Least acidic F Br CI А. "СООН В. COOH COOH "СООН С. "СООH D. COOH

Q: Which equation below describes basic solution?     [H3O+] [OH-]

A: The answer is given below

Q: he strongest acid?

A:

Q: What volume of 1.584 mol L solution of NaOH is required to make 7.00 Lof a solution with a pH =…

A: pH - It is the negative logarithm of the hydrogen ion concentration of a solution.  Given:- pH =…

Q: Part A Asolution with a hydroxide ion concentration of 4.15 x 107 mol L-1 is and has a hydrogen ion…

A:

Q: Calculate [H3O+] for each solution pH = 1.52?

A: pH = -log [H3O+]

Q: Which one of the following statements is true? A. A solution with a pH of 13.10 will have a lower…

A: The statements given are, A) A solution with a pH of 13.10 will have a lower concentration of…

Q: Which values represents the most basic solution, highest pH? A. [H3O+] = 1 x 10-10 B. [OH-] = 1.4 x…

A: Since you have asked multiple type questions, we will solve only first  questions for you. If you…

Q: A 0.735 M solution of a weak base (B:) is made.  The solution has a pH of 10.86. Calculate the Kb of…

A: The concentration of the base solution is = 0.28 M The pH of the solution is = 10.86 The value of Kb…

Q: 2. Which solution is the most acidic? А) 1.0 x 10-7 м ОН В) 2.3 х 10 3 М ОН С) 3.9х 10 8 М ОН D) 5.1…

A:

Q: In the reaction: BCI3 + NH3 The Lewis acid is: (c) B-NH3 1. O cr O H,O O H O NH3 BCly

A: A Lewis acid is a chemical species which has an empty orbital in which it is able to accept…

Q: What is the key equation for finding density? O d = m/V O A = ebC O q_rxn = -q_cal O at endpoint,…

A: There are different formulas used to relate two or more quantities to each other. Each quantity is…

Q: Calculate the pH

A:

Q: Calculate the pH of a solution that is .0400M in  a.) H3PO3  b.) H2S

A:

Q: to maintain the pH at 10 basic pll is needed to deprpto to favorize the formation of sta

A: A buffer solution is an aqueous solution of a weak acid and its salt or a weak base and its salt the…

Q: hat is the PH of a 0.500 M NaCIO solution? Ka of HCIO is 2.9x10- O a. 9.48 O b. 3.38 O c. 10.62 O d.…

A: Which one of the following is correct answer

Q: CH3 H2SO4 (d) SO3 NB. This combination of SO3 and H,SO, is called fuming sulfuric acid. Since SO 3…

A:

Q: 1. Calculate the molarity of H3O+ and the molarity of OH-, as well as the pH of the following…

A: Strong acid are those which can completely dissociate into water to give H+ ion Example = HCl, HNO3…

Q: What is the pH of a solution that is 1 × 10-8 M with respect to H+?

A: Here given, Concentration of H+, that is [H+] = 1 x 10-8 M We know, that---- PH = - log [H+]

Q: In many reactions, the addition of AlCl3 produces thesame effect as the addition of H+.(a) Draw a…

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: (a) What is the concentration of the Acid? D.l [=Mores しLQrs ミ 20 O.005 BasE PL (b) What is the pH…

A: (a)  Reaction between NaOH and H2CO3…

Q: Predict the acid that has the smallest pKa+ O HBRO2 O HBRO3 O HBRO O They have the same relative…

A: the smaller the pKa value, the stronger the acid

Q: H2SO4 (e) SO3 NB. This combination of SO3 and H,SO, is called fuming sulfuric acid. Since SO, is a…

A:

Q: The pOH of 0.050 M HCI is O a. 1.30 b. O b. 0.30 O c. 13.70 O d. 12.70

A: Given- Concentration of HCl= 0.050M pOH=?

Q: Which of the following is the most basic solution (highest [UH ])? O pH 12 %3D O pOH = 1.0 o [OH] =…

A: 1) pH=12 we know, pH + pOH = 14 pOH = 14 - 12 = 2

Q: Calculate pH and pOH of a solution with [OH-] = 5.92×10-8 M

A: Given    [ OH- ]  = 5.92 × 10-8 M    PH        = ?   POH     =  ?

Q: 2. Complete the following tdde with the needed [H3O+], [CH], and pH, and dassify the solution as…

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Q: e highest [OH-]?

A:

Q: c). B (if basic).o

A: Reaction of Salt in Water, K2C2O4(aq.) + H2O(l)--->  2KOH(aq.) + H2C2O4(aq.)

Q: he PH formula is given as PH=-log(H+). The H+ is th umber of free ions of hydrogen. A seven PH is…

A: pH scale is explained by Sorensen  Lower pH indicates acidic  Higher pH indicates basic  PH = 7  it…

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: 16.) A sdution od 8.m g 88.0M unt is othe Ko f a We ak acid, HA, is 0.47% ranized. the Weak acid.…

A: The molarity of given weak acd, HA =8.0 M As HA is a weak acid, it dissociates partially into A- and…

Q: that ar the distimgushing p3oresties f acids and ase. Explain the ability of dissolve Some metals…

A:

Q: A 0.25-M weak base solution has a pH of 11.50. Calculate its Kb.

A:

Q: Give a clear handwritten answer...

A: Acidic strength of molecules can be compared by resonance stabilization of their conjugate bases.…

Q: A) A solution with a pOH of 12.50 will have a higher concentration of hydronium ions than hydroxide…

A: pH + pOH = 14 The concentration of hydronium ion is very high in strongly acidic solution

Q: The pH of a 0.0231 M HNO3 solution is: 4 sig figs if possible please

A: PH=-logH+

Q: An unknown weak base with a concentration of 0.0910 M has a pH of 11.70. What is the Kb of this…

A: A weak base is a substance that do not dissociate completely.

Q: Predict and sort HF, HCI, and HBr starting with the strongest acidity! Explain why!

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Q: Consider 1.3 M HNO2 solution. (a) Show the reaction of dissociation (ionization) of HNO2.  (b)…

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Q: I dentity the tollaming salts as Acidic, Basic or neutiral : HCook Naclos ,kCloy i CoH 5. CH; Nity…

A: Salt is substance produced via reaction between acid and base.  If salt produced via strong acid and…

Q: Which of the following statements is/are true for a 0.10 M solution of a weak acid HA? (a) The pH is…

A: Molarity of HA = 0.10 M

Q: Which of the following is amphoteric (1.e. can behave as an acid or base) in aqueous solution?…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: What is the H,O"| of a solution of HI with a pH = 1.45? O la) 0.0355 O (b) 0.1173 O (c) 0.3548 O (d)…

A:

Q: Number the following acids in decreasing order of acid strength: OH OH OH Br CH,OH Br Br ČH3 1 O a.…

A: Given : some Compounds are given  To find: Decreasing order of acidic strength Solution: Acidic…

Q: The most basic among the ff. aqueous solutions, given the pOH: рон - 2 рон - 10 pOH = 6 рон 3 12 pOH…

A: Option 1 is the correct choice.  Since pH nearly equal or approaches to 14 shows that the base is…

Q: For a 0.0000125 M H2SO4 solution, the hydroxide concentration would be?

A: Answer = 3.98 x 10-10

Q: The common constituent in all acid solutions is O H2 H+ O OH- O H2SO4 O C-

A: When acid is dissolved it form H+ ion

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.53. What is the Kb of this base?

A: The K b represents an equilibrium constant.  If the value of K b is small, then the base will be…

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.