What is the pH of a solution with a hydroxide ion (OH-) concentration of 10-10M?

Q: Calculate [H3O+] given [OH-] in each aqueous solution and classify each solution as acidic or…

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Q: What is the pH of 1.5 x 10-4M solution of H2SO4?

A: pH of a solution determines the concentration of hydrogen ion present in the solution.

Q: Which solution has the highest pH? O 0.065 M HIO (Ka-2.3x10-11) O 3.5x10-4M HBrO (Ka-2.5x10-9) O…

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Q: The ph of a solution for which [OH-]=1.0X10^-9

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Q: What is the [H3O+] for a solution with a [OH-] of 7.79 X 10-6 M? Is the solution acidic, basic or…

A: The solution which have: pH > 7 basic pH = 7 neutral pH < 7 acidic

Q: A solution that has a hydrogen ion concentration equal to 9.61 x 10-7 has a pH =

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Q: What is the pH of a solution that is 2.7×10-9 M in NaOH

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Q: What is the pH of a solution when the [H+] = 6.5 x 10-9

A: pH is defined as the negative logarithm of the concentration of hydroxide ion. where [H+] is the…

Q: What is the pH of a solution when the [OH-] = 1 x 10-3

A: Given that, [OH-] = 1×10-3  Now, we know that, pOH = -log[OH-]     or, pOH = -log[1×10-3]     or,…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 5.4×10-2 M. The hydroxide ion…

A: Use relations  pH= -log[H+] Ph+poh=14 Poh= -log[OH-] PH is power of Hydrogen.

Q: What is the pH of a 2.8 x 10-4 M solution of NaOH? What is the hydronium ion concentration of the…

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Q: Determine the [OH-] of a solution when the [H+] = 4.0 x 10-8

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Q: What is the pH of a 6.2 x 10-5 M NaOH solution?

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Q: determine the [H+], pH, and pOH of a solution with an [OH-] of 9.2 x 10^-10 M at 25 degrees Celsius.

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Q: The [h3O+] of tomato juice is 2.2 x 10^-4 M. What is the pH of the solution

A: Given [H3O+] = 2.2 x 10-4 M

Q: What is a basic solution? H+OH- H+ = OH- H+>7 OH-<7

A: H+ Hydronium ion OH- : Hydroxide ion

Q: The pH of 0.010 M trimethylamine is 10.74 at 25 degrees celisus.  What is the hydroxide ion [-OH]…

A: pH is defined as the negative logarithm to the base 10 of hydrogen ion concentration. pH = -log10[…

Q: A solution has [OH-] = 1×10-10. What is the concentration of H3O+ ion?

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Q: 2. What is the pOH of a solution in which the hydroxide ion concentration is 3.2x10-3M? 3. What is…

A: POH = -log[OH-] [H]+[OH-] = 10-14 M2

Q: A nitric acid solution has a pH of 1.75 what is the [H+] and [OH-].

A: Given, pH of nitric acid solution =1.75we are asked to calculate the [H+] and [OH-]

Q: Adding an acid to water increase the H3O+ ion concentration and decreases the OH- ion concentration.…

A: The statement is true or false has to mentioned

Q: If the [ H+  ] concentration of a water sample is 1 x 10-4 M, the [ OH- ] concentration is:________

A: GIven: The concentration of hydrogen ion [H+]=1 x 10-4 M The concentration of hydroxide ion i.e.  […

Q: concentration of 7.23 x 10^-7 at 100 degrees C. What is the hydrogen ion concentration? Is the…

A: In water,  [H+] = [OH-] [OH-] = 7.23×10-7 M [H+] =  7.23 ×10-7 M Kw =[H+][OH-] =  5.23 × 10-13 pH =…

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

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Q: the [H^+] of a solution is 2.5 x 10^-4M, what is the concentration of the hydroxide ion ? __ Is this…

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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: At 25 °C, a solution has a hydronium ion concentration of 8.80×10-6 M. What is the pH, pOH, and…

A: • The values provided in the question are:-    i) Hydronium ion concentration of a solution, [H3O+]…

Q: pH of a solution having OH-  concentration 10-5

A: We know that, pOH = -log[OH-]                { [OH-] is the molar concentration of OH- ion} Again,…

Q: hat is the concentration of hydronium ions in a solution with a pH of 5?

A: Given- pH of the solution =5  We know formula,  pH = - log [H+]

Q: Calculate [OH-] fore each solution, express each answer to two significant figures: pH = 1.92 pH =…

A: Calculate [OH-] fore each solution, express each answer to two significant figures:

Q: What is the pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M

A: The pH of a solution with a hydroxyl ion (OH−) concentration of 10−12 M is to be calculated

Q: pH

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

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Q: What is the pH of a solution when the [OH^-] = 1 x 10^-3

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Q: The pOH of an aqueous solution at 25°C was found to be 13.00. The pH of this solution is The…

A: The solution is as follows :

Q: Calculate the [OH-] in each of the following solutions, and indicate whether the solution is acidic…

A: The relationships which we will be needing are 1) pH = -log[H+ ] where [H+ ] = concentration of H+…

Q: What is the pH of a solution that has a OH- concentration equal to 1.3x10-10 M?

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Q: Calculate the hydronium ion concentration, [H3O+], for a solution with a pH of 7.59.

A: Given: pH = 7.59

Q: Calculate the hydronium ion concentration, [H3O+], for a solution with a pH of 6.73.…

A: Given pH of solution is 6.73 We have to find out hydronium ion concentration for this solution.

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 &gt;7:…

Q: the pH of a solution with an [OH-] =  8.95x10-11 M

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Q: Determine the pH and [OH-]  of a solution if its [H+] = 7.5 x 10-3M.

A: The pH can be calculated as, pH=-log[H+]

Q: What is the pH of a solution when the [H^+] = 6.5 x 10^-9

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Q: What is the [OH-] , [H+] and pH of a solution containing 0.00086M KOH

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the…

Q: Aq of NH4+  Aq of HF  NH4+=6.25M HF=1.04x10^-6M NH3=5.00x10^-4M F=2.50x10^-5M H3O+=5.00x10^-4M…

A: Both solution are buffer so we will Henderson-hasselbach equation .

Q: pH of a 10-3 M HCI solution is: O - 11 O 1 O -3 O 3

A: Given, Concentration of HCl= 10^-3 M

Q: What is the pH and pOH of a solution with a [OH-] of 7.79 X 10-5 M? Is the solution acidic, basic or…

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Q: What is the pH of a 0.25 M solution of a strong acid?

A: The Formula of pH of solution is        pH = -log10[H+]

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.