calculate [OH−] and pH for each of the following solutions. 4.2×10−2 M Na2S .

Q: Calculate the [H+] in a solution that has a pH of 5.66.

A:

Q: Is it possible for a solution to have a negative pH? If so, would that pH signify a basic or acidic…

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Q: Determine the [H+] in a solution with a pH of 4.39.

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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: Indicate whether the solution is acidic, basic or neutral. (Reminder: You must be in pH to…

A: Given :- molar concentration of HCl solution = 3.1 × 10-6 M  To indicate :- nature of solution i.e.…

Q: predict pH when dissolved in water for the following CaO, NaNO2, (NH4)3PO4, LiCl. choices: neutral,…

A: We have to predict the pH of the given salt when dissolved in water.

Q: Find the pH of the following solutions. First write the balanced equilibrium equation of this salt…

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Q: The pH of an aqueous solution at 25°C was found to be 5.60. The pOH of this solution is . The…

A: Note:- according to our guidelines we are supposed to answer only one question.kindly repost other…

Q: Explain why salts can be acidic, basic, or neutral. Write chemical equations to illustrate each…

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: calculate the hydroxide ion concentration of a solution with pH =9.9

A: Given : pH = 9.9  Since , pH + pOH = 14  => pOH = 14 - pH = 14 - 9.9 = 4.1  pOH = - log[OH-

Q: A solution undergoes neutralization reaction. Does the property describe a solution that is acidic ,…

A: When one acidic Solution mixed with another basic Solution, then these two Solutions give a salt and…

Q: Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the…

A: KC3H5O3 is simply nothing but  potassium lactate.  It is conjugate base of Lactic acid  (Weak acid…

Q: Rainwater is found to be slightly acidic compared to pure water. It has a hydrogen concentration of…

A: Given: H+ of rainwater = 10-5.6

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0184 M solution. The pH of the…

A: Acids are the compounds which donate protons, H+ in the solution. Weak acids partially dissociate…

Q: Calculate the [H+] in each of the following solutions, and indicate whether the solution is acidic…

A: Given, [OH-] = 2.32 × 10-4 M [H+] = ? Note: When pH > 7 , solution is basic. When pH = 7 ,…

Q: What are the concentrations of H,O* and OH in oranges that have a pH of 3.837 [H₂O¹] = I [OH-] = M M

A:

Q: Calculate the hydroxide ion concentration of a solution with pH= 2.8

A: Given: pH= 2.8 To find: The concentration of hydroxide ion

Q: ough of a monoprotic weak acid is dissolved in water to produce a 0.0112 M solution. The pH of the…

A: We have given pH and concentration and have to calculate Ka.

Q: A solution has a higher concentration of hydroxide ion then hydrogen ion. Does the property describe…

A: When the solution  has OH- ,hydroxide ion . Then the solution is basic in nature.

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

A: Since the concentration of H+ ions is always ( in any case) = concentration of H3O+  hence [H+] =…

Q: Using data from Appendix D in the textbook, calculate [OH−] and Ph for each of the following…

A: Given data : Concentration of NaBrO = 0.10 MOH-=6.3×10-4 The ICE table for the process is :…

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: (a)ICE table for the reaction is given below.

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0180 M solution. The pH of the…

A:

Q: 2. Calculate the pH of the solution given that the molar hydroxide ion concentration is [OH]= %3D…

A: Given :- [OH-] = 0.000031 M  To calculate :- pH of solution  pH + pOH = 14

Q: Calculate the hydroxide ion concentration of a solution with pH = 6,4.

A: pH of solution is 6.4 We need to determine [OH-]

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.55 M solution. The pH of the…

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Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

A: pH of solution is defined as negative logarithm of hydrogen ions  present in solution.

Q: Calculate the pH of solutions with the following concentrations. [OH−]= 1×10−12M

A: Given, [OH-] = 1 * 10-12 M   Required,                      pH of the solution   First, have to find…

Q: Calculate the pH of a solution if [H*] is measured to be 5.76 x10-9 M. Is this solution acidic or…

A: Given: Concentration of [H+] ion = 5.76×10-9 M

Q: Calculate pH of 0.508 M solution of NaOH

A: By using the relation between pH and pOH we can solve this problem.

Q: If the pH of a solution was 3.12 determine the H3O and the OH of the solution. Is the solution…

A: pH of a solution denotes the amount of hydrogen ion present in the solution. If the pH of the…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.07 M solution. The pH of the…

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.