Calculate OH- in a solution that is 0.0062M Ba(OH)2 and 0.0105M BaCl2  BaCl2 does not hydrolyze

Q: What pH results when 0.75 mol of acetic acid is dissolved in enough water to make 3.0 litres of…

A: Acetic acid is a weak acid and will partially dissociates into its ion. Molarity is defined as the…

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: Calculate the [H] and pH of a 4.73 x 10 M iodoacetic acid solution. The K, of iodoacetic acid is…

A: Given : Concentration of iodoacetic acid = 4.73 x 10-4 M Ka = 6.68 × 10-5 Ka is the equilibrium…

Q: 2. 50 x 10-5 , wha

A: Given data are as follows: Concentration of acidic solution = 0.05 M Ionization constant = 2. 50 x…

Q: Example: - Calculate the pH and pOH of a 1.0 x 10-7 solution HC1? HCI H+ + Cl-

A:

Q: What is [OH-] in a solution of 0.125 m ch3nh2 and 0.130 m ch3nh3cl?

A: Buffers are the solutions containing a mixture of weak acid and its conjugate base or a mixture of…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 2.8x1o-2 M. The hydroxide ion…

A:

Q: If the pOH of a solution is 7.7, calculate [H*]. 50118723.362727247 1995262.314968879 0.000000501…

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: The pOH of an aqueous solution of 0.461 M hydrofluoric acid is .

A:

Q: Calculate the pH to two decimal places of each of the following solutions at 25 °C for which the…

A: p H can be calculated using the equation given below:

Q: A solution is 0.0500 M in NH4Cl and 0.0300 M in NH3. Calculate its OH- concentration and its pH.

A:

Q: Calculate the molar concentration of H3O+ in a water solutions with the following OH molar…

A: The given data is as follows: (a) The molar concentration of OH- = 0.018 M The molar concentration…

Q: 36. Which will have a lower (the lowest) pH among the solutions shown in each of the following…

A:

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

A:

Q: At certain temperature, the pKb value of NH4OH is 4.70. What is the pH value of a 0.20 M solution of…

A:

Q: 4. Calculate the value of [H3O'Jand [OH] in each solution: a. 0.0001 M NaOH b. 0.0001 M HCI

A:

Q: v much 0.150M HCI wa

A: At Neutralization point, Gram eq. of LiOH = Gram eq. of HCl  Mole×valence factor = N2V2

Q: Calculate [OH-] of NaClO, 0.110M; KaHClO = 3.0 x 10-8.

A: Given: Concentration of NaClO is 0.110 M Ka (HClO) is 3.0×10-8 To determine: [OH-]

Q: What is the pH and pOH of a: a) 0.20M NH4CI solution? b) 0.47M NaCN solution?

A:

Q: Calculate [OH-] and pH for each of the following strongbase solutions: (a) 0.182 M KOH, (b) 3.165 g…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: A solution is found to have a pH of 8.3, what is the hrdroxide ion [OH-] concentration?

A: Introduction If we know the pH of any particular solution, then first [H+] is calculated then with…

Q: A solution has [OH - ] = 4.0 * 10 - 8 . What is the value of [H + ] for the solution?

A: [OH-] = 4.0 × 10-8  [H+] = ?

Q: Calculate the concentration of 45.0 mL of a phosphoric acid solution that neutralized 20.8 mL of…

A: H₃PO₄ + 3NaOH → Na₃PO₄ + 3H₂O Volume of H3PO4 = 45 mL = 0.045 LVolume of NaOH = 20.8 mL = 0.0208 L…

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: HF undergoes dissociation as: HF+H2O→F-+H3O+

Q: pOH and ph of a solution with [OH-] concentration of 1.20x10^-7 M.

