A 50.0 mL sample of H2SO4 is neutralized with a KOH solution having a concentration of 0.400 M. If 22.6 mL of KOH are required to complete the neutralization, what is the concentration of the sulfuric acid solution?

Q: A 35.0 mL solution of NaOH is neutralized with 23.4 mL of 0.250 M HCl. What is the concentration of…

A: Solution C1V1= C2V2 where,  C1, C2 - concentrations V1, V2 - volumes Given, C1= 0.250 M V1= 35 ml,…

Q: Exactly 41.00 mL of 0.100 M NaOH is used to titrate a 25.00 mL sample of HNO3 . What is the…

A: Volume of NaOH = 41.00 mL Concentration of NaOH = 0.100 M Volume of HNO3 = 25.00 mL

Q: If it takes 23.8 mL of a 1.85M stock solution of HCL to neutralize 50.0 mL of an NaOH solution, what…

A:

Q: What is the molar concentration of sodium ions in a 0.350 M Na,sO4 solution? A) 0.350 M O B) 1.05M…

A: Na2SO4 In one Mole of Na2SO4, there are 2 moles of Na

Q: What volume (in mL) of 0.2900 M HCl is required to neutralize 50.00mL of 0.8000M NaOH?

A: Given -> Molarity of HCl = 0.2900 M = M1 Molarity of NaOH = 0.8000M = M2 Volume of NaOH = 50.00…

Q: How many milliliters of 0.100 M HClO₃ are required to neutralize 40.0 mL of 0.235 M KOH?

A: To determine the volume of HClO₃ in millilitres. Using the formula. n1 is the number of equivalent…

Q: In the neutralization reaction below17.3 mL of H2SO4 solution are required to neutralize 32.2 mL of…

A:

Q: It takes 18.5 mL of a 0.24 M HCl solution to neutralize 245 mL of NaOH solution. What is the…

A: Balance chemical equation: HCl + NaOH -----> NaCl  +  H2O By stoichiometry of reaction: Moles of…

Q: Calculate the molarity of a HCl solution when 30.00 mL of it required 28.75 mL NaOH to neutralize…

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Q: An unknown triprotic acid requires 13.33 mL of 0.117 M NAOH to completely neutralize a 0.229 g…

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Q: concentration of OH- in a sample is 2.2 x 10-6 M, what is the molar concentration of H3O+?

A: [OH-] = 2.2 x 10-6 M  we know.   ,  [H3O+] * [OH-] = 10-14

Q: Sg(s) + 24 F2(g) → 8 SF6(g) 1. Single Displacement 2 C5H10(g) + 15 O2(g) → 10 CO2(g) + 10 H20(g) 2.…

A: Since you have asked multiple questions, we will answer the first question for you. For the rest of…

Q: Calculate the molarity for a solution of HNO3 if 4.16 g of Ca(OH)2 is neutralized by 16.5 mL of HNO3

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Q: The molar concentration of an unknown acid solution with general formula H3A is to be determined by…

A: Given Molarity of KOH=0.72 M Volume of KOH=33.33 ml Volume of H3A =17.363ml To determine the…

Q: Calculate the molarity of an HBr solution if 25.0mL of it were neutralized by 17.0mL of 2.50M KOH…

A: Number of moles of solute present in 1 liter of solution is known as molarity of the solution.

Q: 2.37 L solution containing 1.30 mol L-1 potassium hydroxide (KOH) has been left on your bench. How…

A: Given-> Volume of KOH = 2.37L Molarity of KOH = 1.30 mole/L

Q: If 37.5 mL of HNO3 is neutralized with 35 mL of 2.25 M KOH, what is the molarity a HNO3?

A: The neutralization reaction occurs when strong acid and strong base reacts to form salt and water.…

Q: How many milliliters of 0.0100 M Sr(OH)₂ are required to neutralize 65.0 mL of 0.0400 M HCl?

A: Given, M1 =  0.0100 M Sr(OH)₂ V1 =? M2 = 0.0400 M HCl V2 = 65.0 mL

Q: A 0.261 g sample of NaHC2O4 (one acidic proton) required 17.5 mL of sodium hydroxide solution for…

A: The complete balanced Chemical Reaction is - NaHC2O4 + NaOH ----> Na3C2O4 + H2O Thus, one mole of…

Q: Give an example of a strong base, and a strong acid.

