Given the pOH is 12.22 a. what is [H+] b. what os [OH-] c. is it acidic or basic?

Q: the pH of the solution given that Kw=2.93×10^−15 at

A: The pH of the solution given that Kw =2.93×10−15 at this temperature

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: A solution has a [H3O+] of 1 × 10−3 M. What is the [OH−] of the solution?  A)11 M  B)14 M  C)1 ×…

A: Given : [H3O+] = 1 × 10−3 M.            =10−3 M.

Q: solution contains [H+] = 0.0034 M a) What is the pH of the solution?                            pH…

A: Given,  Hydrogen concentration = [H+] = 0.0034 M We need to calculate the pH of the solution using…

Q: A solution is made by dissolving 18.9 g of CH3NH3NO, in 500.0 mL of water. Does NO, have any acidic…

A:

Q: The pOH of an acidic solution is 10.77. What is [OH⁻]? what is the M?

A: Given that --> pOH = 10.77

Q: Determine the [H+] , [OH−] , and pOH of a solution with a pH of 1.03 at 25 °C.

A: Given, pH = 1.03

Q: Determine the [H*], [OH¯], and pH of a solution with a pOH of 7.10 at 25 °C.

A:

Q: Calculate [H3O+] for each solution pH = 1.52?

A: pH = -log [H3O+]

Q: Determine the [OH−], pH, and pOH of a solution with a [H+] of 7.3×10−8 M at 25 °C.

A: Given :- [H+] =7.3×10^−8 M  To calculate :-  [OH−], pH, and pOH

Q: Solution Y has a pH of 7.5 Solution X has a pH of 9.5   a.) what is the [H3O+] in each solution?…

A: We are given pH and we have to tell H+ and OH- ion concentration

Q: The pOH of a 0.25 M weak base is 5.45. Determine Kb

A: To determine kb if the pOH of a 0.25 M weak base is 5.45.

Q: neu as Question 8.07 Carbonic acid is a diprotic acid while formic acid is not. Why? (It may be…

A: Carbonic acid is a weak inorganic diprotic acid in the first step ionisation of carbonic acid gives…

Q: An aqueous solution at 25.0 °C contains |H30*| = 0.09613 M. What is the pOH of the solution?

A: Given that:  [H3O+] = 0.09613M  pH tells the information about free H3O+ ion in a solution. pH =…

Q: Calculate the [H*] in an HCIO2 solution that has a pH of 3.84. (Answer to 4 decimal places).

A: The (H+) in HClO2 is given below

Q: If a solution has a pOH of 12.2, what is its [H3O+]?

A:

Q: What is the pOH of a solution if the [OH-] = 3.5 x 1-^-2?

A: The given data is as follows: OH-1=3.5×10-2 M The pOH of the solution can be calculated as follows:…

Q: Determine the [H+], pH, and pOH of a solution with an [OH−] of 0.086 M at 25 °C.

A:

Q: If the {H3O^+ of a solution is greater then OH^-, which word beat describes the solution A) acidic…

A: Answer:- This question is answered by using the simple concept of nature of a solution which have…

Q: a cetain juice sample has [H+] = 1.0*10-4(exponet)   a. what is the ph for this sample   b. what is…

A: Equations for pH, pOH calculation:

Q: An aqueous solution has [H+] = 1.0 x 10-4 M. What is the [OH−] for this solution?

A: Given, [H+] = 1 × 10-4 M We have to find [OH-] .

Q: Given the pOH for a solution, calculate the other values:   pOH = 5.33   a)   pH =  b)   [H3O+] =…

A: POH=5.33PH=-log H3+O                  POH=-log OH-10-PH=H3O+                     10-POH=OH-a PH=?…

Q: (a) In a sample of lemon juice, [H+] = 3.8 x 10-4 M. What isthe pH?(b) A commonly available…

A: (a) Given:

Q: Determine the (H*]. [OH-], and pH of a solution with a pOH of 7.25 at 25 °C. [H*) = 1.8 x10-7 =…

A: Given that  POH= 7.25  We have to determine [H+] , [OH-]  and PH of a solution  Complete solution is…

Q: 3. Calculate the value of [H3O*] from the given [OH ]in each solution and label the solution acidic…

A: pH  of any solution is expressed as the negative logarithm of hydrogen ion or hydronium ion…

Q: 1.) What is the pOH of a solution with [OH-] of 8.4 x 10-12 M? Is this solution acidic or basic?

