Which of the following salts will form a basic solution in water? Select one: a. NH4Cl b. (CH3)NH3 Cl c. NaCl d. NaF e. NaNO3   Which of the following salts would be acidic Select one: a. NaCl b. NaOH c. NaCH3COO d. NH4Cl e. KNO3

Q: 1. Ephedrine is a naturally occurring drug useful in the treatment of asthma. a. Classify ephedrine…

A: The strength of an acid can be defined by the acid dissociation constant, Ka. The acid with higher…

Q: Apply the Bronsted theory of acids and bases to the following reaction: H3AsO4(aq) + H2O( l ) ⇆…

A: Answer:- This question is answered by using the simple concept of conjugate acid and base. Conjugate…

Q: Which of the following would give the highest pH when dissolved in water to form a 0.10 M solution?…

A: The pH of different types of salts are  1) pH > 7               => the solution is basic 2) pH…

Q: Which beaker best illustrates what happens when the following acids are dissolved in water?a.…

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Q: b Choose balanced equations showing how the HSO3 ion of sodium hydrogen sulfite, NaHSO3, can be a…

A: Bronsted Lowry base is a substance which acts as proton acceptor whereas bronsted Lowry acid is a…

Q: For each of the following solutions A. identify as cither acid or base; B. write the dissociation…

A:

Q: Which solution below has the highest concentration of hydronium ions (H+)? pH = 8.1 pH = 4.3  pH…

A: The concentration of hydronium ions can be calculated by the reverse of the mathematical operation

Q: 1. Arrange the following in order of INCREASING pH of their corresponding solutions. a. CaBr2, NaF,…

A: Answer - pH = pH are measured to have lower pH values than basic or alkaline solutions. The pH scale…

Q: When the pH of a solution changes from 3 to 8, the H+ concentrationa) decreases as the solution…

A: To explain the change in concentration of the H+ ions when the pH of the solution changes from 3 to…

Q: What is the pH of a 0.325M solution of NH4Cl?

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Q: NaH2PO4 - Ph 4.7 NA2HPO4 - Ph 8.8 Dihydrogen phosphate ion and monohydrogen phosphate ion are both…

A: An acid that contains more than one ionizable protons is termed as polyprotic acid. The removal of…

Q: 6. Which solution has the highest pH? A. 0.10 M HCIO4 (aq) B. 0.10 M HBrO4 (aq) C. 0.10 MHCI0(aq) D.…

A: pH is defined as negative logarithm of hydrogen ions

Q: a) Unlike benzoic acid, hydrochloric acid ionizes completely. Calculate the pH of a 0.30M HCI…

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Q: 13.6 mL of an HCl(aq) solution with a pH of 2.65 are mixed with 14.2 mL of another HCI(aq) solution…

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Q: Calculate the pH of a 0.10M solution for each substance pH(NH3)=9.3 pH(NH4Cl)=4.03…

A: Given , Concentration of solution = 0.10 M

Q: Which weak acid solution has the greatest percent ionization? Which solution has the lowest (most…

A: Percentage ionisation of a weak acid can be obtained by dividing concentrationof H+ ions produced by…

Q: A solution has a H3O+ concentration of 1.0 × 10–3 M. This solution is _____. a. acidic b. basic c.…

A: The value of pH can be calculated with the help of given H3O+ ions so that determines the acidic /…

Q: Predict whether dissolving the following makes an acidic basic or neutral solution.(why) CrCl6

A: Reference: Self Introduction: Salts are formed by the combination of both acidic and basic ions. the…

Q: Write the balanced reaction of hydroxide ion with hydrofluoric acid, HF, to for fluoride ion and…

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

Q: Differentiate between weak and strong acid with suitable examples.

A: Strong acids dissociate completely in water to produce the maximum number of H+  ions. This…

Q: 30. Which pH corresponds to the most basic solution? А. 3.0 В. 5.0 C. 7.0 D. 9.0 Е. 11.0

A: Concept: If pH less than 7 is Acidic solution pH more than 7 is the Basic solution pH= 7 is neutral…

Q: Calculate [OH-] in each aqueous solution at 25 °C, and classify the solution as acidic or basic.a.…

A: [H3O+] or [H+] x [OH-] = Kw here Kw = 1.0 x 10-14 from that the [OH-] = Kw / [H+] a) [H3O+] = 1.2 x…

Q: A common scouring powder contains baking soda (NaHCO₃) and Na₂CO₃. What can you say about aqueous…

A: Option B) Both compounds are basic in water so the solution is basic.

