A weak acid has K a = 1.00 × 10 -3. If [HA] = 1.00 M what must be [A -] for the pH to be 2.7?

Q: A weak acid, HA, has a p?apKa of 4.5424.542. If a solution of this acid has a pH of 4.4944.494, what…

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Q: The weak acid HZ has a Ka of 2.55 x 10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

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

A: The equilibrium reaction given is, => HA --------> H+ + A-  Given : Initial concentration of…

Q: Calculate [H+ ], [OH- ], pH and pOH of 2.00 M (weak acid) HF (Ka=6.8 x 10 -4)

A: We have to calculate the hydrogen ion , hydroxide ion concentration , pH and pOH.

Q: 7. A 0.10 M solution of a weak monoprotic acid, HA, nas a pH of 3.14. What is the acid-ionization…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: 1. Calculate the pH of each of the following solutions of a strong acid in water. a. 0.10 М НСІ b.…

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Q: HCIO is a weak acid (Ka = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Ka of HClO = 4.0 × 10-8 Concentration of the solution of NaClO = 0.089 M pH =?

Q: 1    Calculate the pH of a 0.02 M solution of the weak acid, HA.         Ka = 2.46 X 10 –4…

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Q: What is the equilibrium pH of an initially 0.37 M solution of a weak acid HA at 25°C? Ka = 4.89 x 10…

A: Acid dissociation constant Ka is utilized to determine the acidic and basic nature of a solution. It…

Q: Would you expect a solution of ammonium chloride (NH4Cl) to be acidic or basic when added to water?…

A: Introduction- For the salts of strong acids and strong bases, the pH of salt will be neutral that is…

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: 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: For the diprotic weak acid H2A, Kal = 3.9 x 10-6 and K22 = 7.7 x 109 What is the pH of a 0.0400 M…

A: The hydronium ion concentration can be calculated using ICE table as,

Q: Calculate the OH concentration and pH of a 6.1 x 10-3 M aqueous solution of sodium cyanide, NaCN.…

A: Since NaCN is a salt of weak acid and strong base, the pH of the given solution can be determined as…

Q: A weak acid HA has a Ka of 5.3x10-5. A solution of HA has a pH of 3.00 a) Calculate the initial…

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Q: Suppose that ammonia, applied to a field as a fertilizer, is washed into a farm pond containing 3.0…

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Q: HCIO is a weak acid (Ka 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: Given data; Ka=4×10-8Also, Kw=Ka×KbAnd,Kw=1×10-14 Consider the dissociation of given weak acid as;…

Q: Which acid listed below is the weakest? O Hydrogen sulfide, H2S, Ką = 9.5 x 108 Citric acid,…

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Q: Show complete calculations for the pH of a 0.105M solution of ammonium chloride. The Kb for ammonia…

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Q: For a solution of an aqueous hypochlorous acid solution, the Ka is 5.0 x 10-8 and [HOCI] is 0.050M.…

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Q: Hydrofluoric acid (HF) is a weak acid with a Ka = 7.1 x 10-4. What is the pH of a 0.50 M solution of…

A: Given acid is a weak acid, so it will not completely dissociate into products.Construct ICE table…

Q: Which would have a higher pH, a solution whose pOH is 5.00 or a solution whose hydrogen ion…

A: pH of solution is calculated based on the hydrogen ion concentration. pH = -log[H+] pH = 14 - pOH

Q: If the Ka of a monoprotic weak acid is 3.4 × 10-6, what is the pH of a 0.30 M solution of this acid?

A: The dissociation of a weak acid is written as:

Q: HA is a weak acid. Its ionization constant, Ka, is 2.4 x 10-13. Calculate the pH of an aqueous…

A: Given : The solution has salt NaA with concentration 0.063 M Since NaA is an ionic salt. Hence it…

Q: What is the pH of (3.21x10^-1) M C5H5NHBr?

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid…

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Q: What is the pH of a solution which is 0.023M in weak base and 0.039 M in the conjugate weak acid (Ka…

A: This question can be solved using Henderson-Hasselblach equation. The equation is, pH=pKa+…

Q: Kb for ammonia (NH3) is 1.76 x 10-5     What is Ka for ammonium, its conjugate acid. (NH4+)

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Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The Ka of a weak monoprotic acid is 1.85 x 10-5. What is the pH of a 0.0761 M solution of this acid?

A: First, we have calculated the concentration of [H+] with the help of Ka and the concentration of the…

Q: If the Ka of a monoprotic weak acid is 8.3 × 10-6, what is the pH of a 0.19 M solution of this acid?

A: Given, Concentration of monoprotic weak acid = 0.19 M Ka of monoprotic weak acid = 8.3 × 10-6

Q: 5. Calculate the pH of a 0.350 M CH;NH2 solution. The Kb for this weak base is 4.4 x 10ª.

A: The pH of a 0.36 M methylamine (weak base) (CH3NH2) solution is to be calculated, if Kb = 4.4 x…

Q: The Ka for niacin is 1.5 x 10-5. Whatis the pH of a 0.010 M solution of niacin?

A: The dissociation reaction of niacin is as shown below Hence we can see that 1 molar concentration…

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: given  HClO Ka=4.0 x 10-8  concentration of  NaClO IS 0.027  PH =?

Q: What will be the H+ concentration in a 0.25 M solution of a weak acid (HA), of Ka = 6.9x10-3 What…

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Q: Solutions of sodium salts of the acids in the following table are prepared with an initial…

A: Dissociation of a weak acid is given by: HA  ⇌  H+  +  A- The acid dissociation constant of this…

Q: A particular base has Kb= 4.4*10^-4. What is the pH of 0.35M solution of this base ?

A: Since the Kb value is less so the dissociation of base is very less and it is assumed that the…

Q: The organic acid RCOOH has a Ka = 4.1e-5. What is the pH of a 0.50M aqueous solution of this acid?

A: given, Ka = 4.1e-5 [RCOOH]= 0.50M

Q: What is the theoretical pH of a 0.10 M NH4Cl solution when the Kb for NH3 is 1.8 x 10^-5?

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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: For H2CO3, Ka1= 4.3 x 10^-7, Ka2= 4.7 x 10^-11. What is the pH of a 0.28 M solution of carbonic…

A: H2CO3 is a weak acid.  pH = 0.5pKa - 0.5logC ....(1) Here, pKa1 = -logKa1 = -log(4.3*10^-7) = 6.37…

Q: What is the pH of a 0.010 M solution of HF? The Ka for HF is 6.8 x 10^-4.

A: Given,   Concentration of HF = 0.010 M  Ka for HF is = 6.8x10-4

Q: M CH3COOH?

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Q: If the Ka of a monoprotic weak acid is 1.6 x 10-6, what is the pH of a 0.37 M solution of this acid?…

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Q: 7. This weak monoprotic acid, HZ, can be found in many berries. Calculate the Ka of this acid if the…

A: Ka is the dissociation constant of the acid. An acid dissociate in water and the dissociation…

Q: The Ka of a weak monoprotic acid is 1.13 x 10-5. What is the pH of a 0.0777 M solution of this acid?…

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Q: A 10° C solution has a pH of 8.0 . At this temperature , K w =2.93 x 10^ -15 . What is the pOH of…

A: Kw is an equilibrium constant, which is known as ionic product of water. It is the product of the…

Q: HCIO is a weak acid (K, = 4.0 x 10-8) and so the salt NaCIO acts as a weak base. What is the pH of a…

A: pH = 7 +12 (pka + log c)

Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

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Q: 1 Calculate the pH of the following strong base and strong acid solutions: а. 0.075 M Ca(Он) b.…

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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.