A: POH is defined as negative logarithm of the Hydroxide ion Concentration.  A basic solution has poH…

Q: Determine the [OH−] of a strong basic solution with a pH of 5.40 @ 25 degrees C.

A: Given, Temperature , T =25°C pH = 5.40

Q: if the pOH is 3.09 what is the pH?

A: If pH is less than 7 then solution is acidic in nature.If pH is greater than 7 then solution is…

Q: Calculate the pOH in an Al(OH)3 solution that is slightly basic with a pH of 9.50. pOH = = i M

A: Here we have to determine POH  of Al(OH)3 solution which is slightly basic with pH =9.50 .

Q: Determine the (OH], pH, and pOH of a solution with a| H* of 0.0075 M at 25 °C.

A: Given :- [H+] at 25°C = 0.0075 M  To calculate :- [OH-], pH and pOH of solution

Q: Determine the [H+][H+] , pH, and pOH of a solution with an [OH−] of  0.099 M at 25 °C.

A: The concentration of hydrogen ion is calculated as follows:

Q: Determine the [H+] , pH, and pOH of a solution with an [OH−] of 2.0×10−10 M at 25 °C.

A: The pOH of the solution can be calculated as follows-

Q: What are [H*], [OH-] and pH in a solution with a pOH of 12.11 15.

A:

Q: a) What is the pH of 7.52X10⁻⁴ M CsOH? Is the solutionneutral, acidic, or basic? (b) What is the…

A: (a)

Q: The pOH of a solution of NAOH is 11.30. What is the [H ] for this solution?

A: The negative logarithm of the concentration of the hydroxide ions of a solution is known as pOH of…

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 3.47? (b) What are [H₃O⁺],…

A: pH is equal to the negative logarithm of hydronium while pOH is equal to the negative logarithm of…

Q: If HNO3 is added to water, how does [OH-] change? How does pH change? (b) Use the pH…

A: a. HNO3 releases  H+ in the water Therefore, acidity of water increases pH of water decreases HNO3 +…

Q: (a) What is the pH of 0.0333 M HNO₃? Is the solution neu-tral, acidic, or basic? (b) What is the pOH…

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

Q: a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 8.97? (b) What are [H₃O⁺], [OH⁻],…

A: The concentration of the hydrogen ions in the solution is determined in the pH scale.…

Q: (a) What are [H₃O⁺], [OH⁻], and pOH in a solution with a pH of 9.85? (b) What are [H₃O⁺], [OH⁻],…

A: a) pH of a solution is equal to negative logarithm of hydronium ion concentration present in it. So;…

Q: Determine the [H+] , [OH−] , and pH of a solution with a pOH of 8.95 at 25 °C.

A:

Q: An aqueous solution is found to have an OH- concentration ( [OH-] ) of 1.0 x 10-8 M, a) What is the…

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

Q: Which of the following does NOT describe an acidic solution????? a. the pH is less than 7 b. the…

A: We need to find out the, which is not an acidic solution out of these 4:

Q: 300.0 mL of a 0.385 M solution of NaI is diluted to 700.0 mL. What is the new concentration of the…

A: Given,  300.0 mL of a 0.385 M solution of NaI is diluted to 700.0 mL. The new concentration of the…

Q: Which of the following statements is/are true for a 0.10 M solution of a weak acid HA? (a) The pH is…

A: Molarity of HA = 0.10 M

Q: solution has a pH = 11.4.   Calculate [H+]                              Calculate [OH-]…

A:

Q: A truck transported 400 liters of HCl approximately 7.4M a) Is it a strong or weak acid? b) What is…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: Calculate [OH−] for the following solution; [H3O+] = 8.87×10−9 M Is the solution basic at 25°C?

A: pH is negative logarithm of hydronium ion. Given,  [H3O+] = 8.87×10−9 M

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 5.7×10−13 M at 25 °C.

A: Given: [H+] = 5.7*10-13 M

Q: is a weak acid? Of the following acids, a. HBr b. HCI C. HNO3 O d. H3PO4 e. HCIO4 е.

A: The question is based on the concept of acidity. we have to identify which of the given acid is 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.