At 25 °C, how many dissociated OH– ions are there in 1291 mL of an aqueous solution whose pH is 1.39?

Q: Write the Lewis structures of the reactants and product of each of the following equations, and…

A: To determine the Lewis structure of the reactants and product as given below, A Lewis acid is…

Q: The base Ca(OH)2 is almost insoluble in water , only 0,25 g can be dissolved in 0,5 L of water at 25…

A: Base is the substance which gives hydroxide ion in the solution while acid gives proton in the…

Q: The value of K, is 2.55 x 10 for a weak monoprotic acid whose initial concentration is 0.244 M. What…

A:

Q: What should the pH be for a 0.1 M solution of a strong monoprotic acid? If these strong acids are at…

A: pH calculation for a strong monoprotic acid :

Q: c) Define Lewis acid and Lewis base. Identify the Lewis acid and Lewis Base in the following…

A: Given : We have to identify Lewis acid and Lewis base.

Q: What is the pH of an aqueous solution of 1.69×10-² M hydroiodic acid?

A: Concentration of hydronium ion H3O+ present in the solution is known as the pH of the solution.

Q: What is the pH of a solution in which 15 mL of 0.39 M NaOH is added to 25 mL of 0.39 M HCl?

A: Since NaOH and HCl are strong base and acid respectively Hence they will react as per the reaction…

Q: Phosphoric acid H3PO4 is a weak acid, where as hydrochloric acid is a strong acid. Explain how the…

A: A weak acid is defined as an acid which undergoes partial ionisation in aqueous solution. A strong…

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: The ionization of NH4Cl as follows,

Q: What is the pH of an aqueous solution of 1.45×10-2 M nitric acid?

A: Nitric acid i.e HNO3 is a strong acid. Hence it dissociates into ions completely as per the…

Q: The pH of solution of Ba(OH)2is 10.66 at 25oC. What is the hydroxide ion concentration in the…

A: Given that, pH of solution is 10.66

Q: The Ka of hypobromous acid, HOBr, is 2.6x10-9. Calculate the pH of a solution which is composed of…

A: Given :-  [HOBr] = 0.40 M  [NaOBr] = 0.40 M Ka for HOBr = 2.6 × 10-9  To calculate :-  pH of…

Q: How do I calculate pH of a salt? for example in 0.10 M NaClO4(aq)?

A: Salt are produced by the reaction of an acid and a base. For example, The pH of salt is given as :

Q: A sample of 7.5 L of NH3 gas at 22 °C and 735 torr is bubbled into a 0.50-L solution of 0.40 M HCl.…

A: The negative logarithmic concentration of hydronium ions in a solution is called the pH of the…

Q: Calculate pH, pOH, [OH-(aq)] and [H30*(aq)] of a 350.0 mL aqueous solution containing 1.20 g calcium…

A: Mass of Ca(OH)2 = 1.20 g  Molar mass ( MM ) of Ca(OH)2 ,         = MM of Ca +2×  MM of O + 2 × MM oH…

Q: What is the pH of 500 mL of water after the addition of 50 mL of 25 mM HCl?

A: Since,      Numbers of moles  =  Molarity solution×volume of solution                   of…

Q: Given a mixture of 100cm3 of 1.01M HCl and 400cm3 of 0.04 NaOH, calculate the pH of the solution.

A: We have given that Volume of HCl = V1 = 100ml Molarity of HCl = M1 = 1.01M Volume of NaOH = V2…

Q: A weak acid, HA, is a monoprotic acid. A solution that is 0.140 M in HA has a pH of 1.800 at 25°C.…

A: In this question, we will determine the Ka value and degree of ionization.  How we can calculate,…

Q: Suppose a 0.10OM solution of each of the following substances is prepared. Rank the pH of the…

A: There are some substance :-  KF, NH4I ,HBr, NaCl, LiOH . We have to calculate the PH of the  0.100M…

Q: Write complete Lewis structures of the molecules in the following reactions. Which is the Lewis acid…

A: Lewis structures of the molecules: a). In this reaction, NH3 acts as a Lewis base because, the…

Q: Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCI(aq) and 0.060 M in…

A: Answer :-  1) 0.030 M HCl    a) pH = 1.52     b) pOH = 12.48…

Q: What is the pH of a solution made by mixing 40.0 mL of 0.035 M KOH (aq) and 91.3 mL of 0.031 M…

A:

Q: At 10°C, the ion-product constant of water, K w, is 6.88 × 10 –15. What is the pH of pure water at…

A: Autoionization of water takes place as follows: The product of the concentration of the hydronium…

Q: 6.7 x 10, What is the pH of A solution at 25 °C has [OH] = the solution?