A: The term "strong acid" refers to an acid that dissolves in water. The word "strong" relates to the…

Q: What volume (in mL) of 0.2250 M HCl is required to neutralize 60.00 mL of 0.7000 M KOH

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Q: How many grams of LiMnO4 are needed to prepare 1.10 L of a solution that has an ion concentration of…

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Q: What volume (in mL) of 0.2000 M HCI is required to neutralize 75.00 mL of 0.6000 M LIOH?

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Q: 31.2 mL of 0.20 M hydrobromic acid is required to neutralize 75.0 mL of a solution of barium…

A: Two mole of hydrobromic acid react with one mole of barium hydroxide

Q: Calculate the concentration (in molarity) of an N2OH solution if 25.0 mL of the solution is needed…

A: Solution stoichiometry involves the calculation of concentration of solutions in the given…

Q: A 30.0 mL solution of LiOH is neutralized with 28.5 mL of 0.150 M HBr. What is the concentration of…

A: Given: Volume of LiOH solution = 30 mL Volume of HBr = 28.5 mL Concentration of HBr= 0.150 M To…

Q: 76.4 mL of 0.25 M lithium hydroxide are needed to completely neutralize 250.0 mL of a solution of…

A: Using stoichiometric ratio we can determine how many moles of H2SO4 neutralises. From that we can…

Q: If 5.00 mL of HCl requires 4.96 mL of 0.9581 M NaOH to consume the HCl, what is the concentration of…

A: GivenVolume of HCl = 5.00mlVolume of NaOH = 4.96mlMolarity of NaOH = 0.9581MThe objective is to find…

Q: A flask containing 10.0 mL of HCl acid is neutralized by 20.00 mL of 0.125M NaOH.  What is the HCl…

A:

Q: What mass of the antacid CaCO3 is required to neutralize the acid in a 290 mL solution of 0.227 M…

A: Formulas to calculate moles of a substance: Moles = mass (g)molar mass gmol…

Q: A 12.5 mL volume of 0.500 M H2SO4 neutralizes 50.0 mL of NaOH. What is the concentration of the…

A: Given, Volume of H2SO4 =12.5ml Concentration of H2SO4 = 0.5M Volume of NaOH= 50.0 ml Titration of…

Q: 19.42 grams of potassium chromate, K2CrO4, are dissolved in sufficient water To have 500 ml of…

A: The question is based on the concept of solutions.   Molarity is a method of expressing…

Q: What is the concentration of H+ ions in a solution of hydrochloric acid that was prepared by…

A: Given, 20.0 mL of concentrated (11.6 M ) HCl

Q: 2. A 3.0 ml sample of HNO, solution is exactly neutralized by 6.0 mL of 0.5 M KOH. What is the…

A: To neutralize by KOH, the number of moles of HNO3 must be equal to the number of moles of KOH. Given…

Q: Calculate the volume of 2.30 M sodium hydroxide that is needed to neutralize 2.9107 g of potassium…

A: To neutralize whole potassium hydrogen phthalate (KHP) we have to have  Number of moles of NaOH=…

Q: ne molarity c

A:

Q: A 40.0 mL solution of KOH is neutralized with 31.3 mL of 0.300 M HCl. What is the concentration of…

A:

Q: A 45.0 mL solution of LiOH is neutralized with 36.5 mL of 0.350 M HCl. What is the concentration of…

A: The objective of this question is to find the concentration of the original LiOH solution. This can…

Q: It takes 95 mL of a 0.49 M NaOH solution to neutralize 250 mL of an HCl solution. What is the…

A: HCl  +  NaOH  ------>   NaCl  + H2O So, for the neutralization: Number of mmol of HCl = Number of…

Q: A 45.0 mL solution of LiOH is neutralized with 36.5 mL of 0.350 M HCl. What is the concentration of…

A: Given The volume and concentration of HCl and the volume of LiOH.  To find Concentration of LiOH in…

Q: A solution of HCl is prepared by diluting 35.0 mL of a 1.0 M HCl solution with enough water to make…

A: Molarity can be defined as the ratio of number of moles of solute to the volume of the solution. The…

Q: If it takes 88 mL of 5.4 M KOH to neutralize 210 mL of sulfuric acid (H2SO4) solution, what is the…

A: The equivalence point is defined as the point in reaction when moles of acid equals the mole of base…

Q: calculate the volume (mL) of 0.120 M HCl to completely react with 0.1250 g of Na2CO3

A: Given  Molarity of HCl      = 0.120 M  mass of Na2CO3    =  0.1250 gram  Volume of HCl       = ?

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.