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

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: Which of the following is a balanced molecular equation describing the titration of a weak acid with…

A: We have to tell among the given balanced molecular equation, which one balanced molecular equation…

Q: Identify the acid and base pair

A: Brownsted acid : Proton (H+ ) donar is called " acid " acid and its conjugate base has only 1…

Q: conjugate acid-base pairs.

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

Q: NH3 (aq) + H2O (I) 2 NH4* (aq) + OH- (aq)

Q: We can ignore the contribution of water to the concentration of OH− in a solution of the following…

A: Concept introduction: A weak base can ionize partially to form OH- ions and respective anion. The…

Q: Question 10 Which of the following are acid-base reactions? A K₂P (s) +20₂(g) → K₂PO4(s) 3KOH(aq) +…

A: We have to select the acid base reaction

Q: What is the pH of a 0.604 M NH3 solution that has a Kb = 1.8 x 10-5? The equation for the…

Q: What is the reaction associated with the autoionization constant of water, Kw? Group of answer…

Q: What is the pOH of a solution of 0.292 M CH3NH2 and 0.116 M CH3NH3Cl?…

A: Given, Kb = 4.4 × 10^-4 pOH = -log (OH-)

Q: Complete the balanced neutralization equation for the reaction below: HCI(aq) + NaOH(aq)

A: HCl is a strong acid . NaOH is a strong base. When a strong acid and a strong base react with each…

Q: 5. Acetic acid, CH3COOH is the main component of vinegar, apart from water. CH3COO(aq) + H3O* (aq)…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: The objective of the question is to identify the species in the reaction given for Bronsted Lowry…

Q: Which of the following is a balanced molecular equation describing the titration of a weak acid with…

Q: What type of ion is Na+?

Q: Questio Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: The salt given is C3H7NH3Br Since there is a proton on N in the salt ( cation C3H7NH3+ and anion Br-…

Q: What is the ionization percentage of 0.1 M of 500 mL of acetic acid solution, CH3COOH? (KCH3COOH =…

A: Acids that do not ionize completely in their aqueous solution are known as weak acids. Acetic acid…

Q: Identify acid, conjugate acid, base and conjugate base in the reactions below: →NH4* (aq) ◆ +H₂O (1)…

Q: Identify the reactant that is an acid and the reactant that is a base for both reactions. 1. HI(aq)…

Q: What is the pH of a solution of HCL in which (HCI] = 2.6 x 10 M7 (2 decimals only)

Q: What is the percent ionization of a 5.3 X 10-3 M HCN solution? The Ka of HCN is 4.9 X 10-10. HCN…

A: HCN is a weak acid and it is not completly dissociate into ions in solution

Q: grade 12 chemistry: In the following reaction, what is the function of the bolded substance?…

A: The species which can give (donate) H+ in the solution are acids and the base formed by them are…

Q: What is the pH (to two decimal places) of a 0.2 M HBr aqueous solution? HBr(aq) + H₂O(1) H3O+ (aq) +…

Q: 5. The dissociation reactions for several acids and their equilibrium constants are given below:…

A: The acid dissociation constant (Ka) of an acid is used to distinguish between strong acid and weak…

Q: HCl(aq) + Sr(OH)2(aq) ->

A: Law of Conservation of mass - "All atoms of various elements must be equal on both sides in a…

Q: Identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate…

A: Identify the bronsted lowry acid, base, conjugate acid and conjugate base in the following reaction…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Given, the chemical reaction is as follows,C6H5NH2(aq) +H2O(l) → C6H5NH3+(aq)+ OH-(aq)we are asked…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

A: According to Bronsted-Lowry acid-base theory, a pair of substances which differ by proton (H+) ion…

Q: Phosphoric acid, H3PO4, is a polyprotic acid. What is the SECOND ionization reaction for phosphoric…

A: The question is asking for the second ionization reaction of phosphoric acid (H3PO4) in water.…

Q: + H₂BO3(aq) HNO2 (aq) + H₂B03 (aq) In the reaction represented by the equation above, a conjugate…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: We have to predict Bronsted Lowry acid or base.

Q: Only a small fraction of a weak acid ionizes in aqueous solution. What is the percent ionization of…

A: Draw an ICE table for the given chemical reaction as - CH3CO2H(aq) +…

Q: Which one of these equations represents the reaction of a weak acid with a strong base? Group of…

A: Given,The reactions:H+(aq) + OH-(aq) → H2O(aq)H+(aq)+ CH3NH2(aq)→ CH3NH3+(aq) OH-(aq)+ HCN(aq)→…

Q: Which of the following is a balanced molecular equation describing the titration of a strong acid…

A: Given: Titration of a strong acid and a strong base.

