Calculate the pH of a solution (aq., 25 oC) when 20.00 mL of 0.284 M HNO3 is mixed with 30.00 mL of 0.768 M CH3NH2. Kb CH3NH2 = 4.27 x 10–4.

Q: What is the pH and pOH of a 28% KH2PO4?

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Q: Calculate the pH of 2.50M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)

A: The ICE table are utilized to figure out the hydrogen ion's concentration. With the help of hydrogen…

Q: Write the whole acid base equation for the reaction of KOH(aq) with HC4H7O2(aq) b) write the net…

A: (a) Acid base equation  KOH(aq)    +    HC4H7O2(aq)    → KC4H7O2(aq)  + H2O (l)   (b) Net ionic…

Q: What is the pH of a 0.0470 M solution of methylamine (CH&NH2, Kb = 4.4 x 10 4)?

A: Calculate the hydroxide ion concentration released by methylamine. OH- = KbCOH- = 4.4 × 10-4 ×0.047…

Q: Calculate the pH of a solution (aq., 25 oC) when 25.00 mL of 0.250 M KOH is added to 25.00 mL of…

A: Answer :-  pH = 4.20  The pH of a solution, when 25.00 mL of 0.250 M KOH is added to 25.00 mL of…

Q: 1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt…

A: Solving only first question in accordance with guidelines. We will first draw ICE table and then…

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO, is 4.5 x 104)?

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Q: What is the pH of a 0.21 M solution of methylamine (CH3NH2, Kb = 4.4 x 10–4) at 25 degrees C?

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Q: What is the pH of a 0.0730 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A: Given :- concentration of methylamine solution  = 0.0730 M  Kb for methylamine = 4.4 × 10-4  To…

Q: Calculate pH, pOH, [OH-(aq)] and [H;O*(aq)] of a 350.0 mL aqueous solution containing 1.20 g calcium…

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Q: Calculate the pH of a solution that is 1.314 M HF, 0.442 M NaOH, and 0.719 M NaF. For HF K = 7.2 x…

A: Here we have NaOH which is a strong base and will completly dissociate on reacting with HF.

Q: Below is the reaction for the formation of acid rain due to high concentration of atmospheric…

A:

Q: What is the pH of a 0.0650 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: 20.00 mL

A: mmoles of acid = ( 40.00mL • 0.100M ) = 4mmol  mmoles of base = ( 20.00mL • 0.100 M ) = 2mmol

Q: 2. Describe the alkaline error in the measurement of pH. Under what circumstances is this error…

A: The answer to the following question is-

Q: What is the pH of 0.018M C5H5N(aq)?

A: pH is defined as the negative logarithm of the hydrogen ion concentration. The range of pH lies from…

Q: What is the pH of a 0.0490 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

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Q: Calculate the pH of a 0.125 M sodium propionate (NaC3H5O2) solution

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Q: The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its…

A:

Q: Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL…

A: Given,  Mass of CH3COONa = 1.75 g  Molarity of CH3COOH = 0.15 M  Volume of CH3COOH = 53.5 mL  Acid…

Q: 8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a…

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Q: Calculate the pH of a 4.2M solution of hypobromous acid.

A: Ka is the ratio of  product of concentration of products raised to their stoichiometric coefficient…

Q: Calculate the pH of a solution (aq., 25 oC) when 60.00 mL of 0.0500 M NH3 is titrated with 25.00 mL…

A: Ammonia and hydrobromic acid will do acid-base reaction.

Q: What the pH of 0.10 M solution of methylamine (Kb for CH3NH2 is 4.4 x 10*)?

A: A numerical problem based on pH of the weak base, which is to be accomplished.

Q: What is the pH of 0.43 M NH3 solution? (Kb = 1.8 x 105) NH, (aq)+ H,0 (1) NH (aq) + OH (aq)

A: Answer: pOH of solution is equal to the negative of logarithm of hydroxide ion concentration of it…

Q: Calculate the pH of 0.10 M (COOH)½ (aq), oxalic acid. Ka1 = 5.9 x 10-² ; Ka2 = 6.4 x 10-5.

A:

Q: Place the following acids in order of increasing strength: -H​3P​O​4,​ H3P​O​2​ and H3P​O​3.​…

A: We have to explain the acidity order: -H​3P​O​4,​ H3P​O​2​ and H3PO3.

