Calculate the pH of a 0.325 M solution of a weak base whose conjugate acid has a pka-5.155.

Q: Another way to express acid strength is by using pk b:pK a =−logK a Another way to express base…

A: Acidic strength and dissociation constant (Ka) are interrelated concepts. Lower is the value Ka,…

Q: A solution of 0.20 M hydrazoic acid has a pH of 3.21. What is the Ka of hydrazoic acid?

A: We have to calculate the Ka of acid.

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: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: A weak acid has a Ka = 5.78x10. What is its pK3? %3D 9.244 8.238 O 1.660 0.999

A: Given, the Ka for a weak acid = 5.78 × 10-9 We have to calculate the pKa of the acid.

Q: A solution of a weak acid has a concentration of 0.64 M and is found to have a pH of 3.77. What is…

A: The dissociation of a weak acid can be depicted as follows.           HA   +H2O ⇔    A-  +  H3O+I…

Q: The acid ionization constants for species that are listed below can be found by using data given in…

A: The Ka value will be more for strong acids. Ka for H3PO4 = Ka1 x Ka2  x Ka3 = (7.5 x 10–3)( 6.2 x…

Q: The K₂ for a base is 15.3 x 10-13. What is the Ka for its conjugate acid?

A: Given :- kb for a base = 15.3 × 10-13  To determine :- value of Ka for its conjugate acid

Q: Lactic acid (HC3H5O3) has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44.…

A: Given data is as follows: The concentration of lactic acid = 0.10 M The pH of the solution = 2.44 Ka…

Q: What is the Ka of the acid in a solution that is 0.34 M in the acid, and 0.247 M in the conjugate…

A:

Q: The acid dissociation constant Ka of hydrocyanic acid HCN is ×6.210−10. Calculate the pH of a 1.6M…

A: The acid dissociation constant, Ka, of hydrocyanic acid HCN is 6.2×10−10. The pH of a 1.6 M solution…

Q: a general chemistry student measured the pH of a 0.510 M aqueous solution of nitrous acid to be…

A: Here we are required to find the dissociation constant for weak acid nitrous acid

Q: Calculate the pH of formic acid (HCOOH) of 10-2 M (Ka) if the acid ionization constant(Ka) is…

A: Given: Initial concentration of HCOOH = 10-2 M Acid ionization constant (Ka) of HCOOH = 6.75 x 10-4…

Q: According to the following pKa values listed for a set of acids, which would lead to the strongest…

A:

Q: Hydrogen cyanide, HCN, also called hydrocyanic acid is a weak acid with a pKa near 10. What would be…

A:

Q: A 0.12 M solution of hypoiodous acid has a pH of 5.71. Calculate the acid-dissociation constant (Ka)…

A: Solution:- Reaction:-  HIO (aq) + H2O (l) → H3O+ (aq) + IO- (aq) Concentration of HIO = 0.12 M pH =…

Q: Calculate the pH of a 0.05 M solution of iodic acid. Ka for iodic acid = 0.17

A:

Q: Ethylamine (C2H5NH2) has a Kb value of 4.5x10–4. Calculate the pH of a solution that is 0.00789 M…

A: Interpretation - To calculate the pH value of the 0.00789 M ethylamine solution when ethylamine…

Q: Calculate the pH of a 0.25M solution of formate ion (HCOO-) at 250 C.  The pKa for formic acid…

A:

Q: Calculate the pH of a 0.033 M Na2SO3 solution. pK1 = 1.66 and pK2 = 6.85 for sulfurous acid (H2SO3)…

A:

Q: Which of the following is considered a Lewis base? Cl- Cu2+ BCl3 NH4+ Mn2+

A: Which of the following is considered a Lewis base?

