determine the pH of the resulting solutions when the 2 reagents are mixed together. 15.00mL of 0.1000M NH3 and 12.00mL of 0.1000M HCl  25.00mL of 0.2500M HC2H3O2 and 25.00mL of 0.2500M NaOH 25.00mL of .1500M HF and 30.00mL of 0.1500M NaOH

Q: What is the pH of a solution prepared by mixing 25.0 mL of 0.180 M HC,H30, with 40.0 mL of 0.250 M…

A: pH of the solution = 13.71

Q: Calculate the pH of a mixture of 106 mL of 0.112 M HI and 30 mL  of 0.45 M KOH

A:

Q: Calculate the pH of a solution made by mixing 100.0 mL of 0.110 M NaBrO with 75.0 mL of 0.140 M…

A: Given: Concentration of NaBrO = 0.110 M Concentration of HBrO = 0.140 M Volume of NaBrO = 100.0 mL…

Q: Calculate the pH of the solution resulting by mixing 20.0 mL of 0.15 M HCl with 20.0 mL of 0.10 M…

A: Given,Molarity of HCl solution =0.15 Mvolume of HCl solution =20.0 mLMolarity of KOH solution =0.10…

Q: Calculate the pH of a solution prepared by adding 25.0 mL of 0.10 M sodium hydroxide to 30.0 mL of…

A:

Q: Calculate the pH of the resulting solution when 350.0 mL of .400 M HCl is mixed with 35.0 mL of…

A:

Q: Determine the pH if 50.0 mL of 0.50 M HI solution is added to 0.027 L of a 0.10 M KOH solution

A: Given : 50.0 mL of 0.50 M HI solution is added to 0.027 L of a 0.10 M KOH solution  Tip : pH = -log…

Q: A sample of 1.25 L of HCl gas at 21 °C and 0.950 atm is bubbled through 0.500 L of 0.150 M NH3…

A: According to ideal gas law (for HCl moles calculation), PV = nRT where P = pressure = 0.950 atm V =…

Q: Calculate the pH when 15.52 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The neutralization reaction is given below.

Q: Calculate the pH of a solution resulting from the addition of 10.0 mL of 0.50M NaOH to 35.0 mL of…

A: This question belongs to Ionic equilibrium. Given 10.0 mL of 0.50M NaOH to 35.0 mL of 0.50M HCl. We…

Q: What is the pH of the solution obtained by mixing 65.00 mL of 0.220 MM HCl and 60.00 mL of 0.125…

A:

Q: Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: 1 Determine the pH of the resulting solutions when the following reagents are mixed. a. 25.00mL of…

A:

Q: Calculate the pH of a solution prepared by mixing 45.0 mL of 1.45 M sodium hydroxide with 56.0 mL of…

A:

Q: Calculate the pH of the resulting solution when 20.0 mL of 0. 150 M NaOH is added to 50.0 mL of…

A:

Q: Determine the pH of the resulting solution when 35.00mL of 0.2450M (CH3CH2)2NH is mixed with 10.50mL…

A:

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: What is the pH of an aqueous solution that consist 40.0 mL of 0.050 M HCl and 30.0 mL. solution…

A: pH: It is a scale that determines, whether the given compound or solution in acidic, basic or…

Q: Payalben

A: The objective of this question is to calculate the pH of a solution resulting from the mixture of…

Q: Solution A is prepared by adding 50 ml of 0.3M hypochlorous acid solution to 50 ml of 0.2M of sodium…

A: Given solution A prepared by mixing of weak acid - hypochlorous acid (HClO) with its salt with…

Q: Determine the pH of a solution that results when 15.0 mL of 2.00 mol/L NaOH is added to 25.0 mL…

A: This question belong to ionic equilibrium. pH calculation of mixture of strong acid and strong base.…

Q: Calculate the pH of solution obtained by mixing 500.0 mL of 0.10M NH3 with 200.0 mL of 0.15 M HCL

A: Henderson equation for a buffer of weak base and strong acid: pOH = pkb + log [salt]/[base] pH = 14…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.

A:

Q: 4- A liter of solution contains 0.25 M HCOOH and 0.3 M HCOONA, calculate the pH of this solution.…

A:

Q: Calculate the pH of a solution prepared by mixing 10.0 mL of 0.3 M HCl with 15.0 mL of 0.5 M NaOH.

A: We have given that Concentration of HCl = M1 = 0.3 M Volume of HCl = V1 = 10 mL Concentration of…

Q: Calculate the pH of a solution prepared by adding 25 mL of 0.10 M sodium hydroxide to 30 mL of 0.20…

A: Acetic acid is a weak acid & NaOH is a strong base, pH of the solution depends upon whether…

Q: Calculate the volume of 0.4M of Ba(OH)2 solution must be added to 50ml of 0.3M NaOH in order to…

A:

Q: Calculate the pH when 9.06 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: From the molar equation-   M1: molarity of NaOH solution. V1: volume of NaOH solution. M2: molarity…

Q: Calculate the pH of a solution that is 0.250 MM in sodium formate (HCOONaHCOONa) and 0.110 MM in…

A: The pH of the solution is calculated as shown below where pka value is 3.75. pH=pKa+logSodium…

Q: Determine the pH when 48.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 HCl

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: If 0.050 moles of gaseous HCl is bubbled in 1.0 liter of a solution that is 0.15 M in NH3 and 0.10 M…

A:

Q: Which of the following aqueous solutions has the highest pH? a) 0.10 M HCI b) 0.10 M HCIO c) 0.10 M…

A: Given options are : a). 0.10 M HCl  b). 0.10 M HClO  c). 0.10 M HCl in 0.10 M KCl  d). 0.10 M HClO…

Q: Calculate the pH when 4.91 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: The volume of NaOH solution is 4.91 mL which is equal to 0.00491 L and the volume of acetic acid is…

Q: Calculate the pH of the following solution when the 2 reagents are mixed: 25.00mL of 0.550M KOH…

A:

Q: Calculate the expected pH of a solution created by mixing 30.00 ml of 0.125 M Na(OAc), 20.00 ml of…

A: A solution that contains weak acid and its conjugate base becomes a buffer solution. Buffer…

Q: Calculate the pH of a solution prepared by mixing 150.0 mL of 0.200 M hydrobromic acid and 150.00 mL…

A: Applying concept of molarity and pH  pH = -log [H+]

Q: Calculate the pH when 5.48 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A:

Q: Determine the pH for the following salts in water. Assume that you have a 0.20M solutions of each of…

A: since you have posted a multiple questions in a single session, we are entitiled to answer only…

Q: Calculate the pH of a solution containing 200ml of 0.1M HCl and 8ml of 2.5M sodium acetate.

A: Given data,Molarity of HCl=0.1MVolume of HCl=200mL=0.2LMolarity of CH3COONa=2.5MVolume of…

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

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.