HOW DO WE FIND THE pH, H+ and OH- of a 0.10 M Na2CO3.

Q: What is the pH when the [OH-] = 4.26 x 10-2 M at 25 oC?

A: 1- First we need to calculate the pOH of the solution :  We know that,  pOH = -log[OH-]  pOH = -log(…

Q: Calculate the pH of a 7.9 x 10 Maqueous solution of hydrobromic acid (HBr). Round your answer to 2…

A: Given that -  Molarity of hydrobromic acid HBr = 7.9×10-5 M    Now the pH is negative logarithm of…

Q: What is the pH of an aqueous solution of KOH with a concentration of 0.035M? Respond with the…

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Q: What is the pH of 0.88 M NaOH?

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Q: Methylamine, CH3NH2, is a weak base.CH3NH2(aq) + H2O(ℓ) ⇄ CH3NH3+(aq) + OH−(aq)If the pH of a 0.065…

A: Given data contains, pH=11.70 Concentration is 0.065 M. The pOH is calculated as, The pOH is 2.30.

Q: CH3NH2 is a weak base (?b=5.0×10^−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

A: CH3NH3NO3 → NO3- + CH3NH3+ Kb for the above reaction is 5x10-4  CH3NH3 can donate a proton and…

Q: Given that acetic acid has Ka = 1.8 x 10–5, what is the pH of a solution that contains the molar…

A: Given: Ka of acetic acid = 1.8 x 10-5  [CH3CO2–][CH3COOH] = 110   Calculating pKa pKa=-log (Ka)…

Q: The K₂ for a base is 15.3 x 10-13. What is the Ka for its conjugate acid?

A: Given :- kb for a base = 15.3 × 10-13  To determine :- value of Ka for its conjugate acid

Q: ) What is the pH and pOH of a solution with a [H;O*] of 5.72X 10-8 M? Is the solution acidic, basic…

A: Given: Concentration of H3O+ = 5.72×10-8 M Or [H3O+] = 5.72×10-8 M

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

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Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.203 M  solution of…

A: This problem is based upon basic strength of base or dissociation constant for the base. Since…

Q: Determine the [H+][H+] , [OH−][OH−] , and pOH of a solution with a pH of 12.9412.94 at 25 °C.

A: We know that, pH is the negative logarithm of hydrogen ion concentration  i.e.,…

Q: What is the concentration of H3O+ ions in black coffee if [OH-] = 1.3 x 10-9 M? Is black coffee…

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Q: The hydronium ion concentration of an aqueous solution of 0.502 M triethanolamine (a weak base with…

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Q: Complete the following statements about the below solutions at 25 °C? 1. The pOH of 9.95 x 105 M KOH…

A: at 25°C ;  pH + pOH = 14.0  pOH = -log[OH-]

Q: What is the pH of 2.9x10 M

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Q: Ka for ammonium, its conjugate acid. (NH4+) = 5.68 x 10^-10 Using the answer above, what is the pH…

A: Given: Ka = 5.68 x 10-10 Concentration of NH4Cl = 0.140 M

Q: - log10 H*] where H* is the concentration of hydrogen The pH scale for acidity is defined by pH =…

A: pH is defined as the negative logarithm to the base 10 of hydrogen ion concentration expressed in…

Q: The pH of a 0.59M solution of barbituric acid (HC,H,N,0,) is measured to be 2.12. Calculate the acid…

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Q: In the reaction: H2PO4 + H20 H3PO4 + OH", which pair represents an acid and its conjugate base?

A: an acid is a proton donor whereas a base is a proton acceptor  acid after donating a proton turns…

Q: Calculate [OH–] , [H+] , and the pH of 0.20 M solutions of each of the following  amines. a.…

A: Aniline and pyridine both are weak bases. From the equilibrium table we have to determine its…

Q: The hydronium ion concentration of an aqueous solution of 0.377 M ethylamine (a weak base with the…

A: Given, Concentration of of ethylamine solution (C) = 0.377 M [H3O+] = ? M ethylamine (C2H5NH2) is a…

Q: HOW DO WE FIND THE pH, H+ and OH- of a 0.10 M NH4CL HOW DO WE FIND THE pH, H+ and OH- of a 0.10 M…

A: Given concentration of NH4Cl is 0.10M

Q: H NO3 HF K" H* OH OH K OH F NO3 H* 4* HF OH H* NO3 он K* HF HF Mg(OH) a b Which beaker depicts a…

A: Arrhenius gave the definition of an acid and base. According to him, acids are those substances…

Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

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Q: 1. HOW DO WE FIND THE pH, H+ and OH- of a 0.10 M KAI(SO4)2.

