Write the formula a. HCO; b. РО а. 3-

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: Rank the following acids in increasing order of strength (from weakest to strongest) HCIO, | HBrO,…

A: Dear student, the above compounds are acidic in nature on account of their ability to release…

Q: If [H* ] = 4.3 x 10-4 M, what is [OH]?

A: The given problem can be solved by using the formula given below as; H+ OH- = Kw= 1.0×10-14…

Q: What is the pH of a solution with a [H3O*] concentration of 7.44 x 10-5 M?

A: Given: [H3O+] concentration = 7.44 × 10-5 M We have to calculate the pH of the solution.

Q: What acid and what base would react with CsNO3

A: Given salt for formation is CsNO3

Q: Hydrogen fluoride is considered: A a weak base B a weak acid C None of the others D a strong…

A: Strong acid and base are those which are strongly dissociates into ions whereas weak acid and base…

Q: Why does the concentration of H3O+ and OH- equal each other in neutral water?

A: pH = -log[H3O+]   [OH-].[H3O+]  = kw  Kw = 1.0 × 10-14 M2

Q: 6.) If the pH = 8.2, what is [H*]? %3D 7.) If the pH = 4.2, what is [OH]?

A: Answer govt as follows

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: Calculate the pH of the follo 0.39 M NH4CI (рКp fo O a. 2.57 O b.4.83 с. 9.67 O d.4.33 O e. none of…

A: Given, pKb = 4.74  Concentration of Salt(C)= 0.39 M It is salt of weak base -strong acid type salt .…

Q: How would the pH of a 0.175 M solution of NaC4H,O2 compare with that of a 0.175 M solution of…

A: The salt gets hydrolyzed when dissolved in water. Both salt have the same acid and similar strong…

Q: The pH value of 0.1 M ammonium hydroxide is --- -- O 2.87 O 1 11.13

A: Ammonium hydroxide is basic in nature.

Q: Calculate the pH of 0.02 M H;PO4

A:

Q: Write equations for the reaction of each compound with BF3, a Lewis acid

A: Concept introduction: Lewis acid: These are substance that donates proton and accepts a pair of…

Q: Calculate [H3O+][H3O+] given [OH−][OH−] in each aqueous solution. [OH−] = 4.2×10−12 M [OH−] =…

A:

Q: Most Acidic H,PO, H,PO, HPO,? H,O+ H,0 Least Acidic

A: Given that : We have to rank these Bronsted acids according to their acidic character.

Q: Why can't we write OH2 for water instead of H2O???

A: In the nomenclature process,  more electropositive atom is given preference to be written first.

Q: The pH of 0.20 M HNO3 is O a. 0.63 O b. 1.58 O C. 0.70 O d. 0.20

A: pH  =  - log [H+ ]  Strong acids undergo complete ionisation in solution.  Thus, [H+] =…

Q: Calculate the OH-millimolar concentration in an "alkaline water" which the manufacturer claims to be…

A:

Q: 1. Calculate [H] and [OH] for solutions with the following pH values: a) 4.0 b) 8.52 c) 12.60

A: given a) pH = 4 b) pH = 8.52 c) pH = 12.60

Q: b. Bi(OH)3 + Sn(OH)3 Sn(OH),² + Bi (basic) ->

A:

Q: Which of the following statements is false? O A) None of these are false O B) If a solution of…

A: Increase in concentration of methyl amine increases concentration of hydroxide ion.  Greater the…

Q: Acid, base or neutral [H*] [OH'] pH pOH 3.25 х 106 М 4.5 9.5 2.7 11.3

A: Since you have asked multiparts questions, we will solve the first three sub parts questions for…

Q: For  1.15×10−2 M Ba(OH)2, determine [OH−] and [H3O+]

A: Barium hydroxide is a strong base and it undergoes complete dissociation to give two hydroxide ions…

Q: The F- ion is a weaker base in water than NH3 is. Explain what this means.

A:

Q: 1.) What is [OH] if [H'] = 2.3 x 10° M? 2.) Suppose [H] = 8.5 x 10 M. What is the pH?

A: Given, [H+] = 2.3 x 10-5 M [OH-] = ?

