Calcualtw the pH of a 0.217 M HC7H5O2 aqueous solution. Ka for HC7H5O2 is 6.5 x 10^-5.

Q: Hydrofluoric acid, HF(aq), is a weak acid with Ka = 3.5 x 10–4. What isthe pH of 0.10 M HF(aq)?

A: Answer :- Acid dissociation constant :- The equilibrium constant for an dissociation of acid is…

Q: dissociated H+H+ ions

A:

Q: The pH of an aqueous solution of 0.528 M benzoic acid , C,H;COOH is

A: Benzoic acid is a weak organic acid. It does not dissociates completely rather maintains equilibrium…

Q: Calculate the pH of a weak base which dissociates as   BOH ⇌ B+ + OH-   ( like  NH3 (g) + H2O(l) →…

A: The dissociation reaction taking place is BOH ⇌ B+ + OH-

Q: What is the pH of a 0.0520 M solution of HONH,CI (Kb of HONH, is 1.1 × 10*)? 2

A: Solution :      Weak bases show partial ionization on dissociation in an aqueous solution. Here…

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: If an acid, HA, dissociates to 0.1% when added at a final concentration of 0.05M in water, that is:…

A: 1- First calculate the H3O+ ion concentration :  [H3O+] = ( Concentration ) × ( Degree of…

Q: The pH of an aqueous solution of 4.45x102 M ammonium bromide, NH,Br (aq), is This solution is

A: NH4Br is a salt of weak base and strong acid. We have to determine pH of an aqueous solution of…

Q: What is the pH of a 0.750 M solution of C,H,NHB (Kb of C,H̟N is 1.7 10°)?

A:

Q: The pH of a 0.0833 M ethanoic acid (Ka=1.8x10-5) solution is

A:

Q: The pH of a 0.550 M of weak base, A-,  is 9.93 at 25. What is the Kb of the base?

A: Since the base given is a weak base. Hence it will undergo partial ionisation as per the below…

Q: An aqueous solution at 25 ∘C is 14.7% HNO3 by mass and has a density of 1.043 g/mL. What is the pH…

A: The acidity of a solution depends on the concentration of the [H]+ ion. The pH is the most…

Q: What is the pH of a 0.580 M solution of NaCN (Ka of HCN is 4.9 x 1010)?

A:

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: The pH of an aqueous solution of 0.353 M aniline (a weak base with the formula C¿H2NH,) is

A: pH - pH is defined as negative logarithm to the base 10 of H+ ion concentration. Mathematically, pH…

Q: The pH of aqueous 0.10 M pyridine (C5H5N) ion is 9.29. What is the Kb of this base

A: Given , Concentration of pyridine (C) = 0.10 M pH of pyridine solution = 9.29 Dissociation constant…

Q: What is the pH of a 0.380 M solution of NACN (Ka of HCN is 4.9 x 1010)?

A:

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: Calculate the pH of an acqueous solution; 0.0025M Hl

A: HI is a strong acid. 0.0025 M HI results in release of 0.0025 M hydrogen ions.

Q: What is the pH of a 0.730 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: Interpretation: The pH of a 0.730 M solution of NaCN is to be determined. Ka of HCN = 4.9 × 10-10

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: The pH of a solution at 25°C in which [OH]= 2.0 x 10 is: 1 9.52 4.76 4.69 3.30 9.30

A: In this question, we want to determine the pH of the Solution.  You can see details Solution below…

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

A:

Q: dissociated H+H+ ions

A:

Q: If you measure the pH of a carbonic acid solution to be 5.6, what is the concenration of the H3O+ in…

A: pH of carbonic acid=  5.6[H3O+ ] = ?

Q: Pyridine, C5H5N, is a toxic, foul­smelling liquid for which Kb = 1.7 × 10 ­9 . What is the pH of a…

A:

Q: What is the pH of a 0.0380 M solution of HONH,CI (Ka of HONH,+ is 9.1 × 10-7)?

A:

Q: What is the pH of a solution that is prepared by adding 4.0 mL of 0.50 M NAOH(aq) and 4.0 mL of 0.40…

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Q: What is the pH of a solution that is 0.071 M LiCN at 25°C?

A: A solution is made up of 0.071 M LiCN at 25 ◦ C. Here, we have to calculate the pH of the solution.…

Q: The hydroxide ion concentration, [OH], of an aqueous solution of 0.453 M pyridine (a weak base with…

A:

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: What is the pH of a 0.690 M solution of NACN (Ka of HCN is 4.9 x 10 10)?

A: Given, The concentration of the solution of NaCN = 0.690 M Acid dissociation constant (Ka) = 4.9 x…

Q: The hydroxide ion concentration of an aqueous solution of 0.325 M phenol (a weak acid) , C6H5OH, is…

A:

Q: The pH of a O.0086 M solution of Ca(OH)2 is

A: The negative logarithmic concentration of hydrogen ion concentration in as solution is called pH. It…

Q: The pH of a normal raindrop is 5.60. Compute the con- centrations of H,CO;(aq), HCO; (aq), and CO3…

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

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Q: A. One simple way to measure the [H] is to measure pH. If a 10.0mL solution of "acid rain" is…

A: In mixture of strong acid and weak acid pH depends on H+ ion concentration of strong acid.

Q: The pH of a 1.50 M solution of anilinium chloride (C6H5NH3Cl) is _____.   Kb(C6H5NH2) = 4.3 × 10‒10…

A: Given,Kb(C6H5NH2) = 4.3 × 10‒10[C6H5NH3Cl] = 1.5 M

Q: Q6) 200 ml , o.0ol M NAOH is udded to 30oml, o.0005 M HCL. what is the PH of the Soluution ? Ans. :…

A: The balanced Chemical Reaction between HCl and NaOH is - HCl + NaOH ----> NaCl + H2O Here, one…

Q: The hydronium ion concentration of an aqueous solution of 0.558 M isoquinoline (a weak base with the…

A:

Q: The pOH of an aqueous solution of 0.468 M formic acid, HCOOH is _____  .

A:

Q: What is the pH of an aqueous solution of 0.005 M C6H5O- at 298 K of the Ka for phenol at the given T…

A: Given: Concentration of C6H5O- = 0.005 M And Ka of C6H5OH = 1.0 × 10-10

Q: A solution is prepared at 25 °C that is initially 0.29M in chloroacetic acid (HCH,CICO,), a weak…

A:

Q: The pH of an aqueous solution of 0.390 M methylamine (a weak base with the formula CH;NH2) is

A: 12.09

Q: The pH of an aqueous solution at 25.0 °C is 12.36. What is the molarity of H + in this solution?

A: Given information,      The pH of an aqueous solution at 25.0 °C is 12.36

Q: The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature.  What is the initial…

A: Answer:- This question is answered by using the simple concept of calculation of initial…

Q: _s the pH of an aqueous solution that is 0.1M NH4C1?

A:

Q: In the given equation: HCOOH (aq) + H2O (l) ↔ H3O+ (aq) + HCOO– (aq), the initial concentration of…

A:

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

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.