Problem 5: a) Determine the equilibrium concentration of zinc ion (Zn^²) when zinc hydroxide solid Zn (OH); dissolves in water. The solubility constant Kap of zinc hydroxide is estimated to be 8x10-¹8. b) What is the pH of the water at equilibrium?

Problem 5: a) Determine the equilibrium concentration of zinc ion (Zn^²) when zinc hydroxide solid Zn (OH); dissolves in water. The solubility constant Kap of zinc hydroxide is estimated to be 8x10-¹8. b) What is the pH of the water at equilibrium?

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: The expression for the solubility product of Fe₂(CrO4)3 is: O2 [Fe³+] × 3 [CrO²-] O [Fe³+] ²…

Q: The PK, value for H₂S is 7.00. What mole ratio of NaHS to H₂S is needed to prepare a buffer with a…

Q: Which of the following aqueous solutions are good buffer systems? (Select all that apply.) 0.30 M…

A: The mixture of a weak acid and its salt can behave as a good acidic buffer.The mixture of a weak…

Q: Chemical Formulas Scientific Notation Periodic Table Tables Calculate the pH of 1.00 L of a 0.270 M…

A: Information of question

Q: The Ksp of PbCl₂ is 7.28 10-11 M. Calculate the solubility of each ion in a saturated solution: M…

Q: The following concentrations are found in mixtures of ions in equilibrium with slightly soluble…

Q: Determine the pH of a buffer that is 0.95 M HBRO and 0.68 M KBRO. The value of pka for HBRO is 8.68.…

A: Given, Concentration of HBrO = 0.95 M Concentration of KBrO = 0.68 M pKa of HBrO = 8.68 pH of…

Q: 1) Write the solubility constant expression for the following species: a) MnS b) AI(ОH)з с) Саз…

A: As per regulations only first question can be answered.

Q: None

A: So, the answers to the questions are:

Q: Given a K value of 4.6 X 10-12, would you expect a nearly complete reaction at equilibrium Given…

A: The value of K is 4.6 ×10-12. This is a very small value which means that the reaction has not…

Q: Practice 10: What is the pH of a buffer that is 0.200 M HC2H3O2 and 0.100 M NaC2H3O2. K₁=1.8 x 10-5

A: The buffer system in this case is made up of acetic acid (HC2H3O2) and its conjugate base, the…

Q: Question 22 · Buffers are solutions that resist changes in pH. (a) Calculate the solubility (in mol…

A: pH is given to be 8.45 The Ksp of Pb(OH)2 is 1.42 x 10−20 from standard sources. If Ksp changes, the…

Q: They product conants, A25C unds front cartonas FeCO₂, and cadm) CCO, we given by the table Bidance…

A: #Part-B: Ksp of FeCO3 = 2.10*10-11 The equation for the dissociation of FeCO3 is: FeCO3(s) ⇌…

Q: The pK, value for H2S is 7.00. What mole ratio of NaHS to H2S is needed to prepare a buffer with a…

Q: t condition will decrease the solubility High pH Low pH

A: The equilibrium solubility is, BaF2(s) ----> Ba2+(aq.) + 2F-(aq.) As we kn, due to odd ion…

Q: For the 0.5 M Acetic Acid Solution: Chemicals CH3COOH(aq) CH3COO(aq) H3O* (ag) K₁ Calculation:…

A: The concentration of acetic acid solution = 0.5 M To calculate Ka of acetic acid

Q: Complete the mechanism for the DIBAL-H (diisobutylaluminum hydride) reduction of methyl…

Q: Which of the following can be classified as buffer solutions? (Select all that apply.) O0.50 M HOCI…

A: A buffer solution is a solution that can maintain its pH even after the addition of small strong…

Q: Calculate the concentration of IO, in a 7.06 mM Pb(NO,), solution saturated with Pb(IO,),. The Ksp…

A: #Q.1: Since Pb(NO3)2 is completely soluble in water, [Pb2+(aq)] = [Pb(NO3)2] = 7.06 mM [Pb2+(aq)] =…

Q: What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.29? See the Solubility…

A: The concentration of salt that is dissolved to form one liter of its saturated solution at…