Q: Fill in the missing information in the following table. [H*] M [OH]] M pH pOH Acidic, Basic or…

A: The relationships needed to solve the problem are 1) pH + pOH = 14 2) pH = -log[H+]  3) pOH =…

Q: A common scouring powder contains baking soda (NaHCO₃) and Na₂CO₃. What can you say about aqueous…

A: Strong acids and strong bases are those compounds which can dissociate completely into ions in…

Q: What is the pH of a solution if there are 0.00456 grams of H+ present in 1L of solution.

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: Which of the following statements is true about a solution of ammonium acetate, NH4C2H3O2? [Ka(NH4+)…

A: Given :  Ka(NH4+) = 5.56x10-10  Ka(HC2H3O2) = 1.8x10-5

Q: A solution has a pH of 3.10. What is the OH− concentration of the solution at 25°C

A: The sum of pH and pOH of the solution is equal to 14. Calculate the pOH of the solution.…

Q: Which

A: If H2BO3- ion acept proton from another species and make H3BO3 ( Boric acid ) from H2BO3- ion then…

Q: Rank the following solutions from lowest to highest pH. 1.0 M NH3, 1.5 M HC2H3O2, 1.0 M HNO3, and…

A: pH is a measure of concentration of protons in a solution. It tells us about how much acidic or…

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: Which of the following substance/substances yield a basic solution when dissolved in water? (i) NaCN…

A: The solution of following compounds are:

Q: Which of the following statements is true about a strong acid? O a) Dissociates completely when…

A: There are four statements about strong acid :  (a)  Dissociated completely when dissolved in water.…

Q: OH (aq) + H2CO3(aq) HCO, (aq) + H2O(1) [ Select ] [ Select ] + [ Select ] [ Select ] Considering the…

A: According to Bronsted-Lowry Concept, conjugate acid-base pair only differ by one proton (H+). A…

Q: Calculate the [H3O^+] and the pH of each polyprotic acid solution. Please explain. A) 0.125 M H2CO3…

A:

Q: According to the Bronsted theory, which of the following statements is true?

A: According to the Brønsted-Lowry concept of acids and bases :- an acid is a proton (H+) donor and a…

Q: Which ion forms a basic solution when dissolved in water?a) Br- b) NO3- c) HSO4- d) SO32 -

A: An acid donates proton and forms a conjugate base. The strength of an acid depends upon the…

Q: The ph of a solution is 12.65 what is the [H+

A:

Q: Calculate the pH for each expressing each answer two decimal places:  [H3O+] = 6.7×10−8 M [H3O+] =…

A: [H3O+] = 6.7×10−8 M pH of the given compound is, pH = -log [H3O+] pH = -log(6.7×10−8 M) pH = 1.77

Q: Of the following, ________ is a weak acid. A) HF B) HCl C) HBr D) HNO3 E) HClO4

A: Acidic strength of any acid is decided by the ability of acid to produce protons in the solution.…

Q: Calculate [OH−] in the following aqueous solution at 25°C: [H3O+]= 1.7x10-9 M Express your answer…

A: The solution is as follows:

Q: What is the H3O+ ion concentration in a solution with an OH– ion concentration of 4.2 × 10–3 M? Is…

A: [OH–]  =  4.2 × 10–3 M [H3O+] = ..............? [H3O+][OH-]  = 1.0 x 10-14 [H3O+] 4.2 X 10-3 M = 1.0…

Q: 2. Which equation correctly describes the ionization of a weak acid in water? (i) H2SO4(aq) + H2O…

A:

Q: 15. List all the species present in a solution that is 0.25 M in NH,Br and 0.25 M in KBr. Rank the…

A: In this question , we have given a solution containing 0.25 M NH4Br and 0.25 M KBr. We have to…

Q: Calculate the [H3O+] and pH of each polyprotic acid solution.a. 0.350 M H3PO4 b. 0.350 M H2C2O4

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Q: If Solution A has a pH of 4 and Solution B has a pH of 6, which solution is more acidic? by how…

A: We have to compare the given two solution

Q: • Soap - red litmus paper chaned to blue. blue litmust paper showed no change in color • Synthetic…

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Q: Calculate the number of hydronium ions

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Q: Calculate [OH−][OH−] given [H3O+][H3O+] in each aqueous solution. A. [H3O+][H3O+] = 6.6×10−12 M…

A: In given question Kw = [H+][OH-] formula used

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.