Q: Question 1 In terms of acid strength, which of the following does not belong with the others? HC104…

A:

Q: What is the pH of a 0.600 M solution of Na2S?

A: In this question, we want to determine the pH of the salt solution ( Na2S ) How we can calculate,…

Q: What is the volume of 0.0175 M Ba(OH)2 required to neutralize 10.0 mL of 0.0300 M HCl?

A:

Q: What happens when a weak base such as NH3 is dissolved in water? Write a chemical equation to…

A: A base is a species that can donate its non-bonded electron pair or can accept a proton. A weak base…

Q: What volume of 0.50 M KOH would be required to neutralize completely 500 mL of 0.25 M H 3 PO 4…

A: Given data contains, Molarity of potassium hydroxide is 0.50 M. Volume of H3PO4 is 500 mL. Molarity…

Q: Rank the following acids in order of increasing strength: (a) HClO4, H3PO4, H2SO4; (b) H3PO4,…

A: (a) HClO4 >H2SO4 > H2PO4 (b) H3PO4 >H3AsO4 >H3SbO4 (c) HOF >HOCl >HOBr >HOI

Q: Calculate the hydrogen ion concentration in mol/L for each of che following solutions: (a) a…

A: The pH is a measure of the concentration of hydrogen ions, the acidity of alkalinity of a solution.…

Q: The species SO4– 2 is___ A both B None of the others C an acid D a base

A:

Q: Determine the pH of 0.25M CH3COONA solution. Kg of CH3COOH = 1.8×105 Select one: 10.08 O 9.08 O 4.90…

A: Sodium acetate is a salt of a weak acid, acetic acid, and strong base, sodium hydroxide. The salt of…

Q: * A solution of NaOH has a pH of 10.50. How many grams of CaO should be dissolved in sufficient…

A:

Q: Write the dissociation of the acid HClO2.  You may include or exclude water.

A: Chlorous acid, HClO2 is a weak acid. According to the Arrhenius theory, the acids dissociate in an…

Q: Write separate equations representing the reaction of H2 PO4−(a) as a base with HBr(b) as an acid…

A: A base is a substance which accepts proton  An acid is a substance which donates proton

Q: Write separate equations representing the reaction of HSO3−(a) as an acid with OH−(b) as a base with…

A: HSO3- is amphiprotic. It can act as an acid as well as base.

Q: Calculate the theoretical number of moles of HCl equivalent to 1 mole of Al2O3

A: HCl is a strong acid and Al2O3 is an amphoteric oxide. Al2O3 reacts with acid and form salt and…

Q: What is the pH of a solution with a [H3O^+] concentration of 7.44 x 10^-5 M?

A: Given, Concentration of H3O+ ion = [H3O+] = 7.44 x 10-5 M pH of the solution = ? Note: pH: it can…

Q: What is the pH of a solution with [H3O+] of 1.9 x 10-8 M?

A: Given that, [H3O+] = 1.9×10-8 M pH = ?

Q: following aqueous solut (Select all that apply.) O0.32 M NaCiO4 + 0.27 M NaCl O 0.20 M HF + 0.21 M…

A: We have tell which will form buffer.

Q: Calculate the  [ H3O+ ]  corresponding to pH = 8.62.

A: The relation between pH and [H3O+] is: pH=-log[H3O+]                           ...... (1)

Q: Determine the pH of the solution resulting from mixing a solution of 154 mL of HNO2 (Ka = 5.62e –…

A:

Q: Rank the following acids in order of increasing strength: ClCH2SH, CH3SH, H2S.

A: The acidic strength of any acid is proportional to the stability of the anion formed by removing the…

Q: What happens when a weak base such as NH3 is dissolved in water?

A: When a weak base such as ammonia NH3 is dissolved in water, NH3 accepts the proton H+ from water and…

Q: 6. Which formula represents a hydronium ion? A H,O R NH, C. OH D. HOO,

A: water molecule  accept the proton to give hydronium ion. H2O +  H+  ⇄ H3O+

Q: What volume (mL) of 0.10 HNO3 is required to neutralize 125 mL of 0.050 M KOH?

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.