In the reaction below, which reactant is the Lewis acid? Cr* + 6 H2O –→ Cr(H2O)6³+ A) Cr³* B) H2O C) Cr(H2O)3+ D) None of these are Lewis acids.

Q: What volume of (0.45 M) Ca(OH)2 must be added to 50 mL of 0.25-M (KOH) to give a solution 0.8 M in…

A: Concentration of Ca(OH)2 =0.45M Valume of KOH = 50ml Concentration of KOH =0.25M Concentration of…

Q: B: What is the pH of 0.6 M NH.CI solution? Discuss yon

A: It undergo salt hydrolysis  It's pH = 7 - 1/2( pKb + logC) Where  PKb = - log Kb = - log 1.8 x 10-5…

Q: Consider the ionization of the 0.134 M carbonic acid, H₂CO,. H2CO3 + H2O = HCO3 + H3O+ HCO3 + H2O =…

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Q: What will happen when  CH3NH3Cl is added to a CH3NH2 solution? Will it change the pH of the solution…

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Q: A solution is made by dissolving 16.9 g of CH3NH₂NO3 in 500.0 mL of water. 1 As CH3NH3* is an acid,…

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Q: 11. For the weak base piperidine, CsHioNH, K. = 1.30 x 10-3. What is the equilibrium concentration…

A: 11) Reaction- C5H10NH + H2O  →      C5H10NH2+ + OH-

Q: When COCI2 is placed in a container with a pressure of 4.1 atm, determine the equilibrium…

A: Since you have posted multiple questions as per guidelines we can answer only one per session . If…

Q: Consider the reaction below: Pb(NO3)4(aq) + 4 NaOH(aq) ----> _ Compound A + _ Compound B (OR Pb(N…

A:

Q: Done 7 Part A Calculating pH What is the pH of an aqueous solution with the hydronium ion…

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Q: In each of the following acid-base reactions, identify the Brønsted acid and base on the left and…

A: According to Bronsted-Lowry theory,  Acid is species which donates proton and Base is species which…

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH4B (M=98) , is used to make 200 mL of…

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Q: MISSED THIS? Watch KCV 16.6, IWE 16.3; Read Section 16.6. You can click on the Review link to access…

A: The pH of a solution is the negative logarithmic concentration of hydronium or hydrogen ions. The pH…

Q: . The equilibrium constant for the dissociation of a weak acid of the type, HA⇌H++ A-, would be:…

A:

Q: What is the pH of a solution that is 0.250 M in KH2PO4 and 0.600 M in K2HPO4

A: Given -> [KH2PO4] = 0.250 M  [K2HPO4] = 0.600 M

Q: 3. Calculate the equilibrium constant of the following reaction: H;S = 2H* + S Knowing that H;S has…

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Q: 1. What will the color of the extract solution be if the pOH=2? 2. What is the [H30+] for a solution…

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Q: 4. a. What is the pH, and the equilibrium concentrations for [H*], [CH³COO-], [CH3COOH] and [OH-] in…

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Q: H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8 What is the equilibrium constant…

A: When we subtract two equations; value of equilibrium constant gets divided.Equilibrium constant is…

Q: a) Find the pH of a 500 mL aqueous buffer solution prepared with 3.81 g of H3BO3 and 4.55 gof…

A:

Q: What Al(III) species is the major species in aqueous solution at pH 14.0 ?   a) [Al(H2O)6]3+ b)…

A: pH stands for "potential of hydrogen" and is a measure of the acidity or alkalinity of a solution. A…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: What is the [OH–] in an aqueous solution with [H3O+] 1.30 mol L–1

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Q: There is a buffer solution containing 0.50 M acetic acid (CH3COOH, Ka= 1.8 X 10-5) and 0.50 M sodium…

A: A buffer is used to maintain the pH of the solution when the addition of acid or base is done. pH of…

Q: Consider the weak acid, HA, in water as shown in the reaction below. The [HA] initially is 0.3120 M…

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Q: 2. Consider the following reaction: HCO, (aq) = H+(aq)+ CO?-(aq) at room temperature (298 K). a)…

A: For a spontaneous reaction ∆Greaction <0  And ∆G = ∆G° + RTlnQ  Where Q is reaction quotient  T =…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

A:

Q: Which of the following species is amphoteric? CO32– HF NH4+ Two of species listed are amphoteric.…

A: Out of the given species only HSO4- is amphoteric in nature.

Q: 5. Write an equation for the single-proton transfer reaction with water for the following acids.…

A: Since you have asked multiple question as per our company guidelines we are supposed to answer the…

Q: Calculate the pH of a 0.58 M CH3CO2H solution

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Q: Which of the following statements is TRUE? Select one: A solution with a pOH of 9 is basic. A 1 M…

A: The pH is an acidity or basicity measurement in an aqueous solution. The pH levels for acidic…

Q: What are the

A: let us take  ethyl amine concentration "C"                   C2H5NH2    +  H2O   -->   C2H5NH3+…

Q: In the following chemical reaction identify the acid. Don't worry about the charges and no need for…

A: Given [Al(H2O)6]3+ + 3H2O →  [AI(H2O)3(OH)3]2+ +  3H3O+

Q: Calculate the pH of Ka for HCHO₂ is 1.8 × 10 a 0.10 M Na CHO₂ solution. -4

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Q: a) What is the pH and pOH of 0.001 M NaOH solution, which is the strong base? b) The Ka value of…

A: pH + pOH = 14 pOH = -log [OH-] For a weak acid: [H+] = (Ka x C)1/2 Where, C = molar concentration

Q: Calculate the [H+] concentrate if pOH = 5.35

A:

Q: Calculate the pH of the solution that results when 15.0 mL of 0.1600 M lactic acid a. diluted to…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Consider the following acid-base reaction: H3O+ + HPO42- H₂PO4 + H₂O Identify the Bronsted-Lowry…

A: Answer:- This question is answered by using the simple concept of Bronsted Lowry concept of base…

Q: For the reaction below: which base(s) (I – V) will have an equilibrium constant greater than 1 Base…

A: Equilibrium is a condition at which the concentration of different species remains same over time.…

Q: Shoifuton stulib vito gostmenop isaillent elle SECTION 4: APPLICATION 7. Bones and teeth consist…

A: An acid will donate hydrogen ions and a base will donate hydroxide ions in the solution. It can be…

Q: Which of the following K values would indicate the weakest base of the group? O 1.2 x 109 O 6.3 x…

A: Ans:- (1.2×10-9 is the weakest base of the group).

Q: NH3 is a weak base (K, = 1.8 × 10-') and so the salt NH4CI acts as a weak acid. What is the pH of a…

A: Given, Concentration of NH4Cl solution = 0.075 M Kb for NH3 = 1.8 × 10-5 pH of the solution = ?…

Q: Complete the balanced molecular reaction for the following weak base with a strong acid: NaCIO2(aq)…

A: Given,

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.