**Problem Statement:**An acid (HA) dissociates as follows:\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]*Note: The arrow should be interpreted as an equilibrium arrow.*The pH of the 0.15 M solution of HA is 4.31.**Question:**What is the concentration of $\text{H}^+$?*Instructions:*Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit.**Your Answer:**| Answer | Units ||-----------------|-------|| | |

Answered: Image /qna-images/answer/f1564076-5fc1-458f-9268-cd88084ec245.jpg

An acid (HA) dissociates as follows: HA → H+ + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.15 M solution of HA is 4.31. What is [H*]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit. Your Answer:

An acid (HA) dissociates as follows: HA → H+ + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.15 M solution of HA is 4.31. What is [H*]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit. Your Answer:

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: You use a pH meter to measure the pH of a solution that has a pH of 5.0. Determine the concentration…

A: The measure of the acidic and basic strength of any solution is given by its pH value. A strong acid…

Q: Determine the pH and percent ionization for a hydrocyanic acid (HCN) solution of concentration 1.6 x…

A: Given: Concentration of HCN = 0.0016 M And Ka of HCN = 4.9 × 10-10 The…

Q: 6. The pH of a solution is calculated by using the formula pH = -log[H+], where H+ is the…

A: The problem is asking us to find the concentration of hydronium ions (H+) in a solution given the…

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

Q: A chemist must prepare 200.0 mL of hydrochloric acid solution with a pH of 1.00 at 25 °C. He will do…

A: Here we are required to find the volume of the concentrated hydrochloric acid that must a chemist…

Q: A) In the lab, you're working with a solution and measure it's pH with a meter to be 6.9. However,…

A: We know that, pH is the negative logarithm of hydronium ion concentration and pOH is the negative…

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

A: Given :- HA <-----> H+ + A- Initial concentration of HA = 0.37 M pH = 4.91 To be…

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

Q: What is the equilibrium constant expression, Ki, for the following weak acid? H3PO4(aq) + H*(aq) +…

Q: A solution of hydrofluoric acid, HF, has a pH of 4.20. Calculate the initial molarity of HF, whose…

A: Given -> pH = 4.20 Ka = 7.2 × 10-4

Q: The pH of a 0.244 M solution of sodium methanoate, HCOO-Na+, is 8.57. Calculate Kb for the…

Q: A solution of HCN was prepared in 2.5 L of water. The pH of this solution at 25°C was determined to…

A: We have to calculate the moles of HCN.

Q: Part A What is the pH of a 0.440 M ammonia solution?

A: [ NH3 ] = 0.44 M Kb = 1.8 × 10-5 pH = ?

Q: At 100°C and 1000 atm, Kw = 1.10×10-12. Answer the following questions for these conditions.…

A: Given data : Kw = 1.10×10-12

Q: Consider a 1.0-L solution that is initially 0.610 M NH3 and 0.750 M NH4Cl at 25 °C. What is the pH…

A: This is a basic buffer solution. pOH = pKb + log{[salt]/[base]} ...(1) Moles of NH3 = 0.610 Moles…

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

A: Answer:

Q: The concentration of hydronium, [H 30 *], in a solution that contains a weak acid is 5.28 x 10-5 M.…

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

Q: What is the pH of 425.0 mL of an aqueous solution containing 0.559 g of HCI? Round your answer to 3…

A: Volume= 425 ml 1 L = 1000 ml so 425 ml =0.425 L Volume= 0.425 L Weight of HCl = 0.559 gram.…

Q: the pH of a mysterious solution has an H+ concentration of: 1.704 x 10-2 is. After finding the pH,…

Q: None

A: The pH of a solution is a measure of its acidity or alkalinity. It is defined as the negative…

Q: A saturated solution of calcium phosphate has [Ca2*] = 1.5 x 10-6 M and [PO431= = 1.0 x 106 M. What…

A: Given, [Ca2+] = 1.5 x 10-6 [PO4]3- = 1.0 x 10-6 Solubility product describes the equilibrium…

Q: A solution of hydrofluoric acid, HF, has a pH of 2.20. Calculate the initial molarity of HF, whose…

A: pH of the solution = 2.20 Ka of HF = 7.2 × 10-4 Initial molarity of HF (C) = ? Note: HF is a weak…

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

Q: What is the [H+] in a solution with a pH of 3.75? Group of answer choices 5.6 x 103 7.5 x…

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

A: Given that, HA ----> H+ + A- [HA] = 0.11M , pH=4.80 Then,

Q: Each row of the table below describes an aqueous Complete the table. That is, fill in any missing…

