The pH of a 0.206 M solution of a weak acid, HB, is 2.59. What is K, for the weak acid?

Q: The hydrogen concentration of a solution is 1 x 10-14 M. What is the pH? pH =  Is this an acid,…

A: Answer: The pH of the solution is 14 and the solution is Basic.

Q: The pH of an acidic solution is 2.19. What is [OH]?

A: The question is best on the concepts of PH. we have to calculate hydroxide Ion concentration.

Q: 6) If the hydroxide ion concentration of a solution is 1.0 x 10° M Is it an acidic or basic…

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Q: The pH of a 0.173 M solution of a weak acid, HB, is 2.53. What is Ka for the weak acid?

A:

Q: Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the…

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Q: The pH of an aqueous solution of 0.223 M sodium hypochlorite, NaCiO (aq), is This solution is (

A:

Q: For sulfuric acid, K >> 1 and K is 0.012. Calculate the pH of a 1.2 M solution of HSO.

A: Assuming the solution is H2SO4

Q: The pH of an aqueous solution of 0.124 M ammonium nitrate, NH,NO3 (aq), is This solution is

A: NH4+ ion released H+ ion in water so concentration of H+ ion is  [H+] = √(Kw × C / Kb )  Where, Kw =…

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: The pH of a 0.205 M solution of a weak acid, HB, is 2.58. What is K, for the weak acid?

A: The given data is as follows: The pH of solution = 2.58 The concentration of weak acid, HB = 0.205 M…

Q: A 0.54 M solution of chloroacetic acid, CICH2 CO2H, has a pH of 1.57. Calculate K, for the acid. %3D

A: Given: The molarity of the solution of chloroacetic acid = 0.54 M The pH of the solution = 1.57 We…

Q: If the molarity of an unknown substance is expressed as 3.7 x 10-5, what is the pH of the substance?

A:

Q: You have a 0.0685 M solution of Ca(OH)2, what is the pH of your solution?

A:

Q: What is the pH of a solution that contains 6.13 x 10–4 M OH–?

A: pH measures the acidity of the solution whereas pOH measures the basicity of the solution -

Q: The pH of a 0.154 M solution of a weak acid, HB, is 2.72. What is K, for the weak acid?

A:

Q: The pH of an aqueous solution of 8.08×10 M sodium hypochlorite, NaCIO (aq), is This solution is

A: Basic salt is the Salt formed from strong base and weak acid solution 8.08 x 10-2 = 0.0808 M NaCIO…

Q: A solution of barium hydroxide at 25 degrees Celsius is 0.125M Ba(OH)2. What is the pH of the…

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Q: The pH of a solution if 6.2. What is the concentration of H3O+ ions?

A: We have to calculate the concentration of H3O+ ion

Q: The pH of a 0.206 M solution of a weak acid, HB, is 2.74. What is K, for the weak acid?

A:

Q: The pH of a 0.70 mol/L weak base solution is 10.22. What is the Kb of the base?

A:

Q: The pH of an aqueous solution of 0.522 M benzoic acid, C6H5COOH is

A:

Q: The pH of a 0.152 M solution of a weak acid, HB, is 2.53. What is K. for the weak acid?

A:

Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.66. What is Ka for the weak acid?

A:

Q: the pH of an acid solution is 3.59. If the concentration of the acid in the solution is 0.200 mol/L,…

A: Given Concentration of the acid=0.2 mol/LpH of the acid solution=3.59Ka of thel acid=??

Q: Calculate the pH for the coffee solution if [H3O+] = 2.0 x 10-5 M.  Is the solution acidic, basic,…

A: Given data, [H3O+] = 2.0 × 10-5 M pH of a solution is pH = - log [H+] H+ exists in solution as H3O+…

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

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Q: The pH of an aqueous solution of 0.486 M acetylsalicylic acid (aspirin), HC,H¬04, is

A:

Q: . What is the pH of a solution that contains 0.35 mol/L of the strons base NaOH?

A:

Q: If the molar concentration of OH- is 1.0 x 10-7, the pH is what?

A: Applying formula of pH  POH= -log[OH-]

Q: What is the pH if the pOH is 2?

A: Given -pOH=2 UsedFormula- pH+pOH=14

Q: The pH of an aqueous solution of 0.129 M potassium fluoride, KF (aq), is ____________. Therefore,…

A: PH of salt :   The solution is acidic, basic or neutral can be predicted as : If pH = 7, the…

Q: The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.

A: Since pKa for phenol is 9.98 and concentration of phenol is 0.508 M (given)

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 4.85 x 10-5 M.

A: The pH of a solution is defined as the -ve logarithm to the base 10 of the value of the hydronium…

Q: Write the formula for the conjugate acid of each of the following bases: (a) HS¯, (b) HCO,, (c)…

A:

Q: 5 mg of HNO3, which is a strong acid, is added to 750 ml of water. What is the final pH of the…

A:

Q: The pH of a 0.229 M solution of a weak acid, HB, is 2.50. What is K, for the weak acid?

A: Given :-  Concentration of weak acid HB = 0.229 M  pH of solution = 2.50  To calculate :-  Ka for…

Q: The pH of an aqueous solution of 0.223 M sodium hypochlorite, NaC1O (aq), is This solution is…

A: pH of salt produced from reaction of weak acid and strong base would be basic and pH of salt…

Q: The pH of a 0.220M solution of a weak acid, HB, is 2.51. What is Ka for the weak acid?

A: Given  PH of weak acid = 2.51  Concentration of weak acid ( c ) = 0.220 M  Ionization constant ( Ka…

Q: Write the formula of the conjugate base of CH:CO2H.

A: In order to identify the conjugate base of CH3COOH, we must know the concept of Conjugate Base.

Q: A 0.051 M weak acid solution, HA, has a pH of 1.95. What is the Ka of the acid

A: [H+]  = (Ka  × C )1/2

Q: The pH of an aqueous solution of 0.223 M ammonium bromide, NH,Br (aq), is This solution is

A: In this question, we want to determine first the pH of the aqueous solution of NH4Br(aq) and then…

Q: The pH of an aqueous solution of 0.136 M sodium nitrite, NaNO2 (aq), is This solution is

A: NaNO2 is a salt of a weak acid (HNO2) and a strong base NaOH pH = 7 + (pKa + log C)/2

Q: 2) A weak acid has a K,= 6.62 x 10. What is the pH of a solution of this acid that is 2.65 M?

A:

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

A:

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

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Q: The pH of a 0.224 M solution of a weak acid, HB, is 2.63. What is Ka for the weak acid?

A:

Q: What are the pH and pOH of 0.075 M NaOH(aq)?

A: Since NaOH is a strong base Hence it will dissociate completely in solution  Since the dissociation…

Q: The pH of an aqueous solution of 0.176 M ammonium bromide, NH Br (aq), is This solution is

A: 1. Solution - According to the question - pH = pH stand for potential of hydrogen, since pH is…

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.