10. Calculate the pH of a solution in which 32.0 ml of 0.150 M KOH has been added to 28.0 ml of 0.100 M HCI.

Q: Calculate the pH of the following solutions. a) 0.400 M HCl solution  b) Solution containing 0.727…

A:

Q: Determine the pH of a solution of KOH (15. mL of 0.020 M KOH) that has been titrated with 10mL of…

A: 1. **Calculate moles of KOH**:   - Moles of KOH = Volume of KOH in liters × Molarity of KOH  - =…

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 when 80.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH)₂.

A:

Q: Calculate the [OH-] and pH of a mixture formed by adding 50.0 mL of 0.0.20 M HCl to 150 mL of 0.010…

A: Given : Concentration of HCl = 0.020 M                                                     (Assuming…

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: 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: A chemist titrates 60.0 mL of a 0.8409M sodium hydroxide (NaOH) solution with 0.1926M HCl solution…

A:

Q: Calculate the pH when 19.15 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: How many grams of CH3COONa must be added to 1.00 L of a 0.100 M CH3COOH solution in order for the pH…

A: The total volume of the solution is 1.00 L. The concentration of CH3COONa in order to have a pH of…

Q: Suppose 0.5 L of 0.02 M HCI was mixed with 0.1 L of 0.1 M Ba(OH)2. Calculate the final pH of the…

A:

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 pH when 32.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBRO (Ka = 2.5 x 10 9)…

A: Given data is as follows: The concentration of KOH =  0.150 M The volume of KOH = 32.0 mL The…

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 made by adding 150 mL of 1.30 M HCl to 350 mL of 1.50 M NH 3…

A: The objective of this question is to calculate the pH of a solution made by mixing two solutions of…

Q: Calculate the pH when 64.0 mL of 0.250 M HCl is mixed with 40.0 mL of 0.150 M Ca(OH)₂.

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: Consider a buffer solution comprised of HF and F. The K₂ of HF is 6.3 x 10-4. If the pH of the…

A: Given here, a buffer solution comprised of HF and F-. we are asked to  calculate the number of moles…

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: Find the pH of a mixture formed by adding 41.0 mL of 2.5×10−2 M  HCl to 170 mL of 1.0×10−2 M  HI.

A: Since both the acids are strong in nature and hence both will dissociate completely producing H+ ion…

Q: 3. Calculate the pH of a mixture of 30.00 mL of 0.4508 M HBr and 18.00 mL of 0.1162 M Ca(OH)2.…

A: Given,Molarity of HBr = 0.4508 MVolume of HBr = 30.00 mLMolarity of Ca(OH)2 = 0.1162 MVolume of…

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: 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 when 25.36 mL of 0.100M NaOH has been added to the original 30.0mL of 0.100M Acetic…

A: Total volume of the solution (VT) after mixing the 25.36 mL of 0.100 M NaOH to 30.0 mL of 0.100 M…

Q: Calculate the pH of a 26 mL of 0.155 M HCI solution titrated with 12.3 mL of 0.07 M NaOH solution.…

A: Volume of HCl = 26 ml = 0.026L Molarity = 0.155M No. Of moles = volume*molarity = 0.026*0.155 =…

Q: Calculate the pH after addition of 10.20 mL of 0.1907 M NaOH to 25.00 mL of 0.1165 M HBr.

A: Given  Volume of NaOH = 10.20 mL Molarity of NaOH = 0.1907 M Volume of HBr  = 25.00 mL Molarity of…

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.