QUESTION 15Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed?HCI(aq) + LIOH(aq) = H20() + LICI(aq)O CH3CO2H(aq) + LIOH(aq) = H20() + LICH3CO2(aq)O H2SO4(aq) + 2 KOH(aq) 2 H20() + K2SO4(aq)HI(aq) + C5H5N(aq) C5H5NHI(aq)Click Save and Submit to save and submit. Click Save All Answers to save all answers.MacBook AirDDF7F8F9F5F6F3F4F1F2233456.Y.000000%24LL

Which of the following reaction has a pH>7 when equal moles of acid and base is taken ?

QUESTION 15 Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed? HCI(aq) + LIOH(aq) =H20() + LICI(aq) CH3CO2H(aq) + LIOH(aq) = H20() + LICH3CO2(aq) H2SO4(aq) + 2 KOH(aq) =2 H20() + K2SO4(aq) HI(aq) + C5H5N(aq) = C5H5NHI(aq)

QUESTION 15 Which of these neutralization reactions has a pH > 7 when equal moles of acid and base are mixed? HCI(aq) + LIOH(aq) =H20() + LICI(aq) CH3CO2H(aq) + LIOH(aq) = H20() + LICH3CO2(aq) H2SO4(aq) + 2 KOH(aq) =2 H20() + K2SO4(aq) HI(aq) + C5H5N(aq) = C5H5NHI(aq)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 77QAP: Two students were asked to determine the Kb of an unknown base. They were given a bottle with a...

See similar textbooks

Related questions

Q: Hydrofluoric acid, HF, unlike hydrochloric acid, is a weak electrolyte. What is the hydronium-ion…

Q: For HBrO Ka = 2.30 x 10-9. What is the pH of a 0.15 M solution of HBrO? (ICE Problem) HBrO + H2O ↔…

A: Reaction equation for the acid and water is given as: The dissociation of acid is given as: ICE…

Q: Question 14 of 23 Subr Determine if the following salt is neutral, acidic or basic. If acidic or…

A: NaCN is made up of: HCN(aq) + NaOH(aq) .....> NaCN(aq) + H2O(l)

Q: 2. Calculate the following (report to 2 decimals, use scientific notation when calculating H3O*) and…

A: In a given question we have to find out pH of a solution i.e. pH= -log[H3O+] If pH>7 Basic…

Q: 4. Aqua regia (1:3 mixture of nitric acid and hydrochloric acid) is commonly used to remove noble…

Q: QUESTION 13 Which of the following acids is a weak acid? HCl HI HBr HF

A: The weak acids are those acids that are not able to release H+ in the solution. While the strong…

Q: Questions 1. Define pH of a solution. Calculate the pH of a 1.37M solution of HCl. 2. Define pOH of…

A: By using the formula pH = -log10[H(+)] --------------(I) pH+pOH = 14-------------------(II) 1.…

Q: Do you expect KClO4 ( OR "K" ClO4) to be acidic, neutral, or basic when dissolved in pure water?

A: The salts of strong bases and strong acids are neutrals at pH 7. The salts of weak bases and strong…

Q: Question 2: Suppose your supervisor gave you two beakers, one containing 0.1 gm of HCl (mat-1) and…

Q: Choose the true statements about acidic, basic, and neutral aqueous solutions below. Select all that…

A: 1. In a basic solution hydroxide ion concentration is more than proton concentration. 2. In neutral…

Q: Which one of these salts will form a basic solution upon dissolving in water? Question 2 options:…

A: The solution containing a salt of a strong base and weak acid is basic. The solution containing a…

Q: Question 3 of 7 A diprotic acid, H2A, has Ka1 = 3.4 x 10 4 and Ka2 = 6.7 × 10 °. What is the pH of a…

A: Given :- [H2A] = .11M Ka1 = 3.4 × 10-4 Ka2 = 6.7 × 10-9

Q: Which equation represents the auto-ionization of water?

Q: Assuming that the pH of the blood is maintained at 7.4 by H2PO4- acid and its salt, HPO42-,…

Q: Calculate the acid ionization for Ka for propionic acid, HC3H5O2. The pH of a 0.012 M aqueous…

Q: Question 1 A 2.75 x 10 3 M Ba(OH), solution is prepared. a. What is the pOH of the solution? (write…

A: (1) When barium hydroxide Dissociates in water, it gives two Hydroxide ions as - Ba(OH)2 ----->…

Q: Idency ase can Part A Pyridine is a weak base that is used in the manufacture of pesticides and…

A: Calculation of PH

Q: Question 1 Which of the following statements is true of a 2.5 x 10 M HCl solution? Select all that…

Q: HF. (T/F). 24. A vinegar solution (acetic acid) has a hydroxide ion concentration of 0.000000000005…

A: 24 Given Concentration of OH- = 5 × 10-12 M

Q: 11) Do you expect NaCHO3 ( OR "N" a CHO3) to be acidic, neutral, or basic when dissolved in pure…

A: NaHCO3 commonly known as Sodium Bicarbonate or Baking Soda is Basic in Nature.

