Which one of the following solutions is basic?  a. A solution for which [OH-] = 8.3x10-12  M  b. A solution for which [H3O+] = 0.0715 M  c. A solution for which the pH is equal to the pOH d. A solution with a pOH of 3.22  e. All of the above are basic

Q: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

A: The pH of the following solutions will be equal to or less than 7.0 for all of the following…

Q: 10. Identify each solution as acidic, basic, or neutral. Justify your answer. a. NaBr(aq) b.…

A: The compounds given are NaBr, NH4NO3 and K2CO3.

Q: 23. Polyprotic Acids: Write out the formation of the three conjugate bases for H,PO,. When it…

A: The question is based on the concept of acid and bases. we have to write step wise dissociation of…

Q: A weak base, B, has Kb = 4.0X10^-6. Consider a 0.0020 M solution of the base.  a. Calculate pOH b.…

A: Suppose the weak base be A-. It gets hydrolyze according to the equation: A- + H2O <----> HA +…

Q: Determine the [H+] in a 0.0244 M HClO solution. The Ka of HClO is 2.9 × 10 -8.   a. 1.61   b.…

A: The dissociation behavior of a weak Bronsted acid in aqueous solution, is defined according to its…

Q: Arrange in terms of increasing acidic and explain these using partial charges and inductive effects…

A:

Q: Determine if each salt will form a solution that is acidic, basic, or pH-neutral. a. FeCla d. NH,Br…

A: Since you have posted a question with multiple subparts, we will solve the first three subparts for…

Q: Which of the following salts will be Acidic? A. Fe(NO3)3 B. AlCl3 C. NH4Br D. All of them Group of…

A: The salt of strong acid and weak base is acidic in nature. All the given salt is product of a…

Q: If you have 0.80 g of solid KOH dissolved in 2.28 L of water: a. Determine the concentration of H…

A: Given Mass of Solid KOH (W) = 0.80g Molar mass Of KOH = 56.10 g/mol Number of moles dissolved (n)…

Q: For each mixture of acids, find the pH and [A- ] for each conjugate base. a. 0.185 M HCHO2 and 0.225…

A: pH of mixture of any two weak acids(1 and 2) can be determined by the formula- H+=c1k1+ c2k2

Q: 1. For each of the salts (assume at this point completely soluble), write the equation for…

A:

Q: A solution with a pOH of 11.70 has an [H+] of a. 5.0 × 10−3 M.b. 3.2 × 10−4 M.c. 2.0 × 10−12 M. d.…

A: Given data, pOH of the solution =11.70

Q: Which best describes the pH value of a solution with a H3O+concentration of 1.68 * 10 -5M? a. pH =…

A:

Q: A 0.432 M solution of pyridine has a pH of 9.40. What is the K, of pyridine? Oa. 2.7 × 104 Ob. 1.5 x…

A:

Q: 8. Which one of the following ions will NOT produce a basic solution? * O HCOO Br NH2 O NO2 O HST

A: Weak base have strong conjugate acid and strong base have weak conjugate acid .

Q: An aqueous solution has an hydroxide ion concentration of 1E-6 M (10-6 M). Remember to use e…

A: Since, Negative logarithm of concentration of H+ ion is known as pH of the solution. i.e. pH =…

Q: Which solution will have the lowest pH (most acidic)? a. 0.10 M HCIO. b. 0.10 М НСIO с. 0.10 МКОН d.…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: 15. The [H3O+] of a solution with pH = 2 is Group of answer choices 1 × 10-12 M 1 × 10-2 M -10. M…

A: PH = -log[H3O+] Where, [H3O+] is the concentration of H+ in the solution So, PH is 2 when…

Q: Suggest the conjugate base of nitric acid, HNO₃. *

A: As HNO3 is a acid, therefore it will easily release H+ ion as this is the property of acids.  To…

Q: a. What is the hydroxyl concentration of the ammonia solution? b. What is the pOH of the ammonia…

A: Given: Volume of ammonia solution= 300ml Concentration of ammonia solution= 0.05M The density of the…

Q: Which of these could be the pH of a very concentrated solution of a strong acid? a. 6 b. 0  c. 9…

A: CORRECT ANS- B)0

Q: 5. In a NaOH solution [OH2] is 2.9 x 10-24 M. Calculate the pH of the solution.

