Iodic acid, HIO3, has a pK, of 0.77. What is the formula of its conjugate base? O H2IO3+ O HIO3 O OH H2IO4 103 What is the value of K for the conjugate base? the tolerance is +/-2% The conjugate base of iodic acid is a

Q: Calculate the pH at 25 °C of a 0.91M solution of pyridinium chloride (C,H,NHCI). Note that pyridine…

A: pH is a scale used to specify the acidity or basicity of an aqueous solution. Acidic solutions are…

Q: The acid dissociation constant Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a 1.2M…

A: Acetic acid is weak acid and it dissociates partially into [CH3COO-] and [H3O+].

Q: Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.219 M in formic…

A:

Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

A:

Q: Calculate the pH at 25 °C of a 0.53M solution of pyridinium chloride (C5H,NHC1). Note that pyridine…

A:

Q: Sodium stearate (C17H35COONa) is a major component of bar soap. The Ka of the stearic acid is 1.3 ×…

A:

Q: The weak acid HQ has a pKₐ of 4.89.(a) Calculate the [H3O⁺] of 3.5X10⁻² M HQ.(b) Calculate the…

A: Calculation of dissociation constant:

Q: A weak acid has a Ka of 2.5×10^-5.  What is the Kb of its conjugate base?  Which is stronger, the…

A:

Q: The pH of a 0.94M solution of hydrofluoric acid (HF) is measured to be 1.60. Calculate the acid…

A:

Q: Calculate the pH at 25 °C of a 0.46M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A: Given data :

Q: Rank the following acids in order of DECREASING acid strength Acid Ka I. HIO3 1.7e-1 II. HC3H503…

A: pKa is a negative log of acid dissociation constant(Ka). The mathematical expression is pKa = -log…

Q: Calculate the Ka of a weak acid if a 0.065 M solution of acid has a pH of 2.96 at 25 degrees…

A:

Q: 4. pKb of the conjugate base H3C HO H3CO OH

A: Since you have posted multiple questions, we can do only first question.  If you want other…

Q: Calculate the pH at 25 °C of a 0.85M solution of pyridinium chloride (C5H;NHCI). Note that pyridine…

A:

Q: The pKp of 4-hydroxypyridine is 10.80 at 25°C. What is the pH of a 0.0250M solution? Round to two…

A: Please have a look on the solution below:

Q: the following reaction at equilibrium 04 + H20 → cIO41 + H3O*1 O4 is the It is on the list of strong…

A:

Q: Which of the following statements is correct? O The pH of a 0.05 M solution of H2SO3 is equal to 1.0…

A: Solution: The correct statement among the given statements is as follows --- b) In a neutral…

Q: his question relates to aqueous formic acid solutions (HCOOH pK,-3.75) ou will be asked to calculate…

A: pKa of HCOOH = 3.75

Q: Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the…

A: We are given a combination of acidic, basic, and neutral salts.  Each salt has a concentration of…

Q: Calculate the pH at 25 °C of a 0.71M solution of sodium hypochlorite (NaCIO) . Note that…

A: NaClO dissociates into Na+ and -OCl.  NaClO(aq)→Na+(aq)+OCl-(aq)OCl-(aq)+H2O(l)→HOCl(aq)+OH-(aq)

Q: The pka values of a weak acid is directly proportional to basicity. O True O False

A: The given statement is True. It can be explained as below:

Q: Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCI (C14H2]NONH,CI). Note that lidocaine…

A: Solution of iodocain HCl is (C14H21NONH2Cl) = 0.44 M, pKb of weak base iodocaine (C14H21NONH) =7.94…

Q: A 0.1000 M of 1-naphthoic acid solution has a pH of 2.35.  What is the Ka of 1-naphthoic acid?

A: Given information, [1-naphthoic acid] = 0.1000 M pH = 2.35  Find Ka = ?   Molecular formula of…

Q: Which of the following aqeuous solutions has the highest percent ionization? (The Ka of benzoic acid…

A:

Q: 2) The PH of asolution of aweak ronoprotic ucid (HA) is 2.85 what is the Ka of the acid ? Ans.: 2*10

A: Given ,  Concentration of weak mono protic acid ( C ) = 0.1 M pH of the weak acid = 2.85 Acid…

Q: At 60 °C, Kw for water is 1.0 × 10¹³. At 60 °C, a weak acid has a Ka of 1.3 x 10-4. What is the Kb…

A: Acid can be defined as a substance that give hydrogen ions in an aqueous solution.

