An acid (HA) dissociates as follows: HA – H* +A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.35 M solution of HA is 4.83. What is (A minus]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit.

An acid (HA) dissociates as follows: HA – H* +A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.35 M solution of HA is 4.83. What is (A minus]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit.

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: A student is given a 0.1 M solution of an acid and is asked to determine whether it is a solution of…

A: Given: Concentration of acid = 0.1 M And the pH of the solution = 2.3

Q: <, (C,H;CO,H) = 6.5 x 105). • What is the initial pH before any base is added? The first digit is a…

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

A: The equilibrium reaction given is, => HA --------> H+ + A- Given : Initial concentration of…

Q: Determine the OH-] of a solution that is 0.135 M in CO,2-. Express your answer using two significant…

A: Given: Concentration of CO3-2 = 0.135 M Kb of HCO3- = 2.1×10-4

Q: The ionization constant of methylamine, CH3NH2, (Kb) is 4.2 x 10–4. Write the dissociation equation…

A: Please find your solution below : Ionic Equilibrium is the equilibrium in which the ionic substance…

Q: What is the pH of a 3.1 M potassium hydroxide, KOH, solution at 25oC , knowing that Kw = 1.0 x…

Q: What is the equilibrium pH of an initially 0.37 M solution of a weak acid HA at 25°C? Ka = 4.89 x 10…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: 9) Classify each of the following acids as strong or weak. If the acid is weak, write an expression…

Q: Phenol is a weak acid with a Ka = 1.28 x 10-10. As a pure compound, it is rather corrosive but in…

A: The reaction taking place will be PhOH ----> PhO- + H+ Assuming a concentration of PhOH is…

Q: 1. For each neutralization, state if the pH will be acidic (pH 7) when equal number of moles of…

A: According to the company guidelines, we have to answer only the first question. So, please kindly…

Q: Calculate the pH of the following solutions a)1 L 0,100 M malonic acid b)100 ml 0,100 M malonic…

Q: A solution is prepared in which the concentration of propionic acid, HC3H5O2, is 0.250 M and the…

A: The given buffer solution is a mixture of weak acid propionic acid (C2H5COOH) and its conjugate base…

Q: Chemistry The acidity of the water in a swimming pool is considered normal if the average of three…

A: Given the normal average pH range = 7.2 - 7.8 So the lower normal pH average range = 7.2 and upper…

Q: C. For the salts given below, label the pH of the resulting solution as acidic, basic or neutral. If…

A: Here is your answer

Q: 16- The pH value of 0.1 M ammonium hydroxide and 0.01 M ammonium chloride is - -- O 8.26 O 10.26 O…

Q: Which acid listed below is the weakest? O Hydrogen sulfide, H2S, Ką = 9.5 x 108 Citric acid,…

Q: An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium…

Q: Calculate the pH of the following solutions. Give your answers to two significant figures. (a) 0.021…

Q: The pH of an aqueous solution at 25°C was found to be 8.52. Calculate the pOH , and the hydronium…

A: The PH of the solution is given 8.52. The concentration of the hydronium ion and hydroxide ion of…

Q: The Lewis definition of acids and bases is used for reactions that do not involve proton (hydrogen…

A: Since you have posted question with multiple sub-parts, we are entitled to answer the first 3 only.…

Q: The pH of a 1.5M solution of boric acid (H, BO,) is measured to be 4.53. Calculate the acid…

A: Also given that : pH = 4.53 We know that, pH = -log[H3O+] So, [H3O+]=10-4.53 = 2.95 x 10-5 M

Q: of 45 > Assuming equal concentrations, arrange these solutions by pH. Highest pH HCN(aq) HI(aq)…

Q: Tartaric acid is found in many fruits, including grapes, and is partially responsible for the dry…

A: The first dissociation constant gives a major contribution to the calculation of the pH of tartaric…

Q: 5. Complete the table for the following strong acids and strong bases solutions. 0.070 M HCI [H*]…

A: pH = -log[H+] , pOH = -log[OH-] pH+pOH = 14 If pH < 7 then it is acidic If pH > 7 then it is…

