What is the pH of a solution with 10.2mL 0.10M CH3COOH and 0.15mL 1.0M HCl ? Ka = 1.8x10^-5

Q: Calculate the pH value of 0.01M Ba(OH), solution.

A: Given concentration of Ba(OH)₂ solution = 0.01 MTo find :pH Value of the above solution

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH  = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: A diprotic acid has ka1= 4.3×10^-6 and ka2= 5.5×10^-9. What will be the pH of a 0.77 M solution of…

A: In this question, we want to determine the pH of the Solution of the acid.  You can see details…

Q: Calculate the pH when 43.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

A: HBr +CH3NH2 ==> CH3NH3+ + H2O Given volume of HBr = 43.0ml           Molarity of HBr = 0.200M…

Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…

A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…

Q: when

A: A) moles of Acid(HBr) = 39.0mL • 0.200molL-1 = 7.8mmol  B) moles of Base( CH3NH2 ) = 30.0mL •…

Q: Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: What is the pH of 0.024M acetic acid solution at 25°C? (Ka=1.8×10^-5)

A: Given, [CH3COOH] = 0.024 M Ka = 1.8 × 10-5

Q: What is the pH of a solution prepared by mixing 18.00 mL of 0.277M CH3COOH with 50.00 mL of 0.166 M…

A:

Q: What is the pH of a solution composed of 1.0 x 10-6 M sodium hydroxide solution?

A: Acid is commonly sour. An acid is a substance that renders an ionizable hydronium ion (H3O+) in its…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: At 25°C, the pH of HF solution is 2.13. When Ka of HF = 6.6 × 10-4, calculate the molar…

A:

Q: What is the pH of a solution obtained by mixing 100ml of a 0.01M NaOH solution and 100ml of a 0.01 M…

A: NaOH is a strong base and Acetuc acid is a weak acid, thus we will get a overall solution basic.

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

A:

Q: what is the pH?

A:

Q: What is the pH of 0.15 M solution of acetic acid (CH3COOH) Ka=1.75 x 10^-5 A) 2.6 x 10^-6 B) 0.0016…

A: Calculating pH of the acetic acid. CH3COOH + H2O <----------> CH3COO- + H3O+

Q: What

A: Dear student I have given answer to your question in the image format.

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: what is the pH of 0.12795M CH3COOH solution? Ka=1.8x10^-5

A: We have to calculate the pH.

Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

A:

Q: What is the pH of 0.030 M aqueous formic acid (Ka of HCO2H = 1.8× 10^-6)

A: Formic acid dissociates as follows:                               HCOOH (aq) ⇌ HCOO- (aq) + H+ (aq)…

Q: A certain weak base has a K b of 8.40 * 10 ^ - 7 . What concentration of this base will produce a pH…

A: Given, pH of solution =10.36 and base ionization constant Kb =8.40×10-7we are asked to calculate the…

Q: Calculate the pH when 44.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

A: Given, Volume of HBr = 44.0 mL Volume of CH3NH2 = 30.0 mL

Q: 4. Calculate the pH of an aqueous solution containing 6.32x109 H3O* ions per liter.

A:

Q: Calculate the pH of 0.15M CH3COOH. Ka=1.8×10-5

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

Q: Assuming complete dissociation, what is the pH of a 3.39 mg/L 2Ba(OH)2 solution?

A: Given, Mass of Ba(OH)2= 3.39 mg/L= 3.39 × 10-3 g/L We know , pH = -log[H+] Kw = [OH-] × [H+]

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0152 M solution. The pH of the…

A:

Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH when 45.0 mL of 0.200 M HBr is mixed with 40.0 mL of 0.400 M CH₃NH₂ (Kb = 4.4 ×…

A: we have to calculate the pH of solution

Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

Q: Calculate the pH of a 0.5000M NH CI solution. K, of NH, =1.8×10

A:

Q: At 10°C, the ion-product constant of water, K w, is 6.88 × 10 –15. What is the pH of pure water at…

A: Autoionization of water takes place as follows: The product of the concentration of the hydronium…

Q: What is the pH for a solution with 0.10 MCH 3 COOH solution and 0.30 M CH 3 COONa? (K a for acetic…

A:

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

Q: 6) Which of the following has the highest hydroxide ion concentration? 0.1 M HCI 0.1 M H₂SO4 a…

A:

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH of the solution when 35.0 mL of 0.15 M HCN is mixed with 17.5 mL of 0.30 M NaOH. Ka…

A: [NaOH ] = 0.30 M  VNaOH = 17.5 ml  nNaOH = 0.30 M x 17.5ml = 5.25 m mol  [HCN ] = 0.150 M  V HCN =…

Q: A certain weak base B has a base-ionization constant Kb of 5.9 × 10–4 at 25°C. If strong acid is…

A: Ionisation constant Kb of base B=5.9×10-4

Q: %3D What is the pH of a 0.1000 M NACH3COO solution? (Ka CH3COOH = 1.8x10^-5) 4.75 5.13 8.87 7.45…

A: We have find out pH of 0.1000 MNaCH3COO Solution.

Q: A certain weak base has a ?b of 7.50×10^-7. What concentration of this base will produce a pH of…

A:

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: If the ph of a 30.0 mL sample of 1.0 M HOAc is 2.40 what's the equilibrium [H+] and the Ka value?

A: HOAc is a weak acid also known as acetic acid. The pH of a solution is related to the concentration…

Q: Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given Molarity of KOH = 0.150 M Volume of KOH = 10 ml Molarity of HBrO = 0.300 M Volume of HBrO = 20…

Q: What is the Kb for the conjugate base of an unknown acid with a Ka of (8.4x10^-3) What is the pH of…

A:

Q: Calculate the pH of a 120mL of a solution containing 0.5g of hydrofluoric acid. Ka = 6.6 x 10^-4

A: pH = -log[H+]  Molar concentration = number of moles of solute/volume of solution (in L)  number of…

Q: Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given:Concentrations KOH  = 0.150 M    Volume = 50 mLHBrO = 0.300 M   Volume = 20 mLNow number of…

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.