Q: At a certain temperature, silver carbonate has a K = 7.82x10-12 and a solubility of 0.0001250 M in…

A: Given : Ksp = 7.82 x 10-12

Q: 9) Determine the molar solubility of Cd(OH)2 in pure water. Ksp for Cd(OH)2 =2.5 × 10-14. A) 1.84 x…

Q: QUESTION 19 A solution is made from 0.289 M of a weak base. What is the pH if the Kp for this base…

A: The concentration of a weak base is C = 0.289 M, The dissociation constant of the weak acid is Kb =…

Q: Identify Principle Species and Calculate its pH values on H₂A (Oxalic Acid) titration curve…

A: The objective of this question is to identify the principle species and calculate the pH values at…

Q: The molar solubility of P6C12 in 0.10 M NaCl is 1.7 x 10-3 moles in a liter (that is 1.7 x 10-3…

Q: How many grams of solid NaF should be added to a 100-mL 1.0 × 10-³ M solution of LaCl3 at pH 3.00 to…

A: In this chemical calculation, we are presented with a scenario where we need to adjust the…

Q: 4th attempt See Periodic Table See Hint How much lead(II) chloride will precipitate if 185 mL of…

A: The objective of this question is to calculate the amount of lead(II) chloride that will precipitate…

Q: What is the molar solubility of Sn(OH), in a buffer solution containing equal concentrations of NH,…

A: 1.) To calculate solubility of Sn(OH)2 in buffer solution , we would first calculate pOH if buffer…

Q: It's also not 3.44

A: AcOH/NaOAc buffer is an acidic buffer composed of weak acid and its salt of strong base. On adding…

Q: d) Calculate the concentration of free, uncomplexed Cu²+ ions in a solution that originally contains…

A: As here already mentioned that I have to solve only Part- D of question -2 so I am solving this…

Q: Imagine that phenol ("hydroxybenzene") and nitrobenzene are reacted (in separate beakers) with a hot…

A: This question is related to aromatic electrphile substitution reaction . In the phenol OH group is…

Q: The Kp of PbBr, is 6.60 x 10-6. What is the molar solubility of PbBr, in pure water? molar…

Q: Question 3 : The equilibrium constant for the formation of Cu(CN)42 is 2.0 x 1030. Calculate the…

A: The question is based on the concept of chemical equilibrium.we have to calculate concentration of…

Q: [CN A buffer solution made from HCN and KCN has a pH of 9.66 . If pKa for HCN is 9.40 , what is the…

A: Given that, We have a buffer solution containing HCN and KCN which is an acidic buffer The pH of the…

Q: QUESTION 16 A solution is prepared by adding excess CaBr2 (Ksp = 3.2×10-11] to water, what is the…

A: When an ionic salt is dissolved in water, it dissociates to form constituent ions. The extent of the…

Q: Silver chromate (Ag2CrO4; Ksp = 1.1×10-12) has a molar solubility of 6.5×10-5 M. What calculation…

A: To solve this problem we have to write the dissociation of Ag2CrO4 into there ions . Then by using…

Q: An acidic solution is 6 mM in each of the following metal lons: Ph, zn?, Mn, cu. See the Solubility…

Q: What is the value of K,? K, = 22.89 The change in the number of moles of gas for the reaction is…

A: The explanation is given below-

Q: Activity 5: Problem Solving (Henderson-Hasselbalch Equation) 1. A buffer is prepared containing 1.00…

A: Solution : Henderson Hasselbalch equation is very useful to calculate the pH of buffer solution.…

Q: Give experts solution with explanation

Q: Problem 2. 0.10 M sodium lactate, NaC3HsO3? For lactic acid, K = 1.4 x 104 (Use the…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: A 50.0 mL of 2.00 M Fe3+(aq) solution are mixed with 50.0 mL of 2.00 M SCN (aq) solution. What is…

Q: An indicator of pKa = 6.5 can be used for the titration of a reaction that reaches equilibrium at…

A: Indicator in an acid base titration helps to identify the equivalence or end point of titration. It…

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

Problem 5:
a) Determine the equilibrium concentration of zinc ion (Zn¹²)
when zinc hydroxide solid Zn (OH): dissolves in water. The solubility constant Kap of
zinc hydroxide is estimated to be 8x10¹8.
b) What is the pH of the water at equilibrium?

