If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?

Q: What is the original molarity of a solution of ammonia whose pH is 10.48?

A: The original molarity of solution of ammonia whose pH is the 10.48 is calculated as follows

Q: Which of the following 1.0 M solutions would have the highest pH? Weak Acid Ka HCN 4.9 x 10-10 HNO2…

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Q: Calculate the pH of a solution of 100.00 mL of 0.1092 M Ba(OH) 2 and also calculate the pH of a…

A: Ba(OH)2 is a strong base. Hence it will dissociate completely in solution as  Ba(OH)2 ------->…

Q: What is the pH of a solution that has [H3O*]= 4.5x10-³ M?

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Q: The hydroxide ion concentration of a solution is 6.7 X 10-8. What is the pH level of the solution?…

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Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in base…

A: pH is the measure of concentration of H+ ions. Here pH can be calculated with the help of kB values,…

Q: If H+ is equal to 6.9x10^-5, what are the values of pH, POH, and OH-?

A: Given - [H+ ] =6.9*10-5 We have to determine pH, pOH and concentration of OH-.

Q: 8. What is the pH of a cup of coffee that has a [OH-] of 1.200 x 10-10?

A: Detail mathematical calculation is shown below

Q: Which of these solutions has the lowest pH? Rank these solutions: 0.10 M HIO, 0.10 M H2SO4, 0.10 M…

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Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A: Given Hydrogen ion concentration is [H+]=4.5×10-10M As we know, pH=-log[H+] pH=-log[4.5×10-10]use…

Q: What is the pH of a solution if the concentration of H 3 O^ + is 5.6 * 10 ^ - 5 M?

A: Given data contains, Concentration of H3O+ is 5.6×10-5.

Q: What is the pH in a solution consisting of Ba(OH)2 6.17x10-8M.

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Q: 6.84 x 10-2 M OH Calculate the molarity of H*. Enter the value in the first blank (with proper sig…

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Q: 10. What is the pH of a 0.4M ammonia solution? The ionization constant of ammonia is 1.8 X 10.

A: Given: Concentration of ammonia solution = 0.4 M Kb of ammonia = 1.8×10-5

Q: The Ka of hypobromous acid, HOBr, is 2.6x10-9. Calculate the pH of a solution which is composed of…

A: Given :-  [HOBr] = 0.40 M  [NaOBr] = 0.40 M Ka for HOBr = 2.6 × 10-9  To calculate :-  pH of…

Q: What is the pH of a solution that has [OH–] = 6.92x10-11 M.

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Q: A solution that has a hydrogen ion concentration equal to 3.52 x 10-3 has a pH = _____________?

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Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

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Q: If a 5.6 L solution has a pH of 3.6, what will the pH be if the volume is increased to 7.2 L?

A: Given:PH of solution-1 = 3.6V1 = 5.6 L.V2 = 7.2 L

Q: Calculate the pH of each of the following solutions of a strong acid in water. (a) 0.22 М HCI (b)…

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Q: Which would have a higher pH, a solution whose pOH is 5.00 or a solution whose hydrogen ion…

A: pH of solution is calculated based on the hydrogen ion concentration. pH = -log[H+] pH = 14 - pOH

Q: If the pH of a solution is 6.7, the [H*]= 2 x 107 5 x 10 6 8 x 107 5 x 107 O O O O

A: Acids are the chemical compounds which donate proton, H+ in the solution while base is a chemical…

Q: Calculate the pH of a 0.36M methylamine (weak base) (CH3NH2) solution, if Kb = 4.4x10-4

A: In aqueous solution, methylamine undergoes the acid base reaction: CH3NH2 aq + H2Ol  → CH3 NH3+ +…

Q: If the K, of a weak base is 2.7 x 10, what is the pH of a 0.30 M solution of this base?

A: Solution Ph may be a live of however acidic or basic is AN solution.It is measured in terms of…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

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Q: What is the pH of a solution with a pOH of 2.4? Is the solution acidic or basic?

A: We have pOH as 2.4 , we have to calculate pH as well as nature of solution.

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

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Q: What is the pH of an aqueous solution with a hydroxide ion concentration of 4.20 x 10-4 M?

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Q: The pH of a 0.01 M HNO2(aq), Ka=4.0x10^-4  ,solution is in which of the following ranges?  a.)…

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Q: What is the pH of the following solutions? [H+] = 1.5 × 10-3 M ▪ [H+] = 8.7 × 10-12 M %3D [OH-] =…

A: The solutions are given below -

Q: what is the pH of a 7.5x10^-2 M solution of NaOH?

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Q: What is pH of a solutionwith a H+ concentration of 10^-4M

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Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

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Q: If the Ka of a monoprotic weak acid is 6.6x10-6, what is the pH of a 0.32 M solution of this acid?

A: Ka = 6.6 x 10-6 c = 0.32 M

Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

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Q: For questions 7-9 state which species (chemical) is the acid, which is the base, and which are the…

A: Bronsted Lowry acid-base theory. Acid is the chemical species that donates protons in the solution…

Q: Calculate the pH of each of the following solutions at 25°C. a. 0.125 M HONH2 (K = 1.1 x 10-8) pH =…

A: Since you have posted multiple sub-parts questions, as per our company guidelines we are supposed to…

Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: What is the pH of a 5.3 x 10^-6 M HBr solution?

A:

Q: The Kb for aniline (C6H5NH2) is 4.3 x 10-10. What is the pH of a 0.15 M solution of aniline?

A: From the ICE table, we have

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

A:

Q: What is the pH of a solution if the concentration of H+ is 5.3x 10^-9

A: pH of solution = ? H+ = 5.3 × 10-9  We know that, pH = - log [H+]

Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: What is the pH of a 8.7x10^-3 M HI solution

A: given : [HI] = 8.7 × 10-3 M  to calculate :- pH of solution

Q: Step by step please clearly

A: Given reaction,

Q: If the hydronium ion concentration is 2.5 x 10^-4, what is the pH ? __ Is this am acid or base ?

A: The concentration of hydronium ion (H3O+] = 2.5 × 10-4  pH = ?  This is an acid or base ?

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.