)What is the pH of a solution composed from 52.0 mL of 0.128 M HCI with 48.0 mL of 0.235 M NaOH?

Q: The pH of a basic solution is 12.03. What is [H⁺]?

A: Given: pH of solution = 12.03

Q: What mass of KOH would need to be dissolved in 500.0 mL of water to produce a solution with a pH of…

A: KOH completely dissociates since it is strong base.Concentration of KOH is determined as follows,

Q: A solution is made by dissolving 0.02500 moles of Ba(OH)2 in enough water to make 750. ml of…

A:

Q: What is the pH of a solution prepared by mixing 75.10 mL of 0.02250 M NaOH with 19.22 ml of 0.08780…

A: Given:Volume of NaOH = 75.10 mLMolarity of NaOH  = 0.02250 MVolume of HCl = 19.22 mlMolarity of HCl…

Q: A concentrated HCl solution contains 36.0% HCl (density of 1.18 g/mL). How many liters are required…

A: pH: The acidity of the solution is given in the term of pH, it is given by negative logarithm of…

Q: The pH of a solution of 0.200 M NaOH is __________.

A: • The values provided in the question are:-     i) Concentration of sodium hydroxide solution,…

Q: What volume (in mL) of 8.84 M HBr would be required to make 300.0 mL of a solution with a pH of…

A:

Q: what is the pH of a solution obtained by mixing 225 mL of 0.680 M HCl with 565 mL of an HCl solution…

A: Here, we have to calculate the pH of a solution obtained by mixing 225 mL of 0.680 M HCl with 565 mL…

Q: A) What is the PH of a solution in which 15 mL of 0.01 M NaOH has been added to 25 mL of 0.1 M HCI?

A:

Q: Calculate the pH value of a prepared solution by mixing 2 mL of a strong acid solution with a pH of…

A: To calculate the pH of the mixture, first of all, we calculate the hydrogen ion concentration of…

Q: The pH of a solution of household ammonia, a 0.950 M solution of NH3, is 11.612. Determine Kb for…

A: We know that, pH can be expressed as the negative logarithm of H+, i.e.            pH = - log[H+]…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

Q: Calculate the pH of a 1.33x10-9 M solution of LiOH.

A: The reaction will be as shown below. LiOH ----> Li+ + OH-  Assuming complete reaction, we can say…

Q: What is the ph of a 0.214 M weak base solution? The Kb of the weak base is 0.000033.

A: Given :-  Concentration of weak base = 0.214 M  Kb = 0.000033  To calculate :-  pH of solution

Q: What is the pH of a 0.00100 M solution of NaOH?

A: Inorganic chemistry.

Q: The pH of a basic solution is 9.93. What is [OH ]?

A:

Q: Calculate the pH of a solution with [H+] = 0.010 M HCI.

A:

Q: 3.3. Calculate the pH of the solution prepared by adding 35.00 mL of 0.4211 M NAOH and 63.00 mL of…

A: (3.3)  Given -  Molarity of strong base, sodium hydroxide, NaOH = 0.4211 M  Volume of NaOH = 35.00…

Q: What is the pH of a 0.105 M solution of acetic acid? What is the percent ionization of the acid?

A:

Q: A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?

A:

Q: The pH of a basic solution is 12.29. What is [OH]?

A: pH + pOH = 14

Q: Students found that a solution sample had a pH of 7. What are the [H*] and [OH-] of this solution?

A: Given :- pH of solution = 7  To calculate :- [H+] and [OH-]

Q: What is the pH of a solution that contains 0.561g of dissolved KOH in 10.0L of aqueous solution?

A: Mass of KOH =0.561 g Volume of solution = 10 L Molar mass of KOH = 56.10 g/mol pH of solution = ?

Q: what is the pH of solution made by adding 22 g of KoH into water and diluting to 250.0 ml?

A: The mass of KOH is 22g. It is dissolved in water to form of 0.250L of solution. The number of moles…

Q: What is the pH of a solution in which 15 mL of 0.27 M NaOH is added to 25 ml of 0.27 M HCl? pH

A:

Q: Calculate the pH of a solution that is 0.00115 M in HCl and 0.0100 M in HClO2.

A: pH is used to determine the concentration of hydronium ion.

Q: The pH of a basic solution is 12.83. What is [OH ]?

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: Which solution would have the higher pH: 0.010 M HNO2 or 0.010 M HNO3? Explain.

A: pH of any solution is defined as negative logarithm of H3O+ or H+ concentration present in solution…

Q: Calculate the pH of a solution prepared by adding 250 mL of 0.0125 M HNO3 to 500.0 mL of 0.0200 M…

A: Acid is defined as a substance that releases hydronium ion when dissolved in water. Acid is…

Q: NH3 is a weak base (Kb=1.8×10−5 M), so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: If 215 ml of a .01M HBr is reacted with 250 ml of a .007M solution of KOH, what is the resulting pH?

A: HBr    +      KOH            →           KBr  +  H2OINITAL         215×.01…

Q: What is the pH of a 100mL aqueous solution containing 0.023g of HOCN.

A: Given, mass of HOCN =0.023 gvolume of solution=100 mL =0.1 Lwe are asked to calculate the pH of the…

Q: The pH of a basic solution is 12.59. What is [OH⁻]?

A: Given: The pH of a basic solution is 12.59 [OH-] is the concentration of hydroxide ion

Q: What is the pH of a solution that is 0.34 M KOCN and 0.14 M HOCN (cyanic acid)?

A:

Q: What is the pH of a solution containing 0.25 M HCOOH and 0.51 M HCOOK?

A:

Q: What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

A: Moles of NaOH and HCl are determined as follows,

Q: What is the pH of (a) a 0.028 M solution of NaOH

A: Given: Concentration of NaOH=0.028M To find: The pH of the solution

Q: The pH of a basic solution is 12.51. What is pOH?

A:

Q: A 1.57 M solution of a weak acid HA is found to have a pH of 2.05.     Determine the pH of a 2.00 M…

A: The concentration of hydrogen ions can be calculated as follows-

Q: What is the final pH of the solution when 10 mL of 0.1 M NaOH is added to 50 mL of 0.05 M HCl…

A:

Q: For a solution of 0.15 M HCl, the [H+] is 0.15 M.  Why?  What is the pH of the solution?

A: pH = -log(H+)

Q: What is the pH of a solution in which 15 mL of 0.15 M NaOH is added to 25 mL of a 0.10 M HCl ?

A: HCl is a strong acid and NaOH is a strong base. The net ionic equation involved in the titration of…

Q: The pH of a basic solution is 12.89. What is [H⁺]?

A:

Q: What is the pH of a solution in which 15 mL of 0.16 M NaOH is added to 25 mL of 0.16 M HCl? pH =

A:

Q: 6 g of LIOH is added to water to make 500 mL of solution. What is the pH?

A:

Q: What is the ph of a 0.00840 M solution of HCi

A: pH is known as power of hydrogen, it is negative logarithm of hydronium ion.

Q: a 0.365g sample of HCl is dissolved in enough water to give 2.00 x 10 ^2 mL of solution. what is the…

A: pH = -log[H+] [H+] = [HCl] = Number of moles of HCl/Volume of solution (L) Number of moles of HCl =…

Q: The pH of a basic solution is 11.43. What is [OH⁻]?

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.