Balance the following equation in a basic sol Mo2O72- + Br2   ⟶   Mo3+ + BrO3-

Q: pH is a solution containing 0.81M HA and 0.35M A-? KaHA= 5.45 x 10 ^ -8

A: According to the Henderson-hassleblach equation, the pH of any buffer type solution can be…

Q: Calculate the oh of a solution that is prepared by adding 45.0 m, of 0.050M HI to 25.0 ml of 0.050M…

A: Given: The volume of HI = 45 mL. The volume of Ba(OH)2  25 mL. The concentration of HI = 0.05 M. The…

Q: When 14.08 mL of 0.1594 M NaOH is added to 25.00 mL of 0.1235 M HX (an unknown weak acid), the…

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Q: 1.MnO4-(aq) + CH3OH (aq) ...........>Mn2+ (aq) + HCO2H (aq) (acidic solution) 2.Pb(OH)42-(aq) +…

A: (1)Seven steps are required to balance the given redox reaction in acid solution. First reduction…

Q: A solution turns red litmus blue, its pH is likely to be(a) 1(b) 4(c) 5 (d) 10

A: An important concept of pH can be given as: Acids have a pH level below 7 Bases have a pH level…

Q: Calculate the pH of a 0.082 molar NaF solution (Ka for HF is 7.1X10^-4)

A: The pH of a 0.082 molar NaF solution is to be calculated. (Ka for HF is 7.1×10-4).

Q: 5.00 g NaOH and 5.00 g Ba(OH)2 were used to prepare 1L solution each. Which solution will bo more…

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Q: Which of the following species is amphoteric? O co,? O HF O NHA O HPO42 None of the above are…

A: Amphoteric species are those which can act as both Brønsted -Lowry acid and Brønsted -Lowry base.…

Q: What is the pH of a solution made by mixing 0.30 molNaOH, 0.25 mol Na2HPO4, and 0.20 mol H3PO4 with…

A: Record the given data, 0.20 mol of H3PO4 react with NaOH completely to form 0.20 mol of NaH2PO4 (the…

Q: [References] Using the Bronsted-Lowry model, write an equation to show why the following species…

A: PO43- is an acid when it is treated with H2O it will form a pair of conjugate acid and conjugate…

Q: Q3|| A. Calculate the PH of the (0. 1 N) Na;PO, in 250 ml B. What is the Normality of a sulfuric…

A: The given data contains, concentration of Na3PO4=0.1 N

Q: Calculate the hydrogen ion (H") concentraion of a solution with pH of 1.06

A: Given that, pH= 1.06

Q: What [H2C03] needs to be added to 0.0250M NaHCO3 to obtain a buffer solution with a pH of 7.0?

A: A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate…

Q: 2) Calculate the PH of the solution if Ece = 0.10 when [Co*] = 0.45 M, [H:] = 0.30 M, and PH = -log…

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Q: Calculate the pH of a solution that is 0.0100 M in HCl and 0.0150 M in H2SO4. (Ka2…

A: 0.0100 M in HCl and 0.0150 M in H2SO4 As HCl is monobasic it gives one H+ per molecule concentration…

Q: A 1.00 M solution of which electrolyte will have pH = 7.00 at 25 C? I. CaBr2 II. NHẠNO3 III. LICN…

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Q: Calculate the pH of a 0.15M solution of sodium acetate (CH3COONa). What is the percent hydrolysis?…

A: A strong base and weak acid react to form salt and water. The salt will be basic in nature and the…

Q: 3. Carbonic acid, H2CO3, can be found in a wide Calculate the hydronium -ion concentration of a…

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Q: Water with an alkalinity of 2.00 x 10-3 eq/L has a pH of 7.0. Calculate [CO2], [HCO3-], [CO32-], and…

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Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56

A: The concept used here is based on the acid dissociation constant of an acid which is used for…

Q: The acid ionization constant for Fe(H2O6)3+ is 7.7x10^-3. Calculate the pH of a 0.3300 M solution of…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the given…

Q: 0.1 M NaHCO3 solution, using the given pH data, calculate value of (Ka or Kb)

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Q: 3. Complete the following equations for the addition of an acid and base to phosphate buffer…

A: Quick summery:  a) In  acidic solution phosphare buffer act as base and abstract proton. b) In basic…

Q: Balance the equation below assuming it occur in a basic solution. NO3−(??)+H2(?)⟶NO(?)

