂]⁹ [NH 3]2 [N₂][H₂]³ [N₂][H₂]³ (NH3)2 (NH3]1/2 [N2][H₂]1/3
Which of the following is the correct Ksp expression for the insoluble solid, Ag,SO,? A) K sp 2[Ag*][SO}¯] B) K sp = [Ag*][SO}¯] C) Ksp = [Ag*]*[SO?¯] [Ag*]*[SO?¯] D) K en = Ag,SO4 ds 2[Ag*][S0}¯] K sp E) Ag,sO4 A) see problem image A) B) see problem image B) C) see problem image C) D) see problem image D) E) see problem image E)
A student combines Fe(NO3)3 solution and KSCN solution to produce a solution in which the initial concentrations of Fe3+(aq) and SCN–(aq) are both 5.58 × 10–2 M. The chemical equilibrium forms FeSCN2+(aq): Fe3+ + SCN- <=> FeSCN2+ The absorbance of this solution (from FeSCN2+) is measured as 0.161, and Beer's law equation (the trend line from best fitting) as Absorbance = 189 x Concentration of FeSCN2+ + 0.02 Determine the equilibrium concentration for SCN- in mol/L.
Choose the correct solubility constant expression for iron(II) hydroxide in water: Ksp = [Fe2+][OH−]2/[Fe(OH)2] Ksp = [Fe2+][OH−]/[Fe(OH)2] Ksp = [Fe2+][OH−]2 Ksp = [Fe2+][OH−]
Consider the given reaction. A(aq) + B(s) = C(aq) K = 9.40 Suppose 22.1 mol A reacts with excess B in 9.15 L of solution. Calculate the concentration of C at equilibrium. [C] = M
At 25 °C, an aqueous solution has an equilibrium concentration of 0.00217 M for a generic cation, A+(aq), and 0.00109 M for a generic anion, B2−(aq). What is the equilibrium constant, ?sp, of the generic salt A2B(s)?
The solubility of silver chloride can be increased by dissolving it in a solution containing ammonia. AGCI (s) S Ag * (aq) + Cl ¯ (aq) K 1 = 1.6 x 10 -10 Ag * (aq) + 2NH 3 (aq) S Ag(NH 3) 2 * (aq) K 2 = 1.5 x 10 7 What is the value of the equilibrium constant for the overall reaction? AGCI (s) + 2NH 3 (aq) S Ag(NH 3) 2 * (aq) + CI (aq) K net = ? 1.5 x 10 7 2.4 x 10 -3 3.1 x 10 -3 2.3 x 10 14 2.4 x 107
8. You mix a 200.0-mL sample of a solution that is 1.5 X 10-³ M in Cu(NO3)2 with a 250.0-mL sample of a solution that is 0.20 M in NH3. After the solution reaches equilibrium, what concentration of Cu²+ (aq) remains? For [Cu(NH3)4]²+, Kf = 1.7 x 1013 me that
Given the following values of equilibrium constants: [Ag(NH,)2]* = Ag* (aq) + 2NH3(aq) K 6.3 x 10-5 Ag,SO3(s) = 2Ag* (ag) + SO?-(aq) K= 1.50 x 10-14 What is the value of the equilibrium constant for the following reaction? Ag, SO3 (s) + 4NH3 (aq) = 2[Ag(NH,)2]+ +SO (aq)
Write the equation for the equilibrium constant (K) of the reaction studied in this exercise. 2CrO4 2- (aq) + 2H+ (aq) = Cr₂O72- (aq) + H₂O(1) 1E T² B 1 U T₂ 0 Word(s)