What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make 450. mL of solution? Assume that Ba(OH)2 dissociates completely in water to Ba2+ and OH¯ ions. What is the pH of the solution?

Q: Two 0.10 mol samples of the hypothetical monoprotic acids HA(aq) and HB(aq) are used to prepare 1.0L…

A: Given : Two hypothetical monoprotic acids i.e HA and HB. Moles of acid HA = moles of acid HB = 0.10…

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: Calculate the pH for basic solution pOH =6?

A: The relation between pH and pOH is  pH +pOH = 14 Given pOH = 6

Q: Determine the equilibrium constant given: NH4NO3(s)  N2O(g) + 2 H2O(aq)

A: For the given equilibrium reaction: NH4NO3(s) ⇌ N2O(g) + 2 H2O(l) Here decomposition of ammonium…

Q: Calculate the concentration of CO32- in an aqueous solution of 0.168 M carbonic acid, H2CO3 (ag).…

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Q: Suppose that, instead of using NaOH, a base such as Ba(OH)2 had been used. What changes in the…

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Q: Complete and balance the following acid-base neutralization reaction: 1 H2SO4 + 2 NaOH

A: Balance chemical equation is defined as which has equal number of atoms or ions in both sides…

Q: Calculate the pH of a 0.25 M solution of aluminum chloride, which dissolves completely to give the…

A: Concentration of aluminum chloride solution = 0.25 M   The equation for the reaction: Al(H2O)63+(aq)…

Q: What is the pH of a solution containing 3.2 x 10-6 M hydronium ions

A: The pH of a solution determines the acidity and basicity of a solution, which is calculated using…

Q: Potassium sorbate,KC H,O, (molar mass 150. g/mol) is commonly added to diet soft drinks as a…

A: Solution: Dissociation expression is a dissociation constant ( equilibrium constant). For acid…

Q: What is the pH of a 1.00 x 10^-9 molar solution of MgCl2?

A: The pH of a 1.00 x 10^-9 molar solution of MgCl2 is given below

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO, is 4.5 x 104)?

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Q: Calculate the pH, pOH and [OH ] of a 0.0420 mol/L a strong acid, HNO, (aq) solution.

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Q: Write the balanced molecular equation for the neutralization reaction between HIHI and…

A: When an acid and base reacts with each other to form salt and water and involves H+ and OH- ions in…

Q: Calculate the pH of the following solutions in which the [H+] is a) 0.01, b) 1.0 x 10 –8 , and c)…

A: Given that -  Hydrogen ion concentration , [H+] are -  a) 0.01 b)1.0 x 10 –8  c) 4.67 x 10 –4  Then,…

Q: A. What is the pH of an aqueous solution with a hydrogen ion concentration of [H+]=4.9×10−7M? B.…

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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: What is the pH of a 0.0490 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

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Q: complete the balance neutralization of the equation for the reaction HC2H3)2 + Sr (OH)2 .

A: Strontium Hydroxide + Oxalic acid --------- Strontium Oxalate + water.

Q: The pH at the stoichiometric point for the titration of a strong acid with a strong base is (= 7, >…

A: To solve this problem we have to explain the pH of titration of given Solution

Q: What is pH of a 0.1 Molar solution of oxalic acid in water

A: Given : Concentration of oxalic acid i.e H2C2O4 = 0.1 M The Ka1 and Ka2 of oxalic acid are 5.0 X…

Q: Malonic acid, H2C3H2O4 (aq), is a diprotic acid, so 2 moles of hydroxide ions are required per mole…

A: A neutralization reaction can be described as a chemical reaction in which acid and base react…

Q: Phosphoric acid, H3PO4 (aq), is found in soda. Write the balanced chemical equation for the…

A: Given,  The balanced reaction for the neutralization of phosphoric acid (H3PO4 ) and NaOH is:

Q: What is the pH of a 0.103 M aqueous solution of potassium hypochlorite, KCIO? This solution is pH =

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Q: For a tablet containing 1000 mg of vitamin C, calculate the minimum concentration of the NaOH…

A: Given that :  Mass of vitamin C = 1000mg = 1000mg×1g/1000mg = 1.00g Volume of NaOH used to…

Q: The concentration of hydronium ion in a sample is 3.5 x 10-7 mol/L. What is the pH of the above…

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Q: What is the pH of a 0.0338 M nitric acid, HNO3, solution?

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Q: Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when…

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Q: 1. When H2SO<(aq) was reacted with NaOH(aq) in the titration, why was a precipitate not formed? 2.…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: A sample of calcium hydroxide (Ca(OH)2) has a concentration of 0.00473 mol/L. What is the pH of this…

A: The PH of Ca(OH)2 can be calculated as follows

Q: Find the pH of a 0.155 M HClO2(aq) solution

A: As we know that the acid ionization constant (Ka) for HCIO₂(aq) is 0.011. The equation for…

Q: What are the concentrations of H3O+, HC2O4− and the oxalate ion, C2O42−? What is the pH of a 0.10 M…

A: Given data, Concentration of oxalic acid = 0.10M Data taken from google; Ka1 = 6.5 x 10-2 Ka2 = 6.1…

Q: Determine the pH of a 1.2 M solution of ammonia, NH3, with K 1.8 x 105

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Q: Complete and balance the following neutralization reaction: Fe(OH)2 + HNO3 ———->

A: Neutralization reaction: The hydrogen ion of acid reacts with the hydroxide ion of a base to form…

Q: What is the pH of a 0.031 M solution of aqueous Sr(OH)2? 1.21 1.51 12.49 12.79

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: Write the balanced neutralization reaction between Ca(OH), and HBr.

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Q: Fill in the left side of this equilibrium constant equation for the reaction of nitrous acid (HNO,)…

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Q: For H2CO3, Ka1 = 4.3 x 10 7, Ka2 = 4.7 × 10 11. What is the pH of a 0.11 M solution of carbonic…

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Q: Determine the pH of a 0.0400 mol / L solution of H 2 S (aq).

A: The pH of a solution can be determined by the hydrogen ion's concentration. It is the negative…

Q: Lactic acid (ch3ch(oh)cooh) is produced by bacteria in the mouth from food residues and is…

A: Given that,  Concentration of lactic acid sample = 0.528 mol/L Ka value of lactic acid = 1.4×10-4…

Q: Chemists working with fluorine and its compounds some- times find it helpful to think in terms of…

A: (a) would the acid in this system be the fluoride donor or fluoride exceptor  (b) Identify the acid…

Q: According to the Arrhenius concept, if Al(OH)3 were dissolved in water, it would act as: A) a…

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Q: Write the products of the reaction between the acid KHP and the base NaOH, and balance the reaction:…

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Q: Ag+ (aq)  +  Cl–   (aq)     →     AgCl (s)               Delta H = ? What is the enthalpy change…

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Q: How many moles of hydroxide ions can be released into solution from 1.00 mg of Mg(OH)2 that is used…

A: Molar mass of Mg(OH)2 = 58.32 g/mol Given mass = 1 mg = 0.001g Moles = 0.001/58.32 = 1.71*10-5

Q: A. What is the pH of an aqueous solution with a hydrogen ion concentration of…

A: Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What are the pH, pOH and [H3O]+ for a 2.37 x 10-2M HClO4 solution? HClO4 is a strong mineral acid.

A: Given Data

Q: What is the pH of a 2.12.1 M solution of HClO4?

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Q: 0.100 M HCL, what will be the pH of the resulting solution? Ca(OH)2 (aq) + HCl (aq) CaCl2 (aq) + H2O…

A: Applying concept of molarity equation MV= M2V2 -M1V1

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.