Determine the pH of a 0.031 M solution of Mg(OH)2.

Q: Calculate the pH of a solution in which [OH−]=7.1×10−3M.

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: Calculate the pH of a 6.8 x 10-6 M solution of LiOH

A: Given: Concentration of hydroxide ion =

Q: Determine the pH of each solution and classify it as acidic,basic, or neutral.(a) pOH = 8.5(b) pOH =…

A: We have four solution of  pOH = 8.5, pOH = 4.2,pOH = 1,pOH = 7.0 . We have to calculate pH of each…

Q: Calculate the pH of a 0.01 M solution of hydroxyl amine (K, = 1.1 x 10*).

A:

Q: Determine the pH of an aqueous solution that is 0.078 M in HCIO4 and 0.080 M in HNO3. O 1.5 O 0.98 O…

A: By using the formula of pH and by calculating total H+ concentration we can calculate pH.

Q: Calculate the pH of a 0.0250 M solution of Ba(OH)2.

A: The dissociation of Ba(OH)2 is shown below.

Q: Determine the [OH], [H;O*], pOH and pH of a 0.001 M KOH solution.

A: Given,

Q: Calculate the pH of a 0.041 M Ba(OH)2 solution.

A: pH = -log[H+] [H+][OH-] = 1.0 x 10-14 [H+] = 1.0 x 10-14/ [OH-]

Q: Calculate the concentration of an aqueous solution ofCa(OH)2 that has a pH of 10.05.

A: Since Ca(OH)2 is insoluble salt  hence molar solubility of Ca(OH)2 = concentration of Ca(OH)2 in…

Q: Find the pH of 4.2 X 103 M HClO4.

A: pH can be expressed as the negative logarithm of H+ ion, i.e.                            pH =…

Q: Determine the pH of each of the following solutions.   0.115 MM HClO2

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

Q: What is the pH of a solution that contains 6.13 x 10–4 M OH–?

A: pH measures the acidity of the solution whereas pOH measures the basicity of the solution -

Q: Determine the [OH ], [H3O*], pH and pOH in a 1.0 x 103 M Ba(OH)2 solution.

A:

Q: Calculate the pH of a 0.020 M solution of oxalic acid

A:

Q: Determine the pH of each solution and classify it as acidic, basic, or neutral. (a) pOH = 8.5 (b)…

A:

Q: Calculate the pH of a 1.5 x 10-2 M solution of HBr.

A: The concentration of HBr solution is = 1.5 x 10-2 M The pH of the solution is =?

Q: Calculate the PH of:     II. A "1.8x10-2 molar" solution of an unknown strong base: X (OH) 2

A: Bases have Hydroxide ions(OH-) pH + POH = 14 POH = - log [OH-]

Q: What is the pH of an aqueous solution of 2.70×10² M hydrobromic acid?

A:

Q: What is the pH of a 0.0050 M solution of hydrochloric acid?

A: The pH of a solution is calculated by,

Q: What is the pH of a 7.7 x 10® M KOH solution?

A: Here ,the concentration of KOH is less , so we can not neglect the concentration oh OH- comes from…

Q: determine the pH of a 6 x 10^-5 M HNO3 solution

A: pH is defined as  pH=-log[H +] HNO3 is strong acid so we will calculate pH directly with the above…

Q: determine the pH of a 0.24 M Ca(OH)2 solution

A: Given;

Q: Calculate the pH of a 0.0806 M solution of Ca(OH)2

A:

Q: Determine the pH of a 0.0898 M HCIO4 solution.

A: We have to predict the pH of given solution.

Q: calculate the pH of a 0.10 M perchloric ,HCIO4, solution.

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration, [H+] expressed in mol/L…

Q: Calculate the pH of a solution with a H,O* concentration of: 1.5 x 10 6 M

A: The solution’s pH is equivalent to the negative of the log of H+concentration which is generally…

Q: Determine the pH of a 0.50-M solution of NH4OCl.

