Answered: Using the dissociation constant, Kd =…

Using the dissociation constant, Kd = 3.4 × 10–15, calculate the equilibrium concentrations of Zn2+ and OH– in a 0.0465-M solution of Zn(OH)4 2−.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.83QE

See similar textbooks

Related questions

Q: The following 4 questions involve the titration of a 50.00 mL sample of 0.200 M chlorous acid,…

A: pH - It is the negative logarithm of the hydrogen ion concentration of a solution. Given:- Ka =…

Q: An analytical chemist is titrating 91.3 mL of a 0.7000M solution of butanoic acid (HC3H,CO₂) with a…

A: Here we are required to find the pH of the solution.

Q: 1) Calculate the pH of a solution prepared by dissolving 1.45 g of sodium acetate, CH₂COONa, in 50.0…

Q: What is the pH of a buffer solution that is 0.15 M puridine, C6H5N and 0.08 M pyridinium bromide…

Q: n the laboratory, a general chemistry student measured the pH of a 0.578 M aqueous solution of…

A: Aspirin (acetylsalicylic acid) is a weak acid. The dissociation of weak acid is given as:HA ⇌ H+ +…

Q: A natural water sample contains 0.484 M NaCl, 054 M MgBr2 and trace levels Ag+ ions. Write the…

A: Ionic strength of the water sample = 2.1 MExplanation:As Ag+ ion is present in very less amount so…

Q: What is the pH of a buffer solution containing 1.25 M NH₃ and 0.75 M NH₄NO₃? Note that the base…

Q: Determine the pH during the titration of 36.4 mL of 0.299 M ethylamine (C,H;NH, K, = 4.3×104) by…

A: Hello. Since your question has multiple sub-parts, we will solve first three sub-parts for you. If…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: Ka(experiment)

Q: For each of the following cases, decide whether the pH is less than 7, equal to 7, or greater than…

Q: In the laboratory, a general chemistry student measured the pH of a 0.433 M aqueous solution of…

Q: A student does a titration of 86.0 mL of a 0.37 M solution of methylamine (CH3NH2(aq) (pKb =3.36)…

A: PH+Poh=14. This is basic buffer equation Poh=pkb+log[salt]/base Use this equation and get the…

Q: What is the pH of a buffer that is 0.153 M in a weak acid and 0.227 M in the acid's conjugate base?…

A: Weak Acid concentration = 0.153 M. Conjugate base Concentration = 0.227 M. Ka = 5.7 × 10-4 pKa = -…

Q: sample of an aqueous weak base (RNH2, where R is an tion with a standard 0.150 M HBr(aq) titrant.…

A: Given, pH = 5.40 At equivalence point, salt is formed. If equal is mixed, then concentration is…

Q: ulate the pH at the equivalence point in the titration of 50 mL of 0.10 M methylamine = 4.3 × 10)…

Q: Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and…

A: The Ka values for the phosphoric acid areThe phosphoric acid has the following ionizations H3PO4 ⇌…

Q: Calculate the equilibrium concentration of Zn2+ in a 0.30-M solution of Zn(CN)4 2−.

A: As per law of chemical equilibrium, for reversible dissociation of a compound its dissociation…

Q: You are asked to prepare a buffer for an experiment. You have access to the following dolutions of…

Q: water sample

A: Generally, drinking water has a pH of 7, which is neither acidic nor basic and is safe to drink. The…

Q: What is the pH of a 0.455 M solution of lactate, (CH3)2 COO^-1. The pKa of lactic acid, (CH3)2 COOH…

A: Given - Concentration of solution of lactate (CH3)2 COO- = 0.455 M pKa of lactic acid (CH3)2 COOH)…

Q: 1) Write the equilibrium constant expression for the dissociation of acetic acid

A: Below attached file showing the details answer. All the best. As per Bartleby answering guidelines…

Q: Calculate the pH of the buffer system made up of 0.19 M NH3 and 0.48 M NH₂Cl. The K of NH³ is 1.8 ×…

Q: An analytical chemist is titrating 185.8 mL of a 0.9600M solution of butanoic acid (HC3H,CO₂) with a…

Q: Determine the pH and pOH of 0.25 L of a solution that is 0.0201 M boric acid and 0.0366 M sodium…

A: Concentration of boric acid ([B(OH)3])= 0.0201 M Concentration of sodium borate ([sodium borate])=…

Q: At 22 °C, an excess amount of a generic metal hydroxide, M(OH)2, is mixed with pure water. The…

Q: The pH of a saturated solution of a metal hydroxide M(OH)2 is 10.500. Calculate the Ksp for this…

A: ksp : sloublity product Ksp = equilibrium between solids and liquids

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: determine the K, for this acid.

A: Given :- pH = 5.098 concentration of phenol = 0.597 M To calculate :- Ka

Q: A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined with 4.90 mL of 6.20 M NaOH and the…

A: Given:Mass of weak acid (HA) = 5.65 gVolume of NaOH = 4.90 mL 0.0049 LMolarity of NaOH = 6.20…

Q: For the titration of 50. mL of 0.10 M ammonia with 0.10 M HCI, calculate the pH. For ammonia, NH3,…

A: When weak base like ammonia is treated with strong base like hydrochloric acid. Then pH decreases…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: In the laboratory, a general chemistry student measured the pH of a 0.578 M aqueous solution of…

Q: Calculating the pH of a buffer -4 and 0.13M in sodium nitrite α A solution is prepared at 25 °C that…

A: Ph is 3.28Explanation:Step 1:To calculate the pH of the solution, Henderson- Hasselbalch equation,…

Q: A solution is prepared at 25 °C that is initially 0.48 M in propanoic acid (HC₂H,CO₂), a weak acid…

A: Concentration of propanoic acid ([HC2H5CO2] = 0.48 M Concentration of potassium propanoate…

Q: You are running a titration. You have placed 40.0 mL of 0.200 M chlorous acid, HClO2, in a flask…

A: This question can be solved using Henderson-Hesselbech equation.

