Calculate the [OH-] of a solution that contains 1.0 × 10-5 M H3O+ at 25°C.  Note:  Kw = [H3O+][OH-] = 10-14 M2

Q: Determine the (OH-) of a solution that is 0.115M in CO3^2- kb=1.8x10^-4

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Q: Calculate the pH of a solution that has [OH-1] equal to 2.79 x 10-6 M.  Enter your answer with 2…

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Q: NaC14H10Cl2NO2 acidic or basic?

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: Calculate either [H,O] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-] = 2.59 x 107…

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Q: 07-13: The diprotic acid Hal. has Kar-1.4 x 10 and Kaz -1.2 x 10-10 97-Calculate the molarity of H"…

A: The acid H2L is a diprotic acid in which there are two protons that can be released. Frist…

Q: aqueous solutions will have a pH of 2.00 at 25 °C? (Kw = 1.01 × 10–14) 0.020 M HNO3

A: As we know,  Acidic solution has pH less than 7. Basic solution has pH greater than 7 . pH =…

Q: What is the pH of a bleach solution that has a OH = 2.3 x 10-3 M? %3D pH %3D Is bleach acidic,…

A: pH is a method to determine the concentration of hydrogen ions present in a solution. It helps in…

Q: What is the pOH of a solution that contains 6.1 x 10-5 M HCl at 25°C?

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Q: Calculate [H3O+] in each aqueous solution at 250C, and classify each solution as acidic or basic.…

A: [H3O+] in each aqueous solution  [OH-] = 5.1 x 10-4M [OH-] = 1.7 x 10-12M [OH-] = 2.8 x 10-2M…

Q: Calculate the [H +], [OH -], pH , pOH of 005 M NH3     Kb=   1.8 x 10 -5

A: pH is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being neutral. pHs…

Q: pOH of a 10-1 M NAOH solution is: 0 1 O13 -1 -13

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Q: {OH-} =1.5 x 10^-4 M pH=

A: Given: [OH-]=1.5 x 10-4 pH=?   First, calculate pOH. pOH=-log [OH-]

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: The dissociation constant of ammonia is 1.8 x 10 -5. At 0.112 M solution concentration, find the…

A: Given,  The molarity of ammonia solution = 0.112 M.  The dissociation constant = 1.8 × 10-5

Q: Calculate [H, O+] for a 3.43 x 10-3 M HBr solution. [H,O*] = Calculate [H, o*] for a 1.50 x 10-2 M…

A: Strong acid vs Weak acid: Strong acid dissociated completely into its constituents ions while weak…

Q: Rank the following solutions according to their acidity:   Rank Solution 1 [H3O+] =10^-8 M…

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Q: Which solution below has the highest concentration of hydroxide ions?     pH = 8.3     pH = 11…

A: We will use relation pH and pOH to get answer

Q: Determine the [OH. pH, and pOH of a solution with a (H*] of 1.6 x 10-6 M at 25 °C. !3! = [.HO] pH =…

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Q: Calculate the volume of 0.650-M NaOH solution needed to completely neutralize 28.1 mL of a 0.760-M…

A: The neutralisation reaction taking place will be  2 NaOH + H2SO4 --------> Na2SO4 + 2 H2O hence…

Q: alculate [OH -] and pH for each of the following solutions. (a) 0.0027 M NaOH [OH-] =  M pH =…

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Q: Complete the following statements about the below solutions at 25 °C? 1. The pOH of 9.95 x 105 M KOH…

A: at 25°C ;  pH + pOH = 14.0  pOH = -log[OH-]

Q: An aqueous solution at 25 °C has a H,0" concentration of 4.2 × 10 M. Calculate the OH concentration.…

A: Solution : We should know that  [H3O+][OH-]=Kw=1×10-14 Given, [H3O+]=4.2×10-6

Q: What was the original 1. concentration (M) of an aqueous acetic acid (CH3COOH) solution whose pH is…

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Q: What is the OH- concentration for a solution at 25 C that has a pH of 1.86? At this temperature Kw…

A: We have,  At 25oC, Kw=1.0x10-14     -----(1) where Kw is ionic product of water Also, Kw=[H+][OH-]…

Q: Calculate [OH-] of NaClO, 0.110M; KaHClO = 3.0 x 10-8.