Q: Question 2 In which reaction does bicarbonate act as a Bronsted-Lowry base? O HCO (aq) + NaOH (aq) →…

Q: Label the acid, base, conjugate acid, and conjugate base. H,PO, + CI → HPO,² + HCI

A: H2PO4- is Acid, and Conjugate base is HPO4 2-

Q: A 4.28⋅10^−2 M solution of HBr is made. (answer each part) part A: What is the pH of this solution?…

Q: to INCREASING acid strength. HNO2(aq) + HC00"(ag) NO2 (aq) + HCOOH(aq) HN3(aq) + Bro¯(aq) = N3 (aq)…

A: We are given the following equations:

Q: A 4.28⋅10^−2 M solution of KOH is made. (answer each part) part a: What is the pOH of this…

A: We have 4.28*10-2 M solution for KOH. We have to calculate the pOH, pH and hydrogen ion…

Q: In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a…

A: Given :- C6H15O3N(aq) + H2O(l) C6H15O3NH+(aq) + OH-(aq) According to Bronsted and Lowry…

Q: Question 17 On acidity and basicity of aqueous solutions, the following relationships are valid,…

A: 17) Relationship between pH and concentration of H+ and OH- ions:

Q: A person who overdoses on antacids may neutralize too much stomach acid, which causes an imbalance…

A: Antacid pills are composed of compounds which are basic in nature.

Q: Complete and balance the following acid-base neutralization reaction: ___KOH(aq) + ___H2SO4(aq) ——>

A: Neutralization reaction: Acid and base react to form salt and water, this reaction is known as a…

Q: For each of the following equations, indicate whether it represents an acid-base neutralization…

A: The interaction of H+ ions and OH- ions produces water in a neutralisation reaction, which occurs…

Q: Thinking about Le Chatelier's principle, what would happen to this equlibria if sodium hydroxide was…

A: According to Le Chatelier's principle, when an acid , base or salt, there is change in temperature,…

Q: A healthy individual has a blood with [H+] = 4.87× 10–8. Question: What is his/her blood pH?

A: The pH of a solution is a measure of the molar concentration of hydrogen ions in the solution and as…

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

Assuming the forward reactions are favored in the chemical equations below, arrange the acids according to INCREASING acid strength. HNO2(aq) + HCOO (aq) = NO2 (aq) + HCOOH(aq) HN3(aq) + Bro¯(aq) - N3¯(aq) + HBrO(aq) N3- + HCOOH(aq) = HN3(aq) + HC00"(aq) Your answer: HN3 HBRO HNO2 НСООН
In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. C2H;NH,(aq) + H,0(1) — CHNH3" (aq)(аq) + он (аq) В-L В-L The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is
For each reaction, identify the Brønsted-Lowry acid, the Brønsted-Lowry base, the conjugate acid, and the conjugate base. HNO3(aq)+ H2O(l)→H3O+(aq)+NO3−(aq)HNO3(aq)+ H2O(l)→H3O+(aq)+NO3−(aq) Express your answers as chemical formulas. Enter your answers in the order given in the question separated by commas.
Calculate the pH value of the solutions ( with the following parameters: c(H2PO4 ) = 0.23 mol L c(HPO42-) = 0,42 mol/L V(solution) = 0,942 L) (V(solution) = 0,961 L) c(KCl) = 0.30 mol L-1c(NaOH) = 0,30 mol/L
Which equation below is correct when HCI is added to a buffer solution of HCO₂H/NaHCO₂? NaHCO2(aq) + HCO2H(aq) →→ HCl(aq) + NaCl(aq) NaHCO2(aq) + HCl(aq) → HCO₂H(aq) + NaCl(aq) HCO₂H(aq) + HCl(aq) + NaHCO2(aq) + NaCl(aq) NaOH(aq) + HCl(aq) →→→→ H₂O(l) + NaCl(aq)
In the following net ionic equation, identify each reactant as either a Bronsted-Lowry acid or a Bronsted-Lowry base. C2H5NH2(aq) + H2O(l) C2H5NH3+(aq)(aq) + OH-(aq)B-L B-L The formula of the reactant that acts as a proton donor is The formula of the reactant that acts as a proton acceptor is
Idendify ALL of the the TRUE statements (there may be more than 1) A) NH4^(1+) and OH^(1-) form a conjugate acid-base pair B) HCO3^(1-) can act like a base or an acid C) H2O is the conjugate base of a Hydroxide ion D) NaHSO4(aq)+Na2CO3(aq)-->Na2SO4(aq)+NaHCO3(aq) is classified as a acid-base reaction
Rhododendrons are shrubs that produce beautiful flowers in the springtime. They only grow well in soil that has a pH that is 5.5 or slightly lower. What is the hydrogen ion concentration in the soil moisture if the pH is 5.57? [H3O+] = M
Choose the answer that has the appropriate acid and base that would make this neutralization reaction: Acid + Base --> H2O(l) + KCl(aq) HK(aq) + ClOH(aq) HCl(aq) + KOH(aq) H2Cl(aq) + KOH(aq) H2O(l) + KCl(aq)
Identify each of the substances in the reaction as acid, base, conjugate acid, or conjugate base. HSO, (aq) H¸O(1) 1, SO,² (aq) H,O*(aq) 31 --
3. Write equations for the formation of each salt. Write if the salt is,acidic, basic or neutral. Zn (aq) + HCL (D): (aq) ZnCl2 (aq) + H2 HCN__(aq) = NaCN (aq) + H₂O a) b) NaOH(aq) + c) (aq) + (aq) + (aq) + d) e) (aq) → CuSO4 (aq) + H2O (1): (aq) (NH4)2SO4 (aq) + (1): (aq) BaCl2 (aq) + (1):
What is the pOH of a solution of 0.376 M CH3NH2 and 0.111 M CH3NH3Cl?CH3NH2(aq)+H2O(l)⇌CH3NH3+(aq)+OH−(aq) Kb=4.4×10−4