Q: Chloroacetic acid, HC,H, CIO2, has a greater acid strength than acetic acid because the…

A: Given : Concentration of HC2H2ClO2 = 3.00 X 10-3 M And Ka of HC2H2ClO2 = 1.3 X 10-3 The partial…

Q: Determine the OH- and H+ concentration and calculate the pH, pOH of a solution that is 0.70 M NH3…

A: pH of a solution is a measure of acidity of a solution. pH less than 7 indicate that solution is…

Q: Q-3- Calculate the pH for ( four) these solutions. 1- 100 ml. 0.01 M acetic acid. 2- 200 ml. of…

Q: The initial molar concentration of formic acid (HCOOH) is 1.7 M. What is the pH of the solution, if…

A: In this question, we want to determine the pH of the Solution. You can see details Solution below…

Q: HCI, HNO3, HCIO, and HCIO: are strong acids. NaOH, KOH, LIOH, and Ca(OH)2 are strong bases. Complete…

A: A strong acid or a strong base fully dissociates in water. So the number of moles of ions produced…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-1 Ка(нсоон) = 1.77 ×…

A: Given: Ka (HIO3) = 1.6 × 10-1 Ka (HCOOH) = 1.77 × 10-4 We have to calculate the pH of a mixture of…

Q: C6H₂O₂ + H₂O = HC6H₂O₂ + OH- K₂ = 1.7 x 10-5 for sorbic acid, HC6H7O₂ a The potassium sorbate…

Q: Ką for formic acid, HCOOH, is 1.80×10-4. Ką for acetylsalicylic acid (aspirin), HC,H,04, is…

A: ->conjugate base of strong acid is weak base. ->Ka is proportional to acidity. ->conjugate…

Q: Calculate the pH of the following solutions: (a) 0.0500 M NaOH (b) 0.0500 M sodium acetate (c)…

A: A) 0.05 M NaOH As NaOH is a strong base, it will dissociate completey. NaOH (aq) → Na+ (aq)…

Q: Determine the pH of a 0.588 M weak base solution at 25°C. The K b for the weak base is 1.76 x 10 -5.…

A: The given base is weak base hence first determine the hydroxide ion concentration using ICE table.…

Q: Without using a calculator, determine the pH and pOH of each solution. Rank the solutions from most…

A: pH of the solution is equal to the negative logarithm of hydronium ion concentration while pOH is…

Q: HCN is a weak acid that ionizes according to the equation HCN(aq) + H2O(l) ⇄ H3O+(aq) + CN−(aq)…

A: Given that, HCN is a weak acid. This means that HCN will not readily give its proton. So it will not…

Q: The acidic ingredient in vinegar is acetic acid. The pH of vinegar is around 2.4, and the molar…

A: Ionization of acetic acid(CH3COOH): CH3COOH(aq) ⇌…

Q: Grades - BIOL111ASP2020 X 8 Canvas Login at Mary Baldwin U x 6 Chemistry 121 101 Chem101 Question 11…

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: K, for formic acid, HCOOH, is 1.80 × 10-4. K, for hydrocyanic acid, HCN, is 4.00 × 10-10. K, for…

Q: The pH for 6.1 × 10-4 M solution of cocaine, a weak base, is 9.60. Determine the value of Kb for…

Q: Consider the following data on some weak acids and weak bases: name acid acetic acid hydrocyanic…

A: Here we have to determine the increasing order pH of the following salt solution. pH of salt…

Q: A) Please fill in the first blank with the word "acidic", "basic" or "nearly neutral". B) SHOW ALL…

A: NH4Cl, when dissolved in water, shows a different behavior. Ammonium chloride is a neutral salt but…

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: CHo AQU , TV, 1. Determine whether the following solutions are Bronsted-Lowry acids or bases. Then,…

A: There are different type of substances which may be acidic, basic or salty in nature. For…

Q: Answer the following questions about weak acids. Use the K values in the following table to help…

A: First consider 0.10M HC2H3O2 reaction is noted as follows,

Q: For a 0.40 M solution of HCIO4, calculate: [H+], pH, pOH, and [OH"] Determine all pH and pOH values…

A: Given: Concentration of HClO4 = 0.40 M

Concept explainers

States of Matter

The substance that constitutes everything in the universe is known as matter. Matter comprises atoms which in turn are composed of electrons, protons, and neutrons. Different atoms combine together to give rise to molecules that act as a foundation for all kinds of substances. There are five states of matter based on their energies of attraction, namely solid, liquid, gases, plasma, and BEC (Bose-Einstein condensates).

