What is the pH of 0.5 M HBr solution?

Q: What is the [H3O+] of a solution if [OH−] is 5.0 × 10−8 M?

A:

Q: What is the hydroxide ion concentration in a solution that has a pOH of 5.70?

A:

Q: What is the pH of a 0.025 M solution of NaOH

A: Applying formula POH = - log[OH-]

Q: Explain why pH of 0.1M HCl is not the same as the pH of 0.1M HF?

A: Answer  Explain why pH of 0.1M HCl is not the same as the pH of 0.1M…

Q: Find the [OH-] and pH of a 0.100 M NH3 solution.

A: It is given that the concentration of ammonia is 0.100 M.

Q: What is the pH of a 0.087 M solution of HCl?

A: Given  [H+]     = 0.087 M  PH       =  ?

Q: What is the pH of a 0.00360 M solution of HCI?

A: Given, [HCl] = 0.00360 M PH is defined as negative logarithm of concentration of [H+] ions.

Q: What is the pH of 0.15325 M COCA COLA solution?

A: What is the pH of 0.15325 M COCA COLA solution?

Q: What is the pH of an aqueous solution if the [H+] = 0.1M?

A: Given Data :  [H+] = 0.1M  To calculate : pH.  Formula : - log [H+]

Q: What is the pH of a * 1x10-4M HCI solution?

A: The pH of a solution is calculated as shown below: pH=-log(H+) The concentration of HCl is given.…

Q: Calculate the pH of a  0.500 M HCN solution.

A:

Q: What is the pH of a 0.25 M solution of NH4+? What is the percent ionization of NH4+?

A: Here we have to find the pH of 0.25 M aqueous NH4^+ solution and have to determine percentage of…

Q: What is the pH of a 6.00 M HBr solution?

A: We know that, pH is the negative logarithm of hydrogen ion concentration. i.e.,…

Q: What is t pH of an aqueous solution that is 2.7 x 10-3 M HCl

A: Given, Concentration of HCl solution = [HCl] = 2.7 x 10-3 M pH of the solution = ? Note:  HCl is a…

Q: What is the pH of a 0.0025M HCl solution?

A: To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion…

Q: What is the pH of a solution with a concentration of 0.00001 moles/ml (M) of H1?

A: Gvien, concentration of 0.00001 moles/ml (M) of H1

Q: What will be the pH of 0.1 M KOH solution?

A: pH is defined as the negative logarithm of [H3O^+] and pOH is defined as the negative logarithm of…

Q: What is the pH of a 0.00645 M HCl solution?

A: pH can be calculated using the following formula. pH = - log [H+]

Q: What is the pH of a 0.00560 M solution of HCl?

A: pH = -log[H+]

Q: What is the theoretical pH of a 0.00001 M HBr solution?

A:

Q: Find the pH of a 0.0025 M HCl solution.

A: Here we are required to find the pH of 0.0025M of HCl solution

Q: What is the pH of a 2.3 x 10-4 M HCl solution?

A:

Q: What is the pH of a .0832 M HCl solution?

A: Here given, Concentration of HCl = 0.0832 M, therefore-- [H+] = 0.0832 M We know, the formula--- PH…

Q: What is the pH of 0.055 M HBr?

A: pH of a solution is given by, pH = -log[H+] pH tells about the acidity of the solution.

Q: What is the pH of 1.7 x 10-5 M HCl solution?

A: To find the pH: Tm concentration of HCl is, 1.7 x 10-5 M

Q: What is the pH of a 0.250 M solution of KOH?

A:

Q: What is the pH of a solution of 3.7 M HBr?

A: We can calculate pH of a solution by using following equation pH = - log [H+]

Q: What is the pH of a 0.005 M aqueous HCl solution?

A: Given, concentration of HCl = 0.005 M HCl is a strong acid . It dissociates Completely in aqueous…

Q: A solution has a pOH = 9.18. Calculate the following: [OH] = M pH = [H,O*] = M

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

Q: What is the [OH-]  in a solution with a pH of 2.50?

A:

Q: What is the pH of a 0.00890 M solution of HCI?

A:

Q: Be sure to answer all parts. An aqueous solution of a strong base has a pH of 10.69 at 25°C.…

A: pH = 10.69  => pOH = 14 - pH = 14 - 10.69 = 3.31  [OH-] = 10-3.31 = 4.9 x 10-4

Q: What is the pH of a 10-¹⁰M NaOH solution?

A:

Q: What is the pH of a 0.020M HBr solution?

A: 4th ans is correct but not the 5th one Since in 4th we have reaction  HBr ----> H+ + Br-  Hence…

Q: Calculate the pH value of 0.5 M NaOH

A: As NaOH is very strong electrolyte i.e base so it will dissociate completely  :…

Q: What is the pH of a 0.00205 M solution of NaOH?

A:

Q: What is the relationship between H+ and OH- concentrations in a solution that has a pH of 11?

A:

Q: What is the concentration of HNO3 if the solution has a pH = 1.24?

A: Given, the pH of the HNO3 solution is =1.24we are asked to calculate the concentration of HNO3

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: Calculate the concentration of OH ions in a HCl solution whose hydrogen ion concentration is 1.40 M.

A: · We have HCl solution.· Hydrogen ion concentration = 1.40 M∘ We need to calculate the concentration…

Q: What is the pH of a 0.15 M hydroiodic acid solution?

A: Given     Concentration  of HI    = 0.15 M                                  PH   =  ?

Q: pH of a 10-2 M HCI solution is: O 12 O-12

A: Full form of pH = potential of hydrogen. It is used to determine acidity or basicity of given…

Q: What is the pH of a 0.025 M solution of HCl?

A:

Q: What is the pH of a 0.00670 M solution of HCl?

A: pH = -log [H+]

Q: What is the pH of a 0.035 M NaOH solution?

A: Given  Molarity of NaOH  = 0.035              PH  = ?

Q: What is the pH of 0.0137 M NaOH? Is the solution neutral, acidic, or basic? The pH is: The solution…

A: Given that,[NaOH] = 0.0137 Mfind the OH- - log [OH-] = pOHpOH = -log [0.0137] = 1.86

Q: pH of a 10 M KOH solution is: O-10 O 10 O-4 4

A: Given , [OH-] = 10-4 M  PH = ? PH is defined as negative logarithm of concentration of H+ ions.

Q: The pH of 0.10M HNO3 is When a solution has pOH = 5.30, the [OH-] is

A: pH = -log[H+]  pOH = -log[OH-]

Q: What is the pH of a 0.0072 M hydrochloric acid solution?

A: Given, Concentration of HCl = 0.0072M. The dissociation of HCl can be given as follows:

Q: What is the pH of a  0.3 M HNO3 aqueous solution?

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.