7. Calculate the pH value when 10.0mL of 1.0M HCI is added to the solution in question 5. (pH change=-0.09) JOH 1410

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: For each of the following salts, determine the pH of a 2.50M solution of the salt.  You will need…

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: 2. Calculate the pH of a solution that contains 150 mL of 0.25 M NaF and 252 ml of 0.30 M HF. K, =…

A: Given volume of HF is 252 mL and strength is 0.30 M  Given volume of NaF is 150 mL and strength is…

Q: What is the pH of a solution that contains 0.10 M cyanic acid and 0.20 M sodium cyanate?

A:

Q: 6. Consider the reaction of 50.0 mL of 2.0 M nitric acid with 90.0 mL 1.0 M potassium hydroxide.…

A: The equation of given reaction is,

Q: LIOH+HNO3 → H₂O + Li NO3 200.0 mL of a 0.100 M solution of LiOH is mixed with 250.0 mL of a 0.100 M…

A: The question is based on the titrations. we are titrating a strong acid nitric acid with a strong…

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: To a 150.0 ml solution of 0.100 M NH3 solid NH4Cl is added. What will happen to the pH, [H+], [NH3],…

A: The aqueous solution of ammonia consists of ammonium ions. The dissociation constant of base can be…

Q: Calculate the pH of the resulting solution if 25.0 mL of 0.250 M HCI(aq) is added to 30.0 mL of…

A:

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: What is the pH of a solution obtained by mixing 0.75 L of 0.147 M  Ba(OH)2 and 0.28 L of 0.0660 M…

A:

Q: 4. Calculate the pH of an aqueous solution containing 6.32x109 H3O* ions per liter.

A:

Q: Calculate the pH of the solution that results when 10.0 mL of 0.15 M NaOH is added to 50.0 mL of…

A:

Q: Calculate the pH of the resulting solution if 24.0 mL of 0.240 M HCl(aq) is added to 34.0 mL of…

A:

Q: A 13.6 mL solution of 0.100 mol L-1 CH3COOH is titrated using 0.150 mol L-1 NaOH. What is the pH of…

A:

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: Write the basic equilibrium equation for BrO₃⁻.

A: NOTE: Since you have asked multiple question, we will solve the first question for you. If you want…

Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: What is the pH of a solution of 0.15 M formic acid (HCOOH)? (Ka = 1.8 x 10-4) A 5.57 B 2.37 C) 2.28…

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: For a titration of 50.0 mL of 0.100 M HCl, what is the pH of the solution when 40.0 mL of 0.100 M…

A:

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: How much 0.500 M NaOH should be added to 12.0 g of tris hydrochloride to reach pH 7.77 in a final…

A: Given, Molarity of NaOH = 0.5 MAmount of tris-hydrochloride (T-HCl) = 12 gFinal pH = 7.77Final…

Q: If the bicarbonate ion (HCO3-) concentration in a sample of blood is 0.210 M, determine the carbonic…

A: A buffer is a solution which resists any change in pH on adding a small amount of acid or base.It is…

Q: Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl

A: GIVEN:- Calculate the pH of a solution that contains 0.10 M ammonium hydrochloride and 0.010 M HCl…

Q: 36. Which will have a lower (the lowest) pH among the solutions shown in each of the following…

A: a) 0.001 M NaOH and 0.005 M NaOH  Since NaOH is a strong base hence it will dissociate completely…

Q: Calculate the pH when 62.0 mL of 0.250 M HCI is mixed with 40.0 mL of 0.150 M Ca(OH)2.

A: Given that : The volume of HCl = 62.0 mL The molarity of HCl = 0.250 M The volume of Ca(OH)2 = 40.0…

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: Calculate the pH change that results when 12 mL of 2.1 M HCl is added to 560. mL of each of the…

A: pH change = pH of final solution - pH of initial solution pH = pHfinal - pHinitial

Q: . Calculate the resulting pH when 1.00 L of 1.00 M H,SO4 is added to a tank containing 1.00 × 107 L…

A: The dilution of base solution increases the volume of solution and also alter the 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.