A: NaOH is  a strong base so, it completely dissociate into its ions in aqueous solution. NaOH (aq)…

Q: pH pOH [H*] [OH]] Acidic, Basic or Neutral? a. Solution 9.60 a M M pH РОН [H*] [_HO] or Neutral?…

A:

Q: Calculate either [H,O*] or [OH¯] for each of the solutions. Solution A: [OH¯] = 2.55 x 10-7 M;…

A: Use relation:  Kw = [H3O+][OH-]  At 25°C Kw = 10-14  In basic solution pH >7  => [H3O+] <…

Q: From what acid and what base are these salts below made from? a. Ca(NO3)2 b. NH4Br c. BaCl2

A:

Q: What is the pH of an HCl solution if [H*] = 0.03? %3D

A:

Q: What is the pH of a 0.876 MHNO3 solution? 0.420 Ob. 0.057 OC. 0.535 Od. 0.244 a.

A: According to the question, The molarity (molar concentration ) of the HNO3 is given by = 0.876 M The…

Q: 1. If an acid has a aka value of 4.2x10^-7, what does this mean in terms of the strength of the…

A: Ka value can be used to estimate strength of an acid. If Ka value is high (and pKa value is low),…

Q: Calculate the pH of HOCI solution that is 2xE-6 M, Ka =2.8xE-8 а. 2.8 O b. 2.4 O c. 1.3 O d. 6.6

A:

Q: Which acid in each pair has the stronger conjugate base?   a. HI or HPO42−

A:

Q: Which of the following solutions would have the highest pH?  Assume that they are all 0.10 M in acid…

A:

Q: Under normal laboratory conditions (i.e. – as discussed in this class only), how many of the…

A: Lewis acids are the species that accepts a pair of electrons. Lewis acids are electrophilic in…

Q: The concentration of H+ ions in a solution is 0.315 M. a. Calculate the concentration of OH– ions…

A: Applying formula PH= -log[H+]

Q: Acid strength decreases in the series HI > HSO 4 - 1 > HF> HCN. Which of these anions is the…

A: Answer: A

Q: ľ The pH found to The hydr The hyd.

A:

Q: Need help with question 4

A: a) HCl is a stronger acid than HF because fluorine is more electronegative than chlorine. In result,…

Q: Consider the reaction HC1O+F HF+ CIO¯ Which of the following statements is true: A. It is product…

A:

Q: Macmillan Learning Calculate either [H3O+] or [OH] for each of the solutions. Solution A: [OH] =…

A: Before solving the problems, we need to know about few relations.For determining [H3O+] or…

Q: Which of the following acids is the weakest? HF OHBr HI All of the acids are equal in strength. HCI

A: HF is the weakest acid amongst all the options given.

Q: Which one of the following is more acidic? CO2H CO,H а) b) NO2 ОН NH2 c) d) i. b

A: Acidity is defined as the ability of a molecule to release protons.  if a compound  easily donate…

Q: Give a clear handwritten answer...Find out pH  Of Hcl ...given Hcl solution (H+)=0.03?

A:

Q: Calculate the pOH of a 7.68x10-6 M HCl solution. pOH= (round to the nearest 3 sig figs) This…

A: we have to find pOH of HCl solution.

Q: Which of the following species below, when dissolved in H2O,  will not produce a basic solution? A.…

A: Basic Solution is a solution containing more OH- ions than H+ ions.

Q: 1. A solution has a pH of 5.50. a. What is the pOH of this solution? b. Is the solution acidic,…

A: pH = 5.50 pOH = ? Nature of  solution =?

Q: What is the pH of 2.4E-2M barium cyanide?

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Which solution has the higher pH (which is less acidic)? A. 0.1 M HC2H3O2 B. 0.1 M HCl. C.…

A: The solutions given are, A) 0.1 M HC2H3O2  B) 0.1 M HCl

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.