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 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 a solution prepared by adding 25.0 mL of 0.10 M sodium hydroxide to 30.0 mL of…

A:

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 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: Calculate the pH when 19.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: 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: 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: 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 a solution prepared by mixing 5.0 mL of a strong acid solution of pH 4.00 and…

A:

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: 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 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 when 59.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: pH of a solution obtained by mixing of 59.0 mL of 0.150 M KOH with 20.0 mL of 0.300 M HBrO is needed…

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 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…

Q: Calculate the pH of a solution formed by adding 10.0 mL of 0.20 M Benzoic acid to 8.0 mL of 0.30 M…

A: The objective of this question is to calculate the pH of a solution formed by adding a certain…

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Calculate the pH of a solution made by adding 15.0 mL of 0.300 M HCl to 100 mL of 0.450 M NH3…

A:

Q: Calculate the pH of the solution when 35.0 mL of 0.15 M HCN is mixed with 17.5 mL of 0.30 M NaOH. Ka…

A: [NaOH ] = 0.30 M  VNaOH = 17.5 ml  nNaOH = 0.30 M x 17.5ml = 5.25 m mol  [HCN ] = 0.150 M  V HCN =…

Q: Calculate the pH when 29.91 mL of 0.2628 M carbonic acid is mixed with 10.1 mL of 0.1448 M NaOH.

A: For carbonic acid, 29.91 mL of 0.2628 M carbonic acid Ncarbonic acid  = n- factor × M…

Q: What is the pH of a solution prepared by mixing 45.0mL of 0.183 M KOH and 65.0mL of 0.145 M HCL?

A: Moles of HCl = 65 x 10-3 L X 0.145 = 0.009425 mol Moles of KOH = 45 x 10-3 X 0.183 = 0.008235 mol

Q: Calculate the pH of a solution obtained by mixing 438 mL of 0.14 M  nitric acid with 385 mL of…

A:

Q: What is the pH of a solution made by mixing 45.00mL of 0.1256M HCl with 20.00mL of 0.2006M NH3?

A:

Q: A 1.0m HCl solution has a volume of 60.0mL. Calculate pH of the solution that results from adding…

A: Since the moles = concentration X volume in L Hence moles of HCl = concentration of HCl X volume of…

Q: Calculate the pH of the resulting solution when 30.0 mL of 0.500M HBr is added to 25.00 mL of 1.00 M…

A: The reaction of HBr with NaNO2 can be shown by the balanced chemical equation as follows: HBr (aq)…

Q: Calculate the pH of a solution after 47.0 mL of 0.500 M NaOH is titrated with 53.0 mL of 0.250 M of…

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.