What is the pH of an aqueous solution of 1.89×10² M barium hydroxide? pH %3!

Q: What is the pH of an aqueous solution that is 0.123 MNH4Cl?For ammonia pKb= 4.74

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Q: What is the pH of a solution of 8.2 x 10-5 M HCl?

A: GivenConcentration of HCl = 8.2 x 10-5 MHCl a strong electrolyte completely dissociate solutionHCl →…

Q: If the K of a weak base is 8.5 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

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Q: What is the pH of an aqueous solution of 4.96x102 M hydrobromic acid? pH

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Q: What is the pH and pOH of 3.5 x 10-3 M HNO3  solution?

A: • The values provided in the question are:-     i) Concentration of HNO3, [HNO3] = 3.5 x 10-3 M    •…

Q: What is the pOH of an aqueous solution of 3.66×10-2 M barium hydroxide?

A: Given data, Molarity of Barium hydroxide=3.66×10-2Mwe calculate pOH as follows:pOH=-log[OH-]

Q: What is the H3O+ ion concentration in a 5.7 x 10^-4 M Ba(OH)2 solution? What is the pH?

A: Concentration of Ba(OH)2 = 5.7 x 10-4 M To determine : pH = ?

Q: What is the pH of (i) 1.0 X 103 M HBr and (ii) 1.0 X 102 M KOH?

A: We know that, pH and pOH can be expressed as the negative logarithm of hydrogen ion and hydroxide…

Q: What is the pH of a 0.620 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10 4)?

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Q: The H3O+ concentration in coffee is about 1 X 10-5 M. What pH is this?

A: The pH of a solution is equal to –log[H+] where [H+] is the concentration of hydrogen ions present…

Q: What is the pH of a 0.0600 M solution of nitrous acid at 25 C?

A: Since nitrous acid is a weak acid with acid dissociation constant = 5.6 X 10-4  The dissociation…

Q: What is the pH and the pOH of a 0.0215 M HCIO3 solution at 80.0 °C? Kw 2.5 x 10-13 at 80.0 °C pH:…

A: Given: Kw=2.5×10-13 [HClO3]=0.0215 M To find: pH and pOH Formula: pH=-log10[H+] pH+pOH=14

Q: Calculate the number of moles of HF that must be present in 500 mL of solution to give a pH of 3.5.…

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

A: We have to calculate the pH.

Q: What is the pOH of an aqueous solution of 2.59x10² M barium hydroxide? pOH

A: Given, the molarity of barium hydroxide =2.59×10-2 Mwe are asked to calculate the pOH of the aqueous…

Q: What is the pH value of 1x10-3 M CH3COOH solution? (Ka: 1.75x10-5)

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Q: What is the pH of 8.1 x 10-5 M HClO4 solution?

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Q: If 34.6 mL of a 0.68 M NaOH solution is added to a 51.9 mL sample of a 0.68 M weak acid, HA , what…

A: 34.6 mL of a 0.68 M NaOH solution is added to 51.9 mL sample of a 0.68 M weak acid, HA (ka = 1.8 x…

Q: What is the pH of a solution containing 0.30 M NH4OH and 0.52 M NH4Cl? Kb= 1.8 x10-5

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Q: What is the pH when 72 moles of acetic acid are added to 105 L of water? Ka = 1.8X10^‐5

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Q: The pH of saliva is about 7.40 that means the concentration of Hydrogen in it is about: [H+] = x 10

A: The pH of a solution is the negative logarithm of hydrogen ion concentration. It can be written as:…

Q: 2. What is the pH, the pOH and the [OH] of a solution in which the [H*] = 2.43 x 10-6 M? %3!

A: pH is defined as  the negative log of hydrogen ion concentration  pOH is defined as the negative log…

Q: What is the hydroxide ion concentration for a 23 % (m/v) HNO3 solution?

A: The ratio of moles to the volume of solution in liters is known as molarity.

Q: What is the pH of a 3.1 x 10-4 M CsOH solution?

A: Given : concentration of CsOH = 3.1 × 10-4 M  To calculate :- pH of solution

Q: 2. What is the pH of a 0.01 M HNO3 solution? What is the ratio of acid to conjugate base for this…

A: (1) The dissociation of the given acid can be given as: The concentration of the acid is 0.01 M.…

Q: What is the pH of a 7.7 x 10-3 M HI solution?

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Q: What is the pH of a solution prepared by dissolving 0.24 gram of solid MgO in enough water to make…

A: In order to find the pH we first write down the given data: Mass of MgO= 0.24 g. Volume of solution=…

Q: What is the pH of an aqueous solution of 8.92x102 M potassium hydroxide? pH %3D

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Q: A student is required to determine the pH of a water sample that was believed to be contaminated…

A: It is a strong base that means in H2O it will be completely dissociates as Mg+2 and 2 HO-

Q: Calculate the pH of a 1.8 x10-2 M Ba(OH)2 solution.

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Q: What is the pH of a 0.20M solution of nitrous acid? Ka= 4.5x10^-4.

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Q: What is the pH of an aqueous solution of 6.78x102 M barium hydroxide? pH =

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

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Q: What is the pOH of a solution that has a hydroxide ion concentration[OHˉ] of 2.00 x10ˉ 6 M?

A: A solution is made up of solute and solvent. Solvent is present in large amount and solute is…

Q: What is the pH of an aqueous solution of 1.99×102 M perchloric acid? pH =

A: The pH of a solution can be calculated by using formula pH = -log10[ H+]

Q: What is the pH of 5.04 x 10-3 M HI? Is it acidic, basic, or neutral?

A: HI is a strongest acid it dissociates completely .

Q: If the K of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH =

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Q: What is the pH of a 0.862 M NH3 solution that has a Kb = 1.8 x 10-5?

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Q: what is the pH of a 7.1 x 10^-3 M solution of H^+?

A: Given : [H+ ]  = 7.1  x 10-3 M

Q: What is the pH of a 0.25 M NH3 solution? Kb 1.8 x 10-5 = pH = [?] pH Enter

A: The equilibrium constant (Kc) of a reaction is the ratio of product of molar concentrations of…

Q: Calculate the pH of a 3.5 x 10-3 M HNO3 solution.

A: Nitric acid HNO3 is a strong acid. Hence, it completely dissociates in the aqueous solution.

Q: 10. Nitrous acid (HNO2) is a weak acid with a Ka = 4.0 x 104. If 112 mL of a 0.100 M KOH solution…

A: Answer: In this question we have to find out the pH of a buffer solution made of nitrous acid and…

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

Q: pOH

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Q: pOH

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Q: What is the pH of a solution of 0.30 M CH:NH:Cl? Kb for CH:NH2 = 4.4 x 104

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Q: What is the pH of a 0.844 M solution of hypochlorous acid (Ka 2.9 x 10-8)?

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Q: What is the pH of a 1.7 x 10^-3 M HI solution?

A: pH is a measure of acidity and basicity of solution. When pH value is below 7 solution is acidic.…

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.