Q: Calculate the pH at 25 °C of a 0.20 M solution of sodium hypochlorite (NaCIO) . Note that…

A: The pH of the solution has to be calculated

Q: Is prepareu at 25 IS hilialy 0.21M weak acid with K̟=4.5 × 10, and 0.43M in potassium nitrite…

A: Buffer solution is calculated by using Henderson Hassel balch equation

Q: Calculate the pH at 25 °C of a 0.59M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A: Given-> Concentration of NaClO = 0.59 M pKa (HClO) = 7.50

Q: You make a solution of a weak acid with a pH of 3.75 and the pKa is 5.42 1. Is the solution acidic…

A: Answer: These questions are based on basic understanding of the solution that contains a weak acid…

Q: a. What is the base ionization constant for CH2BrCOO ? Kp: CH -5 r ל ל- Ź CH2B CO0 – "CH 2BV COOlH…

A: The conjugate base of the CH2BrCOOH is CH2BrCOO-. Thus we can find the Ka of the weak acid from the…

Q: The acid dissociation constant K, of hydrocyanic acid (HCN) is 6.2 × 10 0. Calculate the pH of a…

A: The acid dissociation constant for the HCN is = 6.2×10-10 The concentration of HCN solution is = 4.9…

Q: Consider the following bases: F A B Which of the following statements is true? (1) The ions increase…

A: An electron-withdrawing group increases the stability of an anion.

Q: Calculate the pH at 25 °C of a 0.41M solution of pyridinium chloride (C;H;NHC1). Note that pyridine…

A: From Ostwald's dilution law  pOH = (1/2) (pKb - LogC)  pOH = power of hydroxyl ions  pKb = - log Kb…

Q: Calculate the pH at 25°C of a 0.58M solution of pyridinium chloride C5H5NHCl . Note that pyridine…

A:

Q: Calculate the pH at 25 °C of a 0.23M solution of sodium hypochlorite (NaClO). Note that hypochlorous…

A:

Q: Calculate the pH of a 5.44x10-3 M solution of H2SO4. (Ka = 0.0120 for HSO4") 1.96 HSO4 is not that…

A: Since the first dissociation of H2SO4 will go completely as H2SO4 is a strong acid. Hence the…

Q: Carbonic acid (H2CO3) and bicarbonate ion (HC0;) are used as a buffer system to regulate the blood…

A: Given,  Ka of H2CO3 = 4.2 x 10-7  pH = 7.15

Q: Would a solution of NH,Y be acidic or basic at equilibrium and 25°C? The K, value for NH, is 5 x 10…

A: e) NH4Y is salt of weak base NH3 and weak acid HY .  Ka of NH4+ = 5 ×10-10 So,Kb of NH3 = 10-14 ÷…

Q: Calculate the pH at 25 °C of a 0.77M solution of pyridinium chloride (C,H,NHCI). Note that pyridine…

A: Here we are required to find the pH of 0.77M pyridiumchloride.

Q: Find the Ka of a weak acid ( HA ) that has a concentration of 0.020 M. The pH is 2.74.

A: Weak acid  [H+] and Ka are related as  [H+] = ( Ka x C)1/2 Where C = concentration of acid = 0.02…

Q: Calculate the [H+] and pH of a 2.35×10−4 M hydrazoic acid solution. The Ka of hydrazoic acid is…

A: We wil use concept of weak acid for H+ and pH.

Q: Calculate the pH at 25 °C of a 0.62M solution of ethylammonium bromide (C,H,NH,Br). Note that…

A: C2H5NH3Br →C2H5NH3+  + Br-C2H5NH3+ =C2H5NH3+                      C2H5NH3+  →C2H5NH2  + H+INITIAL…

Q: 1) Determine the [H30t] and pH of a 0 020 M weak acid solution with a Ka = 3.10 X10 . 2) A 0 34 M…

A:

Q: Hard/Soft Acid Base “theory" can be used to predict stability of Lewis acid/base pairs. Please give…

A: HSAB theory: Ralph Pearson proposed the Hard and Soft Acids and Bases (HSAB) Theory to understand…

Q: A 0.04M solution was found to be 1.6% ionized. what is the concentration of the conjugate base?What…

A:

Q: 36. Lactic acid is a weak acid with the formula HC3H5O3, the Ka for lactic acid is 1.38 x 10-4 In…

A: Given,  HC3H5O3 + H2O ⇔ C3H5O3- + H3O+  The Molarity of Lactic acid = 0.2931 M and it's volume = 250…

Q: Calculate the pH at 25 °C of a 0.72M solution of lidocaine HCI (C4H2,NONH,CI). Note that lidocaine…

A: The value of pKb for the given weak base is = 7.94 The concentration of the base solution is = 0.72…

Q: Rank the cations from least acidic to most acidic: Ag+ , K+ , Pb2+, Zn2+

A: Acidic nature of the given cations will follow

Q: One key to predicting the relative strength of an acid is to Look at its conjugate base and judge…

A: A Bronsted-Lowry acid is a chemical that generates a conjugated base by donating a proton or H + ion…

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.