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

Q: The pH of a solution which contains 0.10 M HNO3 is _______________the pH of a solution which…

A: pH is the negative logarithm of concentration of proton.

Q: Classify the following solutions as either acidic, basic or neutral. 0.0354 M H3o+ Choose... +…

A: Acidic pH < 7  Basic  pH > 7 Neutral pH = 7

Q: What is the pH of a solution that has [OH–] =6.9*10^-12

A: Given : [OH- ] = 6.9 x 10-12 M

Q: e pH of a solution  with [H+]  = 1.5x 10-1

A: The pH of the solution is a measure that how much the given solution is acidic and basic in nature.…

Q: Calculate the ph of the [OH-] = 2x10^-3 M.

A: We have to calculate the pH of given solution.

Q: What is the pH of a solution where [H3O+]  = 2.3*10-9 M?

A: [H3O+ ] = 2.3 × 10-9 M  By the definition of pH, we know that ; pH = - log [H3O+]  pH = - log (2.3 ×…

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…

A:

Q: What is the pH of a solution with hydronium ion concentration equal to 0.0046 M.

A: Given :- concentration of hydronium ion in solution = 0.0046 M  To be calculated :- pH of solution

Q: Calculate the pH corresponding to each of the hydroxide ion concentrations given below, and indicate…

A: pH of any solution in terms of hydroxide ion concentration is given by  pH = 14 + log[OH- ]  where…

Q: Determine the [H*],[OH-], and pOH of a solution with a pH of 13.34 at 25 °C. H*] 4.571 x10-14 OH] =…

A:

Q: Calculate the pH corresponding to each of the hydrogen ion concentration given below, and indicate…

A: pH of any solution is given by  pH = -log[H+ ] where [H+ ] = concentration of H+ ions in the…

Q: In a NaOH solution [OH-] is 2.9 x 10-4 M. Calculate the pH of the solution.

A: Given that,  A solution of NaOH has Concentration of OH- ion [OH-] = 2.9×10-4 M Since, pOH  =…

Q: What is the pH of 0.180M NH4Cl. Ka NH4+: 5.80x10^-10

A:

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: Calculate the pH of the following: [OH-] = 1 x 10-3 M

A: 1) Given, [OH-] = 1 × 10-3 M pH of the solution = ? The formula used here is, pOH = -log[OH-]  pH +…

Q: The hydronium ion concentration in a solution is 3.0x10^-3M what is the PH of the solution at 25…

A: We have, hydronium ion (H3O+) which is same as H+ ion. We can determine pH by using the formula: pH…

Q: hydrogen ion concentration

A:

Q: Determine the [OH-] in a solution with a pH of 4.963.  Your answer should contain 3 significant…

A: Given data: The pH of a solution=4.963. To calculate: The concentration of hydroxide ion is [OH-].

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

A:

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

A: pH is related to pOH by the following expression: pH + pOH = 14  ⋯⋯⋯⋯(1) Also pOH is related to the…

Q: is the pH of a solution when the concentration of hydronium and hydroxide ions are equal. O greater…

A: we are to discuss what is the pH when concentration of hydronium ion and hydroxide ion are same.

Q: The pH of a solution can be calculated from which of the following expressions? 1. pH = –log [OH-]…

A: pH of any solution gives an idea about the concentration of H+ and OH- ion in the solution.

Q: Calculate the pH of each of the following solutions of strong acids A) 1.34e-3 M  HNO3 B) 0.000187…

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

Q: Determine the pH of a solution with [H3O+] = 8.53 × 10-3 M.

A: pH is the measure of acidity or basicity of a solution. Mathematically, it is the negative logarithm…

Q: Calculate the pH of pure water if [H3O+] = 1.0 x 10-7.

A: PH is the power of Hydrogen. PH is used to determine nature of solution like as acidic,basic or…

Q: If the  pH of a solution is 2.000 at 25oC, [ OH-]is .(A) 12.000M (B) 1.00x10-12M (C) 2.000M (D)…

A: The concentration of hydrogen ions in a solution may be determined from its pH as:

Q: If the pH of a solution is 4.52, what is the [H3O+] in the solution? Select one: a. 3.3 x 10-10 M…

A: 1) pH = - log[H+] [H+] = 10- pH  2) pOH = - log [OH-] 3) pH + pOH = 14

Q: what is the ph of a solution that has [OH-]= 6.9x10^-12

A: Given :- concentration of OH- ions = 6.9 × 10-12 M  To calculate :- pH of the solution

Q: Find the pH of the 4M NaH2AsO4 solution (Kai-5.8x10-³, Kaz=1.1x107)

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the given…

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: 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: 3. If the pH of a solution is measured to be 5.45, is the solution acidic, basic, or neutral? 4.…

A:

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

A:

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

A:

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

A:

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

A: Given: pH = 7.59

Q: What is the pH when the hydrogen ion concentration is 1 x 10^-12 M? O a) -2 O b) -12 O c) 12 d) 2

A: Given : Hydrogen ion concentration i.e [H+ ] = 1 X 10-12 M

Q: Indicate whether the following solutions are acidic, basic, or neutral. 5x106 м нзо* 5 x 10-9 M OH…

A: In order to know whether any particular solution is acidic, neutral or neutral, we need to calculate…

Q: The pH of a solution with [H3O+] = 1x10¯4 M is

A: pH = -log [H3O+]

Q: Determine the pH of a solution with [OH-] = 5.88 × 10-3 M.  Your answer should contain 3 decimal…

A: The relationship between the pH and [OH-] is given by  pH = 14 + log[OH-]  where [OH-] =…

Q: What is the [OH-] concentration of a solution with a pH of 3?

A:

Q: A solution of hydroiodic acid has a concentration of 2.00x10-2 M. What is the pH of this solution?…

A: Given: Concentration of hydroiodic acid i.e. HI = 2.00 × 10-2 M.

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

A:

Q: pH of a 10 M KOH solution is: O-10 O 10 O-4 4

A: Given , [OH-] = 10-4 M  PH = ? PH is defined as negative logarithm of concentration of H+ ions.

Q: solution has a [H+] of 2.5 ×10-3 M.  What is the pH of this solution?

A:

Q: An aqueous solution has hydronium concentration [H3O+] = 6.3 x 10-3 mol L-1. What is the pH of the…

A:

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: What is the pH of a solution with an [H+] = 1 x10-6 a) 6 b) -6      c)   8      d) -8

A:

Q: Calculate the pH of the following: [H+] = 1 x 10-7 M

A: Given the concentration of H+ ions           [H+] = 1 x 10-7 M  We have to calculate pH of this…

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.