A: negative logarithm of H3O+ (hydronium ion) concnetration is called pH there fore mathematically…

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

A: An acid is a particular substance which upon dissociation in an aqueous medium gives H+ ions…

Q: At 25 °C, how many dissociated OH ions are there in 1247 mL of an aqueous solution whose pH is 1.97?…

A: Given that At 25 °C, pH of the aqueous solution= 1.97 Volume of the solution= 1247 mL

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

A: Since, pH=-log[H+] and [H+]=110pH

Q: A solution is prepared at 25 °C that is initially 0.16M in acetic acid (HCH3CO₂), a weak acid with…

A: In this solution a acetic acid is a weak acid , and sodium acetate is its salt , so it will make a…

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

A: [H+] can be calculated by using formula

Q: Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA]…

A: we have to calculate the percent ionization

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe. Out…

A: Given, 0.050 M in H2Se 0.075 M in NaHSe

Q: A student planned an experiment that would use 0.10 M propionic acid, HC3H₂O₂. Calculate the value…

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

A: Acid dissociation constant is commonly known as Ka , it measures the strength of acid in solution.

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

A: Given: Molarity of NH3 solution = 0.70 M Kb of NH3 = 1.8 x 10-5

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.59. What is the Ka of the acid?

A: Given :- Concentration of weak acid = 0.037 M pH of solution = 4.59 To calculate :- Value of Ka

Q: The ionization of benzoic acid is represented by this equation. C6H5COOH(aq) ↔ H+(aq) + C6H5COO–(aq)…

Question

**Problem Statement:**

An acid (HA) dissociates as follows:

\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]

*Note: The arrow should be interpreted as an equilibrium arrow.*

The pH of the 0.15 M solution of HA is 4.31.

**Question:**

What is the concentration of $\text{H}^+$?

*Instructions:*

Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit.

**Your Answer:**

| Answer | Units |
|-----------------|-------|
| | |

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

Similar questions

This is a multi- answer question. Please type your properly rounded answers in the next three questions ( starting with this one):Calculate the pH of a 0.70 M solution of sodium sulfite, Na2SO3. Also calculate the concentrations of HSO3 and H2SO3. Type the properly rounded pH below:
Give me expert solutions
5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this solution acidic, basic, or neutral? b. If the hydrogen ion concentration, [H°] = 8.47 x 1012 M, what is the pH? Is this solution acidic, basic, or neutral? 6. Calculate the pH of a 0.10 M solution of propanoic acid (C2H;COOH or generically, HA) and determine its percent ionization. K, = 1.3 x 10:5
help please
An acid (HA) dissociates as follows: HA – H* + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.80 M solution of HA is 1.42. What is the K, of HA? Express your answer as a decimal, not an exponent.
Consider the following data on some weak acids and weak bases: name acetic acid hypochlorous acid 0.1 M KCI acid solution 0.1 M KCIO 0.1 M C6H5NH3Br 0.1 M NH4CI formula HCH3CO₂ 1.8 x 10-5 HCIO Ra Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. 3.0 × 10 pH choose one -8 choose one choose one base choose one ✓ Ko name formula aniline C6H5NH₂ 4.3 × 10¯ - 10 ammonia NH3 1.8 × 10
3.
Answer the 2 questions below: Determine both the H and the pH in a 0.0088 M solution of HCIO, at 25 °C? (H*)= Type your answer here M pH = Type your answer here Determine both the OH and the pOH in a 0.0032 M solution of Ba(OH)2at 25 °C? OH]= Type your answer here M pOH = Type your answer here Unanswered 梦 $ a hp prt sc delete backspace
A solution of HCN was prepared in 2.5 L of water. The pH of this solution at 25°C was determined to be 4.87. The Ka for hydrocyanic acid is 6.17 × 10-10. How many moles of HCN were used to prepare the solution? Report your answer to the hundredths place
In a 0.09 M solution of chlorous acid, what percentage of the acid is ionized to the chlorous anion, ClO2-? Ka = 1.1 x 10-2 include 3 significant figures in your answer
I am having a hard time with pH calculations. I have a chart I am working on trying to complete and it gives you the H+ and OH- and you have to find the pH.
a Calculate the molar concentration of the following ion. OH in a solution that contains 1×10-¹¹ M H30+. (Enter your answer to one significant figure.) [OH-] = M b Calculate the molar concentration of the following ion. H3O+ in a solution that contains 1×10-4 M OH-. (Enter your answer to one significant figure.) [H3O+] = M C Calculate the molar concentration of the following ion. OH in a solution that contains 1×10-4 M H30+. (Enter your answer to one significant figure.) [OH-] = M