A: Given: Concentration of NaClO is 0.110 M Ka (HClO) is 3.0×10-8 To determine: [OH-]

Q: Calculate [A-] and [A2-]of a 0.050 M solution of diprotic acid, H2A, with K1 = 8.5 x 10-5 and K2 =…

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Q: Which of the following conditions indicate an acidic solution at 25°C?     ( OH-) = 3.5 x 10-5 M…

A: pH = -log[H+]  pOH = -log[OH- ]   at 25°C  pH + pOH = 14.0

Q: Which solution would turn blue litmus red A solution of pH 9. O A solution of KNO3 A 0.1 M solution…

A: ANSWER IS

Q: In the scary chemistry lab, you come across a bottle that has "0.15M HNO3" written on it (this means…

A: Given: Initial concentration (C1) of HNO3 = 0.15 M Initial volume (V1) of HNO3 solution = 250 mL…

Q: Calculate the [H3O+], [OH-], pH and pOH of a 0.12 M HNO2

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Q: Calculate the concentration of OH- ions in a H2SO4 solution of 1.42 M at 100 oC

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Q: A solution has [OH]] = 1×10-13. What is the concentration of H3O* ion? [H;O*] = mol/L

A: Answer of this question:- The multiplication of concentration of [H3O+] and [OH-] always equal to…

Q: The pOH of a solution of NaOH is 11.30. What is the [H+] for this solution? O 2.0 x 10-3 O 2.5 x…

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Q: 12. Which one of the following is a strong acid? BNH3 F H2SO4 HF None of the others Ca(OH)2 CH3COOH

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Q: A solution has [H+] = 4.0 x 10-3 M. The [OH"] in this solution is %3D 4.0 x 1011 1.0 x 10 14M 4.0 x…

A: Given data,[H+]=4.0×10-3M

Q: Calculate the [H+1]for this solution.

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Q: what is the pH of 10-12M H3O+ solution

A: The pH of a solution is calculated by the formula: pH=-logH3O+......(1)

Q: Calculate the pH of a solution in which [ OH^- ] = 2.50 x 10^-14

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Q: Given the following value of H3O calculate the corresponding value of [OH¯] for each solution. a.…

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Q: An aqueous solution has a pH = 4.23; what is the [ H3O+ ]? 5.9 x 10-5 M 17,000 M 1.7 M 5.9 x…

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Q: Calculate the [H +], [OH -], pH , pOH of 0.005 M NH3 Kb= 1.8 x 10 -5

A: Ammonia is a weak base hence it dissociated less

Q: Indicate whether each of the following solutions is an acidic, a basic, or a neutral solution. Drag…

A: We need to check with the help of [H3O+] and [OH-], if the solution is acidic or basic.

Q: The pOH of a solution containing 4.93 x 10-3M NaOH is 11.69 and the [H+] is 2.03 x 10-12M True or…

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Q: What is the pH of a solution with [OH-]=2.2 x 10^-7M? Calculate the pH of a 0.0500M solution of…

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Q: pOH of a 10-2 M N2OH solution is: O -2 O -12 O 12 O 2

A: We have to find out the pOH of the 10^-2 M NaOH solution.

Q: To add an O atom in basic solution, add 2 OH to the side that needs the O atom, and also add an H20…

A: Basic solution is an aqueous solution having pH greater than 7. Basic salts contain the conjugate…

Q: Calculate the [H*] of 5.8 x 10-5 M magnesium hydroxide solution. O [H*] = 3.4X10-11 O [H*] =…

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Q: pH of a 0.35 M aqueous solution of sodium formate

A: Given that , Ka for formic acid = 1.8×10-4 pH of 0.35 M aqueous solution of sodium formate (NaHCO2)…

Q: The acid dissociation K, of benzoic acid (C,H5CO,H) is 6.3 × 10 °. Calculate the pH of a 1.0M…

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Q: In a certain acidic solution at 25 °C, [H+] is 100 times greaterthan [OH-]. What is the value for…

A: pH and pOH  are related as follows:

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.