Solve the following Given that pH = 2.4, find (a) pOH (b) H3O+ (c) OH-

Q: (b) What are [H3O+], [OH -], and pH in a solution with a pOH of 4.19?

A: Since we know that pH + pOH = 14  => pH for the above case = 14 - pOH = 14 - 4.19 = 9.81

Q: Write a net ionic equation to show that hydrocyanic acid , HCN , behaves as an acid in water. + H20…

A: The answer to the following question is-

Q: What is the [H3O+]  of an acidic solution that has a ph of 11.25?

A: pH of any solution is given by  pH = -log[H3O+ ]  where [H3O+ ] = concentration of H3O+ ions in the…

Q: Calculate the pH of the following: - 0.10 M disodium hydrogen arsenate

A: To calculate pH , we would use dissociation equation of disodium hydrogen arsenate and it's Ka…

Q: Calculate the H3O+ concentration for a solution with a pOH of 5.68

A: We have pOH as 5.68, we have to calculate the hydrogen ion concentration.

Q: The pH of an acidic solution is 3.67. What is [H⁺]?

A:

Q: What is the pH of a solution with a pOH of 6.7?

A: Given: pOH of the solution = 6.7

Q: Calculate [OH-] for a solution with a pOH of 8.03. What is the[H3O+] of this solution? What is the…

A:

Q: HC2H3O2

A: Calculate the concentration of hydrogen ions released from the acetic acid. If the concentration of…

Q: A solution has a proton concentration of 0.00239 M, what is its pH?

A: Given : Concentration of proton i.e H+ ions, [H+ ] = 0.00239 M

Q: Calculate [OH¯] for a solution where [H,O*] = 0.00379 M. %3D [OH¯] = M

A: For an aqueous solution, we know that the production of the concentration of the hydrogen ions and…

Q: Determine the pH of a 0.65 M solution of HCO₂K. The value of Ka for HCOOH is 1.8 × 10⁻⁴.

A: HCOOK is a salt of a weak acid (HCOOH) and a strong base (KOH). The salt is present as HCOO- and K+…

Q: The pH of a 0.0058 M solution of HNO, is

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Calculate the pH of a 5.714 M solution of NaHS

A: Given Concentration of NaHS is 5.714 M To find pH of the given solution

Q: Calculate the pH of solutions with the following concentrations. [H3O+]= 1×10−8M

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The pH of a 0.0070 M solution of HNO₃ is

A:

Q: Calculate [OH¯] for a solution where [H,O*] = 0.00409 M.

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

Q: The pH Of An Unknown Solution Is 0.46. Calculate [H3O+] In Solution.

A:

Q: Calculate the pH of a solution that is .0400M in  a.) H3PO3  b.) H2S

A:

Q: Calculate the hydrogen-ion concentration and pH of 0.010 M HNO3.

A:

Q: Calculate [H3O+] and [OH-] for a solution with a pH of 8.55.

A: pH is calculated as the negative log of a solution’s hydrogen ion concentration:   pH =−log [H3O+]…

Q: What is the pH of a 0.00065 M solution of HI?

A: The pH of the solution has to be calculated,

Q: What is the pH of a 0.0898576 M solution of HClO3 (which is a strong acid)?

A: Strong acids undergo complete dissociation in aqueous solutions. Therefore, the concentration of H+…

Q: The pH of an acidic solution is 3.39. What is [OH⁻]?

A: Given that pH of acidic solution = 3.39

Q: (Q4) What is the pH of a solution if the pOH is equal to 3.15?

A: We have to determine the PH  of a solution given that POH = 3.15

Q: Question 6 of 27 Write the formula of the conjugate acid of HC0,.

A: Ans An acid donate the proton to form its conjugate base and a base will form its conjugate acid by…

Q: The pH of a 0.0040 M solution of HNO₃ is

A: The concentration of HNO3 is 0.0040M HNO3 is a monobasic acid. So, 1 mol HNO3 after dissociation…

Q: Calculate the pH of solution where [H] = 0.000023

A: pH measure the acidity of the solution.

