What concentration of an aqueous solution of NH4+ has the same pH as that of 6.8 × 10–5 M HCl? The pKb of NH3 is 4.74

Q: El producto principal de la siguiente reacción es HCI OH II II IV

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Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: What is the pH of a solution with [H3O+]=2.42 x 10-4?

A: pH of any solution is given by  pH = -log[H3O+] where [H3O+]= concentration of H3O+ ions

Q: For H2CO3, Ka1 = 4.3 × 10–7, Ka2 = 4.7 × 10–11. What is the pH of a 0.36 M solution of carbonic…

A: We have to predict the pH of 0.36 M of carbonic acid .

Q: CH₂NH₂ is a weak base (K₁ = 5.0 x 10-4), so the salt CH₂NH₂NO3 acts as a weak acid. What is the pH…

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Q: What is the concentration of H+ ions in HCl whose pH is 6.9?

A: Chemical equation of dissociation of HCl is given by, HCl------------> H+ + Cl- Given pH= 6.9 or…

Q: What is the hydronium concentration [H3O+] of a solution with a pH of 7.84?

A: We have given that pH is a measure of the hydrogen ion activity usually in aqueous solution.  pH =…

Q: What concentration of oxalic acid, HOOCCOOH(H2A), will have a pH of 2.50 (pKa1 = 1.25; pKa2 = 4.14)?

A: Given:pH = 2.5pKa1 = 1.25pka2 = 4.14The pH of a solution is determined using the negative logarithm…

Q: What is the pH of a 0.190 M C6H5CO2H M solution if the K₂ of C6H5CO2H is 6.5 x 10-5?

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Q: a) Label each species as an Bronsted-Lowry acid or base. Show the conjugate acid-base pairs. HCO; +…

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Q: Calculate the concentration of H2CO3 and HCO3 in a 0.175 M M solution of H2CO3. (Ka1 = 4.3 × 10-7…

A: Answer:Electrolytes that ionize partially upon adding in water are called weak electrolytes. Due to…

Q: 1. Which of the following solutions are acidic? Which are basic? Distilled H2O NaCl NH4Cl NaCH3COO…

A: Salt of strong acid and strong base is neutral  Salt of strong acid weak base is acidic  Salt of…

Q: Calculate the pH and the pOH of these solutions:     (a) 0.257 M HBr pH =   pOH =     (b) 0.332 M…

A: Since you have posted a question with multiple sub-parts, we will solve first two subparts for you.…

Q: Propionic acid, HC3H5O2, has Ka= 1.34 x 10–5. (a) What is the molar concentration of H3O+ in 0.15 M…

A: HC3H5O2 is a weak acid and dissociates in aqueous solution as: HC3H5O2+H2O↔C3H5O2-+H3O+

Q: In a titration experiment, 32.45 ml of 0.200 M NaOH were required to neutralize 25.00 mL of H2SO4.…

A: Sulfuric acid and sodium hydroxide are strong acid and strong base respectively. They furnish the…

Q: If 0.015 moles of Fe2(SO4)3 is dissolved in enough water to make 2.5 L of solution. What is the Eq/L…

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Q: Calculate the pH and the pOH of these solutions:   (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH =   pOH…

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Q: equilibrium constant, K, for this reaction.

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Q: The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH3NH3* and 0.117…

A: TThe base is the substance that gives OH- or accepts H+ ions in solution. The Henderson Hasselbalch…

Q: What was the original 1. concentration (M) of an aqueous acetic acid (CH3COOH) solution whose pH is…

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Q: 13.3.00 g of pure acetic acid (CH3COOH) is diluted to 25.0 L, What is the PH of the solution? Ka =…

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Q: Given that pKa = 3.14 at 25 deg C for HNO2, what is the pH of 0.173 mol L-1 NaNO2(aq) at 25 \deg C?…

A: The objective of the question is to calculate the pH of a 0.173 mol/L NaNO2 solution at 25°C and the…

Q: The molarity of an aqueous solution of NaOH is 0.0022 M. (a) What is the concentration of H3O+ in…

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Q: needs from the soil if its pH is above 6.5. (a) The hydrogen ion concentration of a soil sample is…

A: A) [H+] =1.58×10-7 pH = -log([H+])  = -log(1.58×10-7) = 6.8 So, pH = 6.8

Q: Calculate the pH of a 0.591 M aqueous solution of benzoic acid (CH₂COOH, K₂ = 6.3x10-5). pH =

A: Here,concentration of benzoic acid = 0.591 MKa = 6.3×10-5We have to find out pH.. Herw first we need…

Q: What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when…

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Q: What is the pH of a 0.138 M solution of H2SO4 (sulfuric acid)?

A: We will use formula of pH

Q: Calculate the pH of a 8.3 x 10-3-M solution of H2SO4 (K, = 1.2 x 10-2). %3D pH =

A: The given acid is H2SO4. It dissociates in solution to give two moles of H+ ions. The given…

Q: What is the pH of a 0.20 M solution of CH3NH3NO3 at 25 °C? At this temperature, the K₁ for CH3NH2 is…

A: Given:Given is a solution of CH3NH3NO3Concentration of solution = Temperature = 25oCThe pH of a…

Q: What is the pH of a solution that has an H+ concentration of                        (a) 1.75 × 10 –5…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: 3. For the following Lewis acid-base reaction, identify the acid, the base, and the new covalent…

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Q: What is the pH of a solution that is 0.0530 M in NaClO at 25 °C? The Ka for HClO is 4.0×10−8

A: Given thatConcentration of NaClO = [ClO–] = 0.0530 MKa for HClO = 4.0×10−8Kb for ClO– =

Q: Mel Ph -Br ~ F 2 3 Br 4 Ph · Cl

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Q: The base protonation constant K₁ of morpholine (C₂H₂ONH) is 2.14 × 100. Calculate the pH of a 0.41 M…

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Q: A diprotic acid (H₂A) has Kal = 4.54 x 10-7 and K₁2 = 5.59 x 10-11. What is the pH of a 0.396 M H₂A…

A: we have to calculate the pH of 0 .396 M diprotic weak acid

Q: Given 0.01 M solutions of each of the following acids, which solution would have the lowest pH? O…

A: The objective of the question is to determine the solution with the lowest pH.

Q: It is found that 41.27 ml of 0.2017 M NaOH is required to neutralize 25.00 ml of HNO3 solution in a…

A: Given : Molarity of NaOH = 0.2017 M Volume of NaOH solution required = 41.27 mL And volume of HNO3…

Q: What is the pH of a 0.40 M solution of benzoic acid, C6H5COOH?

A: Given information: Concentration of benzoic acid = 0.40 M

Q: 3. Consider the following acids Acid Acetic Acid, H CCO-H Trichloroacetic Acid, Cl-CCO,H…

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Q: 2 Na2CO3+Pb(OH)4= Pb(CO3)2 + 4 NaOH TOTAL IONIC EQN: net iomice eqn:

A: We are given a balanced chemical equation and we have to write the total and net ionic equation for…

Q: Suppose a 0.25 M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the equilibrium…

A: Given,Concentration of aqueous Phosphoric acid solution = 0.25 MRequired,…

Q: Carbonic acid (H;CO:) is widely used in the production of sodas, soft drinks, sparkling wines, and…

A: a.) Carbonic acid is a diprotic acid so it have two acidic protons and hence two ionization…

Q: f) Calculate the pH of the following solutions: (i) A 0.045 M solution of sulphuric acid. (ii) A…

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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.