ine the [H+] and [OH-] in:   5.0 x 10-5 MHNO3   2.0 x 10-6 M KO

Q: The Kb of dimethylamine [(CH3)2NH] is 5.90×10-4 at 25°C. Calculate the pH of a 1.15×10-3 M  solution…

A: [H+] [OH-]  =  10-14 PH + POH  = 14 [OH-]  = 10-14/ [H+] [H+]  =  10-14               [ OH-]

Q: Which of the following would be the acid-base pair that can create NaCl? OLICI and NaOH OHCI and Na2…

A: Acid reacts with base to form salt and water. The given salt is NaCl.

Q: Calculate the [OH] and the pH of a solution with an [H] = 5.6 x 10-¹0 M at 25 °C. [OH-] = pH =…

A:

Q: 2. Name each of the fo llowing acids: OH a) CH;CH,CF,CH,COOH b) CH3-CH2-ČH–COOH СООН „COOH d) ОН…

A:

Q: Calculate the [H30+]value of{OH-}=1.2x10-11M

A: We have to calculate the [H3O+]

Q: Calculate the pH of a 3.39×10-3 M  solution of NaF, given that the Ka of HF = 6.80 x 10-4 at 25°C.

A: Given : Concentration of NaF = 3.39 X 10-3 M And Ka of HF = 6.80 X 10-4  Since the salt NaF contains…

Q: Label acidic basic or neutral: (you will first need to find the pH) 9.5 x 10^-11 M NH3

A: As per the given data Concentration of NH3=9.5×10-11MpH=?

Q: Which one of the following will have the strongest conjugate base? HF (Ka = 6.8 x 10 %3D CH3COOH (Ka…

A: The weaker the acid, the stronger it's conjugate base. A large Ka value indicates a strong acid…

Q: In a CH3COOH/CH3COO" pair, which among these is the base? A CH3COO- B Neither CH3COOH D) Both

A: An acid is a substance that give H+ ions in the solution. A base is a substance that accept H+ from…

Q: calculate the [H3O+] value {OH-]=1.2x10-5M

A: [OH-] = 1.2 × 10-5 M  [H3O+] = ?

Q: which of the following is a triprotic acid? 1) H3PO4 2) CH3COOH 3) HNO3 4) NH3 5) Al(OH)3

A: The acids given are H3PO4, CH3COOH, HNO3, NH3 and Al(OH)3.

Q: Calulate the pH of each of the following: 0.05M HCl 0.06M NaOH 0.06M CH3COOH (ka = 1.8 x 10-5…

A:

Q: 8.Which of the following is an acid?  HNO3  NH3  NaCl  CH4  NaOH

A: Arrhenius Concept of Acids and Bases  an acid is a substance which dissociates in aqueous solution…

Q: If [H+] = 9.1x10^-4 M, what is [OH-]?

A: Given that, [H+] = 9.1x10^-4 M We have the following relationship between [H+] and [OH-]

Q: Calculate [OH-] of NaBrO, 0.810M; KaHBrO = 2.0 x 10-9. Group of answer choices 4.5 x 10-4 2.0 x 10-5…

A:

Q: Calculate the [OH-| and the pH of a solution with an [H*] = 2.6 x 10-1" M at 25 °C. [OH-] = pH :…

A: pH measures acidity of the solution. pH of a solution depends on the hydrogen ion concentration.

Q: 2) Rank the Acidity of the following sets of compounds. NH, OH2 "OH он a) OH; NH3 NH2, COOH b)

A: Acidity us defined as tendency to donate lone pair or releasing of H+  Most stable anion is higly…

Q: What is the base of the reaction HSO4^-(aq)+H2O(l) H2SO4(aq)+OH^-(aq) HSO4^- H2SO4 OH^- H2O None

A: A base is that species that accepts H+ ion

Q: Rank the positions from most acidic to least acidic. F iii NH₂ —— i HO O O iv > i > ii > ¡¡¡ Oi> iv…

A:

Q: [H3O+] pH Acid or Base? 4.2 x 10-3       5.3   5.2 x 10 -4       9.5   9.8 x 10-2       8.8

A: pH is measure of acidity or basicity of solution. pH value is between 0 to 14. When pH is less than…

Q: Calculate the pH of a 0.0470 M aqueous solution of the weak base methylamine (CH3NH2, Kb =…

A:

Q: Calculate the pH of 0.15M CH3COOH. Ka=1.8×10-5

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: What is the OH- concentration in 0.5 M NH4Cl (aq)? (Ka of NH4+ = 5.6 X 10-10) A.) 5.6 × 10-10 M…

A: Given: Concentration of NH4Cl = 0.5 M Since NH4Cl is a completely soluble salt that will dissociate…

Q: What is the [OH-] of a solution with pH = 3.17? a. 1.48 x 10-10 M b. 6.76 x 10-4 M c. 1.48 x 10-11…

A: To calculate the hydroxide ion concentration first of all we calculate the pOH of the solution and…

Q: Ka for formic acid, HCOOH, is 1.80 x 10-4. Ka for phenol (a weak acid), C6 H, OH, is 1.00 x 10-10.…