Q: Enter your answer in the provided box. Calculate the pH of a bicarbonate/carbonate buffer in which…

Q: ) Lead(II) hydroxide, Pb(OH)2 consists of lead(II) ion and hydroxide ion. Given that Kyp value of…

A: Solubility product is an equilibrium constant which is determined by multiplying the concentration…

Q: Calculate the pH at the equivalence point for the titration of 0.170 M methylamine ( C H 3 N H 2 )…

Q: Explain what happens to the ratio of the two common forms of free residua! chlorine as the pH of…

A: Hypochlorite, ClO-(aq) is a conjugate base of HOCl. #(i): Since HOCl(aq) and ClO-(aq) are conjugate…

Q: Describe the pH changes that occur during the titration of a weak base by a strong acid. What is…

A: A reaction between a base and an acid to give water and salt as products is known as the…

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

Using the dissociation constant, K_d = 3.4 × 10^–15, calculate the equilibrium concentrations of Zn²⁺ and OH^– in a 0.0465-M solution of Zn(OH)₄ ²⁻.

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 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

For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
What is the pH of a solution prepared by mixing 55.00 mL of 0.10 M methylamine, CH3NH2, with 15.00 mL of 0.10 M methylammonium chloride, CH3NH3CI? Assume that the volume of the solutions are additive and that Kp = 4.4 x 104 for methylamine.
4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.
0.0500 M HF (Ka= 7.20 x 10–4) determine the quilibrium molar concentration of H3O+, equilibrium molar concentration of HF, pOH, and %ionization in 3 sig. figures.
1. The ionization constant (Kb) of aniline (C6H5NH2) is 2.35 x 10^-5. If 7.285 grams of aniline is dissolved in 100.0 mL of water, what are the equilibrium concentration of all species present?2. A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell signaling. A 0.439M solution of this acid is found to have a pH of 2.607. Based on the table below, what most likely is the identity of thisunknown acid?
14- A quality-control technician places a 20.00 mL sample of 0.600 mol/L ethanoic acid, HC₂H3O2(aq) (a weak acid), in an Erlenmeyer flask. She titrates this sample with a standardized 0.300 mol/L solution of sodium hydroxide, NaOH(aq) (a strong base). Predict the pH of the solution (Ka=1.8 3x105) (a) before titration begins (b) at the equivalence point when 40.00 mL of NaOH(aq) has been added (c) beyond the equivalence point when a total of 60.00 mL of NaOH(aq) has been added As Sample Problem 1, this is a titration of a weak acid, HC₂H3O2(aq), by a strong base
Calculate the pH at the equivalence point in the titration of 50 mL of 0.10 M methylamine (к, — 4.3 х 10) with a 0.20 M HCI solution.
(a) Calculate the acetate ion concentration in a solution prepared by dissolving 8.70×10-3 mol of HCl(g) in 1.00 L of 1.10 M aqueous acetic acid (Ka = 1.80×10-5). (b) Calculate the pH of the above solution. Give your answer to two decimal places.
Calculate the pH of a bicarbonate/carbonate buffer in which the concentration of sodium bicarbonate (NaHCO3) is always 0.31 M, but the concentration of sodium carbonate (Na2CO3) corresponds to the following values: 0.83 M. (Ka for HCO3− is 5.6 × 10−11.) Report your answer to four significant figures.
Write the chemical reactions whose equilibrium constants are Kp and Ką for imidazole (C,H,N,) and imidazole hydrochloride (C,H,N,H*CI¯), respectively. K, reaction: 2.865 Incorrect K, reaction: 2.323 Incorrect Calculate the pH of a solution prepared by mixing 1.60 g of imidazole with 1.60 g of imidazole hydrochloride and diluting to 100.0 mL. The pKą of imidazole hydrochloride is 6.993. 2.07 pH Incorrect Calculate the pH of the solution if 2.00 mL of 1.06 M HCIO, are added. pH = Incorrect How many milliliters of 1.06 M HCI,, should be added to 1.60 g of imidazole to give a pH of 6.993? 2.865 volume: mL. Incorrect
6a. Draw the Lewis Dot structure for the following diprotic acid: HOOC-CH,-COOH. 38.5 mL of a 1.15 M solution of this acid is titrated to the equivalence point with 0.69 M KOH. Write the balanced equation for this reaction and determine the volume of base needed to completely neutralize the acid.
(a) Calculate the pH of the 0.30 M NH3 / 0.35 M NH4Cl buffer. What is the pH of the buffer after the addition of 0.030 mol HCl? note: Ka (NH4+) = 5.6 x 10 -10 NH3 (aq) + H+ (aq) → NH4+ (aq) (b) What are the hydronium [H3O+] and hydroxide [OH-] ion concentrations at 25°C in a 4.0 M aqueous Mg(OH)2.