Q: QUESTION 1 In a NaOH solution [OH-] is 2.9 x 10-4M. Calculate the pH of the solution. (Round-off…

A: Note: As per our guidelines, we are supposed to answer the first question when multiple questions…

Q: QUESTION 13 Identify the acid, base, conjugate acid and conjugate base in the following reation:…

Q: The pH of a solution is 9. What is the pOH? pOH = What is the hydrogen concentration? [H+] = M…

A: Given The pH of a solution is 9 We have to find pOH, and tell solution Is this an acid, base or…

Q: Question 4 4.1 Calculate the acid ionization for Ka for propionic acid, HC3H5O2. The pH of a 0.012 M…

A: Weak acids like organic acids have less degree of ionisation and can be correlated by…

Q: QUESTION 26 In a 1.00 M aqueous solution of sulfuric acid, H₂SO4, three processes producing the…

A: Given equations of dissociation of H2SO4 are : 1. H2SO4 (aq) + H2O (l) ---------> H3O+ (aq) +…

Q: QUESTION 1 For the following equation, identify the conjugate acid-base pairs: HCI + H2O → CIT +…

A: Identify the conjugate acid-base pairs ----

Q: Question 15 For a solution equimolar in HCN and NaCN, which statement is false? a) This is an…

A: Que 15

Q: Constants Periodic Tab Pyridine is a weak base that is used in the manufacture of pesticides and…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: For the diprotic weak acid H2A, Ka1 = 3.1 × 10-6 and K2 = 8.4 × 10-9. What is the pH of a 0.0500 M…

A: The concentration of diprotic weak acid H-A is 0.0500 M. The value of acid dissociation constant Ka1…

Q: A certain acidic vitamin is essential for all mammals since it plays a role in DNA repair and cell…

A: Given, Molarity of weak acid [HA] =0.439 M pH = 2.607 Calculate Ka to match the answer ?

Q: For many weak acid or weak base calculations, you can use a simplifying assumption to avoid solving…

Q: QUESTION 23 Calculate the pH when a slightly soluble compound, CoS is dissolved in water. Ksp =…

Q: For the diprotic weak acid H2A, Kal = 3.0 × 10-6 and Ka2 = 7.1 × 10-9. What is the pH of a 0.0700 M…

A: We will calculate pH and the equilibrium concentration of the solution.

Q: Question 16 Select the solution below that is the most acidic. A [H30) 1.0* 10 10 M B [H30) 1.0 10 4…

Q: Question#10. Write the acid dissociation constant expression for nitrous acid, HNO2. Weak acid How…

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

Q: This question requires a file upload. You will need to write your answer paper and take a picture or…

A: To find the names of the below acids and find if they are strong or weak? (a) H2SO3 (b) HBr (c)…

Q: shampoo has a pH of 8.66. what is the [H3O+] and the [OH-] in the shampoo

A: To determine the concentration of H3O+ and OH- ions if the pH is 8.66.

Q: Which of the following equations represents the acid equilibrium associated with Каz for H3PO3? A)…

A: Ka is the ionization constant of acid, for weak acid it refer as equilibrium constant Also called…

Q: 14) Do you expect NaBr to be acidic, neutral, or basic when dissolved in pure water? Question 14…

A: Acid base theory- Acids and bases have their own importance in chemistry. Acids and bases are…

Q: Question Completion Status: QUESTION 20 A solution has a pH of 5.4. What is its pOH? O a.-8.6 O…

A: Given that: pH of solution = 5.4

Q: A solution has H3O4 concentration of 8.2 x 10-4 M H3O+. What is the pH of this solution? Report…

A: Given, Concentration of H3O+ ion = [H3O+] = 8.2 x 10-4 M pH of the solution = ? Note: pH : it can…

Q: what is the (OH-) of the blood plasma

A: The concentration of hydronium ions, determines the value of pH of a solution. pH is a measure of…

Q: Which of the following chemical reactions corresponds to the base dissociation constant, Kb, for…

A: Kb => base dissociation constant It can be represented as follows

Q: 0.010 M aqueous solution of the weak acid, m-Nitrophenol (C6H4NO2OH) has a pH of 3.44. Calculate the…