A: Number 1 :- Given :- [OH-] = 6.7 × 10-3  To calculate :- pH of solution

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 1.4 × 10⁻⁴ M. What is the…

A: Given information: Concentration of hydroxide ions = 1.4×10-4 M

Q: At 25 °C, how many dissociated OH ions are there in 1221 mL of an aqueous solution whose pH is 1.26?…

A: pH of an aqueous solution is given 1.26. we know,  pH + pOH=14 Or, 1.26+ pOH=14 Or, pOH=…

Q: The PH of a solution of HCL in water is found to be 1.20.What volume of water would be added to…

A: Formula used  M1V1= M2V2

Q: The pH of an aqueous solution of 0.508 M phenol (a weak acid) , C6H5OH, is _______.

A: Since pKa for phenol is 9.98 and concentration of phenol is 0.508 M (given)

Q: Which of the following are likely to act as Lewis acids and which as Lewis bases? Explain. (a) AlBrs…

A:

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

A:

Q: How many grams of NaOH must be added to 250 mL of 0.10 M HC2H302 in order to bring the pH to 4.50?

A: To calculate the mass of NaOH, it is required to calculate the number of moles, which can be…

Q: 1. Calculate the pH of a solution prepared by dissolving 2.13 g of picric acid, (NO2);C6H2OH (229.11…

A:

Q: 9. The base ionization constant K, describes which of the following reactions for a weak base, B, in…

A: Base dissociation constant ( Kb ) is the equilibrium constant that refers to the ionisation or…

Q: Complete each of the following equations. Then write the Lewis formulas of the reactants and…

A: Lewis gave the definition of an acid or base. According to him, an acid is a substance which can…

Q: What is the significance of determining the pH of an antacid preparation?

A: ANSWER

Q: What feature must a molecule or ion have for it to act as a Lewis base? A Lewis acid? Explain the…

A:

Q: How many moles of nitric acid do you have in a 0.650 L solution of 0.035 M nitric acid? What is the…

A: Given Data :  Nitric acid molar conc. = 0.035 M Volume of nitric acid = 0.650 L Mole of nitric acid…

Q: 6. How many moles of benzoic acid (HC-HsO2) must be used to prepare 500. mL of a solution that has a…

A:

Q: What is the concentration of hydroxide ion in a 0.150 M aqueous solution of hydroxylamine, NH,OH?…

A: NH4OH is a weak base, hence it can't dissociate completely, hence equilibrium is established between…

Q: The pH of a 1.00 M solution of urea, a weak organic base, is 7.050. Calculate the Ka of protonated…

A: [CH4N2O] = 1.00 M pH = 7.050 Calculating the [H3O+] from the given pH value, pH = -log[H3O+] [H3O+]…

Q: What is the pH, pOH and [H​3O​+​​] of a 0.022M Sr(OH)​2​ solution?

A:

Q: How many grams of NaHCO3 must be added to 4 g K2CO3 to give a pH of 10.80 in 500 ml total solution?

A: Henderson-Hasselbach equation is given by: pH = pKa + logA-HAwhere [HA] is the concentration of the…

Q: The pOH of an aqueous solution of 0.509 M diethylamine (a weak base with the formula (C,H),NH) is

A: Given: concentration of diethylamine = 0.509 M Kb of diethylamine = 6.9×10-4

Q: The concentration of hydroxide ion in an aqueous solution at 25°C is 1.6 × 10⁻⁴ M. What is the…

A: Relation between concentration of hydronium ion and concentration of hydroxide ion: [H3O+] [OH-] =…

Q: A barium hydroxide aqueous solution has pH of 10.87. Calculate its molar concentration

A:

Q: The pH of an aqueous solution at 25°C was found to be 2.90. The pOH of this solution is 11.10 The…

A: Given :-  pH of solution at 25°C = 2.90  To calculate :-  pOH  [H3O+]  [OH-]

Q: What is the pH of a 0.200 M NaHCO, solution? The K, for HCO, is 5.6 x 1011

A:

Q: What is the pH of the resulting solution if 25.0 mL of 1.12 M HCl is mixed with 60.0 mL of 0.25 M…

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.