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 solution that is 0.059 M in NaCIO at 25 °C? pH =

Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is 1.8 x 10-5

A:

Q: What is the pH of a 0.178 M aqueous solution of sodium cyanide, NaCN at 25 "C7 (K, for HCN= 4.0-10

A: The given information is: Concentration of sodium cyanide = 0.178 M Ka for HCN = 4.0 x 10-10 The…

Q: Calculate the concentration of OH and the pH of a solution that is 0.20 M in aqueous NH3 and 0.10 M…

A: This is basic buffer question.

Q: If the K of a weak base is 8.5 x 10-6, what is the pH of a 0.27 M solution of this base? pH =

A:

Q: The value of K, is 2.55 x 10 for a weak monoprotic acid whose initial concentration is 0.244 M. What…

A:

Q: What is the pH of a solution which is 0.021 M in weak base and 0.039 M in the conjugate weak acid…

A: We have a buffer system of weak base (0.021M) and conjugate weak acid (0 .039M) . We also have the…

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: what is the ph of a solution that is 0.100 m in hydrofluoric acid? The Ka of hydrofluoric acid is…

A: Recall the following expression to find pH of the given solution of hydrofluoric acid. Given that…

Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

Q: HCN is a weak acid (Ka=6.20×10−10), so the salt, KCN , acts as a weak base. What is the pH of a…

A: Ka = 6.20×10-10 pKa = -log(Ka)    = -log(6.2×10-10 = 9.21  Concentration(C) of salt =0.0750 M

Q: What is the pH of a solution consisting of 0.70 M HC2H3O2 and 0.60 M NaC2H3O2 ? The Ka of HC,H3O2 is…

A:

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

A: Kw = Ka x Kb  Kw = 1x10-14  given that Ka = 4x10-8 find Kb = (1x10-14) / (4x10-8) = 2.5x10-7 Initial…

Q: Calculate the pH of the following solutions: a. 2.0 M morphine hydrochloride, C,„H,„NO,•HCI (pK, =…

A: In order to solve this question, we will be using simple concepts of chemical and ionic equilibrium.…

Q: Barbituric acid, HC4H3N2O3, is a weak acid that is used to prepare various barbiturate drugs (used…

A:

Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?

A: Given data,pH=2.13Molarity of HA=0.45

Q: If the Ka of a monoprotic weak acid is 7.8×10−6, what is the pH of a 0.47 M solution of this acid?

A:

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: A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant (Ka)…

A: Given:

Q: If the Ka of a monoprotic weak acid is 5.8 x 10-6, what is the pH of a 0.12 M solution of this acid?

A: Negative logarithm of Concentration of [H+] ion present in the solution is known as pH of the…

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

A:

Q: How many moles of NH3 must be dissolved in water to give 813.0 mL of solution with a pH of 11.15? Kb…

A: The value of Kb for the given weak base is = 1.8x10-5 The concentration of the base solution is =?…

Q: If 0.050 moles of gaseous HCl is bubbled in 1.0 liter of a solution that is 0.15 M in NH3 and 0.10 M…

A: When an acid is added to a weak base buffer solution, the concentration of weak base decreases where…

Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

Q: Ammonia is a weak base that is a household cleaner and has a Kb =1.8 x 10-5. What is the pH of a 3.0…

A: Given: Kb =1.8 x 10-5Concentration = 3.0 M pH = ?

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

A:

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

A:

Q: If the K, of a weak base is 3.9 x 10-6, what is the pH of a 0.48 M solution of this base?

A: Kb- is a dissociation constant of weak base. Formula is, pOH - pOH is defined as negative logarithm…

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:

Q: The K, of a weak monoprotic acid is 1.65 x 10-5. What is the pH of a 0.0859 M solution of this acid?…

A: In this question, we want to determine the pH of the weak monoprotic acid,  How we can determine the…

Q: 500

A: Dear student I have given answer to your question in the image format.

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: 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: The Ka for cyanic acid HOCN is 3.5 x 10-4. What is the pH of a 0.37 M solution of the acid? What is…

A:

Q: The K₂ of a weak monoprotic acid is 1.74 x 10-5. What is the pH of a 0.0939 M solution of this acid?…

A:

Q: A 0.150 M solution of a weak base has a pH of 9.65. What is the base hydrolysis constant, K, for the…

A:

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

A:

Q: The pH of a 0.060 M weak monoprotic acid, HA is 3.44. Calculate the Ka of the acid.

A:

Q: If the Ka of a reaction is equal to 1.8x10-5, which is favored- the products or the reactants? How…

A: If Ka of reaction is 1.8 x 10-5 then reaction is reactant favoured because value of equilibrium…

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

A: pH is defined as negative logarithm of hydrogen ions.

Q: 1.4 A 0.015 M solution of hydrogen cyanate , HOCN, has a pH of 2.67 a) What is the hydronium ion…

A: Given: The pH of the solution of hydrogen cyanate is 2.67. The molarity of hydrogen cyanate is 0.015…

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: HCN is a weak acid (?a=6.20×10^−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: Given, HCN is a weak acid with Ka =6.20×10-10 and so the salt, KCN acts as a weak base.we are asked…

Q: The pH of a 0.16 M solution of a weak acid, HA, is 2.85. What is the value of Ka for the weak acid?

A: The question is based on the dissociation of weak electrolyte. We  have been given a weak Acid which…

Q: Calculate the pH of a solution that is 0.450 M HC2H2O2 and 0.730 M NaC2H3O2. The Ka for acetic acid…

A: This problem is solved by using Henderson Hassel baltch equation.

Q: Determine the pH of a solution of a weak acid (HA) that is 0.0072 M. The Ka of the weak acid is 1.9…

A: Given ,  Weak acid is HA Concentration of weak acid (C) = 0.0072 M Dissociation constant (Ka) of the…

Q: (Q12) Hydrazoic acid (HN3) is a weak acid with a Ką of 2.5 x 10³. What will be the equilibrium pH of…

A: We need to calculate the pH of hydrazoic acid at equilibrium

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:

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?…

A:

Q: If the Ka of a monoprotic weak acid is 4.7 x 10-6, what is the pH of a 0.49 M solution of this acid?…

A: Given Ka = 4.7 x 10-6 C = 0.49 M

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)

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.