Q: Calculate the pH of the following solutions: a. 0.34 M hydrocyanic acid. b. 1.5 M solution of…

A: pKa of hydrocyanic acid is 9.2

Q: Common aspirin is acetylsalicylic acid, which has the structure shown below and a pka of 3.5.…

A: Given mass of aspirin = 6.5 × 102 mg = 650 mg  Mass of water = 8 ounces = 8 × 28.35 g  = 226.8 g…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A:

Q: Calculate the pH of a 0.0644 M anilinium chloride solution. pH= Calculate the concentrations of…

A: Let us consider a ICE table below, HA = conjugate acid = 0.0644 M (anilinium chloride ) A- =…

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: a 1L, 0.1M, pH = 7.4 buffer solution. The weak acid is 0.5M, pKa = 8.6. The conjugate base is 0.1M.…

A:

Q: conjugate base is amphiphrotic/amphoteric if the given pka values are

A: Acid which has higher value of Ka, is the strongest acid. HClO4 is strongest strong

Q: Which of the following is the conjugate base of the bicarbonate ion, HCO3-? Group of answer choices…

A: The conjugate bases/alkali or acid concept is furnished in Bronsted-Lowry theory. Any acid gets…

Q: c. H20 = Lewis Base (donate 10. Calculate the pH of 0.3M solution of NH,Br if Ka of NH4* = 5.6x10-10…

A: The pH of a 0.3 M solution of NH4Br is to be calculated if Ka of NH4+ = 5.6×10-10

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: a 0.55 M solution of a monobasic compound B has a pH of 11.32, what is the Kb value of the base B

A:

Q: What is the Ka of bromoacetic acid if a 0.035 M bromoacetic acid aqueous solution has a pH of 2.22?

A: Let us take a reaction,        HX = H+ + X-  The dissociation constant of the above reaction is,  Ka…

Q: A 0.015 M solution of hydrogen cyanate (HOCN) has a pH of 2.67. Calculate the hydrogen cyanate…

A: Calculate the concentration of hydronium ion:

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: For first ionization :  pH = 0.5pKa1 - 0.5logC ..(1) Here, pKa1 = -logKa1 = -log(8*10^-5) = 4.097 C…

Q: Find the pH of a 0.247 M NH4Cl solution given that the Kb of NH3 = 1.8x10-5 at 25 °C. 11.32 2.68…

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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…

A:

Q: Calculate the pH of a solution that is 1.8*10^-3 M morphine if the pKa of its conjugate acid is 8.21

A: We have to predict the pH of the morphine solution.

Q: Sulfurous acid (H2SO3) is a diprotic acid with ?a1=1.39×10^(−2) and ?a2=6.73×10^(−8). Determine the…

A:

Q: Thiamine hydrochloride (vitamin B1 hydrochloride, HC12- H17ON4SCl2) is a weak acid with Ka = 3.4 ×…

A: Molar Mass of thiamine hydrochloride is 337.3 g/mol. Mass of thiamine hydrochloride is 3×10-5…

Q: Calculate the pH of a 0.36M methylamine (weak base) (CH3NH2) solution, if Kb = 4.4x10-4   899 10…

A: The pH of a 0.36 M methylamine (weak base) (CH3NH2) solution is to be calculated, if Kb = 4.4x10-4.

Q: What is the Ka of hydrazoic acid if a 0.020 M hydrazoic acid aqueous solution has a pH of 3.22?

A:

Q: Given Methylamine (CH3NH2). Calculate pH of a 0.0010 M solution of this base. Given Kb for CH:NH2 is…

A: As per guidelines if multiple q uestions , first question is allowed to answer , please post…

Q: Calculate the pH and pOH for the following: a. 10mg of cyanic acid (pKa=9.21) in 1L of water

A:

Q: What is Kb for the conjugate base of CH3COOH (Ka = 1.8 x 10)?

A: The relation between dissociation constant for acid, base and water is given as follows, Kw = ka ×…

Q: Provide your view on this?  Strong bases have weak conjugate acids with high pKa values, usually…

A: Strong base are those which donate hydroxide ions easily in aqueous medium

Q: Calculate the pH of a 27 mg/L solution of hydrocyanic acid (HCN). The pKa of hydrocyanic acid is…

A: Given: The concentration of hydrocyanic acid is 27 mg/L. The pKa of hydrocyanic acid is 9.3.

Q: Sulfuric acid (H2SO4) has two acidic protons with the following ionization constants: Ka1 is…

A: As we know, Strong acid dissociates completely and releases [H+] ion. So, we can calculate directly…

Q: Caffeine (CHiON O2) is a weak base with a pKof 10.4. Calculate the pH of a solution containing a…

A:

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.