12. Calculate [OH] for a solution of pH = 5.88.

Q: Calculate the pH of a 0.165 M  solution of KOH.   Calculate the pOH of a 0.165 M  solution of KOH.

A: Concentration of solution of KOH = 0.165 M

Q: What is the [OH] in a solution with a pH of 9.22? (1.7 X 10 M)

A: Given that pH of solution=9.22

Q: A solution of Mg(OH)2 was found to have a pH of 12.64. Determine the initial concentration of the…

A:

Q: What is the pH of a 8.8 x 102M solution of HCIO4? (value + 0.02)

A: Given: Concentration of HClO4 = 8.8×10-2 M   HClO4 is strong acid, it will completely dissociate in…

Q: if the pH is 1.87 find the pOH, [H3O+], and [OH-] calculation

A:

Q: Calculate the pH of 0.010 M Trisodium arsenate

A: The pH is calculated below

Q: Consider a solution which is [OH-] = 1.0 x 10-5 M. Calculate the pOH of the solution. Is the…

A:

Q: Calculate the pH of a solution that has a pOH of 8.70.

A: Given,  pOH of the solution = 8.70  Calculate the pH of the solution = ?  Use the formula :  pH +…

Q: 28. The pH of a solution is measured to be 10.4. What are the values of (HO] and (OH for this…

A:

Q: Calculate the pH of a 0.020 M solution of oxalic acid

A:

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 0.32M solution of barium hydroxide?

A: The pH of a solution indicates the acidity or basicity of a solution, which is measured using…

Q: A solution has a pOH of 13.12. This tells us   a) solution is very acidic b) solution is slightly…

A:

Q: Calculate [OH ] for a solution where [H,0*] = 0.00567 M. [OH¯] = M

A:

Q: 13. What is pH of a 0.25 M sodium hydroxide solution?

A: Since you have asked multiple questions, we will answer the first question for you. For any specific…

Q: Calculate [H'] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: The concentration of hydrogen ions in an aqueous solution is measured in pH scale. Mathematically,…

Q: Calculate the value of [OH−] from the given [H3O+] and label the solution as acidic or basic. a.2.6…

A:

Q: 2. If the [H'] in a certain tap-water sample is 2.6x107 M, what is the OH° concentration? Determine…

A: Answer 2 :  Given : [H+] = 2.6 × 10-7 M             [OH-] = ?             pH = ?

Q: What is the pH of a 4.7 × 103 M HI solution?

A:

Q: Calculate the [OH in a solution that has a pH of 2.92.

A: We know that, pH can be expressed as negative logarithm of H+. i.e.,                      pH = -…

Q: Calculate the pH and pOH for the solution with [Ca(OH)2]= 4.29x10^-5M Is the solution acidic or…

A: The value of pH can be determined by the concentration of the hydrogen ion present in the solution…

Q: Calculate the pH of a solution that is 0.0400 M in *(a) H,PO4.

A: Answer  H3PO4 is weak acid       PH   = 1/2 [ Pka  - log c]…

Q: A particular solution has a [OH−1] = 9.82×10−5. Calculate the [H+1] for this solution

A:

Q: What is the pH of a 0.00050M Ca(OH), solution? 3.00 3.30 9.50 10.70 11.00

A:

Q: Calculate the concentration of H+ in an aqueous solution with a pH of а. 3.40 b. 9.20

A: Recall the following expression of pH         pH=-logH+ Here, H+ is concentration of H+ ion in the…

Q: The pH of a 0.23-M solution of HF is 1.92. Determine Ka for HF from these data

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is given…

Q: Calculate the concentration of H+ in a solution of pH = 1.25.

A: pH of the solution = 1.25  Concentration of H+ = ?

Q: Calculate the pH of a 0.820 M solution of ammonium bromide, NH₄Br. pH = ___

A:

Q: Calculate the pH and pOH for the solution with [Ca(OH)2] = 4.29 x 10–5 M. Is the solution acidic or…

A: Since the the salt given Ca(OH)2 is a strong base Hence it will dissociate completely as per the…

Q: Using data from Appendix D in the textbook, calculate [OH−] and Ph for each of the following…

A: Given data : Concentration of NaBrO = 0.10 MOH-=6.3×10-4 The ICE table for the process is :…

Q: Calculate the pH of a 0.0500 M  solution of NaOH. Calculate the pOH of a 0.0500 M  solution of NaOH.

A:

Q: Calculate the pH. 0.5 M H3PO4

A: pH is used to determine the concentration of hydronium ion.

Q: Determine [OH] in a solution where [H30*] = 5.82 x 109 M. Identify the solution as acidic, basic, or…

A: Here given, [H3O+] = 5.82 x 10-9 M We know, PH = - log [H3O+] Or, PH = - log [5.82 x 10-9] Or, PH =…

Q: Calculate the ratio at pH 9.90. [HCO,] [HCO5] * TOOLS x10

A: Henderson - Hasselbalch equation:

Q: 4. Calculate the pH and pOH of 0.001 M solution of sodium hydroxide (NaOH) at 25° C.

A: Given  Concentration of NaOH  =  0.001 M                                          =  1 × 10-3 M PH…

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 0.74 M solution of NaOH.

A:

Q: 9. What is the PH of a solution with [OH¯]=1 x 10ªM |10 |9HF O11HCNO |None of the others

A: Given, a solution having [OH-] =1×10-4 Mwe are asked to calculate the pH of the solution.

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: 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: A solution has [OH-] = 8.9 x 10^-3, how would you calculate the ph of the solution ?

A: This problem can be solved by knowing that for any solution, pH + pOH = 14. The pH of a solution is…

Q: Calculate the value of [OH] from the given [H₂O*] and label the solution as acidic or basic. a. 10-¹…

A:

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

A:

Q: Calculate the pH of a 0.00118 M solution of HBr.

A: Given data contains, Concentration of HBr is 0.00118 M. Hydrobromic acid is a strong acid so it gets…

Q: A 0.048g sample of solid calcium hydroxide is dissolved in water to form a 750.0ml solution.…

A: PH =- log [H+] POH =- log [OH-] Where [H+] and [OH-] are the concentration of H+ and OH- Molar…

Q: Determine the H*]. [OH , and pH of a solution with a pOH of 2.65 at 25 °C. (H = M %3D M pH =

A: Given data is as follows: The pOH of the solution = 2.65 As we know that; pH+pOH=14        At 25 °C…

Q: For the reaction of hydrazine (N2H4) in water, H2NNH2(aq) + H2O(l) ⇌ H2NNH3+(aq) + OH- (aq) Kb is…

A: Given: The reaction is as follows: H2NNH2(aq) + H2O(l) ⇌ H2NNH3+(aq) + OH- (aq) The initial…

Q: The weak acid HZ has a Kₐ of 2.55X10⁻⁴.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: For weak acid HZ , pKa = -logKa = -log (2.55 x 10⁻⁴) = 4 -log2.55 = 4 - 0.40 = 3.60 (a)  pH of…

Q: Calculate [OH] for a solution where [H,O*] = 0.00553 M. [OH ] =

A: Given: Concentration of hydronium ion, [H3O+]=0.00553 M To find: The concentration of hydroxide ion,…

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.