What is the pH of 1.65e-3 M Ba(OH)2?

Q: What is the pH of a 2.35 x 10-2 M HCl acid solution?

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Q: (v) Ca(OH)2 is a strong base that completely dissociates in solution. What is the pH and pOH of a…

A: The pH of a particular substance is the negative logarithm of the (H+) hydrogen ion concentration.…

Q: Calculate [H+ ], [OH- ], pH and pOH of 2.00 M (weak acid) HF (Ka=6.8 x 10 -4)

A: We have to calculate the hydrogen ion , hydroxide ion concentration , pH and pOH.

Q: What is the pH of a 0.122 M monoprotic acid whose K, is 5.7 x 104? a

A: question given concentration and Ka using this we can calculate the degree of dissociation  using…

Q: 1    Calculate the pH of a 0.02 M solution of the weak acid, HA.         Ka = 2.46 X 10 –4…

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Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: What is the pH of an aqueous solution of 1.69×10-² M hydroiodic acid?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: What is the pH of a solution of 0.400 M CH,NH, containing 0.100 M CH,NH,l? (Kb of CH;NH, is 4.4 x…

A: This is a basic buffer solution. A buffer resist the change in PH of the solution.

Q: what is the ph of 0.10M Fe(OH)2

A: We know that Ksp of Fe(OH)2=2*10^-15

Q: What is the pH of 3.78 *10^-2 M nitric acid in aqueous solution ?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: Assuming complete dissociation, what is the pH of a 3.25 mg/L Ba(OH), solution?

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Q: What is the pH of an aqueous solution of 1.45×10-2 M nitric acid?

A: Nitric acid i.e HNO3 is a strong acid. Hence it dissociates into ions completely as per the…

Q: What is the pH of a solution containing 9 gram of HCl (MW 18 am) dissolved in 50 ml of water?

A: In order to calculate the pH of solution we need to calculate firstly the number of moles of HCl.…

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: 16- The pH value of 0.1 M ammonium hydroxide and 0.01 M ammonium chloride is - -- O 8.26 O 10.26 O…

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Q: What is the pH of 0.0056 M Ba(OH)2?

A: The pH of a solution is used to specify the solution is acidic or basic in nature. The pH is a…

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

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Q: What is the pH of a 0.16 M solution of methylammonium chloride, CH;NH; Cl? What is the concentration…

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Q: What is the pH of a 0.0650 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

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Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?

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Q: What is the pH of 0.350 M Sr(OH)2 ?

A: pOH of the solution is equal to the negative logarithm of hydroxide ion while the pH of the solution…

Q: What is the pH of a solution containing 6.65 g sodium acetate (NaC2H302, 82.03 g/mol) in 100.0 mL of…

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Q: HCN is a weak acid (Ka = 6.20 x 10-10), so the salt, KCN, acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0675 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: What is the pH of a 3.79×10-3 M  aqueous solution of hydrochloric acid?

A: pH of solution is given the information about acidic and basic nature of solution. If pH = 7 then…

Q: What is the pH of a 0.0600 M solution of calcium hydroxide at 25 C?

A: pH holds an essential role in the survival of every living organism. The [H+] ions potential carried…

Q: pH of a 8.82 x 10M solution of Ba(OH)2?

A:

Q: pH

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Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?

A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…

Q: The pH of 0.010 M trimethylamine is 10.78 at 25 oC.  What is the hydroxide ion [-OH] concentration?

A: pH is defined as the negative logarithm to the base 10 of hydrogen ion concentration. pH = -log10[…

Q: The hydroxide ion (OH-) concentration in skim milk was measured to be  5.4 x 10-8 M. What is the pH…

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Q: What is the pH of a 0.0370 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A:

Q: HCNN is a weak acid (?a=6.20×10^−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Given: Ka of HCN = 6.20×10-10 KCN = 0.0525 M we have to determine the pH ? Kb = Kw / Ka       = 1 ×…

Q: What is the pH of a solution prepared by diluting 25.00mL of 0.020 M Ba(OH)2 with enough water to…

A: Ba(OH)2 is a strong base. It dissociates completely to give Ba2+ and OH- ions.  Ba(OH)2→ Ba2+ + 2OH-…

Q: Calculate the pH of a 0.05 M solution of hydrofluoric acid. The Ka of hydrofluoric acid is 6.6x10^-4

A: Given data, Molarity of HF=0.05MKa of HF=6.6×10-4 pH of a solution is given by -log[H+]

Q: What is the pH of a 7.8×10-5 M Ca(OH)2 solution?

A:

Q: The K₂ of a weak monoprotic acid is 1.74 x 10-5. What is the pH of a 0.0939 M solution of this acid?…

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Q: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

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Q: 6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a…

A:

Q: What is the pH for 2.4 M ammonium chloride aqueous solution (ammonium hydroxide, Kb=1.8×10-5)?

A: Ammonium chloride,  NH4Cl  dissolves in solution to form ammonium ions  NH4+  which act as a weak…

Q: What is the concentration of hydroxide ion in a 0.150 M aqueous solution of hydroxylamine, NH,OH?…

A: NH4OH is a weak base, hence it can't dissociate completely, hence equilibrium is established between…

Q: The pH of 750 mL (3 SF) of an aqueous solution containing only NaNO 2 is 8.42. If HNO 2 has a Ka of…

A:

Q: 1.4 A 0.015 M solution of hydrogen cyanate , HOCN, has a pH of 2.67 a) What is the hydronium ion…

A: Given: The pH of the solution of hydrogen cyanate is 2.67. The molarity of hydrogen cyanate is 0.015…

Q: What is the pH of a 0.0500 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10⁻¹⁰)?

A: Given -> Molarity of HCN = 0.0500 M Ka = 4.9 × 10-10

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10*)?

A: dissociation of Ca(NO2)2 Ca(NO2)2(aq)→Ca2+(aq)+2NO2-(aq) we can see 2mol of NO2- is formed from 1…

Q: What is the pH of an aqueous solution of 5.55×10-3 M potassium hydroxide?

A: The sum of pH and pOH is equal to 14. The relationship between pH and pOH is expressed as:…

Q: What is the pH of a 4.5×102M solution of KOH at 25 °C?

A: Given:   The concentration of KOH is 4.5×10-2 M. The value of temperature is 25 ˚C.

Q: 1.00-l aqueous solution contained 6.78 g of barium hydroxide, ba(oh) 2 . what was the ph of the…

A: We know that, pH can be expressed as the negative logarithm of hydrogen ion concentration i.e.…

Q: A 10° C solution has a pH of 8.0 . At this temperature , K w =2.93 x 10^ -15 . What is the pOH of…

A: Kw is an equilibrium constant, which is known as ionic product of water. It is the product of 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.