Assuming complete dissociation, what is the pH of a 4.94 mg/L Ba(OH)₂ solution? pH =

Q: Assuming complete dissociation, what is the pH of a 4.15 mg/L Ba(OH)₂ solution? pH =

A: Upon dissociation the base will give the hydroxide ions which will make the solution basic and from…

Q: A 25.0 mL volume of a sodium hydroxide solution requires 19.6 mL of a 0.189 M HCl solution for…

A: The objective of this question is to calculate the concentration of the phosphoric acid solution…

Q: What mass of KHP will be completely neutrilized by 32.57 ml 0.175 M standard NaOH solution? The…

A: The solution is as follows:

Q: If 24.6 mL of a Ca(OH)2 solution are added to neutralize 14.2 mL of 0.0140 M HC2H3O2, what is the…

A:

Q: What mass of Ca(OH)2 is required to neutralize 50.00mL of 0.180 M HCI?

A: Balanced chemical equation for the reaction between hydrochloric acid and calcium hydroxide is,

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.3 × 10⁻⁵. What is [H⁺]?

A: Given: [OH- ] = 2.3 × 10-5 M

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 2.7 × 10⁻³. What is [H⁺]?

A:

Q: If 94.92 mL of a solution of HCI are equivalent to 43.76 mL of a solution of NaOH and if 49.14 mL of…

A:

Q: What would be the concentration of X 2- if a 10 mL of a 1 M solution of KOH was added to 50 mL of a…

A: The chemical reaction for the neutralization of a diprotic acid H2X with KOH is needed to be…

Q: Which of these is NOT an example of a strong base? O All of these are strong bases Ba(OH)2 ONH4OH O…

A:

Q: In which container is hydrofluoric acid (HF) least ionized? 0.10 M HF 0.10 M HF 0.10 M HF 0.10 M HF…

A: Common ion effect: According to this effect the solubility of an ionic precipitate will decreases if…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 8.9 × 10⁻³. What is [H⁺]?

A: Product of hydrogen ion concentration and hydroxide ion concentration is equal to the ionic product…

Q: Mg(OH)2 + 2 HCI -> M9CI2 + 2 H2O Use the balanced chemical equation to calculate the mass and volume…

A:

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: Cranberry juice contains significant amounts of malic acid (H2C4H4O5), a diprotic acid, which…

A: Given that Malic acid is diprotic acid. The balanced equation for the reaction between malic acid…

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 8.5 × 10⁻³. What is [H⁺]?

A:

Q: Assuming complete dissociation, what is the pH of a 3.67 mg/L Ba(OH)₂ solution? pH =

A: The mass of barium hydroxide = 3.67 mg =         ( 1.0 mg = 10-3 g)Molar mass of Ba (OH)2, = 171.34…

Q: How many mL of 0.25 M HCl(aq) are needed to neutralize a 116.5 mL solution of 0.1 M Ba(OH)2?

A:

Q: H2SO4 + NAOH → BaCl2 H2O + КОН K3PO4

A:

Q: [Topic: Parts Per Million] Sodium hydrogen sulfate, NaHSO₄ , which is dissolved in water to release…

A: Given information:Mass of NaHSO4 = 550 gVolume of water = 4.5×105 L

Q: Each of the four flasks below contains the same volume of .10 M aqueous acid. All four acids are…

A: Since the volume and concentration of acid taken is same for all acids  Hence the moles of all acid…

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: The OH⁻ concentration in an aqueous solution at 25 °C is 8.3 × 10⁻³. What is [H⁺]

A:

Q: If 0.235 g of KHP requires 16.73 mL of NaOH solution to neutralize it, calculate the molarity of the…

A: The neutralization reaction is given below.

Q: Assuming complete dissociation, what is the pH of a 4.04 mg/L Ba(OH)2 solution? pH=

A: Given :  We have to calculate pH.

Q: Calculate the molar concentration of OH- in a water solution that has a molar concentration of H+…

A:

Q: The pOH of a solution is 9.33. Calculate the hydrogen ion concentration of the solution. Be sure…

A:

Q: What mass of Ca(OH)2 is required to neutralize 50.00 mL of 0.180 M HCl?

A: At complete neutralization, no of moles of the base is equal to the no of moles of acid.

Q: Assuming complete dissociation, what is the pH of a 4.12 mg/L Ba(OH)₂ solution? pH =

A:

Q: 1a) The hydronium ion concentration of an aqueous solution of 0.394 M diethylamine (a weak base with…

A:

Q: if it takes 25 mL of 0.05 M HCl to neutralize 345 mL of NaOH solution, what is the concentration of…

A: The objective of this question is to find the concentration of the NaOH solution. This can be done…

Q: 1. What is the pH of a 0.000012 M KOH? 2. What is the Normality of a 1.0 M Ca(OH)2 solution

A:

Q: Assuming complete dissociation, what is the pH of a 3.73 mg/L Ba(OH)₂ solution? pH: =

A:

Q: The OH⁻ concentration in an aqueous solution at 25 °C is 5.3 × 10⁻⁵. What is [H⁺]?

A: The sum of the concentration of hydroxide and hydronium ion is always 10-14. that means,…

Q: The formula for the conjugate acid of HPO42- is?   A student weighs out a 2.33 g sample of…

A: According Bronsted-Lowry acid and base theory, acids are substance which loses protons H+ to form…

Q: What volume of H2SO4 of concentration 0.04 M is required to completely neutralize 200 mL of Al(OH)3…

A:

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.