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Q: A solution NaOH has 0,04%w/v. Find the pH of the solution, when it is given that the solution NaOH…

A: pH is defined as the negative logarithm of Hydrogen ion concentration. In Chemistry, pH denotes as…

Q: ions? PH of a solution depends on concentration of- ---- O a. Hydrogen O b. Nitrate c. Sulfate O d.…

A: PH is the negative logarithm of concentration of H+.

Q: If

A: Given: 50 mL of 2.00HCN(Ka=6.210×10-10) is diluted to 1.00 L. To find: pH of the solution.

Q: balamıd the Solution. Show each step involud in balaneng the reachon deanly. bedox reaction thaT…

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Q: Write the Mass Balance Equation, Proton-Balance Equation and Charge Balance Equation for the…

A: Charge Balance Equation (CBE): It is based on electroneutrality principle. The molar concentration…

Q: Calculate the [OH] in 0.2110 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2…

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Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…

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Q: When the following equation is balanced properly under acidic conditions, what are the coefficients…

A: The electrochemical method that comprises two half-reactions, in that reaction one is…

Q: Balance the following skeleton reactions and identify the ox-idizing and reducing agents

A: Since you have posted question with multiple sub-parts, we will solve two question for you. To get…

Q: Ht = PH=4 043= A cidic/basic

A: Concept: pH= - log [H+] pOH = - log [OH-] pH+pOH = 14 [H+] = 10-pH  [OH-] = 10-pOH  If pH less than…

Q: Nahso3 titr. In neutral describe how the color goes from Mn04- to MnO2 In basic w NaOH describe…

A: Answer-1 In neutral medium, SO32- ion of NaHSO3 is oxidized by MnO4- ion into sulfate ion and MnO4-…

Q: What

A: Hinderson equation is used for calculating the pH of the buffer solution.  pH = pKa + log( [salt] /…

Q: Calculate the pH of a solution that is 0.66 M HNO, and 1.10 M KNO,. 3.372

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: Calculate the pH of a solution containing 0.085 M nitrous acid (HNO2, Ka = 4.5 * 10-4) and 0.10 M…

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Q: Calculate the pH for a 4.3 × 10−8 M HCl solution with an ionic strength of m = 0.1. yH+ = 0.83, yOH−…

A: We have to Calculate the pH for a 4.3 × 10−8 M HCl solution

Q: Vhat is the pOH of a solution with [H,O)=1x10-5M 9. 4 10

A: This is ionic equilibrium chemistry

Q: A 0.100 M solution of bromoacetic acid (BrCH2COOH) is13.2% ionized. Calculate [H+], [BrCH2COO-],…

A: Solution of bromoacetic acid, 0.100M is ionized 13.2%. The percent ionization is defined as ratio of…

Q: What volume of 0.317 M KOH solution will be required to titrate 25.00 mL of 0.285 M HNO3?

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: Calculate the Fe3+ concentration free in a solution of FeY- 0.10 mol / L at pH 4.0 and pH 10.0.

A: The question is based on complexometric titrations. we have to observe the effect of PH on the…

Q: What. is the addit.on the pH of 25.0mLof resulting from e solution with pH 3,550 I1.25e? (10.9) of…

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Q: CuS will be solub‎le in aci‎dic pH bec‎ause a. S-2 is the con‎jugate b‎ase of a we‎ak acid‎, H2S…

A: Answer - The correct option is (d) S-2 is the conjug‎ate base of a we‎ak acid HS- and Cu+2 is…

Q: Write the molecular equation which completes the following. The reaction occurs in an aqueous…

A: the reaction is  K2S + HCl→ KCl + H2S

Q: Determine the pH of a 0.24 M solution of sodium acetate (CH3COONa) at 25°C.(Ka of acetic acid = 1.8…

A: Equation for the ionization of CH3COONa is: [CH3COONa] is 0.24 M. It implies 0.24 mols of CH3COONa…

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.