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

Q: QUESTION 13 Which of the following reactions shows a weak acid? H20 KOH(s) K*(aq) + OH(aq) O HCI(aq)…

A: A weak acid is an acid that doesn't completely dissociate into the ions when dissolved in an aqueous…

Q: Which one of the following is classified as a base? Question 5 options: HCl (aq) CO2 (g)…

A: Given that : We have to identify which of the following is a base : HCl (aq) CO2 (g)…

Q: The pH value of a liquid A is 3.8 and the pH value of a liquid B is 6.2. How many times as acidic as…

Q: The pH of 0.8567 grams of Ba(OH)2 dissolved in water using a 1-L volumetric flask. Answer must have…

Q: What are the concentrations of all the solute species in 0.150 M lactic acid, HC3HSO2? What is the…

A: Given: 0.150M lactic acid, HC3H5O2 Ka for lactic acid is 1.4x10-4 First the concentration value of…

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

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 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

You want to make up 3.00 L of aqueous hydrochloric acid, HCl(aq), that has a pH of 2.00. How many grams of concentrated hydrochloric acid will you need? Concentrated hydrochloric acid contains 37.2 mass percent of HCl.
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
If an acid solution has a concentration of 0.10 M and a pH of 2.5, what is the [H1+]?And what is the % dissociation?
Pls help Calculate the pH of a solution (aq., 25 oC) prepared by dissolving 23.632 g of solid methylammonium chloride (CH3NH3Cl) in 1.00 L of 1.10 M methylamine (CH3NH2). The Kb for methylamine is 4.40 × 10-4. Report to two decimal places. MM CH3NH3Cl = 67.518 g/mol
13.2) Anisic acid (Ka=3.38x10^-5) is found in anise seeds and is used as a favoring agent. For a 0.867 M solution of anisic acid, calculate [H+], [OH-], pH, and % ionization.
for aqueous solution of the weak acid HCN, f = cin -p+2=2-1+2= 3. cin can be calculated be by c - r - a = 5 (H2O, HCN, H+, OH- and CN-) -2 (h20 -> H+ OH, HCN -> H+CN)-1 = 2. or it can also be calcualted by cin = 2 (H2O, HCN). MY QUESTION: is the second way of calculating only available for aqueous solution? how to use the first method to calculate aqueous solution of two compound (e.g. KCN and HCl)?
No Plagiarism Please! 15. HCl is a strong acid, explain why when the pH is measured the pH of the acid sample is 5.4?
Which expression best represents the ionization of formic acid, HCO2H, in water? A. HCO2H (aq) + 2H2O (l) ⇌ H2CO3 (aq) + H3O+ (aq) B. HCO2H (aq) + H2O (l) → CO2- (aq) + 2H3O+ (aq) C. HCO2H (aq) + H2O (l) → CO2 (aq) + H3O+ (aq) D. HCO2H (aq) + H2O (l) ⇌ HCO2- (aq) + H3O+ (aq) E. HCO2H (aq) + H2O (l) → HCO3- (aq) + H+ (aq)
QUESTION 17 Which of the following chemical reactions corresponds to the base dissociation constant, Kb, for ammonia? NH4+(aq) + H2O (ℓ) ⇌ NH3 (aq) + H3O+(aq) NH3 (aq) + OH−(aq) ⇌ NH2−(aq) + H2O (ℓ) NH3 (aq) + H2O (ℓ) ⇌ NH4+(aq) + OH−(aq) NH3 (aq) + H3O+(aq) ⇌ NH4+(aq) + H2O (ℓ) NH4+(aq) + OH−(aq) ⇌ NH3 (aq) + H2O (ℓ)
What does HC2H3O2 (M)=___________ When pH before HCl added is 2.56 pH after HCl is 1.58 and the pH before and after (pHbefore -pHafter) = 0.98
What would be the [H3O+]for a soda found to have a [OH−]of 1.26 × 10−13 mol/L? Is the solution acidic, basic, or neutral? Note: Write the [H3O+]answer in 3 significant figures
1. What is the PH for a solution that has a volume of 2.50L and contains 5.33 grams of HCL? 2. Complete calculation [H+],[OH-],pH and POH for 0.75M NaOH with 100% ionization? 3. Find [H+],[OH-],pH and pOH for 0.121 M HlO4 with 100% ionization?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry

ISBN:

9781133611097

Author:

Steven S. Zumdahl

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

General Chemistry - Standalone book (MindTap Cour…

Chemistry

ISBN:

9781305580343

Author:

Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS