Which of the following solutions is most basic? [H3O+] = 3x10-7 [H3O+] = 8x10-3 [H3O+] = 2x10-6 [H3O+] = 4x10-12 [H3O+] = 5x10-5

Q: Calculate [OH-] when given the [H3O+] in each of the following aqueous solutions and classify the…

A: The OH- has to be calculated for the given aqueous solutions and whether they were acidic, basic or…

Q: Vhich of the following conditions is acidic? [H30*] = 1.4 x 10 -11 А. [H3O*] = 7.2 x 10 -3 В. С.…

A: pH = -log [H3O+] pOH = -log [OH-]  pH = 14 - pOH  When pH < 7 , acidic solution pH = 7, neutral…

Q: Which of these solutions are basic at 25 °C?25 °C? Solution B: [H3O+]=9.07×10−9 MSolution B:…

A: Solution basic is one which have PH>7 So that we can Calculate PH+POH=14 PH=-log[H+] PH+Poh=14…

Q: Complete the following table with the needed [H3O+], [OH-],  pH, and pOH. Then, classify the…

A: Complete the following table with the needed [H3O+], [OH-],  pH, and pOH. Then, classify the…

Q: Which of the following solutions is acidic?     [H 3O +] 7.0 x 10 -7 M     [H 3O +] = 1.5 x 10…

A: We have to predict the acidic solution.

Q: When would a solution be basic? [H+] > [OH-] When the pH is from 7 to 14 [H+] = 1 × 10-7

A: A solution is basic, when an aqueous solution contains more hydroxide (OH-) ions than that of H+…

Q: Solution 1 has a [H3O+] = 1.70 x 10-² M. Solution 2 has a [H3O+] = 4.30 x 10-4 M. Which of the foll…

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Q: Calculate either [H3O+] or [OH¯] for each of the solutions at 25 °C. Solution A: [OH-] = 1.57 × 10−7…

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Q: Calculate either [H,O*] or [OH¯] for each of the solutions. Solution A: [OH¯] = 2.55 x 10-7 M;…

A: Use relation:  Kw = [H3O+][OH-]  At 25°C Kw = 10-14  In basic solution pH >7  => [H3O+] <…

Q: H2NNH2 is a weak diprotic base.  Calculate [OH-], [H2NNH3+], [H3NNH32+] and [H3O+] in a 0.1M…

A: A weak diprotic base undergoes partial dissociation twice and releases a hydroxide ion OH- and its…

Q: Which acid is weakest?   H3AsO3, Ka=5.1x10-10   HClO2, Ka=1.1x10-2   H3PO4, Ka1=7.5x10-3   H2PO4-,…

A: We have acid dissociation constant of four compound, we have to determine the weakest acid among…

Q: Which of the following is the most basic?  A solution with [H+] = 1.0×10-3.  A solution with [OH-]…

A: The basic nature of a solution can be determined by comparing the concentration of the hydrogen ion…

Q: Acids and Bases Identify the classification of these substances. The choices are: strong acid,…

A: A substance that completely dissociates into its ions after its dissolution in water, is called a…

Q: Arrange the following 0.10 M solutions in order from most acidic to most basic: NH4+…

A: Given question of three compounds. NH4+             HNO3             HNO2 We have to order of most…

Q: How many acids below are polyprotic? HNO3 H2SO4 H2CO3 HCN H2C204 0 1 O 2 O 4 O 5

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Q: Which of the following solutions is acidic? Group of answer choices [OH-] = 1.0 x 10-7 M [OH-] >…

A: Acidic solutions are those solutions which have pH less than 7. And basic solutions are those which…

Q: Which solution below is the most acidic? Group of answer choices [H3O+] = 1.0 × 10–10 M [H3O+] = 1.0…

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Q: Which of the following statements is INCORRECT about strengths of acids?        HClO2 is stronger…

A: --> HClO2 is stronger than HBrO2 This is a correct statement because in the chlorine is more…

Q: Rank the following acids from the least acidic to the most acidic fe HCI H H N H -о-н

A: The acidity of the compound is measured by its  value. The lower , the more acidic the compound is.…

Q: Which of the following pairs of species is not a conjugate acid-base pair? 0 02-, OH- HNO₂, NO₂ O…

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Q: Please use the values in the resources listed below instead of the textbook values. Which is the…

A: The strong acid is HCNO (cyanic acid).

Q: Calculate [OH-] in each aqueous solution at 250C, and classify each solution as acidic or basic. All…

A: At 25°C Kw = [H3O+] [OH-] = 1.008 * 10-14 Or simplicity Kw = [H3O+] [OH-] = 1* 10-14 For acidic…

Q: Calculate either [H,O*] or [OH¯] for each of the solutions. Solution A: [OH¯] = 2.31 × 10-" M;…

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Q: Identify the acids and bases in each of the following reactions. 4. H2O + HCl ⇌ H3O+ + Cl- 5. NH3 +…

A: Identify the acids and bases in each of the following reactions. 4. H2O + HCl ⇌ H3O+ + Cl-5. NH3 +…

Q: Which of the following is a basic solution? [H3O+] = 1.23 × 10-9 pH = 7 [H3O+] = [OH-]

A: The pH of the solution helps in the determination of the acidity or basicity of the solution. It…

Q: List the following bases in order of strength, strongest to weakest. Pb(OH)2, Kb=9.6x10-4 CH3NH2,…

A: The order of strength of base can be arranged considering the Kb value.

Q: Identify each solution as acidic, basic, or neutral. [H3O+ ] = 3 × 10−13 M [OH−] = 4 × 10−11 M…

A: The concentrations given are, [H3O+ ] = 3 × 10−13 M [OH−] = 4 × 10−11 M [H3O+] = 1 × 10−8 M   [OH−]…

Q: Order the following Brønsted acids from strongest to weakest: OH OH A OH OA>B> C>D OD>A>B>C OD > C>…

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Q: Which of the following solutions is most basic? Group of answer choices [OH-] = 1 X 10-4 [H+] = 1…

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Q: If a solution has an [OH-]=1.2x10-3M and an [H3O+]=8.2x10-12M. Is the solution acidic, basic or…

A: The nature of the solution can be determined by calculating the pH of the solution. If pH >7:…

Q: Pick the stronger base from each of the following pairs. NO2− or Br− Br− or CN CN−or F−

A: The conjugate base of a strong acid is weak and the conjugate base of a weak acid is strong.…

Q: Identify the acid, base, conjugate acid, and conjugate base in the following reactions:   HBr+…

A: Bronsted-Lowry theory of acids and bases :-  According this , Acid is a species which donates H+ ion…

Q: Which of the following is an acid/conjugate base pair?  (Which of the following an acid and its own…

A: Since the difference between and acid and conjugate base is only of a H+ ion Hence the pairs which…

Q: INCORRECT about strengths of acids?        HClO is stronger than HClO2                HClO2 is…

A: Stronger acid easily ionized in aqueous solution.  In oxyacids higher the oxidation number of…

Q: alculate [OH-] given [H3O+] in each aqueous solution and classify the solution as acidic or basic.…

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Q: Rank the solutions in order of decreasing [H3O+]. 0.10M HCl 0.10M HC2H3O2 0.10M HClO2 0.10M…

A: In this question, we will arrange these solutions in Decreasing Concentration of H3O+ ion  You can…

Q: Which of the following is the strongest acid? Group of answer choices HClO2 HCl HClO4 HClO HClO3

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Q: Calculate the pH and pOH of the given solutions at 25 -C from the concentration of H3O+ ions. Answer…

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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.