A: Given: OH-=1.20×10-7 M Calculation: pOH=-logOH-pOH=-log1.20×10-7pOH=-log(1.20)-(-7) log…

Q: Calculate [OH-] and molality of an HCl solution with pH= 3.4

A:

Q: 1. An electrolyte which forms OH- in aqueous solution a. Arrhenius acid b. Arrhenius base c.…

A:

Q: Calculate 3OH-4 and pH for each of the following strong base solution a solution formed by mixing…

A: Given parameters are: Volume of Ba(OH)2 = 20.0 mL Molarity of Ba(OH)2 = 0.015 M Volume of NaOH =…

Q: Compounds containing nitrogen are often weak bases. One example is aminoethanol, which has the…

A: Answer:- This question is answered by using the simple concept of ionization of weak base and then…

Q: Calculate [OH-] in a 3.0 × 10-7 M solution of Ca(OH)2.

A: The dissociation is as follows,

Q: Determine the Keq values for the dissociation of arsenic (H3AsO4(aq)) in a liter of solution. Hint:…

A: H3AsO4 is a polyprotic acid or more accurately a triprotic acid. This means that it has three…

Q: The pH of an aqueous solution at 25oC is 2.40. What is the [OH-] concentration in this solution? Kw…

A: Given data :- pH = 2.40 Temperature = 25℃ Kw = 1.0 × 10-14 We know that ., PH + POH  = 14

Q: The molar concentration of OH- in a water solution is 1.5 × 10−9 M. Determine the concentration of…

A:

Q: If the Kh of a weak base is 6.2 × 10-6, what is the pH of a 0.24 M solution of this base? pH =

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Q: Hi, Determine [OH- ] in each base solution.  If the acid is weak, indicate the value that [OH- ] is…

A: c) 0.225 M Ba(OH)2 Ba(OH)2 is a strong base. It dissociates as follows: Since each molecule of…

Q: Complete the neutralization reaction below: NaOH + HCI - Н-0 O. HCI Ob HNa Oc NaCl O d CIOH

A: Neutralization reaction can be defined as the chemical reaction between an acid and base to produces…

Q: Calculate the pH to two decimal places of each of the following solutions at 25 °C for which the…

A: NaOH completely dissociated to form Na+ and OH-. Here, the concentration of OH- is 0.016 M pOH of…

Q: What is the pH of a solution if 90 mL of 1.0 M NaCl is added to 10 mL of a 1.0 M NaOH solution?

A: Answer

Q: Calculate the pH of 3.0 X 10-5 M Mg(OH)-, which completely dissociates to Mg2+ and OH-.

A: Given that the Mg(OH)2 completely dissociates, so the dissociation reaction is, Mg(OH)2 →Mg2++2OH-

Q: What is the final pH of the solution when 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl…

A:

Q: What is the pOH of a solution that has ​[OH^-] = 2.7E-4 M

A: pOH can be expressed as -log[OH-]. It is used to represent basicity of a solution. If the pOH value…

Q: Calculate the pH of the following: 5) A solution that contains 0.10 M ammonium hydrochloride and…

A: In this solution we have a strong acid HCl which dissociate completely .  And another is a weak acid…

Q: Calculate [H+] in a solution

A: Given :- [OH-]=2.0 x 10-2 M To calculate :-  [H+]  nature of solution

Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL solution…

A: Strong acids dissociate fully in aqueous solutions while weak acids dissociate partially in aqueous…

Q: Calculate the ph and poh for a solution that is 0.63 M in NH3 and 0.4 M in NH4Cl, Ki for NH3 is…

A: Given,  The molarity of NH3 = 0.63 M  The molarity of NH4Cl = 0.4 M The Ki for NH3 = 1.9 × 10-5  The…

Q: The pOH of a solution made by combining 150.0 mL of 0.10 M KOH(aq) with 50.0 mL of 0.20 M HBr(aq) is…

A:

Q: what do you expect to happen to the pH of the same if you add 1 ml of i M NaOH instead of 1 ml of 1…

A: Answer PH  does not effect by adding acid or base in the system 1ml of…

Q: what do you expect to happen to the pH of the same if you add 11 ml of i M NaOH instead of 11 ml of…

A: 1st it depends on the solution where you are adding it.  for example, if the original solution is…

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.