The weak acid HZ has a Ka of 2.55x10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of 0.045 M HZ.

Q: The pH of a solution that contains 0.010 M H3O+ is

A: The concentration of [H3O+] = [H+] = 0.01 M.

Q: The pH of a 1.00 × 10² M solution of cyanic acid (HOCN) is 2.77 at 25.0 °C. Calculate Ka for HOCN…

A: Solution :         The process of dissociation involves the segregation of molecules into smaller…

Q: The pH of a 0.0081 M solution of HNO₃ is

A: Given values-> [HNO3] = 0.0081M HNO3 ---> H^+ + NO3^- [H^+] = 0.0081M pH =-log [H^+] =…

Q: The pH of a 0.0057 M solution of Ca(OH)₂ is

A: Given- Concentration of Ca(OH)2= 0.0057 M

Q: determine the pH of 0.251M acid HA solution. The Ka of the HA is 3.77x10^-7

A:

Q: b. [OH]=1 x 10$ M

A:

Q: The pH of a 0.0084 M solution of HNO₃ is

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: the Ph of a 0.050 M weak acid solution is 5.25. Calculate the Ka of the acid.

A: Given, pH of weak acid= 5.25 [weak acid ] =0.050 M Ka = ?

Q: Calculate the pH and the pOH of 0.78M NaOH

A: NaOH(aq) ---------> Na+ (aq) + OH-(aq) 0.78 M NaOH will give 0.78 M Na+ ions and 0.78 M OH- ions.…

Q: Which of the following has the highest acidity: pH 1, pH 5, or pH 9?

A: To find: Which pH has the highest acidity

Q: calculate the pH of the solution eith an H+1 concentration of 2.90×10-12 and identify the solution…

A: Given,  The concentration of H+ = 2.90 × 10-12 M The pH of the solution is:

Q: What is the pH of a 0.0355M KOH solution?

A: pH can be defined as negative logarithm of concentration of [H+] ions as the KOH is a base first we…

Q: The [H3O+] of a solution is 1.3x10−5, Calculate the [OH−], pH and pOH of the solution. Is the…

A: The given data contains, H3O+=1.3×10-5M

Q: The pH of a 0.10 M solution of formic acid (HCOOH) is 2.39. What is the Ka of the acid?

A: pH is the universal indicator , that not only help in detecting the acidic/ basic character but also…

Q: The pH of a basic solution is 10.59. What is pOH?

A: The sum of pH and pOH for a solution is equal to 14. pH + pOH = 14 Given that,pH = 10.59

Q: calculate the {H3O} of the solution of hydrochloric acid with pH = 2.00

A: Given, PH = 2.00 PH is defined as negative logarithm of concentration of [H+] ions.

Q: When the pH is equal to pKa, the solution is said to be A) Basic [B Charged C. On its stoichiometric…

A: Given : pH and pKa are equal for a solution. To find: Type of solution. Solution: As we know, on the…

Q: If the ?b of a weak base is 5.9×10−6,5.9×10−6, what is the pH of a 0.28 M 0.28 M solution of this…

A:

Q: The pH of a 0.0042 M solution of HNO is

A:

Q: A 0.050 M solution of a weak acid (HA) has a pH of 4.70. What is the Ka of the acid?

A: We will have the below reaction taking place. HA ----> H+ + A- Since pH = -log[H+] where [H+] =…

Q: The pH and pOH of 0.05 M of NaOH is ..

A:

Q: Calculate The pH 0.09M solution of magnesium hydroxide

A:

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

A:

Q: If the pH of a 2.54-cm rainfall over 4600 km is 3.50, how many kilograms of sulfuric acid, HSO4, are…

A: Given: pH of acid rain = 3.50 height of rainfall = 2.54 cm Area of rainfall = 4600 km2

Q: An aqueous solution of 0.40M Mg(C6H5COO)2 has a pH of__________.

A: Given: The concentration of Mg(C6H5COO)2 0.40 M To find: pH Formula:

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: The pH of a 0.0046 M solution of HNO, is

A: Ph is the negative logarithm of the concentration of Hydrogen ion for dilute solutions. Thus, pH is…

Q: Determine the pH of the following solutions, using the information provided. 3.00 × 10–9 M KOH

A:

Q: Determine the pH of each of the following solutions (Ra and K, values are given in Appendix D): (a)…

A: Interpretation: The pH of each solution using given concentration is to be determined.   Concept…

Q: If the [H3O+] concentration is 0.00047M, what is the pH?

A: Given, Concentration of H3O+ ion = [H3O+] = 0.00047 M pH of the solution = ? Note: pH: It can define…

Q: The pH of a 0.0047 M solution of HNO, is

A: As HNO3 is a strong acid, it completely ionises in the solution.

Q: What is the pH of 0.014 M solution of hydroiodic acid?

A: pH is a value that represents the concentration of hydrogen ions in solution. Hydrogen ions in…

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: calculate the ph of the following solution and tellw hether it is acidic, basic, or neutral…

A: Given, [H3O+] = 4.53 ×10-8 M

Q: Calculate the pH of the following solutions.  - 0.10 M pyridine

A:

Q: If you measure the pH of a carbonic acid solution to be 5.6, what is the concenration of the H3O+ in…

A: pH of carbonic acid=  5.6[H3O+ ] = ?

Q: If the pH of a 0.55 M solution of acid is 5.4, what is the KA?

A:

Q: Provided that a chemist prepared a 1.00 M acetic acid solution (HC2H3O2) wherein he found out that…

A: The weak acids are those that partially dissociate in aqueous solution to give protons. The pH is…

Q: Aspirin, which is acetylsalicylic acid, was the first NSAID used to alleviate pain and fever. If a…

A: Introduction If the value of hydronium ion of any particular solution is known then one can easily…

Q: Calculate the [H3O+] of a solution of hydrochloric acid with pH = 1.00 .

A: The relation between pH and [H3O+] is: pH=-log[H3O+]                        ...... (1)

Q: Calculate the pH. 0.5 M H3PO4

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

Q: How many moles of H₃O⁺ or OH⁻ must you add to 5.6 L of HA solution to adjust its pH from 4.52 to…

A: Strong acids and strong bases dissociate completely in their aqueous solution to provide H3O+ and…

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: Calculate the pH of a 0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K.

A: Given  0.20 M solution of HCN, which has a Ka of 4.9×10-10 at 298 K. pH has to be determined for…

Q: The pH of a 0.0071 M solution of HNO3 is

A:

Q: A solution is made by dissolving 0.05700 moles of Ba(OH)2 in enough water to make 330.0 mL of…

A:

Q: Lemon juice has a pH of about 2. What [H3O+] is this?

A: Given that the pH of lemon juice is 2. To calculate the concentration of H3O+ ions in the lemon…

Q: A truck transported 400 liters of HCl approximately 7.4M a) Is it a strong or weak acid? b) What is…

A: According to the Arrhenius theory, the substance that gives hydrogen ion H+ in the aqueous solution…

Q: The weak acid HZ has a Kₐ of 2.55X10⁻⁴.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: For weak acid HZ , pKa = -logKa = -log (2.55 x 10⁻⁴) = 4 -log2.55 = 4 - 0.40 = 3.60 (a)  pH 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.