Q: 1. Methanoic acid, HCO,H, also known as formic acid, is partly responsible for the characteristic…

A:

Q: Calculate the pH of the weak acid, lactic acid (HC3H5O3), if the concentration is 0.10 mol/L and the…

A: Given data,Molarity of lactic acid=0.10mol/LKa of lactic acid=1.4×10-4

Q: Calculate the pH of a 0.100 M CH 3NH 3CI solution. Kb for methylamine, CH 3NH 2, is 3.7 × 10 4.…

A:

Q: Calculate the pH of a 1.50 M (CH»),NHB solution (aq., 25 °C). 3) Kb (CH3)N - 6.31 x 105

A: (CH3)3NHBr is a salt of weak base and a strong acid formed by the reaction of  trimethyl amine…

Q: What is the pH of a 0.10 M N(CH3)3(aq)? The base ionization constant  of trimethylamine is Kb=…

A:

Q: Calculate the pH of a 2.0 x 10–3 M solution of pyridine (C5H5N). Kb = 1.7 x 10–9

A: The Bronsted-Lowry acid-base theory was purposed by Bronsted and Lowery is called Bronsted-Lowry…

Q: What is the pH of a 0.0270 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10¬1º)?

A: Here, hydrocyanic acid is weak acid as compared to mineral acids , thus when it ionized it will form…

Q: Calculate the pH of a 0.100 M HC2H3O2(aq) solution.

A: The acid in the given problem is depicted by the formula C2H3O2H is acetic acid . It can be written…

Q: Calculate the pH of a mixture made by adding 54.6 mL of 0.015 M HHNO3(aq) to 142.9 mL of water at…

A: Given,  The pH of a mixture made by adding 54.6 mL of 0.015 M HNO3(aq) to 142.9 mL of water at 26.6…

Q: Acidic water can be treated with basic substances to increase the pH, although such a procedure is…

A: Given Volume of lake = 4x109 L The pH of lake water = 5 -log [H+] = 5 [H+] = 10-5 Therefore the…

Q: Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution…

A: For weak base CH3NH2 : [OH-] = Kb×C          = 4.4×10-4×0.20           = 9.38 x 10-3 M pOH = - log…

Q: What is the pH of a 1.63 M solution of XOH, a weak monobasic compound (Kb = 1.7 x 10^-9)?

A: Given data in above Concentration of XOH = 1.63 M  Kb = 1.7 ×10-9

Q: The Kb of pyridine, C5H5N, is 1.7 x 10−9.  Calculate the pH of a 0.124 M solution of pyridinium…

A: Given: The Kb of pyridine (C5H5N) = 1.7 x 10−9  The molarity of the solution of pyridinium bromide…

Q: In the following reaction in aqueous solution, identify (a) which of the reactants is the acid and…

A: Applying conjugate acid base concept.

Q: 3b.) The Ka of acetic acid is 1.8 x 105. Calculate the pH of the following solutions: b. A solution…

A:

Q: Calculate the pH of a solution (aq., 25 oC) when 50.00 mL of 0.150 M HClO4 is added to 30.00 mL of…

A: Normality = n factor * Molarity  for HClO4 , n factor =1  for Ba(OH)2 , n factor =2

Q: Calculate the pH and the concentrations of all species present in a 0.20 M soltuion of ethylammonium…

A: In this question we have to calculate the pH and concentration of species formed i.e C2H5NH3+,…

Q: Nitrous acid, HNO2 (aq) has a Ka value of 4.0 x 10-4. What is the pH and POH of a 0.0500 M solution…

A: The question is based on the concept of equilibrium. we have to determine PH and pOH   of weak acid…

Q: Calculate the pH of 1.00M acetic acid, HC2H3O2(aq). (Ka = 1.8 x 10-5)

A: Dissociation constant, Ka = 1.8 x 10-5 Concentration of acid = 1 M

Q: 1) Calculate the pH of a solution prepared by dissolving 1.60 g of sodium acetate, CH3COONa, in 64.0…

A: Given; The given mass of CH3COONa, (W)  = 1.6 g. The molar mass of CH3COONa, (M) = 82.0343 g/mol.…

Q: If the pH of a 0.0850 M solution of HBrO2 is 2.29, then what is the value for the acidity constant,…

A: pH = -log[H+] Relation between [H+], Ka and C of a weak acid solution: [H+] = (Ka x C)1/2

Q: If the KbKb of a weak base is 1.6×10−6,1.6×10−6, what is the pH of a 0.18 M0.18 M solution of this…

A: Concentration of the solution is 0.18 M. Kb = 1.6 x 10-6 The Ka value is calculated by following…

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.