Given 0.114 M HNO2 in water with a Ka for that acid of 4.6x10-4, what is the molarity of NO2-1present in that solution

Q: What’s the PH of a 0.14M HA solution if Ka for HA is 4.0x10^-2

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Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.630 M? (Kb = 1.3…

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Q: A 0.035 M solution of a weak acid (HA) has a pH of 4.88.What is the Kₐ of the acid?

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Q: What is the pH of a solution of 0.300 M HNO, containing 0.180 M NANO,? (Ka of HNO2 is 4.5 x 10-4)

A: Given- Concentration of HNO2=0.300M Concentration of NaNO2=0.180M Ka of HNO2= 4.5×10-4

Q: If the Ka of a monoprotic weak acid is 5.8 × 10-6, what is the pH of a 0.47 M solution of this acid?

A: Given: Ka=5.8×10-6 Molarity of acid = 0.47 M

Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

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Q: 4. A 0.020 M weak acid HA, has a pH of 3.21. What is the Ka of the acid?

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Q: Calculate the percent ionization of formic acid (HCOOH) in a solution that is 0.311 M in formic acid…

A: According to Henderson-Hasselbalch equation Since formic acid concentration given = [HA] = 0.311 M…

Q: Sodium stearate (C17H35COONa) is a major component of bar soap. The Ka of the stearic acid is 1.3 ×…

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Q: The hydronium ion concentration of an aqueous solution of 0.599 M formic acid, HCOOH (Ka =…

A: Given :  Concentration of HCOOH = 0.599 M  Ka = 1.8 x 10-4

Q: Calculate the [OH−] of a solution of 0.1595 M C5H5NH3F if Kb = 1.800e-9 for C5H5NH2?

A: The equilibrium constant for a reaction is expressed in terms of the ratio of the concentration of…

Q: mL, what wi

A: Given as,   Density of solution ρs=1.05gcm-3 volume  of solution infinityv1=50 ml Final…

Q: Four so v s of an acid dissolved in water are sketched below, as if under a micoscope so powerful…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: A 0.050 M concentration of weak base, CH3CH2NH2, was found to ionize at 1.7%. What is the…

A: Interpretation: A 0.050 M concentration of weak base, CH3CH2NH2, was found to ionize at 1.7%. The…

Q: B is a weak base with Kp = (4.11x10^-9). What is the percent ionization of a (7.060x10^-1) M…

A: Since you have asked multiple questions, we will answer only first question for you. In order to get…

Q: A 0.050 M solution of a weak acid HA has a pH of 4.12 at equilibrium. What is the Ka of the acid?

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Q: What is the pH of 0.0100mol.dm3 solution of a weak.,monoprotic acid K3=3.4×10-3 at 25°C?

A: Given concentration(C) = 0.0100mol/dm3 Dissociation constant ( K ) = 3.4×10-3

Q: An acetic acid solution is 1.0% ionized. What should be the concentration of acetic acid and [H +]…

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Q: For an unknown weak acid HA, the Ka is known to be 1x10-5. What percent dissociates in a 0.15 M…

A: In this question, we want to determine the percent Dissociation for a weak acid HA  You can see…

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: At 60 °C, Kw for water is 1.0 × 10¹³. At 60 °C, a weak acid has a Ka of 1.3 x 10-4. What is the Kb…

A: Acid can be defined as a substance that give hydrogen ions in an aqueous solution.

Q: In humans, blood pH is maintained within a narrow range:acidosis occurs if the blood pH is below…

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Q: Calculate the pH of a solution prepared by dissolving 3.90 g of sodium acetate (NAC2H3 of solution.…

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Q: calculate the percent ionization of formic acis in a solution that is 0.322 M in formic acid and…

A: Using Henderson-Hasselbalch equation first, the pH is determined.

Q: Sodium stearate (C₁₇H₃₅COONa) is a major component of bar soap. The Kₐ of the stearic acid is…

A: The pH of 10.0 mL of a solution containing 0.42 g of sodium stearate has to be given, Given, The Kₐ…

Q: An acid solution is made by diluting 30.6 mL of 0.2360 HI to 1.000 L. 1. What is the pH of this…

A: pH measures the acidity of the solution. The concentration of hydronium ion. pH determined as…

Q: THe pOH of 0.5 M solution of weak base is 4.72. What is its pKa?

A: Given-> pOH = 4.72  Molarity =0.5 M

Q: For the diprotic weak acid H2A, ?a1=3.3×10^6 and ?a2=7.7×10^9. What is the pH of a 0.0800 M solution…

A: The Ka values of the diprotic acid, H2A are: Ka1 = 3.3*10-6  Ka2 = 7.7*10-9  Initial concentration…

Q: An acid (HA) dissociates as follows: HA – H+ + A minus Arrow should be interpreted as an equilibrium…

A: Given that,[HA] = 0.80 MpH = 1.42but pH = -log10[H+] [H+] = 10-pH = 10-1.42 = 0.0380 MHA…

Q: Carbonic acid (H2CO3) and bicarbonate ion (HC0;) are used as a buffer system to regulate the blood…

A: Given,  Ka of H2CO3 = 4.2 x 10-7  pH = 7.15

Q: In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was…

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Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11. What is the…

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Q: Kb for NH3 is 1.8 × 10-5. What is the pH of a 0.45 M aqueous solution of NH4Cl at 25.0 °C? Show

A: This question is related to salt hydrolysis of salt. By applying certain formula for that, required…

Q: How many moles of benzoic acid, a monoprotic acid with Ka = 6.4 × 10–5, must be dissolved in 650. mL…

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Q: NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a…

A: Given : concentration of NH4Cl = 0.088 M Since the salt given is a soluble ionic salt. Hence it will…

Q: A 0.100 M solution of bromoacetic acid (BrCH2COOH) is13.2% ionized. Calculate [H+], [BrCH2COO-],…

A: Solution of bromoacetic acid, 0.100M is ionized 13.2%. The percent ionization is defined as ratio of…

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HBrO, at 25oC is 4.48. What is the value of…

A: The concentration of HBrO solution = 0.55 M. pH of aqueous HBrO solution = 4.48.

Q: ASA (also known as Aspirin) contains acetylsalicylic acid, C16H12O6. Acetylsalicylic acid is a weak…

A: 0.015 mol/L acetylsalicylic acid has a Ka of 3.3 × 10-11.We have to calculate the pH and pOH at…

Q: What is the pH of a 0.870 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 × 10*)?

A: dissociation of Ca(NO2)2 Ca(NO2)2(aq)→Ca2+(aq)+2NO2-(aq) we can see 2mol of NO2- is formed from 1…

Q: The Ka of hypochlorous acid (HClO) is 3.0*10-8 at 250C. What is the % ionization of hypochlorous…

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Q: a) Write a balanced equation representing the reaction of the acid, H2PO4- with the base, water.…

A: a) Balanced chemical equation =  H2PO4-(aq) + H2O(l) ⇔ HPO42-(aq) + H3O+(aq)

Q: True or false ___________1. The acidity of the solution is higher with higher pH. ___________2. pH…

A: In the given question we have to do True or false of the following question.  1.  False ,  because…

Q: 5. Calculate the pH of a solution that is 0.050 M NH, and 0.150 M NH,CI. The Ka=5.62 x 10-10 for…

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Q: By mixing 3L of 2M H2SO4 and 4L of 2M NH4OH , the produced solution will be ......... a) Acidic b)…

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Q: Calculate the pH of the following solutions: a) 400ml containing 7.5g Na2CO3 + 6g NaHCO3.

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

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.