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1: Determine the equilibrium concentration of Cu2+ and pH of the water :

VIEW

Step 2: a. Calculation for concentration of Zn2+ ion at equilibrium is:

VIEW

Step 3: b. Calculation for pH of the water at equilibrium is:

VIEW

Solution

VIEW

Step by step

Solved in 4 steps with 2 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

Practice chemistry question
5) What is the effective pH range of buffers formed with the following acids? Hint for b notice you are given a pK, not a pK.. a) Propanoic acid pK = 4.87 b) dimethylamine pK, = 3.23
Study material: In the Henderson-Hasselbalch equation below, explain the relationship of the pH and pKa when the ratio of [A-] and [HA] =1? The second part of the question is explain the buffer capacity of the buffer, when the ratio of [A-] and [HA] =1. pH=pKa - log [A+]/[HA]
Question 4 A buffer solution consists of 0,25 mol·dm3 acetic acid (HC,H,O,; 1,8 x 10) and 0,35 mol·dm3 potassium acetate K. (KC,H;O,). a) Calculate the pH of the buffer solution. a. 3
The pK value for HSO3 is 7.19. What mole ratio of K2 SO3 to KHSO3 is needed to prepare a buffer with a pH of 7.46? [SO32 ] [HSO3-] Submit Answer Retry Entire Group 7 more group attempts remaining
Problem 10.76 The pH of a buffer solution containing 0.10 M acetic acid and 0.10 M sodium acetate is 4.74. 61°F Mostly cloudy Write the Henderson-Hasselbalch equation for this buffer. Check all that apply O pH=pKa - log- [CH3CO₂] [CH,CO,H O pH=pKa + log O pH=pKa + log- O pH=pKa - log- Part B [CH3CO₂] [CH,CO,H ΑΣΦ [CH3CO,H [CH3CO₂] Submit Request Answer [CH3CO₂H] [CH3CO₂] Write the equations for reaction of this buffer with a small amount of HNO3 Express your answer as a chemical equation. Identify all of the phases in your answer ?
A 26.9 mL sample of 0.282 M ethylamine, C,H;NH,, is titrated with 0.262 M nitric acid. After adding 12.2 mL of nitric acid, the pH is Use the Tables link in the References for any equilibrium constants that are required. Submit Answer Try Another Version 5 item attempts remaining
A buffer solution is 0.448 M in HCIO and 0.210 M in KCIO. If Ką for HCIO is 3.5×10-8, what is the pH of this buffer solution? Submit Answer Retry Entire Group
question 21 The solubility product, Ksp, for Fe(OH)3 is 1.6 × 10–39. What is the solubility of Fe(OH)3 in a buffer solution with pH = 10, in moles per litre? Question 21 options: 4.0 × 10–23 mol.L–1 1.1 × 10–9 mol.L–1 8.8 × 10–11 mol.L–1 1.6 × 10–27 mol.L–1
Solve an equilibrium problem (using an ICE table) to calculate the pH of each of the following solutions. a) a solution that is 0.195M0.195M in HC2H3O2 and 0.120M in KC2H3O2 b)a solution that is 0.200M in CH3NH2 and 0.135M in CH3NH3Br
A Which of the following aqueous solutions are buffer solutions? (Select all that apply.) 0.40 M Cal2 + 0.23 M Ca(NO3)2 0.18 M HCIO + 0.20 M NACIO 0.27 M NH4 Br + 0.39 M NH3 0.24 M HCl + 0.21 M NaCl 0.13 M NaOH + 0.22 M NaCl 0 0 0 0 [Review Topics] [References] Use the References to access important values if needed for this question. Submit Answer Retry Entire Group 9 more group attempts remaining engage Learning
What is the solubility product expression for Pb3(PO4)2? Question 3 options: A) Ksp=[Pb2+][PO43-] B) Ksp=[Pb2+]3[PO43-]2 C) Ksp=[3Pb2+]3[2PO43-]2 D) Ksp=[Pb33+][PO43-] E) Ksp=3[Pb2+]2[PO43-]