A: Given acids with Ka :-  HCOOH   Ka = 1.80 × 10-4  C6H5COOH    Ka = 1.00 × 10-10  C6H5COOH   Ka =…

Q: Fill in the table below and answer the questions using these formulas. pH = -log [H*] pOH = -log…

A: # The ionic product of water in we used to calculate the hydrogen ion concentration or hydroxide Ion…

Q: Find the [H+] and the [OH-] from the following values 1. pH = 2.5   2. pH = 11.3   3. pOH = 4.6…

A:

Q: For the system here: HOBR +OH-1 ------H2O +OBr -1 Bronsted would classified the base species as OBr…

A:

Q: Use the definitions of acid and base to identify the first compound in each equation as an acid or a…

A: Bronsted Lowry Concept of acid and Base: As per this concept, acids are proton donor while bases are…

Q: Calculate [OH-] of a 4.40×10-1 M aqueous solution of triethylamine ((C2H5)3N, Kb = 4.0×10-4).…

A: (C2H5)3N is a weak base. Hence it undergoes hydrolysis reaction in solution as, => (C2H5)3N (aq)…

Q: Tell the concentration and if it’s an acid or base 1. [OH-]=5.48 X 10 ^-9 M 2.[OH-]=2.0 X 10^-13 M

A:

Q: Which of the following states the correct [H+] and [OH-] at pH 10.0? a) [H+] = 4 M;  [OH-] = 10 M…

A:

Q: What is the pH of an acetic acid, CH3COOH, solution that has an initial concentration of CH3COOH of…

A: Acetic acid is a weak monoprotic acid. In water it is dissociated as acetate ion and protons.

Q: H2O                                                        HCN (Ka = 6.2 x 10-10)      HCl (Ka >…

A: Answer : the order of acidic strength:  HCl >HF>H2O>HCN .

Q: Calculate the pH of a 0.600 M solution of methylamine CH3NH2.  Kb = 4.4 x 10–4

A: CH3NH2 is a base and CH3NH3+ is its conjugated acid. pKb of CH3NH2 is 4.4×10-4. Expression for Kb is…

Q: Which of the following is a conjugate acid/base pair?   NH4+/NH3 H2SO4/SO42– HCl/OCl– H3O+/OH

A:

Q: la formula name -4 6.8 x 10 -4 ethylamine C2H5NH2|6.4 × 10 - 10 hydroxylamine HONH, 1.1 × 10 8- 4.9…

A: Acidic solution has pH less than 7, Basic solution has pH greater than 7 .and neutral solution has…

Q: Which of the following acids would be able to neutralize the most base? 100 mL of 0.5 M H2SO4 300…

A: Introduction: According to Bronsted and Lowry concept, an acid is a substance that can donate…

Q: 3. Calculate the [H3O+], [OH-], pH, and pOH of a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: here is the solution of question

Q: Indicate if each set of lone pair electrons on the heteroatoms are basic or not basic. N. :0

A: If lone pair is not a part of resonance so it will be basic.

Q: calculate the [OH-] of a solution that has [OH+] = 6.2 × 10-6 M at 25°C PLEASE ANSWER EVERYTHING ON…

A: Note: as per guidelines if multiparts question, first three only allowed, please post questions…

Q: Calculate the pH value of 0.10 M NaH2PO4 solution. Ka1 （ H3PO4 ）= 7.52×10－3; Ka2 （ H3PO4 ） =…

A: Sodium dihydrogen phosphate is a salt of strong base and weak acid. The pH of such salts is…

Q: Calculate [OH-] of a 1.30×10-2 M aqueous solution of diethylamine ((C2H5)2NH, Kb = 1.30×10-3). (b)…

A: (C2H5)2NH is a weak base. Hence it undergoes hydrolysis reaction in solution as, => (C2H5)2NH…

Q: [OH] - 1.6 x 10 8 M [H*]- M PH - POH - [OH']-8.2 x 10 12 M [H*)- DH - POH -

A: Interpretation- To determine the  concentration of [ H+ ] , pH and pOH in the given question.…

Q: Identify if it's a strong acid, weak acid, strong base, weak base, or neutral.  hc1 secreted in…

A: Strong acid and base- Acid and base that completely dissociates into its ion in aqueous solution…

Q: Calculate the [OH-] and the pH of a solution with an [H*] = 8.2 × 10-12 M at 25 °C. -9 [OH"] 1.2 x10…

A: Answer given as follows

Q: hydronium-ion concentration of a 2.13 ✕ 10−4 M solution of p-bromobenzoic acid, BrC6H4COOH, for…

A: Degree of dissociation is the number of moles dissociated per unit concentration of any electrolyte.

Q: Calculate the pH of the ammonium chloride solution of concentration 0.1M if the acid dissociation…

A:

Q: Given the following data, Base K, NH3 1.8 x 10-5 CH3NH2 5.0 x 10 C6 H6 NH2 4.2 × 10-10 Calculate the…

A: Hey, since you have asked multiple question, we will solve the first question for you.  If you want…

Q: Given [OH-] = 1.75 x 10-4M, calculate [H3O+]. A. 1.25 x 10-4M B. 8.0 x 10-11M C. 5.71 x 10-11M…

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.