Identify the Lewis acid and Lewis base in the reaction: Co3+(aq)+6NH3(aq)⾮Co(NH3)63+(aq)

Q: What is the equilibrium constant expression, Ki, for the following weak acid? H3PO4(aq) ↔ H+(aq) +…

A: We have to predict equilibrium constant expression for dissociation of weak acid.

Q: Boron trifluoride (BF) has no dipole 2) (a) moment. Explain how this observation confirms the…

A: a) We Know that boron and fluorine are compounds with different electronegativity and the central…

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

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Q: In which of the following does no reaction occur? K,CO3(aq) + Ca(NO3)2(aq) → O HNO3(aq) +NaOH(aq) –…

A: A reaction is said to occur when the reactants present in the reaction vessel/container gets…

Q: A monoprotic weak acid, HAHA, is ionized according to the reaction…

A: Given ionization reaction : HA(aq) + H2O (l) ⇌ A- (aq) + H2O+ (aq) pKa = 3.95

Q: Order the following solutions from lowest to highest pH: 1. 0.10 M NACIO II. 0.10 M KBr III. 0.10 M…

A: pH is the measure of acidity. It is obtained by negative logarithm of concentration of H+

Q: Calculate the pH of a 0.56 M HF solution at 25 °C. HF (aq) = H* (aq) + F¯ (aq), K₂ = 6.9 × 10-4 at…

A: Given: [HF]=0.56M;Ka​=6.9x10−4;pH=???Step 1: Write the dissociation…

Q: Using this table of ionization constants, calculate the overall equilibrium constant, Koverall for…

A: The given equilibrium is HCOOH(aq) +S2-(aq) ⇔HCOO-(aq) + HS-(aq) Koverall=HCOO- HS-HCOOH S2-

Q: Classify each of the following species as a Lewis acid or a Lewis base: (a) CO2, (b) H20, (c) I-,…

A: Lewis base donates pair if electron and Lewis acid accepts pair of electron.

Q: what is the pH of a 0.40 M Solution of NH 4 NO3(aq)? Kb for NH ₂ (aq) = 1.76X10²5

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Q: СН.ОН (аq) + CN (ag) — HCN(aq) + CH,О (aq)

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Q: The pH of a 0.10 M solution of a weak acid was determined to be 4.0 once equilibrium was established…

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Q: Which of the following has the highest acidity: pH 1, pH 5, or pH 9?

A: To find: Which pH has the highest acidity

Q: In the reaction HPO 2 (aq) + H20(1) PO,3-(aq) + H3O* (aq) HPO (aq) is the H20(1) is the PO43 (aq) is…

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Q: Co** (aq) + 6NH;(aq) = Co(NH;);*(aq)

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Q: What is the pH of 3.7 x 103 M NH¼Br(aq)? Ο 10.4 O 2.4 Ο 11.7 O 5.8 O 4.6

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Q: In the following equilibrium, identify the conjugate base of the weak acid? HA(aq) + H2O(1) A (aq) +…

A: Answer

Q: 8) What is the pH of a 0.035 M HNO, solution? HNO; (aq) + H,O (1) H3O* (aq) + NO3 (aq)

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Q: Select the conjugate  acid-base pairs for the reaction:

A: Bronsted acid is proton(H+) donar, Where as Bronsted base is proton acceptor. Acid and it's…

Q: Using this table of ionization constants, calculate the overall equilibrium constant, Koverall, for…

A: HCN (aq) + S-2(aq) <---> CN-(aq) + HS-(aq) Koverall…

Q: Identify the conjugate acid-base pairs in the following reaction: HCO3 - (aq) + H2O(l) ⇌ CO3 2- (aq)…

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Q: Calculate the pH of each of the following solutions of strong acids.

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Q: What is the Ka for a 0.1733 M nitrous acid solution, HNO2, if it had a pH of 2.065? HNO2(aq) +…

A: Given, Concentration of nitrous acid (C) = 0.1733 M pH of HNO2 = 2.065  Dissociation constant of…

Q: What is the the PH and POH of the following solutions: 1. 0.05 M Ba(NO3)2 2. 0.01 M Na2SO4

A: The given solutions are 0.05 M Ba(NO3)2 and 0.01 Na2SO4.

Q: For each chemical reaction in the table below, decide whether the highlighted reactant is a…

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Q: Which of the following shows the correct chemical equation for the ionization of HBRO? HBrO(aq) +…

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Q: Consider the following dissociation reaction of a weak acid, HA: HA(aq) + H20(4) H,O* (aq)+ A (aq)…

A: HA H2O H3O+ A- I C - 0 0 C -Ca - +Ca +Ca E C-Ca - Ca Ca a = 2.0 %   = 0.020  [H3O+] = Ca…

Q: Identify the conjugate acid-base pairs in the following reaction: CH3COOH (aq) + NH3 (aq) →CH3COO−…

A: Given , Reaction CH3COOH (aq) + NH3 (aq) →CH3COO− (aq) + NH+4 (aq)

Q: Label the Brønsted-Lowry acids and bases in the follow- ng equations, and tell which substances are…

A: Answer:- this question is answered by using the simple concept of Bronsted Lowry concept of acid and…

Q: Write balanced net ionic equations for the following reac-tions, and label the conjugate acid-base…

A: Given: (a) The ionic equation of the above equation is, The net ionic equation is obtained by…

Q: what is the acid, base, conjugate acid, and conjugate base in this reaction NaOH(aq) + RCOOR’(aq) ➝…

A: NaOH (aq) + RCOOR' (aq)    → RCO2Na(aq) + R'OH (aq)

Q: 12+ + (n-1)+ + How does the equilibrium constant of this acid-base reaction between a hydrated metal…

A: Reaction of a metal cation with water molecule is a type of acid-base reaction more specifically it…

Q: What is the pH of .03 M HC2H3O2 (aq)? O 10.07 O 1.52 O 4.74 O 3.13 O 6.27

A: Ka is acid dissociation constant which determines strength of acid. Stronger acid dissociates more…

Q: Lalculate the pH of the resulting solution if 29.0 mL of 0.290 M HCI(aq) is added to 39.0 mL of…

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Q: why does the equilibrium concentration of H+(aq) increase as the concentration of a weak acid…

A: Acid dissociation constant is the physical constant used to determine the strength of an acid. It is…

Q: Select the conjugate acid-base pairs for the reaction:   CH3CO2H(aq) + H2O(l) ↔ CH3CO2-(aq)  +…

A: Conjugate acid -base pair - When an base abstract a proton from a acid it forms it's conjugate acid…

Q: hat is the equilibrium constant expression for the following reaction?   2 NaHCO3 (aq) ⇌ Na2CO3…

A: Let , consider a general reaction aA +bB →cC +dDThe equlibrium constant  in term of…

Q: Calculate the value of the equilibrium constant for the below reaction: HF (aq) + CN (aq) = HCN (aq)…

A: The reaction given is, => HF (aq) + CN- (aq) ------> HCN (aq) + F- (aq)

Q: (a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH,…

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Q: What is the pH of 2.7 x 102 M NaOH(aq)? O 3.6 O 1.6 Ο 12.4 O 13.1 O 10.4

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Q: Ammonium nitrate NH4NO3 is a salt used in fertilizers and in making matches. The salt is made by the…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

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.