A solution is prepared by dissolving 75 g HCl in enough water to make 350 L of solution. the pH of the solution is?

Q: if 0.1L of 0.2 HCL is added to 0.9 L of water what is the resultant pH?

A:

Q: A solution consisting of a strong acid with a concentration of 1721 millimoles has a volume of…

A: Number of moles =1721 millimoles  ...Or because, 1milli = 10-3    so,  = 1721 × 10-3 moles. = 1.721…

Q: the final volume is 1.00 L. Calculate,, and the pH for this solution. [Hint: Concentrated is 38% (by…

A: We are given 49.7mL HCl, 19.1mL nitric acid added in water to make 1 L solution  We have to find pH…

Q: A solution contains 0.160 M sodium cyanide and 0.255 M hydrocyanic acid. The pH of this solution is

A:

Q: When 150.0 mL of a weak base (which can only accept a single proton) were titrated with 0.100 M HCI…

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: calculate the K, of the acid?

A: Given ;-  Initial concentration of monoprotic acid = 0.060 M  pH = 3.44   To calculate ;- Ka

Q: A solution has a pH of 7.6. What does that say about the solution? A) The solution is slightly…

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.2×10-2 M. The hydronium ion…

A: Concentration of OH- in aqueous solution is 3.2*10-2M.

Q: Calculate the pH of each of the following solution? a) 0.10 M HCl b) 0.10 M NaOH

A:

Q: a solution with a pH of 12.0 is

A: Answer to the following question is given as:

Q: Does pH depend on the concentration of the solution? why?

A: Yes the pH of the solution depends on the concentration of acid in it.

Q: A solution contains 0.354 M potassium cyanide and 0.401 M hydrocyanic acid. The pH of this solution…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log SaltAcid…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.4×10-2 M. The hydronium ion…

A:

Q: contains

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

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.