A: Given concentration of KAl(SO4)2 is 0.10M

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

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Q: 24. Methylamine, CH3NH4 is a weak base that ionizes in solution as shown by the following equation.…

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Q: If the [H3O+] is 4.95 x 10–12 M, what is the pH?

A: Given :-  [H3O+] =  4.95 x 10–12 M  To calculate :- pH of solution

Q: Determine the [H+], [OH-], and pOH of a solution with a pH of 6.81 25 ° C.

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Q: What are the concentrations of H,O* and OH- in tomatoes that have a pH of 4.10? [H,O*] = M [OH] = M

A: pH is defined as negative log of concentration of hydronium ions. If the pH belongs in between 1 to…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: : Find the Kw of pure water at 50.0°C, if the pH is 6.630? 2: Find the pOH in an aqueous solution…

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Q: Ascorbic acid (vitamin C, C6H;O6) is a diprotic acid (Ka1 = 8.0x10 and Ka2 = 1.6×10-12). What is the…

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Q: What is the pH of a 1.00*10-°M solution of KOH at 25 °C? 5.000 9.000 12.400 13.980 7.004

A: pOH= -log[OH-] = -log 10-9 = 9

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: For first ionization :  pH = 0.5pKa1 - 0.5logC ..(1) Here, pKa1 = -logKa1 = -log(8*10^-5) = 4.097 C…

Q: Which of the acids listed below has the weakest conjugate base? O H₂02; K₂ = 2.400x10-12 O HBr, K₂=…

A: The larger the value of ka stronger the acid and weaker the conjugate base.

Q: Will an aqueous solution of Ni(NO3)3 form an acidic, basic, or neutral solution? O neutral basic O…

A: When any Substance is Dissolved in water, then it will give an acid and a base from which it is…

Q: The value pKw is 11.05 at 78 °C. What is the pH of a neutral solution at the same temperature? Enter…

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Q: For C5 H10NH2™, enter an equation that shows how the cation acts as an acid.

A: According to Bronsted-Lowery acid-base theory, acids are proton donors and bases are proton…

Q: What is the [OH-] and pH of a 0.35 M solution of hydroxylamine (a weak base, NH3OH)? Kb = 1.10 x…

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Q: If the pH of a certain soft drink is 3.60, what is the H3O+ concentration in the soft drink

A: Given, pH of soft drink = 3.60 The concentration is defined as the abundance of the constituent that…

Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (C6H3O7)? C6H3O7(aq) +…

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Q: The Kb of dimethylamine [(CH3)2NH] is 5.90x10–4 at 25°C. Calculate the pH of a 0.103 M  solution of…

A: Given : Concentration of (CH3)2NH = 0.103 M And Kb of (CH3)2NH = 5.90 X 10-4  Since (CH3)2NH is a…

Q: pH of a 0.35 M aqueous solution of sodium formate

A: Given that , Ka for formic acid = 1.8×10-4 pH of 0.35 M aqueous solution of sodium formate (NaHCO2)…

Q: At pH = 3.9, a weak acid has a concentration of 0.75 M. If the pKa = 4.5, what is the concentration…

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Q: What is the pH of a solution prepared by dissolving 20.26 g of NaOH (strong base) in enough water to…

A: First of all we have to calculate the concentration of NaOH, from which we get the concentration of…

Q: The hydronium ion concentration of an aqueous solution of 0.393 M caffeine (a weak base with the…

A: Caffeine is a weak base with formula C8H10N4O2. Hence it will dissociate partially as per the…

Q: If the pH of a 1.00-in. rainfall over 1800 miles^2 is 3.90, how many kilograms of sulfuric acid,…

A: Given: pH = 3.90Area= 1800 miles2Ka2 = 0.012.

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.