Q: The pH of a 0.0042 M solution of HNO is

A:

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (a) 0.10 M…

A:

Q: Find the pH of a 0.22 M AlCl3 (aq) solution if Ka of Al3+ is 1.2 × 10–5

A:

Q: ph level of  NH4OH, HFO, HIO4, Be(OH)2

A: We have to level the pH of the following NH4OH, HFO, HIO4, Be(OH)2

Q: The pH of an acidic solution is 3.07. What is [OH⁻]?

A: Given data is as follows:  The pH of the solution = 3.07 OH- = ? As we Know that; pH+pOH=14

Q: What is the ph of a solutiong with a pOH of 4

A: pOH of the solution = 4  pH of the solution = ?

Q: The pH of a 0.0031 M solution of HNO, is 3

A:

Q: What is the Ph of a solution which has an (H3O+) = 0.043 M?

A:

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solution 0.035 M Na2S

A: 0.035 M Na2S hydrolyze in water to produce OH- ions. The ICE table is as follows:

Q: If your acid has a [H3O+] = 2.310-2 M, what is the pH of the solution?

A: The pH of the solution is given by: pH = -log[H3O+]                ......(1)

Q: The pH of a 0.0046 M solution of HNO, is

A: Ph is the negative logarithm of the concentration of Hydrogen ion for dilute solutions. Thus, pH is…

Q: If the [H3O+] concentration is 0.00047M, what is the pH?

A: Given, Concentration of H3O+ ion = [H3O+] = 0.00047 M pH of the solution = ? Note: pH: It can define…

Q: The pH of a 0.0047 M solution of HNO, is

A: As HNO3 is a strong acid, it completely ionises in the solution.

Q: Calculate the [OH-] and pH given that it is a mixture of 0.12 M in NaNO2 and 0.23 M in Ca(NO2)2

A: Given,  A mixture of 0.12 M in NaNO2 and 0.23 M in Ca(NO2)2

Q: Calculate the pH of a 0.00852 M  solution of HNO3.

A: When any particular acid is dissolved, H+ ion  gets shifted towards water molecule and as a result,…

Q: The pH of an acidic solution is 2.11. What is [H⁺]?

A: PH is defined as negative logarithm of concentration of [H+] ion. Given PH = 2.11

Q: The pH of a 0.0065 M solution of HNO3 is

A: pH of a solution is the measure of its acidity or basicity. The values on the pH scale lie between 0…

Q: Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3

A: pH is the measure of the acidity or basicity of the solutions. pH ranges from 0 to 14. If the pH…

Q: Be sure to answer all parts. What are [H2o), [OH]], and pOH in a solution with a pH of 9.70? [H,O*)…

A: pH = 9.70  [H3O+] = ?  [OH-] = ?  pOH = ?

Q: What is the formula for calculating the [OH−] from the [H3O+]?

A: ANSWER

Q: Calculate the [H3O+] of a solution of hydrochloric acid with pH = 1.00 .

A: The relation between pH and [H3O+] is: pH=-log[H3O+]                        ...... (1)

Q: Calculate the pH for 0.43 M NH4ClO4

A: pH can be calculated by following formula  pH = - log [H+]

Q: Calculate the pH of a 2.00 M NH,CN solution,

A: NH4CN is a salt made up of weak acid, HCN (Ka = 6.2×10-10) and a weak base NH4OH (Kb = 1.8×10-5).

Q: Lemon juice has a pH of about 2. What [H3O+] is this?

A: Given that the pH of lemon juice is 2. To calculate the concentration of H3O+ ions in the lemon…

Q: What is the pH of a 0.0025 molar acidic solution?

A: Concentration  given  [H+] =0.0025 M

Q: What is the pH of a 0.975 M solution of acetic acid, HC2H3O2?

A:

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.