A: The question is based on the concept of salt hydrolysis. we have to calculate pH of the given salt…

Q: Find the pH of a 0.337 M aqueous solution of hydrofluoric acid (HF), for which Ka = 6.8 × 10–4.

A: Weak acids :-  Acids which do not undergo complete dissociation and produce very less number of H+…

Q: Calculate the pH of a 0.10 M HNO, solution.

A:

Q: Calculate the pH of a solution that has a hydronium ion concentration, [H,O*], of 4.85 x 10-5 M.

A: The pH of a solution is defined as the -ve logarithm to the base 10 of the value of the hydronium…

Q: Calculate the pH of a 0.0331 M solution of calcium hydroxide.

A: Given  Molarity of Ca( OH )2   = 0.0331 M            PH  = ?

Q: Calculate the pH of a solution in which the molar concentration of H+ is 1.6 x 10-9. a. 1.60 b.…

A: Given information,     Molar concentration of H+ is 1.6 x 10-9.

Q: Calculate the pH of a 0.10 molar solution of sodium formate

A: Acid dissociation constant of formic acid is:  The chemical equation for the reaction involved with…

Q: Determine pH of a solution containing 0.0153 M HClO4 containing 0.105 M NaClO4 .

A: pH = -log[H+]  Given [HClO4]= 0.0153 M

Q: Determine the pH of a 0.285 M solution of NaClO

A: Given : Concentration of NaClO = 0.285 M Since NaClO is a soluble ionic compound. Hence it will…

Q: Determine the [OH'], [H;O*], pOH and pH of a 0.001 M KOH solution.

A: KOH ----> K+  + OH-  [OH-] = [KOH] = 0.001 M [ H3O+ ] = Kw÷ [ OH- ]               = 10-14/0.001 =…

Q: Calculate the pH of a 0.0015 M solution of the strong base Sr(OH)2

A:

Q: Calculate the pH of a solution that has a hydroxide ion concentration, [OH–], of 3.30 x 10-5 M.

A: The acidity or bascity of a solution is defined in terms of pH.pH, mathematically, is -log[H+].…

Q: Determine the pH @ 25 ºC of a solution that has [OH−] = 2.5 x 10−9 M.

A:

Q: Determine the pH of a 0.100 M solution of (NH4)2C2O4.

A: The reaction for the above process can be written as : (NH4)2C2O4 + H2O ------> 2NH4+  +C2O4^2-…

Q: Calculate the pH of a 2.00 M NH,CN solution,

A: NH4CN is a salt made up of weak acid, HCN (Ka = 6.2×10-10) and a weak base NH4OH (Kb = 1.8×10-5).

Q: What is the pH of a 0.0128 M solution of Sr(OH)2 solution?

A: pH can be defined as the potential of the hydrogen. It is the measurement of how acidic or basic the…

Q: The pH of an acidic aqueous solution with a pOH of 9.25

A: Given data is as follows: The pOH of the aqueous solution = 9.25 The pH of the aqueous solution = ?…

Q: Calculate the pH of 0.2 M solution of sodium acetate

A: This is how we can prepare 0.2 M solution. Weigh 27.20 g of Sodium Acetate Trihydrate into a one…

Q: Calculate the pH of a 0.100M solution of arsenic acid, H3AsO4.

A:

Q: Calculate the pH of a 0.250 M solution of Sr(OH)2

A: pH is a measure of how acidic or basic water is. The range goes from 0 to 14, with 7 being neutral.…

Q: Calculate the pH of a 4.3 x 10-3 M solution of HBr

A: pH is negative logarithm of hydrogen ion concentration. HBr is a strong acid meaning it will ionize…

Q: Determine the concentration of a solution of the weak acid HClO2 (Ka = 1.10  10–2)  if it has a pH…

A: Solution :     pH is a quantitative measure to determine the acidity of the solution. It is given as…

Q: determine the pH of an pOH if the concentration of OH is 6.31x10^4 M

A: Given,  Concentration of OH- = [OH-] = 6.31 x 10-4 M  Determine the pH of the solution = ?…

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.