In an aqueous solution at 25°C, if [H,0*] = 3.5 x 10-4 M, then [OH-] is:

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: If [H3O+] = 2.7x10^-5m  Find [OH-], pH

A: Given : [H3O+] = 2.7 * 10-5 M we have to find pH and [OH-].

Q: Calculate [OH-] in a solution with [H3O+] = 1.5 * 10-4 M.

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

Q: What is the molar concentration of H3O+ in an aqueous solution with a concentration of OH-  that…

A: We have to calculate the molar concentration of H3O+ in an aqueous solution with a concentration of…

Q: Write formula for the conjugate acid of the foll F O H2F O HF O H+ O 2HF

A: Conjugate acid of F-  ?

Q: Find the OH- and pH of 0.25g of Ba(OH)2 dissolved in enough water to make 0.655 L  solution?

A: Given, the amount of Ba(OH)2 =0.25 gramvolume of solution =0.655 Lmolar mass of Ba(OH)2 =171.34…

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 6.1*10^-12 M

A: The pH of solution indicates the number of H+ ions in the solution. The pH scale ranges from 0 to 14…

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]=3.3*10^-3 M

A: pH of the solution is given by,                               By using given concentration to get…

Q: What is the pH of a 0.087 M solution of H2SO4? Round to two decimal places.

A: Given, Concentration of Sulfuric acid = 0.087M

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: From the list of the given compounds, choose the strong acid in an aqueous solution. H, SO, CH;CO,H…

A: To solve this problem we have to know about the strong and weak acids .

Q: Determine the [H+], [OH-], and pH of a solution with a pOH of 12.67 at 25 °C. [H*] : [OH] = pH =

A:

Q: In an aqueous solution the [H3O+] is 2.0 x 10 -6 M. What is the [OH-]?

A:

Q: Find the [OH-] in an acidic solution where [H+] = (6.0x10^-5)

A: An acid is a molecules which can donates protons or they are capable of donating hydrogens. Bases…

Q: Example2: Calculate [H;0"], [OH] concentration and pH and pOH of 0.2 M aqueous solution of NaOH.

A:

Q: If in a solution [H,01-10 [OH ], what is the pH of the solution?

A: Given that :  [H3O+] = 10 [OH-]  We need to determine pH of this solution.

Q: For a given aqueous solution if [H+]=1.0x10^-9 M, what is [OH-]

A: Concentration of [H+]=1.0x10^-9 M in aq.solution. Concentration of [OH-] = ? Formula: Ionic…

Q: Calculate the pH of a 0.063-M Al (NO3), solution. The K, value for Al (H2O),* is 1.4 x 10-º. pH =|

A: Given that: concentration of Al(NO3)3 = 0.063 M Ka = 1.4 ×10-5  To find: The pH?

Q: For a given aqueous solution, if [OH-]=1.0x10^-12 M what is [H+]

A: For the aqueous solution, the concentration of the hydrogen ion and hydroxide ion is constant at a…

Q: Determine the [OH-], pH, and pOH of a solution that is 0.125 M in CO3 2-.

A: Given information: Concentration of carbonate ion = 0.125 M

Q: Which of the following is the most basic solution (highest [OH ])? O pOH = 1.0 O pH = 12 O [OH¯] =…

A:

Q: Calculate [H3O+][H3O+] given [OH−][OH−] in each aqueous solution. [OH−] = 4.2×10−12 M [OH−] =…

A:

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

A: Given, a solution with [OH-] =8.4×10-12 Mwe are asked to calculate the value of pOH and predict the…

Q: For a given aqueous solution if [H+]=7.92x10-5M, what is [OH-]

A:

Q: for a given aqueous solution if [OH-]=7.11x10^-10 M what is [H+]

A: For the aqueous solution, the product concentration of the hydrogen ion and hydroxide ion is…

Q: If H+ is equal to 6.9×10^-5, what are the values of pH, pOH, and OH-?

A: Given: [H+]=6.9×10-5 To find: pH, pOH and [OH-]

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: The OH- concentration in an aqueous solution at 25 celcius  is 7.1 x 10^-5. what is [H+]?

A: Given,  Concentration of OH-ion = [OH-] = 7.1 x 10-5 M  What is [H+] = ?

Q: Calculate [OH-] given [H3O+] in the aqueous solution. [H3O+]= 7.1 * 10^-9 M

A: Given information: Concentration of H3O+ = 7.1×10-9 M

Q: At 25 degrees C, a solution has a pH of 10.69. What is the [OH-] in the solution?

A: Given : pH = 10.69

Q: Find the [OH-] of the solution, if the [H3O+] is: 2 ´ 10-11 M

A: Given that,  Concentration of [H3O+]   = 2×10-11 M

Q: The pain reliever codeine is a weak base with a K, equal to 1.6x10-6. What is the pH of a 0.05 M…

A: pH of a solution is defined as the negative  logarithm of H+ ion concentration. Given codeine…

Q: What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M?

A:

Q: Which of the following is the most basic solution (highest [UH ])? O pH 12 %3D O pOH = 1.0 o [OH] =…

A: 1) pH=12 we know, pH + pOH = 14 pOH = 14 - 12 = 2

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: Calculate the pH of an aqueous solution where the [OH-] is 6.9 × 10^-9 M.

A:

Q: In an aqueous solution, if the ​[OH^-] is 4.0E-9 M what is the ​[H3O^+]?

A: Given :- [OH-] = 4.0E-9 M To calculate :- [H3O+]

Q: What is the pH of an aqueous solution with an OH- concentration of 0.00250 M?

A: Solution:- Given concentration of OH- = 0.00250 M  [OH-] = 0.00250 M  As we know, p(OH) = -…

Q: If the [H*] is 1 x 10-2 M, what is the [OH ]?

A: Given :-  Concentration of H+ ions = 1 × 10-2 M  To calculate :-  Concentration of OH- ions i.e.…

Q: find [OH-] and [H3O+] if the pH= 2.75

A:

Q: The pOH of a basic solution is 3.47. What is [OH-]?

A: pOH is the negative logarithm of OH- ion concentration. pOH = -log[OH-] pOH is given here 3.47 3.47…

Q: Calculate the hydronium ion concentration in an aqueous solution of 0.195 M carbonic acid, H,C03…

A:

Q: What is the pH of a solution in which [OH⁻] = 0.000005 M?

A: The concentration of OH- = 0.000005 M OH-=0.000005 M=5×10-6 M

Q: The [OH-] of an aqueous solution is 3.5x10 -5. What is the [H+]

A: The relationship between pH/pOH and concentration is :   pH= -log [H+]             pOH= - log [OH-]…

Q: Determine the [OH-], pH, and pOH of a solution with a [H+] of 3.4 x 10-5 M at 25 °C. [OH-] pH = POH…

A: Since, Negative logarithm of concentration of H+ ion is known as pH. Then,

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: NH3(aq) + H₂O(1) ⇒ NH(aq) + OH- (aq) The equilibrium hydroxide concentration in a 0.0220 M NH3…

A: Concept based on the dissociation constant of an weak base.

Q: Determine the [OH-], pH, and pOH of a solution with a [H*] of 3.3 x 10-7 M at 25 °C. [OH¯] = M pH…

A:

Q: 5) What is the pH and pOH of a solution with a [H,0'] of 5.72X 10* M? Is the solution acidic, basic…

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

Q: Calculate [OH-] for a solution where [H,O*] = 0.00575 M. [OH¯] = M

A: For the given aqueous solution the concentration of the hydronium ion, [H3O+] is = 0.00575 M The…

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.