Chemical Reactions and Equations

When a chemical species is transformed into another chemical species it is said to have undergone a chemical reaction. It consists of breaking existing bonds and forming new bonds by changing the position of electrons. These reactions are best explained using a chemical equation.

Question

An acid (HA) dissociates as follows:
HA – H* +A minus
Arrow should be interpreted as an equilibrium arrow.
The pH of the 0.35 M solution of HA is 4.83.
What is (A minus]?
Express your answer as a decimal, not an exponent.
Please include a proper (abbreviated) unit.

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

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 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

Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Students are often surprised to learn that organic acids, such as acetic acid, contain OH groups. Actually, all oxyacids contain hydroxyl groups. Sulfuric acid, usually written as H2SO4, has the structural formula SO2(OH)2, where S is the central atom. Identify the acids whose structural formulas are shown below. Why do they behave as acids, while NaOH and KOH are bases? a. SO(OH)2 b. ClO2(OH) c. HPO(OH)2
Using the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
Consider the following ions: NH4+, CO32, Br, S2, and ClO4. (a) Which of these ions in water gives an acidic solution and which gives a basic solution? (b) Which of these anions will have no effect on the pH of an aqueous solution? (c) Which ion is the strong base? (d) Write a chemical equation for the reaction of each basic anion with water.
Strong Acids, Weak Acids, and pH Two 0.10-mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0-L stock solutions of each acid. a Write the chemical reactions for these acids in water. What are the concentrations of the two acid solutions? b One of these acids is a strong acid, and one is weak. What could you measure that would tell you which acid was strong and which was weak? c Say that the HA(aq) solution has a pH of 3.7. Is this the stronger of the two acids? How did you arrive at your answer? d What is the concentration of A(aq) in the HA solution described in part c? e If HB(aq) is a strong acid, what is the hydronium-ion concentration? f In the solution of HB(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), B(aq), HB(aq), or OH(aq)? How did you decide? g In the solution of HA(aq), which of the following would you expect to be in the greatest concentration: H3O+(aq), A+(aq), HA(aq), or OH(aq)? How did you decide? h Say you add 1.0 L of pure water to a solution of HB. Would this water addition make the solution more acidic, make it less acidic, or not change the acidity of the original solution? Be sure to fully justify your answer. i You prepare a 1.0-L solution of HA. You then take a 200-mL sample of this solution and place it into a separate container. Would this 200 mL sample be more acidic, be less acidic, or have the same acidity as the original 1.0-L solution of HA(aq)? Be sure to support your answer.
Composition diagrams, commonly known as alpha plots, are often used to visualize the species in a solution of an acid or base as the pH is varied. The diagram for 0.100 M acetic acid is shown here. The plot shows how the fraction [alpha ()] of acetic acid in solution, =[CH3CO2H][CH3CO2H]+[CH3CO2] changes as the pH increases (blue curve). (The red curve shows how the fraction of acetate ion, CH3CO2, changes as the pH increases.) Alpha plots are another way of viewing the relative concentrations of acetic acid and acetate ion as a strong base is added to a solution of acetic acid in the course of a titration. (a) Explain why the fraction of acetic acid declines and that of acetate ion increases as the pH increases. (b) Which species predominates at a pH of 4, acetic acid or acetate ion? What is the situation at a pH of 6? (c) Consider the point where the two lines cross. The fraction of acetic acid in the solution is 0.5, and so is that of acetate ion. That is, the solution is half acid and half conjugate base; their concentrations are equal. At this point, the graph shows the pH is 4.74. Explain why the pH at this point is 4 74.
Using the diagrams shown in Problem 10-37, which of the four acids is the weakest acid?